Note: Organic chemistry is no longer assessed on the APC … Chem summe… · Summer Assignment...

AP Chemistry Dr Kalish

Summer Assignment

Dear Students

Welcome to AP Chemistry a little early We will have a fabulous year together in which

you will be taught everything you need for success in the course and on the AP Chemistry Exam

in May 2015 I apologize for the summer assignment but I want to have at least a month to

review with you prior to the AP Chemistry Exam The assignment is mostly review and NOT

comprehensive of all material covered in honors chemistry I would recommend that you start

the assignment one week before school starts as summer should be reserved for fun

Summer Assignment

1 Read the Chapter 1 notes provided These notes as well as the two other packets

correspond with an older textbook and do not match the chapters in your book perfectly

Complete problems from Hwk 11 (the homework for the three chapters has been

packaged as a unit) and Clwk 11

2 Read the Chapter 2 notes provided Complete problems from Hwk 12 and Clwk

12A and B (12B is NOT available on line) Note Organic chemistry is no longer

assessed on the APC Exam but is assessed on the SAT Chemistry Subject Test 2 so I

have included some information on this concept

3 Read the Chapter 3 notes provided Complete problems from Hwk 13 We will

review this section extensively as stoichiometry is a critical component of APC The

advanced stoichiometry was not covered at the honors or pre-APC level

4 Memorize the chemical symbols for elements on the periodic table (PT) For example

Mg represents Magnesium You can use a PT on every assessment but the name of the

element is NOT listed The periodic table that you will use all year and on the AP

Chemistry Exam is provided in this packet Also included are formula sheets (p 160-

161) which are provided on the APC Exam polyatomic ions which are not and other

pertinent information Please do not lose these sheets You must memorize all of the

polyatomic ions that have been provided

You will take Quiz 11 at the beginning of the second week of school This quiz will assess

material from the summer assignment (ie compound naming formula writing

stoichiometry empirical formula etc NOT kinetics equilibrium etc)

If you have any questions or concerns please email me at jenniferkalishpalmbeachschoolsorg

Have a wonderful and safe summer I look forward to working with all of you next year

Dr Kalish

I

( I () 6t (]i M I 67 Mi (9 71)is 59

iLantrmnidi Scrrs Dv I Ho Er Tm YbCc Pr 16250 II ~J-lB 167 26 16~93 171()-lI I yen11I

I 1291 1i7 07l2(H91I(2()t))

X7 XX

Fr Ra 22 22()J)21227()1

nO

Nd Pm

1)0 l) I )l t9 l()() li)1 IU~

Th Pa Cf Es (m Md Not Aetinide SCI Ci

2J211-l HO-1 (21 L~52) (257) (2~X) (5Q )

no NOT DETACH FROM nOOK

PERIODIC TABL~E OF THE ELElVlENTS

21 )~ 2 24 I 25 I 16 n 2H

- 6 I 7

n C I N HUd Imiddottol

I 1

AI P 1(1(X -(N ~C97

Sc Ti v Cr I Mn I Fe Co Ni 29 30 1 1 H n

Cu Zn Ga Ge As - 9lt1 -I7lt() )()t)-I i~O( )-l9 c +569 6155 6UtJ (912

Jtj 40 41 +~ +3 44 45 6 47 41 9

Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Ml91 9112 tJ2tJI 95)-1 lgtX) 1011 10291 lOll IOiC 112-11 11-1-2 IIX71 12175

51 72 73 74 75 76 77 lX 71) XI) Xl X2 amp1

La I Ht Ta I Re OS Ir Pt Au Hg TI Ph Hi nX91 17H-I9 ISOYi 1K1Xi IX()21 )(12 1922 1950X 19IJ9~P()()591[)-lX

HltJ IOl 10 106 107 lOX 109 1 10 I I I

tAc Rf Ob Sg Bh Hs Vlt Os Rg (261) 1~()2) I (266 I (2b-l11 [277) I (26~) (211) 1(272)

o 1600

16

s 3206 q

Se 71196

52

Te 12760

XJ

Po

I

CI n g 3 iii ltI n g Ul ()

III l Q l1

~ 3 11 ~ n S omiddot l

tv

S tJ

rt

J s ~

CfQ

~ ~ 0

0 CD M gt 4 rt o

r-JPgt )CD 0 ~

(j 0

g gs ct C]

H (lOX

Li 09-1

II

Na 22lt)9

19

K NIO

17

Rb Xil7

55

Cs

Mg ~o

20

Ca OCK

3H

Sr 1-7e

56

B~l

F IC)OO

Ii

el

Yi

Br 7990

5i

I 12691

It)

At 2Jf))

I

Lu 17middot197

1m

Lr 2()2)

lie

10

~e l(lIK

I

Ar

lAS I ~9()l36

Kr X30

54

Xc UI ~9

X6

Rn I (~22)

51

STANDARD REDUCTION POTENTIALS IN AQUEOUS SOLUTION AT 25 c C

Hal f-reaction

) + 2 eshy

+ 1shy

Au + 31shy

K)+2eshy

O(K) + 4H + 41shy

Br2 () + 2

2 Hg2 + 21shy

Hg2+ + 2 eshy

+1

Hg++2eshy

+1

12(~)+2eshy

Cu+ + 1-

Cu 2+ + 21shy

Cu 2+ + 1shy

Sn-+-+2eshy

Sis) + 2 H+ + 21shy

2H++2eshy

Pb2+ + 21shy

Sn 2-+2eshy

Ni 2+ + 21shy

Co 2+ + 2eshy

Cd+ + 21-

Cr+ + 1shy

Fe+ + 21shy

Cr3++3cshy

Zn 2+ + 21shy

2H 20()+ 21shy

Mn 2+ + 21shy

AI)+ + 31shy

Be 2+ + 2cshy

Mg2+ + 21-

Na+ + e-

Ca=- + 2eshy

Sr2+ + 2eshy

Ba + 2eshy

Rb+ + eshy

K+ +eshy

Cs+ + eshy

Li+ + eshy

Au(n

2CIshy

2 HO()

2 Brshy

Hg+

Hg()

Ag(s)

2 Hg()

21shy

curs)

Cuts)

H

H(g)

PhIs)

Sn(s)

Ni(s)

Cots)

Cd(s)

Cr2+

Fe(s)

Cr(s)

Zn(s)

H 2 (g)+20Hshy

vines)

Al(s)

Be(s)

Mgtraquo

Na(s)

Cats)

Sr(s)

Ba(s)

Rb(s)

K(s)

Cs(s)

Lien

287

182

150

136

123

107

092

085

080

079

077

053

052

034

015

015

014

000

013

014

025

028

040

041

044

074

076

083

118

166

170

-237

271

-287

289

290

-292

292

292

-305

GO ON TO THE NEXT PAGE 3

AP Chemistry Course and Exam Description

Appendix B AP Chemistry Equations and Constants

Throughout the test the following symbols have the definitions specified llnles othemise nOled

LmL liter(s) milliliter(s) mm Hg millimeters or menury g gram(s) J kJ jOllle(s) kilojoule(s) nm nanometer( S) V olts)

atm atmosphere(s) mol mole(s)

ATOMIC STRUCTURE E = energy

E = Ill = frequency

=

Plancks constant II = 6626 x 1 J s

Speed of light c = 29l)1 x 108 111 s

ogadro s number = 6022 x I mo)

Electron charge e = 1602 A 10)1 coulomb

EQUILIBRIUM

[C][D]dK = where a A + b B ~ c C + d D

( [A]lrBt

(p ltP ItK = C D

I (P)(P13

K - fOWJlHB h - [B]

K = IWIIOWj = 10 x 1Oj4 at 25degC

pH =-log[WJ pOH [OWl

14 = pH + pOH

_ [A]pH - pK + log rHAl

Equilibrium Constants

K (molar conccntrations)

Ki pressureraquo

K (weak acid)

K1 (weak base)

Kit (waler)

KINETICS

InlAL InfAln = -kr k rate constant

_1_ =kl r =time [Alo rVl halflife

f _ 12 -

0693-k-

Retllrn to the Taj~e 0 Contents

Appendix B

GASES LIQUIDS AND SOLUTIONS

PV IlRT

PA Plot)1 x X where X = mole A

p + Pfl + Pc +

111 11

M

K degc + 273

D= V

1 KE per molecule = - 1111-

Molarity M = moles of solute per liter of olution

A =abc

P == pressure

V = volume

T = temperature

n = number of mole

III == mas

JJ = molar mass

D =- denily

KE kinetic energy

= velocity

A == absorbance

(I = molar absorptivity

h = path length

c = concentration

Gas constant R = 8314 J mol-I

= 008206 L atm mol-I K- 1

== 6236 L torr mol-I K I

I atm = 760 111m

== 760 tOIl

STP == OOOcC and 1000 atm

THERMOCHEUSTRY ELECTROCHEMISTRY

q lIlcfT

fSC I so products -ISo reactants

MIG I JH~ products - I JH reactants

tG C I tGi products -I tGf reactants

-RTln K

1=9 t

q 11

c T

So

He

GO 11

E O

q

Faradays constant F

volt

heat mas specific heat capacity

temperature

lttamlanl entrop

qandard enthalpy

tandard free energy

number of moles

standard reduction potential

current (amperes)

charge (coulombs)

lime (seconds)

96485 coulombs per mole of electrons

I joule [coulomb

Returr to the Table of Corcterts

2013 The College Board

I

i

I

Chemistry Reference Tables Dr Kalish

Activitv Series Polvatomic Ions

I M~tal I Li

Rb

I Sr Ca Na ~Ig

Mil Zn Cr Fe Cd Co Ni Sn Ph II Sb Bi Cu Hg Ag

Pt Au

lOll Name Formula lOll lame Formula 1011 lame Formula i

Acetatc CHCOO Dihvdrogen phosphate HP04 Oxalate C20 4

i Ammonium ~m Hydrogen carbonate or I-ICO Perchlorate U04

i bicarbonate I Arsenate AsO( Hvdrogen sulfate HSOj Pennanganate Mn()j i

Azide N Hydroxide OH Peroxide 0 I Bromate BrCh Hvpochlorite ClO Phosphate P04

i Carbonate CO Iodate 10 Phosphite PO

I Chlorate CIO Iodite 10 Sulfate I SOj Chlorite CIO l1erc ury (l) Hgmiddot Sulfite S( )

Chromate Cre Methvlammonilllll CHNH Thiocvanate seN Cyanide i CN Monohydrogen HPOjmiddotmiddot fhiosull1te SO I

phosphate Dichromate CrOmiddotmiddotmiddot Nitrate NO Uranvl un

Nitrite NO

Important Constants

Avogadros constant I mole = 0022 x 10 atoms

Speed oflight (c) cc- 2991 x ]0 111 S

Plancks constant h 66262 x I J-scc

Prefix Monomiddot Oishy

~

lumber 1 2 I

Trimiddot 1 I f--

T etra-Penta-Hexashy

4 5 6

I

Heptamiddot 7 I Octamiddot 11

Nonashy 9

Oecashy 10

Electroneaativities Atomic Element [lectroIlegathit~ Atomic Element Electronegativity ~umber limber

I It I I 28 Ni 19-shy1 Li 10 29 Cu 19 4 Be 16 30 Zn 16 5 B 20 34 Se 6 6 C 25 35 Hr 10 7 N 30 17 Rb () 11 1 0 34 47 Ag 19 i

9 F 40 4x Cd 17 II -la 09 50 Sn 20 12 Mg 13 51 Sb 20 13 AI 16 53 I 27 14 Si 19 55 Cs OX

15 P ) I 56 Ba 09_shy16 S 20 78 Pt I I_shy17 CI )) shy 79 Au 24 19 K OX 80 Hg 19

20 Ca 10 fP- Pb 18 25 Mn 111 x3 Bi 19

26 Fe 1X 84 Po 20

I n Co 19

i

Reference Tables for 2nd Semester

Table I lsefu I (onstants

Solvent Til I

(0C) ktJ

(nC-kgmole) Tr

(0C) kr(OC-kgmole)

Acctic acid I 17l)O 2530 1666 390 Bellelle 10100 I 253 5533 512 Camphor 20742 5611 17 1 5 ~1 77

Cvelohexltlnc ~O725 275 ()54 2()()

Cvciohexlt1nol -shy -shy 25 i 39

Nitrohcllene 2101 524 57() (152

Phefwl 1l1~W 3MO 40lt)0 740 Wain IOOOO() 0515 O()OO 1153

gatiro - Numbr 6J)22 x 10 panicl Planck OlbWnt Ii 6J262 10 )--c l illi ral Gl- Clhtallt R 001121 L-Jtlll ll1(lle-K or Srd of light (in iKUum) 2)91 x I () 1l sec

R I 14 L-kPa lllok-K lolar Vlull1e (STP) I = 22414 Lnwle Ion rrodut till water f 10 X IOIJ

Table 2 Propertles degfC ~ 0 ventsommon S I

I

a) e peCIIC

Substance TlliS TH eat 0 fCommon Substances at 20(

Specific Heat

(Jig 0c) Table 4- Polvatomic Ions I Of)Air

(J895Aluminum ~

Carh)ll O5()2 (di1I1Hlllti) Carb11 () 71 I ilrarhlte)

