UNIT 2

MATTER - PROPERTIES AND CHANGES

MATTER (pp 21 - 24)

1. Matter is anything that has mass and volume.

2. The amount of matter in an object is known as --'.-M_A_S_S _

3. The amount of space an object occupies is known as VOUJME'

Basic Units of Matter

I. __A_TO_n.5__ · are the basic units of matter.

2. There are over 110 different kinds in the known universe. These are catalogued on the periodic table.

3. Atoms combine to form MOLEtLlU:Sby chemical bonds.

. Molecules are a neutral group of atoms held together

4. A molecule may contain any number of atoms, but it behaves as one unit.

http://www.youtube.com/watch?v=Gxwj24mREyA

PROPERTIES OF MATTER (pp. 29 - 34)

.---...., I. Different types of matter are described by listing their characteristics, or properties.

2. Some properties of matter used to describe things are:COLOR.. fiAQ..DI\{E'SS DDo/(

MA S S t<.t="'):\tTlVIT"f mSre"OLUIY\~ ':;LAMW1t1'BlL'T"f MPov en LIT 'f s.o wI.! J L I r 'f

SOlt!)

UCylVI.!)

b4J

3. Properties fall into two basic categories: PH,/SICt+L

Physical Properties

I. These are properties that can be observed or measured without changing the composition of matter.

2. Examples are: COLull, ODOfl f\.lP. occ ri L l T"f fit D/:'N5', rt, J I

3. The .srn·T1? of matter is also a physical property.

4. The three common states of matter are: So Ll t) I L\ ~ V I()I GA.5

• Phases of MatterGlerm

ResearchCenter

SolidHolds Shape

Rxed Volume

LiquidShape of Container

Free SurfaceFixed Volume

• •• •• ••

• • • • •• •• • • • •• ••• • ••• •

•

Gas

Shape of Container

Volume of Container

5. Solids have a fixed volume and shape. The atoms and molecules are held tightly in a rigid structure, butdo vibrate slightly about fixed positions.

6. Liquids have a fixed volume, but a variable shape. The atoms and molecules are not held together in arigid manner. This allows them to move past one another and flow.

7. Gases have no fixed shape or volume and therefore expand to fill any container they occupy.

8. The word _v_A-_p_O_Q. refers to the gaseous state of a substance that is a solid or a liquid atroom temperature. (Sfk'"A-M)

9. A fourth state, P Ll1.5 W\ A , exists at very high temperatures.

10. In this high-energy state the atoms are torn apart into smaller pieces called _

II. A fifth state of matter, called the 13oSt;- 8 t-i.H"EltJ CoNDt.')1JAflfas proposed in 1925 by aphysicist from India, Syendra Bose, and confirmed by Albert Einstein. It exists as temperatures nearingabsolute zero.

http://www.youtube.com/watch?v=1 RpLOKgTcSk

Intensive and Extensive Properties

1. A way to further describe physical properties.

2. An Ex TlEI-i S I VEpresent. (MA::'$ VOLUMe=.

"

property is a physical property that depends on the quantity of matter1.c.-"Nc,n4 b IAMI::/l::"12... )

, I

properties are physical properties that depend on how matter is structured.

Chemical Properties

1. These are properties that can be observed only when substances interact with one another.

2. Examples are: R.~c..TI V IT 'fF U\I\I\N\.l\'8IL IT .•...(

***** Classify the following as a chemical property, intensive physical property, or extensive physicalproperty:

blue color rdensity :rflammability C.solubility rhardness :rodor rboiling point I

reacts with an acid Csour taste Imelting point :7combustibility Creacts with water Cluster rliquid .r

CONSERVATION OF MASS

I. Although matter can undergo both physical and chemical changes, the total amount of matter does notchange.

2. This is obvious for physical changes, but not always so for chemical changes.

3. Early scientists used analytical balances to determine the mass of the reactants and products. Theydiscovered both were equal.

c.ONSav.l\nO,J4. The tA~v 0 F of MA.s..s state that mass is neither created nor destroyed during a chemicalreaction - it is conserved.

