MATTER - PROPERTIES AND CHANGES...MATTER CHANGES (pp. 29 - 34) tVJjO I. A ~1-\'1.sICAL. CHAtJG8s one that affects physical properties only. The basic identity and structure of the

UNIT 2

MATTER - PROPERTIES AND CHANGES

MATTER (pp 21 - 24)

I. Matter is anything that has mass and volume.

2. The amount of matter in an object is known as __ n_'1_A_SS_~ _

3. The amount of space an object occupies is known as VOL \J 1\112"

Basic Units of Matter

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 .('10LE'CUU=:-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.

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:c.oU),t.. DVC.:'ILIT-{ .li:JLU~\LIT 1DENSlT'f \·t/-\ILDNIo:S S W\f

,:lH 'f 51(A L :;,c~n;-- 1<(::""'AC.TI\l1 T "i l.,or\-\ASS' FL~ ""'VIA 'BlLIT"1 'n'H n.::VOLl.'IV1G- (joo,e"

3. Properties fall into two basic categories: el-\ 'f S I LA L

IHM4Ll~!J\LIT1

Physical Properties

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

2. Examples are:cOl.-oILODO R..I"'41(.t);U(;'S .5

-rn s..11.?WV+LLV'l BIL II'!t>vcn L\ T'1

3. The __ ~",--r_J~~1_.l::_::- of matter is also a physical property.

4. The three common states of matter are: SOL I l)) L \410 i\)) 6AS

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 VAPOr(.room temperature.

refers to the gaseous state of a substance that is a solid or a liquid at

9. A fourth state, PLA ~ vr\f-l , exists at very high temperatures.

10. In this high-energy state the atoms are tom apart into smaller pieces.S"rAe..5

FUJOlt G'~(1::;;\.\T Ll6 1-\ ~

Intensive and Extensive Properties

I. A way to further describe physical properties.

2. An t.::)(Tl::-,\.ISI"';~ property is a physical property that depends on the quantity of matterpresent.

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3. .:!:'N11::'~SIv' ~

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

»vc Tn.' r'f , ScJL.-ul3l LI T'f

Chemical Properties

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

2. Examples are: a.~c.n VI T'"

FLA 11f\tl\A BI L\ Tl

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

blue color Jj) reacts with an acid cdensity r sour taste .rflammability e, melting point .I:solubility I combustibility e,hardness r reacts with water C-odor I luster ..rboiling point .r liquid .r

CONSERV AT ION 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. .

u~w of4. The Cu,oJ SI;:J2.YAn VI\.I of n~tate that mass is neither created nor destroyed during a chemicalreaction - it is conserved.

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

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

••••• A 1O.Ogsample of magnesium reacts with oxygen to form 16.6g magnesium oxide. How manygrams of oxygen reacted?

~ Mj (S) + O~~) -~ DJ fYJJO~)

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MATTER CHANGES (pp. 29 - 34)

tVJjO

I. A ~1-\'1.sICAL. CHAtJG8s one that affects physical properties only. The basic identity and structureof the material does not change.

2. Changes of state are physical changes.

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

4. These are called c'1~8l'\1(/4L CJ-\4JGtiJ ..\

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 t;Nl):)iH",'1LHlIC m.oQ:-SS is a physical/chemical change during which the system absorbsenergy from its surroundings.

8. An t;X01\-\E.f)W\\ c. f£aC.6s.5energy to its surroundings.

is a physical/chemical change during which the system releases

••••• 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 f \8JL:lo) slicing bread Pmelting ice cream p (t.:-'")J Dc))

Jell-O solidifying f (€'JC.O)

digesting toast C (\?"i0)

toasting a marshmallow C ~. P (1E)JJX.)

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

Mixtures and Pure Substances

I. A t'1J.e.t? ;;.uf;STArJC l: is matter made up of only one kind of atom or molecule.

rtLotJ I GOL \) I OKClvrn (!AR-;f;o;JAn;:) F0I'2..n1ALD/:;/f'f DG , 1:171A00/..

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

3. Both elements and compounds can be pure substances.

4. A (VII X/V,~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."sALAD M~.sSI~6J blaT G2ANIIG, A-I,z

Classification of Mixtures

I. Mixtures can be further classified as either 1-to'1106{:;AltlJ US

2. A homogeneous mixture is one in which the substances are uniformly distributed throughout.3. A heterogeneous mixture contains substances that are not evenly distributed.