(U132Cillholl dinxide Copper O3l7

Ethyl alcohol 245 ()129Gold f)803Granite 0441Iron 012-Lad

29Parutlin 0233

Stainless steel Sihcr

051 Water 4IX

T bl E hi f Fa c nt a rlles 0 ormatIOn Substance ~H n (kJmole) IH -459 NlljCI -3144 NIljFI -125

Substance Hr

HO H-Ol

~Ht (kJimole) -23 -241x2 -2858

Ion -ame Formula Ion ~ame Formula Ion -lame Formula Acetate CH 1COO Dihydrogen phosphate HePO Oxalate C20 1

Ammonium NHj Hydrogen carbonate or bicarbonate

HC01 Perchlorate ClO

Arsenate AsOj Hydrogen sulfate HSOj Pemlananate M1104 Azide N Hydroxide OH Peroxide () -

Borate 80 Hypochlorite CIO Phosphate PO+ Bromate BrO Iodate 10 Phosphite PO Carbonate CO- Iodite 102 Sulfate SOj-Chlorate CIO Mercury (I) Hg2 - Sulfite SO Chlorite C10 Methylammoniul11 ClhNH ThiocYanate SCN Chromate CrOj Monohydrogen

phosphate I HP01shy Thiosu I fate SOshy

Cyanide eN Nitrate NO Lranvl LO-Dichromate (rO-middot Nitrite NO

Table 6 Heats of Fusion and Vaporization for Some Common Substances

-3(l556 -187-

Br

NHNO HO() on - J19ilJH2SOj I

-~155-12076CaCO FeO1 -649 -111-4

CI1 1 bull middot

FcOCaU -52()()

CJ I -1047 -749 lnO-

-il21 916

NcO -1257 IOJ(4II Iltllel

noo-3009 0 iC1H -4142-3935CO NaO

noo -110 I

HgtshyFc Na-SO

(lOn -28so -3629 -3957

HC) HBrJ SOe

middot9U

Substance lIeat of Fusion Heat of (Jg aporization (Jig)

Coppcr i 205 472(

Ell1 I koho 109 gt179

Gold ()45 157i Lead 247 X5S Silcr 88 200 Vater 334 22ltgt0

i

AP Chemi-try Dr Kalish II and P Chapter 1 Page I

Chemistry latter and Measurement

I Introduction

Chemistry enables us to design all kinds of materials drugs (disease) pesticides fertilizers fuels fihers (clothing) building materials plastics etc

A Key Terms

1 Chemistry study of the composition structure properties and reactions of matter a Matter anything that has mass and occupies space

Examples wood sand water air gold ctc

1) llass quantity of matter in an ohject a) use a balance to measure mass the unit on a balance is the gram but the

fundamental unit is the kilogram (kg) 2) Volume space that object occupies

a) use a ruler to measure a regular solid and a graduated cylinder to measure an irregular solid (water displacement) or a liquid

b) the units vary em~ ml L [1 ml = I em]

2 Atoms smallest distinctive units in a sample of matter (huilding blocks)

3 Molecules larger units in which two or more atoms are joined together a The way in which matter hehaves depends on the atoms present and the manner in

which they are comhined

4 Composition types of atoms and their relative proportions in a sample of matter

B Properties

1 Physical property characteristic displayed hy a sample of matter without it undergoing any change in its composition what you can see or measure without altering the chemical nature of the material Examples color mass density state Tm Tr Tb

2 Chemical property characteristic displayed by a sample of matter as it undergoes a change in composition Examples flammability ability to react with acids

C Types of changes

1 Physical change change at the macroscopic level but no change in composition the same substance must remain after the change Examples Phase changes dissolving

AI Chemistry Dr Kalish [I and P Chapter 1 Page

2 Chemical change or chemical reaction change in composition andor the structure of its molecules one or more substances is altered--new substances arc formed Examples cooking and spoiling of foods burning digestion fcnnentation a Reactants -7 Products h Evidence of a Chemical Change

1) Evolution of a gas 2) Fonnation or a ppt 3) Evolution or absorption of heat (exo- vs endothennic reactions) 4) Emission of light 5) Color change

D Classifying latter

1aterial

Homogeneous IVlaterialshy

Substance

Elements Compounds

Homogeneous vlixtures

(Solutions)

Heterogeneous Mixtures

1 Material any specific type of matter a Homogeneous Materials unifonn matter b Heterogeneous Materials nonunifo1111 matter

2 Mixture consists of two or more different atoms or compounds with no fixed composition the atoms or compounds are mixed together physically a Heterogeneous Mixture variable composition andor properties throughout

two or more distinct phases interface Examples blood granite Oil and water

b Homogenous Mixture or Solution has the same composition and properties throughout Examples salt water sugar water

3 Substance type of matter that has a definite or fixed composition that docs not vary from one sample to another Examples Elements or compounds

AP Chemistry Dr Kalish Hand P Chapter 1 Page -

a Element substance that cannot be broken down into other simpler substances by chemical reactions substances composed of one type of atom represented by a chemical symbol

h Compound substance made up of atoms of two or more elements that combine in fixed propoltions or definite ratios represented by a chemical fonnula Example H20 with 111 and 1 0

4 Key differences behveen mixtures and compounds a The properties of a mixture ret1ect the properties of the substances it contains the

properties of a compound bear no resemblance to the properties of the elements that comprise the compound

h Compounds have a definite composition by mass of their combining elements while the components of a mixture may be present in varying propOitions

E Scientific lethods 1 Observation 2 Hypothesis tentative prediction or explanation concerning some phenomenon 3 Experiment procedure used to test a hypothesis

a Data 4 Scientific Laws summary of patterns in a large collection of data 5 Theory multi-tested and contlnned hypothesis

II Scientific Measurement A International System of lnits

1 Length the SI base unit is the meter 1 Mass the quantity of matter in an object

a SI base unit is the kilogram 3 Time SI base unit is the second 4 Temperature property that tells us in what direction heat will t10w

a S I base unit is Kelvin (K)

Seven Fundamental Units ill Sf IQllautity

I Symholfi)1 qlumti(r

lnit I Abbreviation for unit i i

Length meter 111

Mass III kilogram kg Time r second s Them10dvnamic Temperature T kelvin K Amount of Substance 11 mole mol Electric Current [ ampere A Luminous Intensity 1 candela cd

AP Chemistry Hand P Chapter I

B

254 centimeters = I in 12 inches 1 foot 3 feet = 1 yard 5280 feet = 1 mile 1 meter = 3937 inches I metcr 109 yards 1 km 062 miles

Problems

sityDen 1 mass per unit volume of a substance

d=mV

Density of water is 100 giml

Problems

Common Sf prefixes Prefix lnit abbreviation I Exponential1 ultiplier

i

GiEa- G 10

Megashy lvl 10 bull Kilo- k 10

Hectoshy h lO-

Decashy da 10 1

10 decishy d 10

centi shy c 1crshymillishy m H)

micro- Jl 10(

i nanoshy n 10

pleoshy p 10 1

femtoshy f 10

i

Jfea 11 illJ( I

I 000 000 000 i

t 000 000 1000

tOO

10 1

1 ]0

1 I U()

1 1000

1 1 000000

I 1 000 000 000

I 1 000 000 000 000

1 I 000 000 000 000 000

C Conversions within the same quantity vs those behYeen different quantities I Same Quantity

2 Different Quantities Factor-Labelllethod or Dimensional Analysis

Eq utllities and Collversioll Factor

2 cups== 1 pint 2 pints 1 quart 4 cups 1 quart 1 liter = 106 quarts 16 ounces = I pound I molc= 6022 x 1O~i awm

31 ml 1 cm

Dr Kalish Page 4

~ -Lowcst density

Greatest density

shy

283 gramsmiddot= 1 ounce 1 kilogram = 22 pounds 4536 g = J lb 2835 g I ounce 3785 L = 1 gal 2957 ml I tl oz

AP Chemistry Dr Kalish Hand P Chapter 1 Page )

D Precision and Accuracy in Measurements I Precision how closely individual measurements agree with one another 2 Accuracy closeness of the average of the set to the correct or most probable value

Precise measurements are 1OT always accurate Example Darts--Ifyou hit the same spot outside the bulls-eye five times you have precision but not accuracy You are accurate vhen you hit thc bulls-eye

Percent Error =~(Measured Value -Accepted VaIUC) I 00 1 Accepted Value

Eo Significant Figures I All digits known with certainty plus the tirst uncertain one (estimated) arc significant

digits or significant figures 2 Significant figures reflect the precision of the measurement 3 D S degfi 19ltsetermmmg Igm Icant D

Number Digits to Count Example Number of Significant Digits

i All ionzero Digits 3279 4 ~ )112

i

None 0()O45

before an integer) Leading Zeroes (zeroes

OO()OOO5 1

Captive Zeroes (zeroes All 5007 4 between two integers) 6f)OOOm~ 7

Counted only if the 100Trailing Zeroes (zeroes I after the last integer) number contains a 100 3

decimal point 1000 4 )00100

17 x 10-1Scientific Notation All BCT be careful 2 of incolTcctly 130 x l((~ 3

0(0) x 10written scicntitic 1 notatilll1

4 Rules a vIultiplying and Dividing Round the calculated result to the same number of

significant figures as the measurement having the least number of significant figures [carryall numbers through and then round oft]

2Example 345 cm 45555 cm -7 157 cm (Answer is expressed in 3 significant figures)

P Chemistry Dr Kalish Hand P Chapter 1 Page 6

b Addition and Subtraction The answer can have NO more digits to the right of the decimal point than there are in the measurement with the smallest number of digits to the right of the decimal point Example 345 cm + 1001 em ~ 1036 em (Express answer to the tenth place)

c Rounding Fives If the last significant digit before the five is odd round up If the last significant digit before the five is even (and therc are not any numbers other than zero after the tive) do NOT round up (leave it alone) Example 315 ~ For two significant digits or to the tenth place round to ]2 Example 345 ~ For tVO significant digits round to 34 Example 3451 ~ For two signiticant digits round to 35

28 Chapter 1 Chemistry Matter and Measurement

Matter is made up of atoms and molecules and can be subdivided into two broad catshyegories substances and mixtures Substances have fixed compositions they are either eleshyments or compounds Compounds can be broken down into their constituent elements through chemical reactions but elements cannot be subdivided into simpler substances Mixtures are either homogeneous or heterogeneous Substances can be mixed in varying proshyportions to produce homogeneous mixtures (also called solutions) The composition and properties are uniform throughout a solution The composition andor properties of a hetshyerogeneous mixture vary from one part of the mixture to another

Substances exhibit characteristics called physical properties without undergoing a change in composition In displaying a chemical property a substance undergoes a change in composition-new substances are formed A physical change produces a change in the appearance of a sample of matter but no change in its microscopic structure and composishytion In a chemical change the composition andor microscopic structure of matter changes

Four basic physical quantities of measurement are introduced in this chapter mass length time and temperature In the SI system measured quantities may be reported in the base unit or as multiples or submultiples of the base unit Multiples and submultiples are based on powers of ten and reflected through prefixes in names and abbreviations

nanometer(nm) micrometer (fLm) millimeter (mm) meter(m) kilometer (km) 10-9 m 1O-6 m 10- 3 m m 103 m

The SI base unit of temperature the kelvin (K) is introduced in Chapter 5 but in this chapter two other temperature scales Celsius and Fahrenheit are considered and compared

tF = 18 tc + 32 tc = ------shy18

To indicate its precision a measured quantity must be expressed with the proper numshyber of significant figures Furthermore special attention must be paid to the concept of sigshynificant figures in reporting calculated quantities Calculations themselves frequently can be done by the unit-conversion method The physical property of density also serves as an imshyportant conversion factor The density of a material is its mass per unit volume d = mV When the volume of a substance or homogeneous mixture (cm3

) is multiplied by its densishyty (glcm volume is converted to mass When the mass of a substance or homogeneous mixshyture (g) is multiplied by the inverse of density (cm3g) mass is converted to volume

In this chapter and throughout the text Examples and Exercises illustrate the ideas methods and techniques under current discussion In addition Estimation Examples and acshycompanying Exercises deal with means of obtaining estimated answers with a minimum of calculation Conceptual Examples and accompanying Exercises apply fundamental conshycepts to answer questions that are often of a qualitative nature