5. In the form of an equation, it looks like:

M AS (1 - IV1ASS AD.~ """c.::r-r..)~J\cn::v..ns - '\ I !UJ uv ~

6. Lavoisier discovered that when mercury(II) oxide decomposes to form mercury and oxygen, the mass ofthe reactants will equal the mass of the products.

d~O ~7 dijy ~ O~I~

***** A IO.Ogsample of magnesium reacts with oxygen to form 16.6g magnesium oxide. How manygrams of oxygen reacted?

~ J1j (S) of O;1J) -7 oJ JlfJ () (s)

(0 4- X := I~.C,

'X - {,'(,J--

-~

MATTER CHANGES (pp. 29 - 34)

1. A PHi SICA L tHANG (isone that affects physical properties only. The basic identity and structureof the material does not change.

2. Changes of state are physical changes.

Changes in States of Matter

3. Some changes involve the rearrangement of atoms and the production of new materials.

4. These are called tH 1::1111U.l L CHatJ6 <SJ

5. During a chemical change atoms are rearranged, but there is no loss or gain in the total number ofatoms.

6. In the process of both physical and chemical changes, energy can be either released or absorbed. Thesechanges, where energy is transferred from the system to, or from, the surroundings, have been given specialnames.

7. An ENJX)~111IC CHAt-16fenergy from its surroundings.

is a physical/chemical change during which the system absorbs(MI::"l...niJ6 / /?JoIL/lJ6)

8. An c)(O·TU~J'1(C C.H-AJ6~energy to its surroundings.

is a physical/chemical change during which the system releases( PtLEF2:J,J 6· / CON i)C1J S't4TlO,..J )

***** Classify each of the following as either a physical or chemical change. If applicable, also indicatewhether the change is endothermic or exothermic:

grinding coffee beans P slicing bread f

digesting toast C melting ice cream P l:7.J.D()

toasting a marshmallow P {' CE""iVDO

Jell-O solidifying 7>

CLASSIFICATION OF MATTER (pp. 24 - 29; 34 - 39)

Mixtures and Pure Substances

I. A PlJf2E sua Sfl.)iJ ~ is matter made up of only one kind of atom or molecule.lrTlo i-J I Gol-D I DI5nl-4--n W4~ I t::OIlM4l-/)l.:f.I'fDl:)

2. Pure substances have a fixed composition and a unique set of properties.

3. Both elements and compounds can be pure substances.

4. A MI ~ TVR.t=" is a collection of two or more pure substances that are physically mixedtogether. Thus, a mixture cannot be represented by a chemical formula.

5. The properties of different substances in a mixture can vary.

6. The properties of mixtures can vary. Each substance in a mixture retains its chemical identity.(nY-\UA.J S4l4D Dh:"""jSluG} 77l41L mIX I tuer GllArJiTG" I4lftJ

Classification of Mixtures 'I

1. Mixtures can be further classified as either l-/ofVI06/::/J &7JvJ

2. A homogeneous mixture is one in which the substances are uniformly distributed throughout.(GL\SOLII'JE I h1ILK, ALLOY)

Homogeneous Mixture

3. A heterogeneous mixture contains substances that are not evenly distributed.

(l)/(l.:r I 120(.K.S J A Ie. )

4. Some parts of a heterogeneous mixture have different properties than other parts.

5. Homogeneous mixtures are also known as.5tJLV710rJS

6. Solutions can be gaseous, liquid, or solid.(He.JO,- I3flt:'JW.I."J6 Altl)

Elements

4LLcV-.S- ST1::'"bL.

- PI:1N 17:'"Il.

1. FL.FrYl El-JTS are the simplest pure substances because they contain only one type of atom.An element cannot be separated into simpler substances by physical or chemical means.

2. Every element has its own unique set of physical and chemical properties.

3. There are 91 naturally occurring elements 118 known elements.

4. About one dozen elements compose the things we notice every day.

5. Elements can consist of single atoms or be diatomic. ,~~, A, ) Cu, h.6. Some elements have f-\ Ll.() Ti20P 1E.s

7. Allotropes are different molecular forms of an elements that exist in the same physical state.

a. Diamondb. Graphitec. Lonsdaleited. C'60 Fullerenee. C'MO Fullerener. C'70 Fullereneg. Amorphous carbonh. Carbon nanctubes

Compounds

1. COI'l"lPou A.l CS are pure substances that are composed of two or more different elements thatare chemically combined.

2. They are created when atoms of different elements join together in a chemical reaction.

3. Every compound has a unique set of properties. These properties are often very different from theproperties of the elements that make up the compound.

