Intermolecular Forces (l) & (s) phases: 1.Molecule-molecule 2.Molecule-ion.
Chapter 5 Molecules and Compounds 2006, Prentice Hall Sucrose molecule (sugar), contains C, H, and O...
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Transcript of Chapter 5 Molecules and Compounds 2006, Prentice Hall Sucrose molecule (sugar), contains C, H, and O...
Chapter 5 Molecules and Compounds
2006, Prentice Hall
Sucrose molecule (sugar), contains C, H, and O atoms.
However, the properties of sucrose are very different
from those of C, H, and O alone. The properties of a
compound are, in general, different from the properties
of the elements that compose it.
molecular formula C12H22O11
2
CHAPTER OUTLINE
Definitions of Molecules and Compounds Law of Constant Composition Types of Compounds Binary Ionic Compounds (Type I and Type II) Polyatomic Ions Binary Molecular Compounds Naming Acids and Oxyacids Formula Mass
• molecule - consist of at least two different atoms in a definite arrangement held together by very strong chemical bonds.
• compound is a substance consisting of two or more elements in fixed and definite proportions
Definition of Molecule and Compound
Molecules and Compounds
• Salt– Sodium – shiny, reactive,
poisonous– Chlorine – pale yellow gas,
reactive, poisonous– Sodium chloride – table salt
• Sugar– Carbon – pencil or diamonds– Hydrogen – flammable gas– Oxygen – a gas in air– Combine to form white crystalline
sugar
Law of Constant Composition• all pure substances have constant composition
– all samples of a pure substance contain the same elements in the same percentages (ratios)
– mixtures have variable composition
H2O molecules
always a 2 H to 1 O
ratio
H2 & O2 mixture;
we could vary the
amount of either
element
6
LAW OF DEFINITECOMPOSITION
In a pure compound, the elements are always present in the same definite proportion by mass.
Mass of sample
Mass of N Mass of H
Sample 1 1.840 g 1.513 g 0.327 g
Sample 2 2.000 g 1.644 g 0.356 g
% N in Sample 1 =
% N in Sample 2 =
1.513 gx100 = 82.23%
1.840 g1.644 g
x100 = 82.20%2.000 g
Based on this law, the mass of an element can be determined from its mass percent in a compound.
7
Barium iodide, BaI2, contains 35.1% barium by mass. How many grams of barium does an 8.50 g sample of barium iodide contain?
Example 1:
22
g Ba8.50 g BaI x = g Ba
g BaI
35.1
1002.98
3 significant figures
8
When 12.66 g of calcium are heated in air, 17.73 g of calcium oxide is formed. What is the percent of oxygen in this compound?
Example 2:
3 significant figures
Mass of oxygen = 17.73 g – 12.66 g = 5.07 g
Percent oxygen =5.07 g
x 100 = 28.6%17.73 g
Formulas Describe Compounds
• a compound is a distinct substance that is composed of atoms of two or more elements
• a compound can be described by the number and type of each atom in the simplest unit of the compound– molecules or ions
• each element is represented by its letter symbol• the number of atoms of each element is written
to the right of the element as a subscript
Formulas Describe Compounds
water = H2O two atoms of
hydrogen and 1 atom of oxygen
table sugar = C12H22O11 12
atoms of C, 22 atoms of H and 11
atoms O
Tro's Introductory Chemistry, Chapter 5
11
Order of Elements in a Formula• metals written first
– NaCl
• nonmetals written in order from Table 5.1– CO2
– there are occasional exceptions for historical or informational reasons
• H2O fits rule, but does NaOH?
Table 5.1Order of Listing Nonmetalsin Chemical Formulas
C P N H S I Br Cl O F
Types of Chemical Formulas• An empirical formula gives the relative number of
atoms of each element in a compound. • A molecular formula gives the actual number of
atoms of each element in a molecule of the compound.
• For example, the molecular formula for hydrogen peroxide is H2O2, and its empirical formula is HO.
• The molecular formula is always a whole number multiple of the empirical formula.
• For many compounds, such as H2O, the molecular formula is the same as the empirical formula.
• A structural formula uses lines to represent chemical bonds and shows how the atoms in a molecule are connected to each other.
Comparison of Formulas and Models for Methane, CH4
• The molecular formula of methane indicates that methane has 1 carbon atom and 4 hydrogen atoms.
• The structural formula shows how the atoms are connected: each hydrogen atom is bonded to the central carbon atom.