1

1

1

A inl yo pil pn de tic PI

AP Chemistry Dr Kalish Summer Assignment

Homework Problems Note Numbers in the left margin correspond with book problems from the PH textbook and your answer key Hwk 11 Chapter 1 1) Which of the following are examples of matter

a) Iron b) Air

c) The human body d) Red light

e) Gasoline f) An idea

2) Which of the following is NOT a physical property a) Solid iron melts at a temperature of 1535 oC b) Solid sulfur as a yellow color

c) Natural gas burns d) Diamond is extremely hard

3) Which of the following describe a chemical change and which a physical change a) Sheep are sheared and the wool is spun into

yarn b) A cake is baked from a mixture of flour

baking powder sugar eggs shortening and milk

c) Milk sours when left out d) Silkworms feed on mulberry leaves and

produce silk e) An overgrown lawn is mowed

4) Which of the following represent elements Explain a) C b) CO

c) Cl d) CaCl2

e) Na f) KI

5) Which of the following are substances and which are mixtures Explain a) Helium gas used to fill a balloon b) Juice squeezed from a lemon

c) A premium red wine d) Salt used to de-ice roads

6) Indicate whether the mixture is homogeneous or heterogeneous a) Gasoline b) Raisin pudding

c) Italian salad dressing d) Coke

7) Convert the following quantities a) 546 mm to meters b) 876 mg to kg

c) 181 pm to microm d) 100 h to micros

e) 463 m3 to L (careful) f) 55 mih to kmmin

8) How many significant figures are there in each of the following quantities a) 4051 m b) 00169 s

c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC

9) Perform the indicated operations and provide answers in the indicated unit with the correct number of significant digits a) 1325 cm + 26 mm ndash 78 cm + 0186 m (in cm) b) 48834 g + 717 mg ndash 0166 g + 10251 kg (in kg)

10) Calculate the density of a salt solution if 500 ml has a mass of 570 g 11) A glass container has a mass of 48462 g A sample of 400 ml of antifreeze solution is added and the container

with the antifreeze has a mass of 54513 g Calculate the density of the antifreeze solution expressed in the correct number of significant figures

12) A rectangular block of gold-colored material measures 300 cm x 125 cm x 150 cm and has a mass of 2812 g Can the material be gold if the density of Au is 193 gcm3 Calculate the percent error

Hwk 12 Chapter 2 1) When 243 g of magnesium is burned in 160 g of oxygen 403 g of magnesium oxide is formed When 243 g

of magnesium is burned in 800 g of oxygen (a) What is the total mass of substances present after the reaction (b) What mass of magnesium oxide is formed (c) What law(s) isare illustrated by this reaction (d) If 486 g of magnesium is burned in 800 g of oxygen what mass of magnesium oxide is formed Explain

2) What is the atomic nucleus Which subatomic particle(s) isare found in the nucleus 3) Which of the following pairs of symbols represent isotopes Which are isobars

a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22

4) What do atomic mass values represent 5) What type of information is conveyed by each of the following representations of a molecule

2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)

AP Chemistry Dr Kalish Summer Assignment Page 2

a) Empirical formula b) Molecular formula c) Structural formula 6) A substance has the molecular formula C4H8O2 (a) What is the empirical formula of this substance (b) Can

you write a structural formula from an empirical formula Explain 7) Are hexane and cyclohexane isomers Explain 8) For which of the following is the molecular formula alone enough to identify the type of compound For which

must you have the structural formulas a) An organic compound b) A hydrocarbon

c) An alcohol d) An alkane

e) A carboxylic acid

9) Explain the difference in meaning between each pair of terms a) A group and period on the periodic table

(PT) b) An ion and ionic substance

c) An acid and a salt d) An isomer and an isotope

10) Indicate the numbers of electrons and neutrons in the following atoms a) B-11 b) Sm-153

c) Kr-81 d) Te-121

11) Europium in nature consists of two isotopes Eu-151 with a mass of 15092 amu and a fractional abundance of 0478 and Eu-153 with a mass of 15292 amu and a fractional abundance of 0522 Calculate the weighted average atomic mass of Europium

12) The two naturally occurring isotopes of nitrogen are N-14 with an atomic mass of 14003074 amu and N-15 with an atomic mass of 15000108 amu What are the percent natural abundances of these isotopes Hint set one at x and the other at 1-x

13) The two naturally occurring isotopes of rubidium are Rb-85 with an atomic mass of 8491179 amu and Rb-87 with an atomic mass of 8690919 amu What are the percent natural abundances of these isotopes Hint set one at x and the other at 1-x

14) Identify the elements represented by the following information Indicate whether the element is a metal or nonmetal a) Group 3A (13) period 4 b) Group 1B (3) period 4 c) Group 7A (17) period 5

d) Group 1A (1) period 2 e) Group 4A (14) period 2 f) Group 1B (3) period 4

15) Write the chemical symbol or a molecular formula for the following whichever best represents how the element exists in the natural state a) Chlorine b) Sulfur

c) Neon d) Phosphorus

e) Sodium

16) Which of the following are binary molecular compounds a) Barium iodide b) Hydrogen bromide

c) Chlorofluorocarbons d) Ammonia

e) Sodium cyanide

17) Write the chemical formula or name the compound a) PF3 b) I2O5 c) P4S10

d) Phosphorus pentachloride

e) Sulfur hexafluoride

f) Dinitrogen pentoxide

18) Write the chemical symbol or name for the following monatomic ions a) Calcium ion b) Cobalt(II) ion

c) Sulfide ion d) Fe3+

e) Ba2+ f) Se2-

19) Write the chemical formula or name for the following polyatomic ions a) HSO4

- b) NO3

- c) MnO4

-

d) CrO42-

e) Hydrogen phosphate ion

f) Dichromate ion g) Perchlorate ion h) Thiosulfate ion

20) Name the following ionic compounds a) Li2S b) FeCl3 c) CaS d) Cr2O3 e) BaSO3

f) KOH g) NH4CN h) Cr(NO3)3 9H2O i) Mg(HCO3)2 j) Na2S2O3 5H2O

k) K2Cr2O7 l) Ca(ClO2)2 m) CuI n) Mg(H2PO4)2 o) CaC2O4 H2O

21) Write the chemical formula for the following ionic compounds a) Potassium sulfide b) Barium carbonate

c) Aluminum bromide hexahydrate

d) Potassium sulfite e) Copper(I) sulfide

20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)


f) Magnesium nitride g) Cobalt(II) nitrate h) Magnesium dihydrogen

phosphate

i) Potassium nitrite j) Zinc sulfate

heptahydrate

k) Sodium hydrogen phosphate

l) Iron(III) oxide

22) Name the following acidsa) HClO(aq)

b) HCl(aq) c) HIO4(aq)

d) HF(aq) e) HNO3(aq) f) H2SO4(aq)

g) H2SO3(aq) h) H2C2O4(aq)

23) Write the chemical formula for the following acids a) Hydrobromic acid b) Chlorous acid c) Perchloric acid d) Nitrous acid

e) Acetic acid f) Phosphorous acid g) Hypoiodous acid h) Boric acid

Hwk 13 Chapter 3 1) What are the empirical formulas of the compounds with the following molecular formulas

a) H2O2 b) C6H16

c) C10H8 d) C6H16O

2) Calculate the molecular or formula mass of the following a) C2H5NO2 b) Na2S2O3 c) Fe(NO3)3 9H2O

d) K3[Co(NO2)6] e) Chlorous acid f) Ammonium hydrogen phosphate

3) Calculate the mass in g of the following a) 461 mol AlCl3 b) 0314 mol HOCH2(CH2)4CH2OH

c) 0615 mol chromium(III) oxide

4) Calculate the mass percent nitrogen in the compound having the condensed structural formula CH3CH2CH(CH3)CONH2

5) Calculate the mass percent of beryllium in the mineral Be3Al2Si6O18 Calculate the maximum mass of Be obtainable from 100 kg of Be

6) The empirical formula of apigenin a yellow dye for wool is C3H2O The molecular mass of the compound is 270 amu What is the molecular formula

7) Resorcinol used in manufacturing resins drugs and other products is 6544 C 549 H and 2906 O by mass Its molecular mass is 110 amu What is the molecular formula

8) Sodium tetrathionate an ionic compound formed when sodium thiosulfate reacts with iodine is 1701 Na 4746 S and 3552 O by mass The formula mass is 270 amu What is its formula

9) A 00989 g sample of an alcohol is burned in oxygen to yield 02160 g CO2 and 01194 g H2O Calculate the mass percent composition and empirical formula of the compound

10) Balance the following equations a) TiCl4 + H2O TiO2 + HCl b) WO3 + H2 W + H2O c) C5H12 + O2 CO2 + H2O d) Al4C3 + H2O Al(OH)3 + CH4

e) Al2(SO4)3 + NaOH Al(OH)3 + Na2SO4 f) Ca3P2 + H2O Ca(OH)2 + PH3 g) Cl2O7 + H2O HClO4 h) MnO2 + HCl MnCl2 + Cl2 + H2O

11) Write a balanced chemical for each of the following a) Decomposition of solid potassium chlorate upon heating to generate solid potassium chloride and oxygen

gas b) Combustion of liquid 2-butanol c) Reaction of gaseous ammonia (NH3) and oxygen gas to generate nitrogen monoxide gas and water vapor d) The reaction of chlorine gas ammonia vapor and aqueous sodium hydroxide to generate water and an

aqueous solution containing sodium chloride and hydrazine (N2H4 a chemical used in the synthesis of pesticides)

12) Toluene and nitric acid are used in the production of trinitrotoluene (TNT) an explosive ___C7H8 + ___HNO3 ___C7H5N3O6 + ___H2O

a) What mass of nitric acid is required to react with 454 g of C7H8 b) What mass of TNT can be generated when 829 g of C7H8 reacts with excess nitric acid

13) Acetaldehyde CH3CHO (D = 0789 gml) a liquid used in the manufacture of perfumes flavors dyes and plastics can be produced by the reaction of ethanol with oxygen gas

8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)


___CH3CH2OH + ___O2 ___ CH3CHO + ___H2O a) How many liters of liquid ethanol (D = 0789 gml) must be consumed to generate 250 L acetaldehyde

14) Boron trifluoride reacts with water to produce boric acid and fluoroboric acid 4BF3 + 3H2O H3BO3 + 3HBF4 a) If a reaction vessel contains 0496 mol BF3 and 0313 mol H2O identify the limiting reactant b) How many moles of HBF4 should be generated

15) A student needs 625 g of zinc sulfide a white pigment for an art project He can synthesize it using the reaction Na2S(aq) + Zn(NO3)2(aq) ZnS(s) + 2NaNO3(aq) a) What mass of zinc nitrate will he need if he can make the zinc sulfide in a 850 yield

16) Calculate the molarity of each of the following aqueous solutions a) 250 mol H2SO4 in 500 L solution b) 0200 mol C2H5OH in 350 ml of solution c) 4435 g KOH in 1250 ml of solution d) 246 g oxalic acid in 7500 ml of solution e) 2200 ml triethylene glycol (CH2OCH2CH2OH)2 (D = 1127 gml) in 2125 L of solution f) 150 ml isopropylamine CH3CH(NH2)CH3 (D = 0694 gml) in 225 ml of solution

17) A stock bottle of nitric acid indicates that the solution is 670 HNO3 by mass (670 g HNO31000 g solution) and has a density of 140 gml Calculate the molarity of the solution

18) A stock bottle of potassium hydroxide solution is 500 KOH by mass (500 g KOH1000 g solution) and has a density of 152 gml Calculate the molarity of the solution

19) If 5000 ml of 191 M NaOH is diluted to 200 L calculate the molarity of NaOH in the diluted solution

74) 82) 84) 89) 90) 92)

AP Chemistry Dr Kalish Clwk 11 Page 1

Date Period

Matter--Substances vs 11ixtures

All matter can be classified as wither a substance (element or compound) or a mixture (heterogeneous or homogeneous)

Directions Classify each of the following as a scompound in the substance column mixture column

ubstance or a mixture Ifit is a mixture writ

If it is a substance write element or a e heterogeneous or homogeneous in the

Mixture

cream

Physical vs Chemical Changes

In a physical change the original substance still exists It has changed in form only In contrast a new substance is produced when a chemical change occurs Energy always accompanies chemical changes

Directions Classify each of the follOving as a chemical (C) or physical (P) change

I Sodium hydroxide dissolves in water

2 Hydrochloric acid reacts with potassium hydroxide to produce a salt water and heat

3 A pellet of sodium is sliced in two

4 Water is heated and changed to steam

5 Potassium chlorate decomposes to potassium chloride and oxygen gas

6 Iron rusts

7 When placed in water a sodium pellet catches on tire as hydrogen gas is liberated and sodium hydroxide forms

8 Evaporation

9 Ice Melting

10 Milk sours

5


11 Sugar dissolved in water

12 Wood rotting

13 Pancakes cooking on a griddle

14 Grass growing in a lawn

15 A tire is intlated with air

16 Food is digested in the stomach

17 Water is absorbed by a paper towel

Physical vs Chemical Properties

A physical property is observed with the senses and can be determined without destroying the object For example color shape mass length and odor are all examples of physical properties A chemical property indicates how a substance reacts with something else The original substance is altered fundamentally when observing a chemical property For example iron reacts with oxygen to form rust which is also known as iron oxide

Directions Classify each of the following properties as either chemical or physical by denoting with a check mark

Physical Property Chemical Property

I Blue color 2 DeI1~ity 3 Flammability 4 Solll~ili~y

Reacts with acid to form He

6 llPPI~ combustion -

7 Sour taste

_ 8 ~J~I~il1g Point 9 Reacts with water to form a gas 10 Reacts with base to form water II Hardness 12 Boiling Point 13 Can neutralize a base 14 Luster IS Odor