***** Classify each of the following as an element, a compound, a homogeneous mixture, or aheterogeneous mixture:

air 4eT' bronze ItO""e

mercury (Hg)

wine /iOIYlO iron ore I~~I

copper (II) sulfate(CuSO~) (.

table salt eNaCI) C mayonnaise Horn oil & vinegar dressing H I:-T

Family Tree

I. In summary the family tree for matter looks like:

MaHer

!--'PURESU8STANCES

~-~-l

1IMPURESU8STANCES

(MIXTURES)

~-~'---lELEMENTS COMPOUNDS

(Hydrogen. Carbon (Wofer,Ammonlo) HOMOGENEOUSIron) MIXTURES

i (Salt solulion. Ale.ahotand WoterJr--- --~--1

HETEROGENEOUSMIXTURES

(Soli. Wood)

NON·METALS(Sulphut)

METALLOIDS NOBlE GASES(Arsenic) (Helium)

METALS{Sliver}

SEPARATION TECHNIQUES (pp. 39 - 41)

I. In order to study the composition of mixtures, they must be separated. This can be accomplished usinga variety of physical means.

2. These separation techniques make use of differences in the physical properties of the materials in themixture.

3. Thus, the materials obtained are not chemically changed by the process.

Techniques

I. FlLn2An0 ~( is used to separate heterogeneous mixtures of solids and liquids by using aporous barrier. The liquid passes through leaving the solid behind.

$OL- eo l..sOL-uqLtQ·· LlCf

GAS - GAS

SOL- GAJ

FiltratIon/SOlYGnI

/ filterpaper

Lrillerrunnel

/L--- resklua

~)==t="""= Qnsoluble solid)

clamp

l hltlllto(soluble &OIiddissolYGd in soMlnl)

2. t?VAtA?QA.no~leaving the solid behind.

is used to separate solids and liquids by allowing the liquid to evaporate,

LIQ - S/O) LII> f': t I;.f'Y''' : : ~ :I:!.. _. "<. ' ,

1'1: '.' <, ~,.;,,·~T.... ;-'.,'::'1 ' •• " , f' ...;} :.' ':..,.' I : :- •

:';\ I • :', : ; ; l';. :

3. e.~1ll.1j:\J6~ uses spinning forces to pull all suspended solids to the bottom of the tubeleaving a liquid layer on top.

Ll~-S()L

4. "be-U\rJ.n,.j (; is pouring the liquid layer off the top of a solid-liquid mixture once the solidhas settled or been centrifuged to the bottom, This can be done with liquid layers, but it is more difficult.

1Iq - So L

1Undissolved solid

5. tl+/l{)m4 Tll6/lA PH Y separates the components of a solution. The components (mobile phase) travelacross the surface of another material (stationary phase) at different rates based on each other's attraction tothe stationary phase.

Simple chromatography

6. ))tSn lLADON separates the components ofa solution based on differences in the boilingpoints of the substances involved.

LlCV - LI 9Ltc? - SoL

***** Ocean water can be made suitable for drinking by boiling the water and then condensing the vaporback to the liquid state. What is the name of this process?

]),.snL..lIl,T1(}~ - D~Sl\L11\J1-\17D~1

***** A forgetful student leaves an uncapped watercolor marker on an open notebook. Upon returning shediscovers the leaking marker has produced a rainbow of colors on the top page.

a. Is the ink a pure substance or a mixture?

n11 XWe.I:-

b. How do vou know?

c. What separation technique is involved.

.--_._ .._-------------------------;------------------------.

STANDARD UNITS

I. In 1960, scientists adopted a part of the metric system to use as the standard scientific system ofmeasurement units. This is called the "Systeme Internationale" or SI.

2. There are seven basic units. These base units can be combined in various ways to describe nearly allphysical measurements. They are:

Quantity Unit Symbol

Length M~ I'V\

Mass K lLOGI2A t\I\%,3

Time SECONb S

Electric current A MP82·.E AThermodynamic

KELVIN t<temperature

Amount of Mo\..E Molsubstance

Luminous intensity Cl'\rJOELA cd.PREFIXES

I. Any SI unit can be modified with prefixes to match the scale of the object being measured. Metersmight be suitable for measuring a person's height, but not the diameter of a living cell.