• The ball-and-stick model and the space-filling model illustrate the geometry of the molecule: how the atoms are arranged in three dimensions.
Tro's Introductory Chemistry, Chapter 5
Classifying Materials• atomic elements = elements whose
particles are single atoms
• molecular elements = elements whose particles are multi-atom molecules
• molecular compounds = compounds whose particles are molecules made of only nonmetals
• ionic compounds = compounds whose particles are cations and anions
15
Molecular Elements• Certain elements occur as 2 atom molecules• Rule of 7’s
– there are 7 common diatomic elements– find the element with atomic number 7, N– make a figure 7 by going over to Group 7A, then down– don’t forget to include H2
H2
Cl2
Br2
I2
7VIIA
N2 O2 F2
Molecular Compounds
• two or more nonmetals
• smallest unit is a molecule
Ionic Compounds
• metals + nonmetals
• no individual molecule, instead these have 3-dimensional array of cations and anions made of formula units (NaCl)
Classify each of the following as either an atomic element, molecular element,
molecular compound or ionic compound
• aluminum, Al
• aluminum chloride, AlCl3• chlorine, Cl2• acetone, C3H6O
• carbon monoxide, CO
• cobalt, Co
= atomic element
= ionic compound
= molecular element
= molecular compound
= molecular compound
= atomic element
19
TYPES OF COMPOUNDS
Compounds are pure substances that contain 2 or more elements combined in a definite proportion by mass.
Compounds can be classified as one of two types:
Metals and non-metals
Two non-metals
Nomenclature of Compounds
Common Names – Are Exceptions(like nicknames)
H2O = water, steam, ice
NH3 = ammonia
CH4 = methane
NaCl = table salt
C12H22O11 = table sugar
Metal Cations• Type I
– metals whose ions can only have one possible charge
• IA, IIA, (Al, Ga, In)
– determine charge by position on the Periodic Table
• IA = +1, IIA = +2, (Al, Ga, In = +3)
• Type II– metals whose ions can have more
than one possible charge– determine charge by charge on
anion
How do you know a metal cation is Type II?
its not Type I !!!
22
BINARY IONICCOMPOUNDS (TYPE I)
Binary compounds contain only two elements. Ionic compounds are formed by combination of a
metal and a non-metal. Type I ions are those cations that form only one
ion. In these compounds, charges of the cations must
equal the charges of the anions since the net charge is zero.
23
BINARY IONICCOMPOUNDS (TYPE I)
Subscripts are used to balance the charges between cations and anions.
sodium bromide
Na+ Br
+1 -1 = 0
NaBr
No subscripts
needed
potassium sulfide
K+ S2
+1 -2 0
K2+
+2 -2 = 0
K2S
24
Write formulas for the following ionic compounds:
calcium chloride
Ca2+ Cl
+2 -1 0
CaCl2
sodium sulfide
Na+ S2
+1 -2 0+2 -2 = 0
Na2S
Example 1:
Cl2
+2 -2 = 0
Na2+
25
Type I Binary Ionic Compounds
• Contain Metal Cation + Nonmetal Anion
• Metal listed first in formula & name
1. name metal cation first, name nonmetal anion second
2. cation name is the metal name
3. nonmetal anion named by changing the ending on the nonmetal name to -ide
26
BINARY IONICCOMPOUNDS (TYPE I)
MgCl2 magnesium chloride
NaI sodium iodide
AlF3 aluminum fluoride
27
Name the following ionic compounds:
barium chloride
Na3P sodium phosphide
BaCl2
Example 2:
28
BINARY IONICCOMPOUNDS (TYPE II)
Type II ions are those cations that form more than one ion.
When naming compounds formed from these ions, include the ionic charge as Roman numeral, in parentheses, after the metal’s name.
This method of nomenclature is called the “stock” system.
29
1. name metal cation first, name nonmetal anion second
2. metal cation name is the metal name followed by a Roman Numeral in parentheses to indicate its charge (only difference from type II!)– determine charge from anion charge
3. nonmetal anion named by changing the ending on the nonmetal name to -ide
BINARY IONICCOMPOUNDS (TYPE II)
30
BINARY IONICCOMPOUNDS (TYPE II)
FeCl2
? -1
? -2 = 0
+2 -1iron (II) chloride
FeCl3
? -1
? -3 = 0
+3 -1iron (III) chloride
31
BINARY IONICCOMPOUNDS (TYPE II)
Cu2O
? -2
2? -2 = 0
+1 -2copper (I) oxide
Roman numeral DOES NOT
represent the subscriptCuO
? -2
? -2 = 0
+2 -2copper (II) oxide
32
BINARY IONICCOMPOUNDS (TYPE II)
Type II cations can also be named by an older method (classical).