AI Chemistry Dr Kalish Ii and P Chapter 2 Page 1

Atoms lo1ecules~ and Ions

I Las and Theories A Brief Historical Introduction A Laws of Chemical Combination

I Lavosier (1743-1794) The Law of Conservation of 11 ass a The total mass remains constant during a chemical reaction

Example HgO ~ IIg -+ O2

Mass of reactants = Mass of products

) Proust (1754-1826) The Law of Constant Composition or Definite Proportions a All samples of a compound have the same composition or the same proportions

by mass of the elements present Example NaCI is 3934 lia and 6066 CI

Example OMg in MgO is 06583 I What mass ofMgO will faTIn when 2000 g Mg is converted to MgO by buming in pure 02

2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO

B John Dalton (1766-1844) and the Atomic Theory of Matter (1803) 1 Law of Vlultiple Proportions

a When two or more different compounds of the same two elements are compared the masses of one element that combine with a fixed mass of a second element are in the ratio of small vhole numbers Examples CO vs CO2 S02 s SO

2 Atomic Theory a All matter is composed ofetreme~v small indivisible particles called atoms b All atoms ofa given clement are alike in mass and other properties but atoms of

one clement differ from the atoms of every other element c Compounds are fanned when atoms of different elements unite in fixed

proportions d A chcmical reaction involvcs a rearTangemcnt of atoms lio atoms are creatcd

destroyed or broken apart in a chemical reaction

Examples

3 Dalton used the Atomic Theory to restate the Lav of Conservation of Mass Atoms can neithcr be created nor destroyed in a chcmical rcaction and as a consequence the total mass remains unchangcd

AP Chemistry Dr Kalish Hand P Chapter Page

C The Divisible Atom I Subatomic Particles

a Proton 1) Relative mass = 1 2) positive electrical charge

b Neutron I) Relative mass 1 (although slightly greater than a proton) 2) no charge == 0

c Electron 1) mass = I 1836 of the mass of a proton 2) negative electrical charge -I

Particle I Symbol Approximate Relative llass

Relative Charge

Location in Atom

Proton p 1 I Inside nucleus Neutron n L 0 Inside nucleus Electron e 0000545 1shy Outside nucleus

1 An atom is neutral (has no net charge) because p = e- t The number of protons (Z) detennines the identity of the element 4 Mass number (A)== protons + neutrons

a neutrons A - Z

Example ticr Detennine the number ofp e- and n

5 Isotopes atoms that have the same number of protons but different numbers of neutrons Examples IH 2H 3H [or H-J H-2 H-3J 32S S 5l)CO 6JCO

6 Isobars atoms with the same mass number but different atomic numbers 1-1 H [a ExampIe C N

D Atomic Masses 1 Dalton arbitrarily assigned a mass number to one atom (H-l) and detennined the

masses of other atoms relative to it 2 Current atomic mass standard is the pure isotope C-12 3 Atomic mass unit (amu) l12themassofC-12 4 Atomic Mass weighted average of the masses of the naturally occurring isotopes of

that element a Example Ne-20 9051 1999244 u

Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u

AP Chel1li~try Dr Kalish II and P Chapter 2 Page J

E The Periodic Table I Dmitri Mendeleevs (1869) Periodic Table

a Arranged elements in order of increasing atomic mass from left to right in ros and from top to bottom in groups

b Elements that most closely resemble each other are in the same vertical group (more important than increasing mass)

c The group similarity recurs periodically (once in each row) d Gaps for missing clements predict characteristics of yet to be discovered

clements based on their placement 2 Modern Periodic Table

a Elements are placed according to increasing atomic number b Groups or Families vel1ical columns c Periods horizontal roVS d Two series pulled out

1) Lanthanide and Actinide Series e Classes

1) Most elements arc Metals which are to the len (NOT touching) the stair-step line a) luster good conductors of heat and electricity b) malleable (hammered into thin sheets or f()il) ductile (drawn into wires) c) Solids at room temperature (except mercury)

2) Nonmetals are to the right (NOT touching) of the stair-step line a) poor conductors of heat and electricity b) many are gases at RT

3) Metalloids touch the vertical and or horizontal of the stair-step line (except Al and Po

11 Introduction to Vlolecular and Ionic Compounds A Key Terms

1 Chemical Symbols are used to represent clements 2 Chemical F0l111Ulas are used to represent compounds

a Subscripts indicate how many atoms of each element are present or the ratio of Ions

B Molecules and Molecular Compounds I Molecule group of two or more atoms held together in a definite spatial arrangement

by covalent bonds ) Molecular Compound molecules arc the smallest entities and they detennine the

propcI1ies of the substance 3 Empirical Formula simplest fOl111Ula for a compound

a indicates the elements present in their smallest integral ratio Example CH~O = 1 C 2 H 10

4 Molecular Formula true fonnula for a compound n = MFmassEFmassl a indicates the elements present and in their actual numbers

Example C6Hl~06 = QC 12 H Q0 5 Diatomic Elements two-atom molecules which dont exist as single atoms in nature

a Br~ h N2 Ch Hgt O2bull F~ 6 Polyatomic Elements many-atom molecules

AP Chemitry H 3nd P Chapter 2

Dr Kalish Page --l

a Sg P-l 7 Structural Formulas shows the alTangement of atoms

a lines represent covalent bonds between atoms

C Writing Formulas and Names of Binary Molecular Compounds I Binary Molecular Compounds comprised of 10 elements which are usually

nonmctals a The first element symbol is usually the element that lies farthest to the lcft of its

period andlor lowest in its group (exceptions Hand 0) [Figure 27] b Molecular compounds contain prefixes far subscripts (exception mono is not

used far the first element) c The name consists of two ords

(prefix) element prefix~ide fonn

rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i

tetrashy 4 pcntashy hexashy f

heptashy 7 octashy 8

110113shy 9

dec ashy 10 i

D Ions and Ionic Compounds 1 Ion charged particle due to the loss or gain of one or more electrons

a 1onatomic Ion a single atom loses or gains one or more eshy1) use the PT to predict charges 2) more than one ion can fann with transition elements

b Cation positively charged ion [usually a metal] c Anion negatively charged ion [usually a nonmetal] d Polyatomic Ion a group of covalently bonded atoms loses or gains one or more

e e Ionic Compounds comprised of oppositely attracted ions held together by

electrostatic attractions no identifiable small units 2 Formulas and Names for Binary Ionic Compounds

a Cation anion (~ide fonn) b Cation (Roman Numeral) anion (-ide fann)

3 Polyatomic Ion charged group of bonded atoms a suftixes are often -ite (1 less 0) and ~ate b prefixes arc often hypo- (1 less 0 than ~ite fonn) and per-( 1 more 0 than -~atc

fann) c Example Hypochlorite CIO

Chlorite CI02shy

Chlorate ClO Perchlorate CIO-lshy

4 Hydrates ionic compounds in which the tonnula unit includes a fixed number of water molecules together with cations and anions a Example CaCI 2 6H20 Calcium chloride hexahydrate

AP Chemistry Dr Kalish II and P Chapter 2 Page

b Anhydrous without water

Acids Bases and Salts 1 Basic Characteristics of Acids and Bases when dissolved in water

a Acids I) taste sour 2) sting or prick the skin 3) turn litmus paper red 4) react with many metals to produce ionic compounds and fllgi

5) react with bases b Bases

1) taste bitter 2) feel slippery or soapy 3) turn litmus paper blue 4) react with acids

2 The Arrhenius Concept ( 1887) a Acid molecular compound that ionizes in water to form a solution containing If

and anions b Base compound that ionizes in water to tltmn a solution containing OH- and

cations c Neutralization the essential reaction betvmiddoteen and acid and a base called

neutralization is the combination of H - and OH- ions to fonn vater and a salt 1) Example HCl NaOH -7 iaCli- HO

3 Formulas and ~ames of Acids Bases and Salts a Arrhenius Bases cation hydroxide

1) Examples NaOH = Sodium hydroxide KOH Potassium hydroxide Ca(OHb Calcium hydroxide

b 1olecular Bases do not contain OH- but produce them when the base reacts with water 1) Example NIh = Ammonia

c Binary Acids H combincs with a nonmetal 1) Examples HCl1g1 = Hydrogen chloride HCl1a4 )= Hydrochloric acid

HI1gi = Hydrogen iodide HI1lt141 = Hydroiodic acid HSlg) Hydrogen sulfide HS (aql Hydrosulfuric acid

d Ternary Acids FI combines with two nonmetals 1) oxoacids H combines with 0 and another nonmetal

a) Examples Hypochlorous Acid HCIO Chlorous Acid 11CIO Chloric Acid HCI03 Perchloric Acid HCIO-1 Sulfurous Acid H2S03

Sulfuric Acid H2S04

b) ate-ic ite-ous

AP Chemistry Dr Kalish 1 I and P Chapter 2 Page 6

I II Introduction to Organic Compounds (Carbon-based Compounds) A Alkanes Saturated Hydrocarbons (contain H and C)

I molecules contain a maximum number of H Atoms 2 Formula C1H2n-2

a Methane CH4 b Ethane C2H c Propane C1H~ d Butane C4H10

1) Two possible structural fOl11mlas

Stem Number Ill1ethmiddot

ethshy 2 prop 3 butmiddot 4 pentshy 5

hexshy (

heptmiddot 7

octmiddot R nonmiddot 9 decshy lO

--except methane ethane amp propane I2) Compounds with the same molecular formula

but different structural fOl11mlas are known as isomers and they have di t1crent properties

B Cyclic Alkanes 1 FOl11mla CnHn 2 prefix cyc1oshy

C Alkenes unsaturated hydrocarbon 1 Formula CJhn

a Ethene CH4 b Propene C3H6 c Butene C4H~

D Alkynes unsaturated hydrocarbon 1 Fonnula Cnl1n2

a Ethyne C2H~ b Propyne C3H4 c Butvne CH6

E Homology 1 a series of compounds vhose fonnulas and structures vary in a regular manner also

have properties that vary in a predictable manner a Example Both the densities and boiling points of the straight-chain alkanes

increase in a continuous and regular fashion with increasing numbers ofC

F Types of Organic Compounds 1 Functional Group atom or group of atoms attached to or inserted in a hydrocarbon

chain or ring that confers charactcristic properties to the molecule a usually where most of the reactions of the molecule occur

2 Alcohols (R-OII) where R represcnt the hydrocarbon a Examples CH30H methanol

CH3CH20H = ethanol CH3CH2CH20H = I-propanol CfhCH(OH)CH 3 2-propanol or isopropanol

b Not bases

3 Ethers (R-O-R) where R can represent a different hydrocarbon than R a Example CHCH20CH-CH = Diethyl ether

AP Chemistry Dr Kalish If and P Chapter 2 Page 7

4 Carboxylic Acids (R-COOH) a Examples HCOOH methanoic or formic acid

CH3COOH ethanoic or acetic acid

b the H of the COOH group is ionizable the acid is classified as a weak acid

5 Esters (R-COOR) a Flavors and fragrances b Examples CHCOOCHCrh = ethyl acetate

CH1COOCHCH 2CHCHCH] pentyl acetate

6 Ketones (R-CO-R )

7 Aldehydes (R-CO-H)

8 Amines (R-NH R-NHR R-NRR) a most common organic bases related to ammonia b one or more organic groups are substituted for the H in NH3 c Examples CHNH = methyl amine

CH 3CHNlh ethyl amine

68 Chapter 2 Atoms Molecules and Ions

TABLE 21

Class

Some Classes of Organic Compounds and Their Functional Groups

General Structural Name of Formula Example Example

Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3

CH3C==CCH2CH2CH2CH2CH3

CH3CH2CH2CH2OH

CH3CH2CH2CH2CH2CH2Br

CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane

I-methoxypropane (methyl propyl ether)

l-aminopropane (propylamine)C

butanal (butyraldehyde)

3-hexanone (ethyl propyl ketone)C

butanoic acid (butyric acid)

methyl butanoate (methyl butyrate)C

butanamide (butyramide)

ethylbenzene

bromobenzene

4-chlorophenol

Section 29 68 Chap 23

Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23

Section 21deg Sections 210 42

Chap 15

Section 46 Chap 23

Section 46 Chap 23

Sections 210 42 Chap 1523

Sections 210 68 (fats) Chap 23 Chap 24 (polymers)

Section 116 Chap 23 Chap 24 (polymers)

Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na

EI C( an Rshyiar ie co

C

The functional group is shown in red R stands for an alkyl group su b X stands for a halogen atom-F Cl Br or I C Common name d Ar- stands for an aromatic (aryl) group such as the benzene ring

11

o II

R-C-O-R or RCOOR

where R is the hydrocarbon portion of a carboxylic acid and R is the hydrocarshybon group of an alcohol R and R may be the same or different

Esters are named by indicating the part from the alcohol first and then naming the portion from the carboxylic acid with the name ending in -ate For instance

o II

CH3-C-O-CH2CH3

is ethyl acetate it is made from ethyl alcohol and acetic acid Many esters are noted for their pleasant odors and some are used in flavors and

fragrances Pentyl acetate CH3COOCH2CH2CH2CH2CH3 is responsible for most of the odor and flavor of ripe bananas Many esters are used as flavorings in cakes candies and other foods and as ingredients in fragrances especially those used to perfume household products Some esters are also used as solvents Ethyl acetate for example is used in some fingernail polish removers It is a solvent for the resins in the polish