51 51PREFIX SYMBOL

yotta y

zetta Zexa Epeta Ptera. Tgiga Gmega M

kilo k

hecto h

deca da

deci dcenti cmilli m

micronano n

pico p

femto f

atto azapto zyocto y

SI UNIT CONVERSION FACTOR(STANDARD FORM)

FACTORLANGUAGE

FACTOR(POWER)

1 yottametre = 1 000 000 000 000 000 000 000 000 metres septillion

1 zettametre = 1 000 000 000 000 000 000 000 metres sextillion

1 exametre = 1 000 000 000 000 000 000 metres quintillion1 petametre = 1 000 000 000 000 000 metres quadrillion1 terametre = 1 000 000 000 000 metres trillion1 gigametre = 1 000 000 000 metres billion

1 megametre = 1 000 000 metres million1 kilometre = 1 000 metres

1 hectometre = 100 metres1 decametre = 10 metres

thousand

hundredten

1 metra= l:nietre1decimetre = 0.1 metres 10-1 tenth

1 centimetre = 0.01 metres hundredth1 millimetre = 0.001 metres thousandth

1 micrometre = 0.000 001 metres millionth

1 nanometre = 0.000 000 001 metres billionth1 picometre = 0.000 000 000 001 metres trillionth

1 femtometre = 0:000 000 000 000 001 metres quadrillionth

1 attometre = 0.000 000 000 000 000 001 metres1 zeptometre = 0.000 000 000 000 000 000 001 metres1 yoctometre = 0.000 000 000 000 000 000 000001 metres

quintillionth

sextillionthseptillionth

2. The prefixes can be combined with various units to describe the size of a measurement.

***** Suggest appropriate SI units and prefixes to measuring the following objects:

- the length of your chemistry book

eM- the volume of a bathtub

l- the mass of an eyelash

VVlj ofL 10- the volume of an aluminum soda can m LDERIVED UNITS - VOLUME

1. The seven base SI units cannot measure every observable property; therefore derived units are createdby multiplying or dividing the seven base units in various ways.

2. The derived unit for volume is obtained by using length, width and height measured in meters:

" z: ..Q xw- x: h:: VVl X vY\ X V\f)::: ;11 3

3. We are more familiar with using the liter, L, as a volume unit.

1000 L:: I fI1 3

4. More commonly we use the following units to measure volume:

"'~ f LLI L-/T/;;It. »t LCU!3IC. C.ENTI fVlETC~ em 3

***** Speed is calculated from length and time according to the following equation.S! unit?

.3I em

What is the derived

Speed = distance / time t: z:

DENSITY CPp 142 - 146)

I. Density is an intensive property. It does not depend on the quantity of matter present.

2. Density represents a ratio of mass to volume.

MASS

v 0 Lv l\I\ <::

3. One interpretation of density is that it is a measure of how tightly matter is packed together.

- _.A substance with the

same amount ofmatter but with asmaller volume ismore dense and

viceversa

A substance which occupies thesame volume and has more

matter is more dense.

4. Because the density of a substance is the same for all size samples of that substance, density can be usedas a means of identifying materials.

5. To calculate density, one uses the following equationbl3JS ITi:= VVlAS.s s: fY\

Va...Ul'V\l.: V

6. The units for density are usually:

***** Determine the density of a piece of iron whose mass is 31.2 g and volume is 4.00 mL.d::: W( 31. d.

Y tj.OO 7. 6'0 ~.mL

***** Clover honey has a density of 0.498 g/rnl.. Determine the mass ofa sample having a volume of225mL.

***** Determine the volume of a piece of copper whose mass is 10.5g. The density of copper is 8.94g/mL.

10, Sf,9t(

I. 17 /11. L

***** To determine the density of ethyl alcohol, a student pipets a 5.00 mL sample into an empty flaskwhose mass is 15.246g. She finds that the mass of the flask and the ethyl alcohol is now 19.171 g.Calculate the density of the ethyl alcohol. JI1.(,3, q,;.J

d:: Vv z: S. (90 mLIq~n(-IS.J4-"

,3. qJSj***** A solid with an irregular shape and a mass of 12.65g is added to a graduated cylinder filled withwater to the 29.7 mL mark. After the solid sinks to the bottom, the water level of the graduated cylinder isread to be 36.6 mL. Calculate the density of the solid.

77-1I S .IS rue u)1tT7:::7C.. DI s,aLA Cf:;?rIl::.AJT /VI eTN ()b

5.00

e 7FS

V :: 3t,. 0- ;J q. 7

~,'1 h1LJ...:= 1;;2, (05

u,q

I. e3 3333 3 33

3/.23 rot:=