In this system, cations with the higher charge end in –ic, while cations with the lower charge end in –ous.
In this system, some cations are named based on their Latin roots.
33
CLASSICAL SYSTEM (DERIVED FROM LATIN)
gold (aurum for Aurora the Roman goddess of the dawn)
silver (argentum for 'bright')
copper (cuprum for 'Cyprus' where the Romans first obtained copper)
tin (stannum for alloys containing lead)
lead (plumbum for 'lead')
mercury (hydrargyrum for 'liquid silver' or quick silver)
antimony (stibium for 'not alone')
iron (ferrum for 'firmness‘)
potassium (kalium via the Arabic qali for alkali)
sodium (natrium for soda)
34
BINARY IONICCOMPOUNDS (TYPE II)
FeCl2
+2 -1ferrous chloride
FeCl3
+3 -1ferric chloride
Lower charge
Higher charge
35
BINARY IONICCOMPOUNDS (TYPE II)
Cu2O+1 -2
cuprous oxide
CuO+2 -2
cupric oxide
Lower charge
Higher charge
36
SnCl2
? -1
? -2 = 0
+2 -1tin (II) chloride
Example 1:
Name each of the following compounds using the stock and classical nomenclature system:
Stock
ClassicalLower chargestannous chloride
37
Cu2S
? -2
2? -2 = 0
+1 -2copper (I) sulfide
Example 1:
Name each of the following compounds using the stock and classical nomenclature system:
Stock
ClassicalLower chargecuprous sulfide
38
Sn
Example 2:
Write formulas for each of the following compounds:
Tin (II) bromide Br
+2 -1
+2 -1 0
Br2
SnBr2
+2 -2 = 0
39
Sn
Example 2:
Write formulas for each of the following compounds:
Stannic oxide O
+4 -2
+4 -2 0
SnO2
+4 - 4 = 0
O2
ExamplesWhat, if anything, should go into the parenthesis
• LiCl = lithium ( ) chloride
• AlCl3 = aluminum ( ) chloride
• PbO = lead ( ) oxide
• PbO2 = lead ( ) oxide
• Mn2O3 = manganese ( ) oxide
XX
II
IV
III
41
POLYATOMIC IONS
Some ionic compounds contain polyatomic ions, an ion composed of several atoms bound together.
Patterns for Polyatomic Ions
1. elements in the same column form similar polyatomic ions
– same number of O’s and same charge
ClO3- = chlorate BrO3
- = bromate
2. if the polyatomic ion starts with H, the name adds hydrogen- prefix before name and add 1 to the chargeCO3
2- = carbonate HCO3-1 = hydrogencarbonate
Periodic Pattern of Polyatomic Ions
-ate groups
BO3-3 NO3
-1
SiO3-2
PO4-3
SO4-2
ClO3-1
AsO4-3
SeO4-2
BrO3-1
TeO4-2
IO3-1
CO3-2
IIIA IVA VA VIA VIIA
Patterns for Polyatomic Ions• -ate ion
– chlorate = ClO3-1
• -ate ion + 1 O same charge, per- prefix– perchlorate = ClO4
-1
• -ate ion – 1 O same charge, -ite suffix– chlorite = ClO2
-1
• -ate ion – 2 O same charge, hypo- prefix, -ite suffix– hypochlorite = ClO-1
© 2012 Pearson Education, Inc.
Naming Ionic Compounds Containing a Polyatomic Ion
• Some examples of more than two ions in the series.
ClO − hypochlorite BrO
− hypobromite IO −
hypoioditeClO2
− chlorite BrO2− bromite IO2
− ioditeClO3
− chlorate BrO3− bromate IO3
−
iodateClO4
− perchlorate BrO4− perbromate IO4
− periodate
When naming these ions in the homework, be sure to include the word ion in your answer, as in “perchlorate ion.”