Amines The most common organic bases the amines are related to ammonia Amines are compounds in which one or more organic groups are substituted for H atoms in NH3 In these two arnines one of the H atoms has been replaced

H H H H H I I I I I

H-C-N-H I H

or CH3NHZ H-C-C-N-H I I H H

or CHFH2NH2

Methylamine Ethylamine

The replacement of two and three H atoms respectively is seen in dimethylarnine [(CH3hNH] and trimethylamine [(CH3hN] In Chapters 4 and 15 we will see that mUch of what we learn about ammonia as a base applies as well to arnines

~ummary

The basic laws of chemical combination are the laws of conservation of mass constant comshyposition and multiple proportions Each played an important role in Daltons development of the atomic theory

The three components of atoms of most concern to chemists are protons neutrons and electrons Protons and neutrons make up the nucleus and their combined number is the mass number A of the atom The number of protons is the atomic number Z Electrons found outside the nucleus have negative charges equal to the positive charges of the proshytons All atoms of an element have the same atomic number but they may have different mass numbers giving rise to isotopes

A chemical formula indicates the relative numbers of atoms of each type in a comshyPOUnd An empirical formula is the simplest that can be written and a molecular formula ~fle~ts the actual composition of a molecule Structural and condensed structural formulas

~ scnbe the arrangement of atoms within molecules For example for acetic acid

Summary 71

APPLICATION NOTE Butyric acid CH)CHzCH2COOH is one of the most foul-smelling substances known but turn it into the ester methyl butyrate CH3CH2CH2COOCH3 and you get the aroma of apples

APPLICATION NOTE Amines with one or two carbon atoms per molecule smell much like ammonia Higher homo logs smell like rotting fish In fact the foul odors of rotting flesh are due in large part toamines that are given off as the flesh decays ----------~shy


Key Terms

acid (28) alcohol (210) alkane (29) amine (210) anion (27) atomic mass (24) atomic mass unit (24) atomic number (Z) (23) base (28) carboxylic acid (210) cation (27) chemical formula (p 47) chemical nomenclature (p 35) electron (23) empirical formula (26) ester (210) ether (210) formula unit (27) functional group (210) hydrate (27) ion (27) ionic compound (27) isomer (29) isotope (23) law of conservation of mass

(21) law of constant composition

(21) law of definite proportions

(21) law of multiple proportions

(22) mass number (A) (23) metal (25) metalloid (25) molecular compound (26) molecular formula (26) molecule (26) neutron (23) nonmetal (25) periodic table (25) poly atomic ion (27) proton (23) salt (28) structural formula (26)

Acetic acid

Empirical Molecular formula formula

H 0 I II

H-C-C-O-H I H Structural formula

f

Condensed structural formula

The periodic table is an arrangement of the elements by atomic number that places elshyements with similar properties into the same vertical groups (families) The periodic table is an important aid in the writing of formulas and names of chemical compounds A moleshycular compound consists of molecules in a binary molecular compound the molecules are made up of atoms of two different elements In naming these compounds the numbers of atoms in the molecules are denoted by prefixes the names also feature -ide endings

Examples NI3 nitrogen triiodide S2F4 = disulfur tetrafluoride

Ions are formed by the loss or gain of electrons by single atoms or groups of atoms Posshyitive ions are known as cations and negative ions as anions An ionic compound is made up of cations and anions held together by electrostatic forces of attraction Formulas of ionic compounds are based on an electrically neutral combination of cations and anions called a formula unit The names of some monatomic cations include Roman numerals to designate the charge on the ion The names of monatomic anions are those of the nonm~allic eleshyments modified to an -ide ending For polyatornic anions the prefixes hypo- and per- and the endings -ite and -ate are commonly found

Examples MgF2 = magnesium fluoride Li2S = lithium sulfide CU20 copper(I) oxide CuO = copper (II) oxide Ca(CIOh calcium hypochlorite KI04 = potassium periodate

Many compounds are classified as acids bases or salts According to the Arrhenius theory an acid produces H+ in aqueous (water) solution and a base produces OH- A neushytralization reaction between an acid and a base fornls water and an ionic compound called a salt Binary acids have hydrogen and a nonmetal as their constituent elements Their names feature the prefix hydro- and the ending -ic attached to the stem of the name of the nonshymetal Ternary oxoacids have oxygen as an additional constituent element and their names use prefixes (h)po- and per-) and endings (-ous and -ic) to indicate the number of 0 atoms per molecule

Examples HI = hydroiodic acid HI03 = iodic acid

HCI02chlorous acid HCI04 = perchlonc acid

Organic compounds are based on the element carbon Hydrocarbons contain only the elements hydrogen and carbon Alkanes have carbon atoms joined together by single bonds into chains or rings with hydrogen atoms attached to the carbon atoms Alkanes with four or more carbon atoms can exist as isomers molecules with the same molecular formula but different structures and properties

Functional groups confer distinctive properties to an organic molecule when the groups are substituted for hydrogen atoms in a hydrocarbon Alcohols feature the hydroxyl group -OH and ethers have two hydrocarbon groups joined to the same oxygen atom Carboxylic acids have a carboxyl group -COOH An ester RCOOR is derived from a carboxylic acid (RCOOH) and an alcohol (ROH) Arnines are compounds in which organic groups are subshystituted for one or more of the H atoms in anmlonia NH3

7

Dr Kalish Page 1

AP Chemistry Clwk 12A

Name ___________________________________________ Date _______

Molecular Formula -riting and Naming

Name the following compounds

1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)

Vrite the chemical formula for cach of the follOving compounds

carbon dioxide

R sulfur hexafluoride

9 dinitrogen tetroxide

10 trisulfur heptaiodide

11 disulfur pentachloride

12 triphosphorus monoxide

Ionic Formula Writing and Naming

Directions Name the following ionic compounds

13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN

Compounds that include Polyatomic Ions

23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh

Directions Write the correct formula for each of the following compounds

1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride

12 Nickel(Il) bromide --~-----~-----~--

13 Lead(lV) phosphide

14 Tin(H) sulfide

Compounds that include Polyatomic Ion~

15 Aluminum phosphate

IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate

20 Magnesium chromate

21 Sodium dichromate

22 Zinc hydroxide

23 Copper(Il) nitrite

24 Manganese(II) hydroxide

25 Iron(II) sulfate

26 lron(III) oxide ---bull- bull-shy

AI Chemistry fk Kabil II and P Chapter 3 Band S Ch

Stoichiometr~ Chemical Calculations

I Stoichiometry of Chemical Compounds

A Molecular Masses and Formula Masses I Molecular Mass sum of the masses of the atoms represented in a molecular formula

Example Mass of CO2

1 C = 1 x 120 amu mass of CO2 =c 440 amu l 0 = 2 x 160 amu

Fonnula Mass sum of the masses of the atoms or ions represented in an ionic fonnula Example Mass of BaCb

1Ba= I x D73al11u mass of BaCl 2 20X3 amu lCl2x355amu

B The 1ole and Avogadros Number I Mole amount of substance that contains as many elementary entities as there are

atoms in exactly 12 g of the C -12 isotope a The elementary entities are atoms in elements molecules in diatomic elements

and compounds and t(mnula units in ionic compounds b Avogadros Number (1) 6()22 x 1O~ mor l

I I I mole 6022 x 10-- atoms molecules partIcles etc

e one mole of any element is equal to the mass of that element in grams I) For the diatomic elements multiply the mass of the element by two

2 Molar Mass mass of one mole of the substance Example Mass of BaCb

1moleBa=1 x D73g mass of 1 mole BaCI2 20X3 g I mole CI 2 x 355 g

C Mass Percent Composition from Chemical Fon11ulas I Mass Percent Composition describes the prop0l1ions of the constituent elements in a

compound as the number of grams of each element per 100 grams of the compound

Example What is the C in butanc (CH1n) Mass ofCs x 100deg) 4(201g) x 100deg0

MassofCH iIl 5S14g

D Chemical Formulas from Mass Percent Composition I Steps in the Detennination of Empirical FOI111Ula

a Change ~O to grams h Convert mass of each elemcnt to moles c Detennine mole ratios d lfneccssary multiply mole ratios by a t~lctor to obtain positic integers only c Write the empirical fonnula

P Chemistry Dr Klil~h II and P Chapter 3 Band S CI1 4

Example Cyclohexanol has the mass percent composition 7195 C 1208 H and 1597deg0 O Determine its empirical timl1ula

A compound has the mass percent composition as 1()llows 3633 C 549 H and 5818 (~o S Detcnninc its empirical t(mmtia

Relating Molecular F0ll11ulas to Empirical F0ll11ulas a Integral Factor (n) Molecular Mass

Empirical Fonnula Mass

Example Ethylene (M 280 u) cyclohexane (M 840 u) and I-pcntcnc (700 u) all have the empirical f0ll11ula CH Vhat is the molecular t(mnula of cach compound

II Stoichiometry of Chemical Reactions

A Writing and Balancing Equations 1 chemical equation shorthand description of a chemical reaction using symbols and

formulas to represent clements and compounds respectivcly a Reactants -7 Products h C oefficicnts c States gas (g) liquid (1) solid (s) aqueous (aq)

d ll Heat 2 Balancing Equations

a For an element the same number of atoms must he on each side of thc equation h only coefticients can be changed

1) Balance the clement that only appears in one compound on each side of the equation first

2) Balance any reactants or products that exist as the free clcment last 3) Polyatomic ions should he treated as a group in most cases

Example _SiCI4 + __H~O -7 _SiO~ ~ _He)

B Stoichiometric Equivalence and Reaction Stoichiometry 1 Mole Ratios or stoichiometric factors

Example _SiCIt + lHO -7 _SiO ~middot1HCI What is the mole ratio ofreactmts

2 Problems a Mole-tn-mole h Mole-to-gram c Gram-to-mole d Gram-to-gram

AP Chemistry Dr Kalish If and P Chapter 3 Band S Ch 4

C Limiting Reactants I Limiting reactant (LR) is consumed completely in a reaction and limits the amount of

products tltmned J To detenninc the LK compare moles 3 Usc the LR to detennine theoretical yield

Example FeS(s) + 2 HCI(aq) ~ FeCI 2(aq) HS(g)

If 102 g HCI is added to 13 g FeS what mass of HS can he formed What is the mass of the excess reactant remaining

102 g HCI x 1 mole HCI 0280 moles HCI LR 3646 g HCI

[32 g FeS x 1 mole FeS 0150 moles FeS 8792 g FeS

0280 moles HCI x 1 mole H2S x 34()1) g HS- 4n g I oS 2 mole HCI 1 mole H2S

0150 mole FeS - 0140 mole FeS = 0010 mole FcS x 8792 g FeS = (l~79 g FeS 1 mole FcS

D Yields of Chemical Reactions I Percent Yield Actual Yield x 100

Theoretical ield

J Actual Yield may be less than theoretical yield hecause of impurities errors during experimentation side reactions etc

Example If the actual yield of hydrogen sultidc was 356 g calculate lhc percent yield

If the percent yield of hydrogen sulfide was 847 (~o what was the actual yield

Solutions and Solution Stoichiometry I Components of a Solution

a Solute substance being dissolving b Solvent substance doing the dissohing

1) water universal solvent solutions made i(h water as the solent arc called aqueous solutions

J Concentration quantity ofsolutc in a given quantity ofsolwnt or solution a ()i1ute contains relaticly little solutc with a large amount of solvcnt

P Chel1li~try Dr Kalish 1I and P Chapter3 Rand S Ch -4 [icl -+

b Concentrated contains a relatively large amount of solute in a given quantity or solvent

3 Molarity or Molar Concentration Molarity moles solute

Liters of solution

Example Calculate the molarity of solution made by dissolving 200 moles NaCI in enough water to generate 400 L of solution Molarity moles solute lnO moles NaCI= OSO() M

Liters of solution 400 L

Example Calculate the molarity of solution made by dissolving 351 grams NaCI in enough water to generate 300 L of solution

351 g aCI x I mole NaCI 060 I moles NaCI 5844 g NaCI

Molarity moles solute 0601 moles NnCI f)lOI) M Liters of solution 300 L

4 Calculating the lolarity of Ions and Atoms

Example Calculate the molarity of Ca and cr in a 0600 M solution of Calcium chloride

CaCI -7 Ca- + leT I I Moles

0600 M CaCh x I mole Ca2 ooon 1 Ca2

shy

I mole CaCI

0600 M CaCb x mole cr 120 M cr I mole CaCI

Example Calculate the molarity of C and H in 150 1 propane CJ-lx

C311~ = 3C 8H Moles I 3 8

150 M CHx x 3 mole C = 450 M C I mole C 3Hx

150 M CHx x 8 mole H 120 M H I mole CH~

AI Chmistry Ik Kalish II and P Chaptr 3 Band S eh 4

5 Dilution the process by which dilute solutions are made by adding solvent to concentrated solutions a the amount of solute (moles) remains the same but thc solution concentration is

altered b M enllc x VWile = Moil X Vcli1

Example What is the concentration of a solution made by diluting sOn 1111 of 100 M NaOH with 200 ml of water