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

5. Homogeneous mixtures are also known as .sCL0T1 0 t'-lS

6. Solutions can be gaseous, liquid, or solid.

Elements

I. 81::/11\ E=N'T S 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 113 known elements.

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

5. Elements can consist of single atoms or be diatomic.

Hq 'j 0;) } Fe. I C.A H» J /8l~

6. Some elements have p,u....crrrll.)f1C5

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

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Compounds

I. CVrv\,,"OcJrJ ()5 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 bronze

wine Ch1.PD

table salt (NaCI) CoWl? C> mayonnaise HOfl1

oil & vinegar dressing Hffmercury (Hg) EL

iron ore Hl?i copper (II) sulfate (CUS04) C-Vl-l P J)

Family Tree

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

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\

\,.-\ ~-------'\

~C.!V\f(} l,)i">.iJ)

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SEPARATION TECHNIOUES (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

1. F\ \.CreAT! 0 tV is used to separate heterogeneous mixtures of solids and liquids by using aporous barrier. The liquid passes through leaving the solid behind.

2. tNA ,t:tIi;?A T1O.Jleaving the solid behind.

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

3. C,e-klTe \ ~ v 6G'"- -uses spj~ing forces to pull all suspended~olids to the' bottom of the tubeleaving a liquid layer on top.

4. DE'MNTI 0 (; 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.5. c.HtoI114Tov/2AP8'f separates the components ofa solution. The components (mobile phase) travelacross the surface of another material (stationary phase)at different ratesbased on each other's attraction tothe stationary phase. . " -,

, 6, -OISTlL-LA-T70,J , •- 'separates the components -of a solution based. on differences in the boiling' -points of the substances involved: - . -

-,-, "

--.*.*.Ocean water can be made suitable for drinking by boiling the \Vater and then'condensingthev~porback to the liquid state. What is the name of this process? .

D\ !!:'ill-L .--\-110.0 -

***** 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?

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b. How doyou know?

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c. What separation technique is involved:

6-HQL'111/:tTO~j2A? 'H"1.

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· 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 "Systerne Intemationale" 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 Symbol

Length

Mass

Time S~CON .D s

Electric current

Thermodynamictemperature 1<

Amount ofsubstance

Luminous intensity

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 ofa living cell.

Prefix Symbol Meaning Power ofTen

GI<;(\ G IlILLlON /0 'I

MEGA M VHIU ..IO~ /0 '1: -rHO\Jf4A1 0 J/

I<\LO 10

01ett' ol Tl::7J'TH 10 -/

NUN iliZ&iYTH - ~ee~\+~' e 10f1itJ1)S4 "[OH-I

.. ..3/Vll' " (' /0J'Vl

IY! t cro_c,

1'< 1~11 LLIO~Jn-t 10

nanD ;1 fo ILUOk..I'71-l - r/0,°1:(,0 p lil IL.L iC;J '11-1 _IJ

/0

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 CYI-1

- the volume of a bathtub L

• the mass of an eyelash)+j /lr- NI.3

- the volume of an aluminum soda can f'Vl LDERIVED UNITS - VOLUME

I. 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:\/OL-UlVlG" Ll<-NGn-t l' WI/)H-f i I..J<=IGHT

s: h-'1 YVVl X ~

- 1''133. We are more familiar wi~husing the liter, L, as a volume unit.

4. More commonly we use the following units to measure volume: ..3i\'\ L .3miLl I L.. IH.nL. /YVI L;:- I em

t.W! CU81c CbJJ n tV! C:rTFrZ••••• Speed is calculated from length and time according to the following equation. What is the derivedSI unit?

Speed = distance / time s:/'11 8/:"7lJ

S eca-i» =

DENSITY (pp 142 - 146)

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

2. Density represents a ratio of mass to volume.

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

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 equation

lf

6. The units for density are usually:

.s!em J 012. f., L

••••• Determine the density of a piece of iron whose mass is 31.2 g and volume is 4.00 mL .

of. = .31. ;JJ:: :

'1.001>1 L

••••• Clover honey has a density of 0.498 glmL. Determine the mass ofa sample having a volume of225mL.

01..-=

••••• Determine the volume ofa piece of copper whose mass is 10.5g. The density of copper is 8.94glmL.

1'\1

d=v»1 10.:5.j

V ~ cJ.. z ? q<f ~ L ::. I. I 7 IrI 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 19.17Ig.Calculate the density of the ethyl alcohol.

tv] z: ,q./11 - IS. J.l/~ = .3. q;J.Sd-

v.:- S.oO h1 L- d > .s. : J. t{cJ Sj :: 0, TPS 4;;LV s.oo» L

••••• 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.

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