46
POLYATOMICCOMPOUNDS
When writing formulas for polyatomic compounds, treat the polyatomic ion as one group.
potassium nitrate
K+ NO3–
+1 -1 = 0
KNO3
calcium hydroxide
Ca2+ OH–
+2 -1 0
(OH–)2
Ca(OH)2
+2 -2 = 0
47
POLYATOMICCOMPOUNDS
ammonium acetate
NH4+ C2H3O2
–
+1 -1 = 0
NH4C2H3O2
sodium sulfate
Na+ SO42–
+1 -2 0
Na2+
Na2SO4
+2 -2 = 0
48
POLYATOMICCOMPOUNDS
copper (II) nitrate
Cu2+ NO3–
+2 -1 0
Cu(NO3)2
(NO3–)2
+2 -2 = 0
Type IIRoman numeral
represents charge of ion
Alternate name =cupric nitrate
49
Mg(OH)2magnesium hydroxide
NaCN
Example 2:
Name the following polyatomic compounds:
Type I ion(Does not require roman numeral)
sodium cyanide
Fe2(SO4)3
Type II ion(Requires roman
numeral)
+3 2
iron (III) sulfate
ferric sulfate
Subclasses
• Compounds containing a metal and a nonmetal = binary ionic– Type I and II
• Compounds containing a polyatomic ion = ionic with polyatomic ion
51
BINARY MOLECULAR COMPOUNDS
Molecular compounds are formed by combination of 2 or more non-metals.
The smallest particles of molecular compounds are molecules.
These compounds are named similar to ionic compounds, with the second element named based on its root and suffix “-ide”.
52
BINARY MOLECULAR COMPOUNDS
Greek prefixes are used to indicate the number of atoms in these compounds.
Number Prefix Number Prefix
1 mono- 6 hexa-
2 di- 7 hepta-
3 tri- 8 octa-
4 tetra- 9 nona-
5 penta- 10 deca-
53
Examples:
Name the following binary molecular compounds:
CS2
carbon disulfide
First atom uses a prefix only when more than one
atom is present
Second atom always uses a
prefix
indicates 1 carbon atom
indicates 2 sulfur atoms
54
Examples:
Name the following binary molecular compounds:
IF7
iodine heptafluoride
indicates 1 iodine atom
indicates 7 fluorine atoms
55
SUMMARY OF BINARYNOMENCLATURE
Ionic Molecular
Type I
Type II
Naming Acids
• Contain H+ cation and anion– in aqueous solution
• Binary acids have H+ cation and nonmetal anion
• Oxyacids have H+ cation and polyatomic anion
Naming Acids• Binary Acids = hydro prefix + stem of the name of the
nonmetal + ic suffix
Example: HCl hydrochloric acid
• Oxyacids– if polyatomic ion ends in –ate = name of polyatomic ion with –ic
suffix
Example: HNO3 nitric acid– if polyatomic ion ends in –ite = name of polyatomic ion with –
ous suffix
Example: H2SO3 sulfurous acid
base name of oxyanion + -ic acid
base name of oxyanion + -ous acid
58
ACIDS
Acids are molecular compounds that form ions when dissolved in water.
Binary Acids
Formulas are written similar to binary ionic compounds, assigning a +1 charge to hydrogen.
HCl+1 -1
H2S+1 -2
59
NAMING BINARY ACIDS
When naming the acids, use hydro- prefix, followed by the name of the non-metal with an –ic ending, followed with the word acid.
HCl
H2S
acidhydrochloric
hydrosulfuric acid
HF hydrofluoric acid
60
POLYATOMICACIDS
Several polyatomic acids are important in the study of chemistry, and their names must be learned.
These acids and the polyatomic ions that form from their ionization are as follows:
Most of these are oxyacids
61
POLYATOMICACIDS
sulfuric acid H2SO4SO4
2
sulfate
phosphoric acid H3PO4PO4
3
phosphate
nitric acid HNO3NO3
nitrate
62
POLYATOMICACIDS
carbonic acid H2CO3
CO32
carbonate
HCO3
bicarbonate
acetic acid HC2H3O2C2H3O2
acetate
The names of acids containing oxyanions ending with -ite take this form:
The names of acids containing oxyanions ending with -ate take this form:
base name of oxyanion + ous
base name of oxyanion + ic
Names of Some Common Oxyacids and Their Oxyanions
Formula Mass: The Mass of a Molecule or Formula Unit
• also known as molecular mass
• For any compound, the formula mass is the sum of the atomic masses of all the atoms in its chemical formula:
Mass of 1 molecule of H2O = 2(1.01 amu H) + 16.00 amu O = 18.02 amu
66
THE END