IIIAdvanced Stoichiometry A Allovmiddots fiJr the conversion of grams of a compound to grams of an clement and deg0

composition to detem1ine empirical and molecular f0l111ula

Examples t A 01204 gram sample of a carboxylic acid is combusted to yield 02147 grams of

CO- and 00884 grams of water a Determine the percent composition and empirical ft)Jl11ula of the compound

Anslcr CIIP (I(()

b If the molecular mass is 222 gimole vvhat is the molecular tt)llnula c Write the balanced chemical equation showing combustion of this compound

Dimethylhydrazine is a C-H-N compound used in rocket fuels When burned completely in excess oxygen gas a 0312 g sample produces 0458 g CO and 0374 g H20 The nitrogen content of a separate 0525 g sample is cOl1clied to 0244 g N a What is the empirical t(mTIula of dimethylhydrazinc 1111 C(

b If the molecular mass is 150 gmo)c what is the molecular ttmnula c Vrite the balanced chemical equation showing combustion of this compound

2

Empirical fonnulas can be detennined from indirect analyses

In practice a compound is seldom broken down completely to its elements in a quantitative analysis Instead the compound is changed into other compounds The reactions separate the elements by capturing each one entirely (quantitatively) in a separate compound whose formula is known

In the following example we illustrate an indirect analysis of a compound made entirely of carbon hydrogen and oxygen Such compounds bum completely in pure oxygen-the reaction is called combustion-and the sole products are carshybon dioxide and water (This particular kind of indirect analysis is sometimes called a combustion analysis) The complete combustion of methyl alcohol (CH30H) for example occurs according to the following equation

2CH30H + 30z--- 2COz + 4HzO

The carbon dioxide and water can be separated and are individually weighed Noshytice that all of the carbon atoms in the original compound end up among the COz molecules and all of the hydrogen atoms are in H20 molecules In this way at least two of the original elements C and H are entirely separated

We will calculate the mass of carbon in the CO2 collected which equal~ the mass of carbon in the original sample Similarly we will calculate the mass of hyshydrogen in the H20 collected which equals the mass of hydrogen in the original sample When added together the mass of C and mass of H are less than the total mass of the sample because part of the sample is composed of oxygen By subtractshying the sum of the C and H masses from the original sample weight we can obtain the mass of oxygen in the sample of the compound

A 05438 g sample of a liquid consisting of only C H and 0 was burned in pure oxyshygen and 1039 g of CO2 and 06369 g o( H20 were obtained What is the empirical formula of the compound

A N A L Y SIS There are two parts to this problem For the first part we will find the number of grams of C in the COz and the number of grams of H in the H20 (This kind of calculation was illustrated in Example 410) These values represent the number of grams of C and H in the original sample Adding them together and subshytracting the sum from the mass of the original sample will give us the mass of oxygen in the sample In short we have the following series of calculations

grams CO2 ----lgt grams C

grams H20 ----lgt grams H

We find the mass of oxygen by difference

05438 g sample - (g C + g H) g 0

In the second half of the solution we use the masses of C H and 0 to calculate the empirical formula as in Example 414

SOLUTION First we find the number of grams of C in the COz and of H ia the H20 In 1 mol of CO2 (44009 g) there are 12011 g of C Therefore in 1039 g of CO we have

12011 g C 02836 g C1039 g CO2 X 44009 g CO 2

In 1 mol of H20 (18015 g) there are 20158 g of H For the number of grams of H in 06369 g of H20

20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2

The total mass of C and H is therefore the sum of these two quantities

total mass of C and H = 02836 g C + 007127 g H 03549 g-c=

The difference between this total and the 05438 g in the original sample is the mass of oxygen (the only other element)

mass of 0 05438 g - 03549 g = 01889 g 0

Now we can convert the masses of the elements to an empirical formula

ForC 1 molC 02836 g C X 12011 g C = 002361 mol C

ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0

Our preliminary empirical formula is thus C1J02361H0D70700001I81 We divide all of these subscripts by the smallest number 001181

CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181

The results are acceptably close to ~H60 the answer

Summary 123

Summary

Molecular and formula masses relate to the masses of molecules and formula units Moshylecular mass applies to molecular compounds but only formula mass is appropriate for ionic compounds

A mole is an amount of substance containing a number of elementary entities equal to the number of atoms in exactly 12 g of carbon-12 This number called Avogadros number is NA 6022 X 1023

bull The mass in grams of one mole of substance is called the molar mass and is numerically equal to an atomic molecular or formula mass Conversions beshytween number of moles and number of grams of a substance require molar mass as a conshyversion factor conversions between number of grams and number of moles require the inverse of molar mass Other calculations involving volume density number of atoms or moshylecules and so on may be required prior to or following the grammole conversion That is

Molar mass

Inverse of molar mass

Formulas and molar masses can be used to calculate the mass percent compositions of compounds And conversely an empirical formula can be established from the mass percent composition of a compoundmiddotto establish a molecular formula we must also know the moshylecUlar mass The mass percents of carbon hydrogen and oxygen in organic compounds can be determined by combustion analysis

A chemical equation uses symbols and formulas for the elements andor compounds inshyVolVed in a reaction Stoichiometric coefficients are used in the equation to reflect that a chemical reaction obeys thelaw of conservation of mass

Calculations concerning reactions use conversion factors called stoichiometric facshytors that are based on stoichiometric coefficients in the balanced equation Also required are ~lar masses and often other quantities such as volume density and percent composition

e general format of a reaction stoichiometry calculation is

actual yield (310) Avogadros number NA (32) chemical equation (37) dilution (311) formula mass (31) limiting reactant (39) mass percent composition (34) molar concentration (311) molarity M (311) molar mass (33) mole (32) molecular mass (31) percent yield (310) product (37) reactant (37) solute (311) solvent (311) stoichiometric coefficient (37) stoichiometric factor (38) stoichiometric proportions

(39) stoichiometry (page 82) theoretical yield (310)

~

124 Chapter 3 Stoichiometry Chemical Calculations

no mol B

no mol A

no mol A

no molB

The limiting reactant determines the amounts of products in a reaction The calculatshyed quantity of a product is the theoretical yield of a reaction The quantity obtained called the actual yield is often less It is commonly expressed as a percentage of the theoretical yield known as the percent yield The relationship involving theoretical actual and percent yield is

actual X 0007Percent yield = I 70 theoretical yield

The molarity of a solution is the number of moles of solute per liter of solution Comshymon calculations include relating an amount of solute to solution volume and molarity Soshylutions of a desired concentration are often prepared from more concentrated solutions by dilution The principle of dilution is that the volume of a solution increases as it is diluted but the amount of solute is unchanged As a consequence the amount of solute per unit volshyume-the concentration-decreases A useful equation describing the process of dilushytion is

tv1conc X Vcone = Mdil X Vdil

In addition to other conversion factors stoichiometric calculations for reactions in solution use molarity or its inverse as a conversion factor

Review Questions

1 Explain the difference between the atomic mass of oxyshygen and the molecular mass of oxygen Explain how each is determined from data in the periodic table

2 hat is Avogadros number and how is it related to the quantity called one mole

3 How many oxygen molecules and how many oxygen atoms are in 100 mol 0 2

4 How many calcium ions and how many chloride ions are in 100 mol CaCh

5 What is the molecular mass and what is the molar mass of carbon dioxide Explain how each is determined from the formula CO2

6 Describe how the mass percent composition of a comshypound is established from its formula

7 Describe how the empirical formula of a compound is deshytermined from its mass percent composition

S bat are the empirical formulas of the compounds with the following molecular formulas (a) HP2 (b) CgHl6 (e) CloHs (d) C6H160

9 Describe how the empirical formula of a compound that contains carbon hydrogen and oxygen is determined by combustion analysis

10 bat is the purpose of balancing a chemical equation 11 Explain the meaning of the equation

at the molecular level Interpret the equation in terms of moles State the mass relationships conveyed by the equation

12 Translate the following chemical equations into words

(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)

(e) 2 AI(s) + 6 HCI(aq) ~ 2 AICI3(aq) + 3 H2(g)

13 Write balanced chemical equations to represent (a) the reaction of solid magnesium and gaseous oxygen to form solid magnesium oxide (b) the decomposition of solid ammonium nitrate into dinitrogen monoxide gas and liqshyuid water and (e) the combustion of liquid heptane C7H16 in oxygen gas to produce carbon dioxide gas and liquid water as the sole products

14 bat is meant by the limiting reactant in a chemical reshyaction Under what circumstances might we say that a reaction has two limiting reactants Explain

15 by are the actual yields of products often less than the theoretical yields Can actual yields ever be greater than theoretical yields Explain

16 Define each of the following terms

(a) solution (d) molarity

(b) solvent (e) dilute solution

(e) solute (0 concentrated solution

I

( I () 6t (]i M I 67 Mi (9 71)is 59

iLantrmnidi Scrrs Dv I Ho Er Tm YbCc Pr 16250 II ~J-lB 167 26 16~93 171()-lI I yen11I

I 1291 1i7 07l2(H91I(2()t))

X7 XX

Fr Ra 22 22()J)21227()1

nO

Nd Pm

1)0 l) I )l t9 l()() li)1 IU~

Th Pa Cf Es (m Md Not Aetinide SCI Ci

2J211-l HO-1 (21 L~52) (257) (2~X) (5Q )

no NOT DETACH FROM nOOK

PERIODIC TABL~E OF THE ELElVlENTS

21 )~ 2 24 I 25 I 16 n 2H

- 6 I 7

n C I N HUd Imiddottol

I 1

AI P 1(1(X -(N ~C97

Sc Ti v Cr I Mn I Fe Co Ni 29 30 1 1 H n

Cu Zn Ga Ge As - 9lt1 -I7lt() )()t)-I i~O( )-l9 c +569 6155 6UtJ (912

Jtj 40 41 +~ +3 44 45 6 47 41 9

Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Ml91 9112 tJ2tJI 95)-1 lgtX) 1011 10291 lOll IOiC 112-11 11-1-2 IIX71 12175

51 72 73 74 75 76 77 lX 71) XI) Xl X2 amp1

La I Ht Ta I Re OS Ir Pt Au Hg TI Ph Hi nX91 17H-I9 ISOYi 1K1Xi IX()21 )(12 1922 1950X 19IJ9~P()()591[)-lX

HltJ IOl 10 106 107 lOX 109 1 10 I I I

tAc Rf Ob Sg Bh Hs Vlt Os Rg (261) 1~()2) I (266 I (2b-l11 [277) I (26~) (211) 1(272)

o 1600

16

s 3206 q

Se 71196

52

Te 12760

XJ

Po

I

CI n g 3 iii ltI n g Ul ()

III l Q l1

~ 3 11 ~ n S omiddot l

tv

S tJ

rt

J s ~

CfQ

~ ~ 0

0 CD M gt 4 rt o

r-JPgt )CD 0 ~

(j 0

g gs ct C]

H (lOX

Li 09-1

II

Na 22lt)9

19

K NIO

17

Rb Xil7

55

Cs

Mg ~o

20

Ca OCK

3H

Sr 1-7e

56

B~l

F IC)OO

Ii

el

Yi

Br 7990

5i

I 12691

It)

At 2Jf))

I

Lu 17middot197

1m

Lr 2()2)

lie

10

~e l(lIK

I

Ar

lAS I ~9()l36

Kr X30

54

Xc UI ~9

X6

Rn I (~22)

51


Hal f-reaction

) + 2 eshy

+ 1shy

Au + 31shy

K)+2eshy

O(K) + 4H + 41shy

Br2 () + 2

2 Hg2 + 21shy

Hg2+ + 2 eshy

+1

Hg++2eshy

+1

12(~)+2eshy

Cu+ + 1-

Cu 2+ + 21shy

Cu 2+ + 1shy

Sn-+-+2eshy

Sis) + 2 H+ + 21shy

2H++2eshy

Pb2+ + 21shy

Sn 2-+2eshy

Ni 2+ + 21shy

Co 2+ + 2eshy

Cd+ + 21-

Cr+ + 1shy

Fe+ + 21shy

Cr3++3cshy

Zn 2+ + 21shy

2H 20()+ 21shy

Mn 2+ + 21shy

AI)+ + 31shy

Be 2+ + 2cshy

Mg2+ + 21-

Na+ + e-

Ca=- + 2eshy

Sr2+ + 2eshy

Ba + 2eshy

Rb+ + eshy

K+ +eshy

Cs+ + eshy

Li+ + eshy

Au(n

2CIshy

2 HO()

2 Brshy

Hg+

Hg()

Ag(s)

2 Hg()

21shy

curs)

Cuts)

H

H(g)

PhIs)

Sn(s)

Ni(s)

Cots)

Cd(s)

Cr2+

Fe(s)

Cr(s)

Zn(s)

H 2 (g)+20Hshy

vines)

Al(s)

Be(s)

Mgtraquo

Na(s)

Cats)

Sr(s)

Ba(s)

Rb(s)

K(s)

Cs(s)

Lien

287

182

150

136

123

107

092

085

080

079

077

053

052

034

015

015

014

000

013

014

025

028

040

041

044

074

076

083

118

166

170

-237

271

-287

289

290

-292

292

292

-305








E = Ill = frequency

=





EQUILIBRIUM


( [A]lrBt

(p ltP ItK = C D

I (P)(P13

K - fOWJlHB h - [B]



14 = pH + pOH




Ki pressureraquo

K (weak acid)

K1 (weak base)

Kit (waler)

KINETICS



f _ 12 -

0693-k-


Appendix B


PV IlRT


p + Pfl + Pc +

111 11

M

K degc + 273

D= V



A =abc

P == pressure

V = volume

T = temperature

n = number of mole

III == mas

JJ = molar mass

D =- denily

KE kinetic energy

= velocity

A == absorbance


h = path length

c = concentration


= 008206 L atm mol-I K- 1


I atm = 760 111m

== 760 tOIl



q lIlcfT




-RTln K

1=9 t

q 11

c T

So

He

GO 11

E O

q

Faradays constant F

volt


temperature

lttamlanl entrop

qandard enthalpy

tandard free energy

number of moles


current (amperes)

charge (coulombs)

lime (seconds)


I joule [coulomb



I

i

I



I M~tal I Li

Rb

I Sr Ca Na ~Ig


Pt Au










Nitrite NO

Important Constants





~

lumber 1 2 I

Trimiddot 1 I f--


4 5 6

I


Nonashy 9

Oecashy 10





20 Ca 10 fP- Pb 18 25 Mn 111 x3 Bi 19

26 Fe 1X 84 Po 20

I n Co 19

i



Solvent Til I

(0C) ktJ

(nC-kgmole) Tr

(0C) kr(OC-kgmole)




Nitrohcllene 2101 524 57() (152





I

a) e peCIIC


Specific Heat


(J895Aluminum ~




29Parutlin 0233


051 Water 4IX


Substance Hr

HO H-Ol

~Ht (kJimole) -23 -241x2 -2858









-3(l556 -187-

Br


-~155-12076CaCO FeO1 -649 -111-4

CI1 1 bull middot

FcOCaU -52()()

CJ I -1047 -749 lnO-

-il21 916


noo-3009 0 iC1H -4142-3935CO NaO

noo -110 I

HgtshyFc Na-SO

(lOn -28so -3629 -3957

HC) HBrJ SOe

middot9U


Coppcr i 205 472(



i



I Introduction


A Key Terms











B Properties



C Types of changes






1aterial


Substance

Elements Compounds


(Solutions)






















Length meter 111



B


Problems


d=mV


Problems


i

GiEa- G 10


Hectoshy h lO-

Decashy da 10 1

10 decishy d 10


micro- Jl 10(

i nanoshy n 10

pleoshy p 10 1

femtoshy f 10

i

Jfea 11 illJ( I

I 000 000 000 i

t 000 000 1000

tOO

10 1

1 ]0

1 I U()

1 1000

1 1 000000

I 1 000 000 000

I 1 000 000 000 000

1 I 000 000 000 000 000





31 ml 1 cm

Dr Kalish Page 4

~ -Lowcst density

Greatest density

shy










i

None 0()O45


OO()OOO5 1


















tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)










Hal f-reaction

) + 2 eshy

+ 1shy

Au + 31shy

K)+2eshy

O(K) + 4H + 41shy

Br2 () + 2

2 Hg2 + 21shy

Hg2+ + 2 eshy

+1

Hg++2eshy

+1

12(~)+2eshy

Cu+ + 1-

Cu 2+ + 21shy

Cu 2+ + 1shy

Sn-+-+2eshy

Sis) + 2 H+ + 21shy

2H++2eshy

Pb2+ + 21shy

Sn 2-+2eshy

Ni 2+ + 21shy

Co 2+ + 2eshy

Cd+ + 21-

Cr+ + 1shy

Fe+ + 21shy

Cr3++3cshy

Zn 2+ + 21shy

2H 20()+ 21shy

Mn 2+ + 21shy

AI)+ + 31shy

Be 2+ + 2cshy

Mg2+ + 21-

Na+ + e-

Ca=- + 2eshy

Sr2+ + 2eshy

Ba + 2eshy

Rb+ + eshy

K+ +eshy

Cs+ + eshy

Li+ + eshy

Au(n

2CIshy

2 HO()

2 Brshy

Hg+

Hg()

Ag(s)

2 Hg()

21shy

curs)

Cuts)

H

H(g)

PhIs)

Sn(s)

Ni(s)

Cots)

Cd(s)

Cr2+

Fe(s)

Cr(s)

Zn(s)

H 2 (g)+20Hshy

vines)

Al(s)

Be(s)

Mgtraquo

Na(s)

Cats)

Sr(s)

Ba(s)

Rb(s)

K(s)

Cs(s)

Lien

287

182

150

136

123

107

092

085

080

079

077

053

052

034

015

015

014

000

013

014

025

028

040

041

044

074

076

083

118

166

170

-237

271

-287

289

290

-292

292

292

-305








E = Ill = frequency

=





EQUILIBRIUM


( [A]lrBt

(p ltP ItK = C D

I (P)(P13

K - fOWJlHB h - [B]



14 = pH + pOH




Ki pressureraquo

K (weak acid)

K1 (weak base)

Kit (waler)

KINETICS



f _ 12 -

0693-k-


Appendix B


PV IlRT


p + Pfl + Pc +

111 11

M

K degc + 273

D= V



A =abc

P == pressure

V = volume

T = temperature

n = number of mole

III == mas

JJ = molar mass

D =- denily

KE kinetic energy

= velocity

A == absorbance


h = path length

c = concentration


= 008206 L atm mol-I K- 1


I atm = 760 111m

== 760 tOIl



q lIlcfT




-RTln K

1=9 t

q 11

c T

So

He

GO 11

E O

q

Faradays constant F

volt


temperature

lttamlanl entrop

qandard enthalpy

tandard free energy

number of moles


current (amperes)

charge (coulombs)

lime (seconds)


I joule [coulomb



I

i

I



I M~tal I Li

Rb

I Sr Ca Na ~Ig


Pt Au










Nitrite NO

Important Constants





~

lumber 1 2 I

Trimiddot 1 I f--


4 5 6

I


Nonashy 9

Oecashy 10





20 Ca 10 fP- Pb 18 25 Mn 111 x3 Bi 19

26 Fe 1X 84 Po 20

I n Co 19

i



Solvent Til I

(0C) ktJ

(nC-kgmole) Tr

(0C) kr(OC-kgmole)




Nitrohcllene 2101 524 57() (152





I

a) e peCIIC


Specific Heat


(J895Aluminum ~




29Parutlin 0233


051 Water 4IX


Substance Hr

HO H-Ol

~Ht (kJimole) -23 -241x2 -2858









-3(l556 -187-

Br


-~155-12076CaCO FeO1 -649 -111-4

CI1 1 bull middot

FcOCaU -52()()

CJ I -1047 -749 lnO-

-il21 916


noo-3009 0 iC1H -4142-3935CO NaO

noo -110 I

HgtshyFc Na-SO

(lOn -28so -3629 -3957

HC) HBrJ SOe

middot9U


Coppcr i 205 472(



i



I Introduction


A Key Terms











B Properties



C Types of changes






1aterial


Substance

Elements Compounds


(Solutions)






















Length meter 111



B


Problems


d=mV


Problems


i

GiEa- G 10


Hectoshy h lO-

Decashy da 10 1

10 decishy d 10


micro- Jl 10(

i nanoshy n 10

pleoshy p 10 1

femtoshy f 10

i

Jfea 11 illJ( I

I 000 000 000 i

t 000 000 1000

tOO

10 1

1 ]0

1 I U()

1 1000

1 1 000000

I 1 000 000 000

I 1 000 000 000 000

1 I 000 000 000 000 000





31 ml 1 cm

Dr Kalish Page 4

~ -Lowcst density

Greatest density

shy










i

None 0()O45


OO()OOO5 1


















tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)















E = Ill = frequency

=





EQUILIBRIUM


( [A]lrBt

(p ltP ItK = C D

I (P)(P13

K - fOWJlHB h - [B]



14 = pH + pOH




Ki pressureraquo

K (weak acid)

K1 (weak base)

Kit (waler)

KINETICS



f _ 12 -

0693-k-


Appendix B


PV IlRT


p + Pfl + Pc +

111 11

M

K degc + 273

D= V



A =abc

P == pressure

V = volume

T = temperature

n = number of mole

III == mas

JJ = molar mass

D =- denily

KE kinetic energy

= velocity

A == absorbance


h = path length

c = concentration


= 008206 L atm mol-I K- 1


I atm = 760 111m

== 760 tOIl



q lIlcfT




-RTln K

1=9 t

q 11

c T

So

He

GO 11

E O

q

Faradays constant F

volt


temperature

lttamlanl entrop

qandard enthalpy

tandard free energy

number of moles


current (amperes)

charge (coulombs)

lime (seconds)


I joule [coulomb



I

i

I



I M~tal I Li

Rb

I Sr Ca Na ~Ig


Pt Au










Nitrite NO

Important Constants





~

lumber 1 2 I

Trimiddot 1 I f--


4 5 6

I


Nonashy 9

Oecashy 10





20 Ca 10 fP- Pb 18 25 Mn 111 x3 Bi 19

26 Fe 1X 84 Po 20

I n Co 19

i



Solvent Til I

(0C) ktJ

(nC-kgmole) Tr

(0C) kr(OC-kgmole)




Nitrohcllene 2101 524 57() (152





I

a) e peCIIC


Specific Heat


(J895Aluminum ~




29Parutlin 0233


051 Water 4IX


Substance Hr

HO H-Ol

~Ht (kJimole) -23 -241x2 -2858









-3(l556 -187-

Br


-~155-12076CaCO FeO1 -649 -111-4

CI1 1 bull middot

FcOCaU -52()()

CJ I -1047 -749 lnO-

-il21 916


noo-3009 0 iC1H -4142-3935CO NaO

noo -110 I

HgtshyFc Na-SO

(lOn -28so -3629 -3957

HC) HBrJ SOe

middot9U


Coppcr i 205 472(



i



I Introduction


A Key Terms











B Properties



C Types of changes






1aterial


Substance

Elements Compounds


(Solutions)






















Length meter 111



B


Problems


d=mV


Problems


i

GiEa- G 10


Hectoshy h lO-

Decashy da 10 1

10 decishy d 10


micro- Jl 10(

i nanoshy n 10

pleoshy p 10 1

femtoshy f 10

i

Jfea 11 illJ( I

I 000 000 000 i

t 000 000 1000

tOO

10 1

1 ]0

1 I U()

1 1000

1 1 000000

I 1 000 000 000

I 1 000 000 000 000

1 I 000 000 000 000 000





31 ml 1 cm

Dr Kalish

~ -Lowcst density

Greatest density

shy










i

None 0()O45


OO()OOO5 1


















tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)









Appendix B


PV IlRT


p + Pfl + Pc +

111 11

M

K degc + 273

D= V



A =abc

P == pressure

V = volume

T = temperature

n = number of mole

III == mas

JJ = molar mass

D =- denily

KE kinetic energy

= velocity

A == absorbance


h = path length

c = concentration


= 008206 L atm mol-I K- 1


I atm = 760 111m

== 760 tOIl



q lIlcfT




-RTln K

1=9 t

q 11

c T

So

He

GO 11

E O

q

Faradays constant F

volt


temperature

lttamlanl entrop

qandard enthalpy

tandard free energy

number of moles


current (amperes)

charge (coulombs)

lime (seconds)


I joule [coulomb



I

i

I



I M~tal I Li

Rb

I Sr Ca Na ~Ig


Pt Au










Nitrite NO

Important Constants





~

lumber 1 2 I

Trimiddot 1 I f--


4 5 6

I


Nonashy 9

Oecashy 10





20 Ca 10 fP- Pb 18 25 Mn 111 x3 Bi 19

26 Fe 1X 84 Po 20

I n Co 19

i



Solvent Til I

(0C) ktJ

(nC-kgmole) Tr

(0C) kr(OC-kgmole)




Nitrohcllene 2101 524 57() (152





I

a) e peCIIC


Specific Heat


(J895Aluminum ~




29Parutlin 0233


051 Water 4IX


Substance Hr

HO H-Ol

~Ht (kJimole) -23 -241x2 -2858









-3(l556 -187-

Br


-~155-12076CaCO FeO1 -649 -111-4

CI1 1 bull middot

FcOCaU -52()()

CJ I -1047 -749 lnO-

-il21 916


noo-3009 0 iC1H -4142-3935CO NaO

noo -110 I

HgtshyFc Na-SO

(lOn -28so -3629 -3957

HC) HBrJ SOe

middot9U


Coppcr i 205 472(



i



I Introduction


A Key Terms











B Properties



C Types of changes






1aterial


Substance

Elements Compounds


(Solutions)






















Length meter 111



B


Problems


d=mV


Problems


i

GiEa- G 10


Hectoshy h lO-

Decashy da 10 1

10 decishy d 10


micro- Jl 10(

i nanoshy n 10

pleoshy p 10 1

femtoshy f 10

i

Jfea 11 illJ( I

I 000 000 000 i

t 000 000 1000

tOO

10 1

1 ]0

1 I U()

1 1000

1 1 000000

I 1 000 000 000

I 1 000 000 000 000

1 I 000 000 000 000 000





31 ml 1 cm

Dr Kalish Page 4

~ -Lowcst density

Greatest density

shy










i

None 0()O45


OO()OOO5 1


















tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)









I

i

I



I M~tal I Li

Rb

I Sr Ca Na ~Ig


Pt Au










Nitrite NO

Important Constants





~

lumber 1 2 I

Trimiddot 1 I f--


4 5 6

I


Nonashy 9

Oecashy 10





20 Ca 10 fP- Pb 18 25 Mn 111 x3 Bi 19

26 Fe 1X 84 Po 20

I n Co 19

i



Solvent Til I

(0C) ktJ

(nC-kgmole) Tr

(0C) kr(OC-kgmole)




Nitrohcllene 2101 524 57() (152





I

a) e peCIIC


Specific Heat


(J895Aluminum ~




29Parutlin 0233


051 Water 4IX


Substance Hr

HO H-Ol

~Ht (kJimole) -23 -241x2 -2858









-3(l556 -187-

Br


-~155-12076CaCO FeO1 -649 -111-4

CI1 1 bull middot

FcOCaU -52()()

CJ I -1047 -749 lnO-

-il21 916


noo-3009 0 iC1H -4142-3935CO NaO

noo -110 I

HgtshyFc Na-SO

(lOn -28so -3629 -3957

HC) HBrJ SOe

middot9U


Coppcr i 205 472(



i



I Introduction


A Key Terms











B Properties



C Types of changes






1aterial


Substance

Elements Compounds


(Solutions)






















Length meter 111



B


Problems


d=mV


Problems


i

GiEa- G 10


Hectoshy h lO-

Decashy da 10 1

10 decishy d 10


micro- Jl 10(

i nanoshy n 10

pleoshy p 10 1

femtoshy f 10

i

Jfea 11 illJ( I

I 000 000 000 i

t 000 000 1000

tOO

10 1

1 ]0

1 I U()

1 1000

1 1 000000

I 1 000 000 000

I 1 000 000 000 000

1 I 000 000 000 000 000





31 ml 1 cm

Dr Kalish Page 4

~ -Lowcst density

Greatest density

shy










i

None 0()O45


OO()OOO5 1









P Chemistry Dr Kalish Hand P Chapter 1









tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)









i



Solvent Til I

(0C) ktJ

(nC-kgmole) Tr

(0C) kr(OC-kgmole)




Nitrohcllene 2101 524 57() (152





I

a) e peCIIC


Specific Heat


(J895Aluminum ~




29Parutlin 0233


051 Water 4IX


Substance Hr

HO H-Ol

~Ht (kJimole) -23 -241x2 -2858









-3(l556 -187-

Br


-~155-12076CaCO FeO1 -649 -111-4

CI1 1 bull middot

FcOCaU -52()()

CJ I -1047 -749 lnO-

-il21 916


noo-3009 0 iC1H -4142-3935CO NaO

noo -110 I

HgtshyFc Na-SO

(lOn -28so -3629 -3957

HC) HBrJ SOe

middot9U


Coppcr i 205 472(



i



I Introduction


A Key Terms











B Properties



C Types of changes






1aterial


Substance

Elements Compounds


(Solutions)






















Length meter 111



B


Problems


d=mV


Problems


i

GiEa- G 10


Hectoshy h lO-

Decashy da 10 1

10 decishy d 10


micro- Jl 10(

i nanoshy n 10

pleoshy p 10 1

femtoshy f 10

i

Jfea 11 illJ( I

I 000 000 000 i

t 000 000 1000

tOO

10 1

1 ]0

1 I U()

1 1000

1 1 000000

I 1 000 000 000

I 1 000 000 000 000

1 I 000 000 000 000 000





31 ml 1 cm

Dr Kalish Page 4

~ -Lowcst density

Greatest density

shy










i

None 0()O45


OO()OOO5 1


















tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases


AP Chemistry Dr Kalish If and P Chapter 2






6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)











I Introduction


A Key Terms











B Properties



C Types of changes






1aterial


Substance

Elements Compounds


(Solutions)






















Length meter 111



B


Problems


d=mV


Problems


i

GiEa- G 10


Hectoshy h lO-

Decashy da 10 1

10 decishy d 10


micro- Jl 10(

i nanoshy n 10

pleoshy p 10 1

femtoshy f 10

i

Jfea 11 illJ( I

I 000 000 000 i

t 000 000 1000

tOO

10 1

1 ]0

1 I U()

1 1000

1 1 000000

I 1 000 000 000

I 1 000 000 000 000

1 I 000 000 000 000 000





31 ml 1 cm

Dr Kalish Page 4

~ -Lowcst density

Greatest density

shy










i

None 0()O45


OO()OOO5 1


















tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)













1aterial


Substance

Elements Compounds


(Solutions)






















Length meter 111



B


Problems


d=mV


Problems


i

GiEa- G 10


Hectoshy h lO-

Decashy da 10 1

10 decishy d 10


micro- Jl 10(

i nanoshy n 10

pleoshy p 10 1

femtoshy f 10

i

Jfea 11 illJ( I

I 000 000 000 i

t 000 000 1000

tOO

10 1

1 ]0

1 I U()

1 1000

1 1 000000

I 1 000 000 000

I 1 000 000 000 000

1 I 000 000 000 000 000





31 ml 1 cm

Dr Kalish Page 4

~ -Lowcst density

Greatest density

shy










i

None 0()O45


OO()OOO5 1


















tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)
























Length meter 111



B


Problems


d=mV


Problems


i

GiEa- G 10


Hectoshy h lO-

Decashy da 10 1

10 decishy d 10


micro- Jl 10(

i nanoshy n 10

pleoshy p 10 1

femtoshy f 10

i

Jfea 11 illJ( I

I 000 000 000 i

t 000 000 1000

tOO

10 1

1 ]0

1 I U()

1 1000

1 1 000000

I 1 000 000 000

I 1 000 000 000 000

1 I 000 000 000 000 000





31 ml 1 cm

Dr Kalish Page 4

~ -Lowcst density

Greatest density

shy










i

None 0()O45


OO()OOO5 1


















tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)










B


Problems


d=mV


Problems


i

GiEa- G 10


Hectoshy h lO-

Decashy da 10 1

10 decishy d 10


micro- Jl 10(

i nanoshy n 10

pleoshy p 10 1

femtoshy f 10

i

Jfea 11 illJ( I

I 000 000 000 i

t 000 000 1000

tOO

10 1

1 ]0

1 I U()

1 1000

1 1 000000

I 1 000 000 000

I 1 000 000 000 000

1 I 000 000 000 000 000





31 ml 1 cm

Dr Kalish Page 4

~ -Lowcst density

Greatest density

shy










i

None 0()O45


OO()OOO5 1


















tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)

















i

None 0()O45


OO()OOO5 1


















tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)


















tF = 18 tc + 32 tc = ------shy18




1

1

1




a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)











a) Iron b) Air











c) Cl d) CaCl2

e) Na f) KI









c) 00430 g d) 500 x 109 m

e) 160 x 10-9 s f) 00150 oC








a) E7033 and E70

34

b) E5728 and E66

28

c) E18674 and E186

74

d) E73 and E8

4

e) E2211 and E44

22


2) 11) 12) 13) 14) 15) 32) 36) 42) 46) 48) 50) 2) 8) 10) 12) 19)











c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)



















c) Kr-81 d) Te-121








e) Sodium



e) Sodium cyanide







e) Ba2+ f) Se2-


- b) NO3

- c) MnO4

-

d) CrO42-









20) 24) 25) 26) 38) 47) 48) 50) 52) 54) 56) 58) 60) 62) 64) 68)



phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)











phosphate


heptahydrate


l) Iron(III) oxide








a) H2O2 b) C6H16

c) C10H8 d) C6H16O



















8) 22) 26) 36) 37) 40) 43) 44) 50) 56) 58) 64) 68)









74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)

















74) 82) 84) 89) 90) 92)


Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)










Date Period






Mixture

cream









6 Iron rusts


8 Evaporation

9 Ice Melting

10 Milk sours

5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)









5



12 Wood rotting













7 Sour taste











2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)


















2000 g Mg x 06583 0 1317 gO 1 Mg

2000 g Mg 1317 gO 3317 g MgO







Examples








Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)















Relative Charge

Location in Atom



a neutrons A - Z







Ne-21 027 2099395 u Ne-22 922 ~O 2199138 u























Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)































Dr Kalish Page --l








rule with oxide

Prefix monoshy

umber 1

di- I-

trishy 3 i



110113shy 9

dec ashy 10 i









Chlorite CI02shy




















Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)


























Sulfuric Acid H2S04

b) ate-ic ite-ous








hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)
















hexshy (

heptmiddot 7
















b Not bases








6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)















6 Ketones (R-CO-R )





TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)










TABLE 21

Class



Cross Reference

H

Alkane

Alkene

Alkyne

Alcohol

Alkyl halide

Ether

Amine

Aldehyde

Ketone

Carboxylic acid

Ester

Amide

Arene

Aryl halide

Phenol

R-H

C=C

-C=Cshy

R-OH

R_Xb

R-O-R

R-NH2

0 II

R-C-H

0 II

R-C-R

0 II

R-C-OH

0 II

R-C-OR

0 II

R-C-NHz

Ar-Hd

Ar-Xb

Ar-OH

CH3CH2CH2CH2CH2CH3

CH2=CHCH2CH2CH3


CH3CH2CH2CH2OH


CH3-0-CH2CH2CH3

CH3CH2CH2-NH2

0 II

CH3CH2CH2C-H

0 II

CH3CH2CCH2CH2CH3

0 II

CH3CH2CH2C-OH

0 II

CH3CH2CHzC-OCH3

0 II

CH3CH2CH2C-NH2

(8j-CH2CH3

o-B CI-Q-OH

hexane

I-pentene

2-octyne

I-butanol

I-bromohexane








ethylbenzene

bromobenzene

4-chlorophenol


Section 910 Chap 23

Section 910 Chap 23

Section 210 Chap 23

Chap 23


Chap 15

Section 46 Chap 23

Section 46 Chap 23




Section 108 Chap 23

Chap 23

Section 910 Chap 23

In or bo

an cl~

by C3 21 na


C


11

o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)









o II

R-C-O-R or RCOOR



o II

CH3-C-O-CH2CH3




H H H H H I I I I I

H-C-N-H I H


or CHFH2NH2



~ummary





Summary 71




Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)










Key Terms






Acetic acid


H 0 I II


f











7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)









7

Dr Kalish Page 1


Name ___________________________________________ Date _______



1 SF4

~ R1Cl

3 PBrs

4 NcO

5 S L)

6 SoO)


carbon dioxide








13 MgCh

14 NaF

15 NacO

16 AhOl

17 KI

IR AIF

19 Mg1N2

20 FeCh

21 MnO

22 erN


23 Ca(OHh

24 (NH4hS

25 Al(S04h

2A H 1P04

shy~ Ca(N01)

Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)









Dr Kalish Page 2


2R CaCO

29 1acSO

30 Co(CHCOOh

31 Cuc(S03h

32 Pb(OHh


1 Magnesium sultide

2 Calcium phosphide

3 Barium chloride

4 Potassium nitride

5 Aluminum sulfide

6 Magnesium oxide

7 Calcium fluoride

R Lithium fluoride

9 Barium iodide

10 Aluminum nitride

II Silver nitride



14 Tin(H) sulfide



IIi Sodium bromate

17 Aluminum sulfite

18 Ammonium sulfate

19 Ammonium acetate



22 Zinc hydroxide



25 Iron(II) sulfate






Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)













Example Mass of CO2














MassofCH iIl 5S14g






























Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)




































Theoretical ield











Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)












Liters of solution










shy

I mole CaCI



C311~ = 3C 8H Moles I 3 8











Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)

















Anslcr CIIP (I(()




2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)









2




2CH30H + 30z--- 2COz + 4HzO








05438 g sample - (g C + g H) g 0



12011 g C 02836 g C1039 g CO2 X 44009 g CO 2


20158 g H 06369 g H20 X 180]5 g H 0 007127 g H

2




mass of 0 05438 g - 03549 g = 01889 g 0



ImolH 007127 g H X 1008 g H = 007070 mol H

1 malO

ForH

For 0 01889 g 0 X 15999 gO = 001181 mol 0


CQ02361 HO07070 O~ = C1999HS9870 1 OO1l81 001181 001181


Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)









Summary 123

Summary




Molar mass








~


no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)










no mol B

no mol A

no mol A

no molB






Review Questions













(a) 2 Hig) + 02(g) ~ 2 Hz0(l)

(b) 2 KCl03(s) ~ 2 KCI(s) + 3 Gig)









Note: Organic chemistry is no longer assessed on the APC … Chem summe… · Summer Assignment...

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Transcript of Note: Organic chemistry is no longer assessed on the APC … Chem summe… · Summer Assignment...