Matter & Energy Chapter 3 Universe Matter Universe Classified Matter is the part of the universe that has mass and volume Energy is the part of the

Matter & Energy

Chapter 3

UniverseUniverse

UniverseUniverse

MatterMatter

Universe Classified

• Matter is the part of the universe that has mass and volume

• Energy is the part of the universe that has the ability to do work

• Chemistry is the study of matter– The properties of different types of matter– The way matter behaves when influenced

by other matter and/or energy

THREE STATES OF MATTER

• Solid -- has definite shape and definite volume ( stone, gold ring, NaCl crystal)

• Liquid -- has definite volume but no definite shape ( water, alcohol, blood, gasoline)

• Gas -- neither definite shape nor definite volume (air, helium, oxygen)

• solid, liquid, gas

States of Matter

State Shape Volume Compress Flow

Solid KeepsShape

KeepsVolume

No No

Liquid TakesShape ofContainer

KeepsVolume

No Yes

Gas TakesShape ofContainer

TakesVolume ofContainer

Yes Yes

Figure 3.1: Liquid water

takes the shape of its container

THREE STATES OF MATTER

Figure 3.11: In ice, the water molecules vibrate randomly about their positions in the solid

STATE OF MATTER DEPENDS UPON:

• Strength of the forces between the particles in the sample of matter (Stronger forces favor solids.)

• Conditions under which the sample exists -- the temperature and pressure (Lower temperatures and higher pressures favor solids.)

Properties

• Characteristics of the substance under observation

• Properties can be either directly observable orthe manner something interacts

with other substances in the universe

PHYSICAL PROPERTY

• - characteristic of a substance that can change without the substance becoming a different substance.

• Physical properties include:– color -density– odor - melting point– volume - boiling point– state (solid, liquid, gas)

CHEMICAL PROPERTY

• - the ability of a substance to change to a different substance.

• Chemical properties include the ability to:– react with acids– burn (combine with oxygen)– corrode or rust– sour or spoil– to ferment

Classify Each of the following as Physical or Chemical Properties

The boiling point of ethyl alcohol is 78°C.

Diamond is very hard.

Sugar ferments to form ethyl alcohol.

Classify Each of the following as Physical or Chemical Properties

The boiling point of ethyl alcohol is 78°C.– Physical property – describes inherent characteristic of

alcohol – boiling point

Diamond is very hard.– Physical property – describes inherent characteristic of

diamond – hardness

Sugar ferments to form ethyl alcohol.– Chemical property – describes behavior of sugar –

forming a new substance (ethyl alcohol)

PHYSICAL CHANGE

• -change in the form, size, shape, or state of a substance, but not its chemical nature; no chemical bonds are broken.

• Physical changes include:– melting - crushing – freezing - grinding– boiling - dissolving– evaporating - breaking

Figure 3.7: No chemical

change occurs when salt water is distilled

CHEMICAL CHANGE

• - the formation of new substance(s) with new properties through the reorganization of atoms -- a chemical reaction.

• Chemical changes include:– corroding - burning– rusting - rotting– souring - reacting with acids– fermenting - reacting with water

IS ELECTROLYSIS A

CHEMICAL OR

PHYSICAL

CHANGE?

Chemical

Classify Each of the following as Physical or Chemical Changes

Iron metal is melted.

Iron combines with oxygen to form rust.

Sugar ferments to form ethyl alcohol.

Classify Each of the following as Physical or Chemical Changes

Iron is melted.– Physical change – describes a state change, but the

material is still iron

Iron combines with oxygen to form rust..– Chemical change – describes how iron and oxygen

react to make a new substance, rust

Sugar ferments to form ethyl alcohol.– Chemical change – describes how sugar forms a new

substance (ethyl alcohol)

UniverseUniverse

MatterMatter EnergyEnergy

MatterMatter

HomogeneousHomogeneous HeterogeneousHeterogeneous

Pure SubstancePure Substance SolutionSolution

Physical Change

MixtureMixture

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HomogeneousHomogeneousPhysical Change HeterogeneousHeterogeneous

Pure SubstancePure Substance SolutionSolution MixtureMixture

Pure SubstancePure Substance

ElementElement CompoundCompound

ELEMENT

• - a substance that cannot be decomposed into simpler substances by chemical or physical means.

• Elements include:– oxygen - iron– silver - aluminum– carbon - nitrogen– gold - neon

02_29

1H

3Li

11Na

19K

37Rb

55Cs

87Fr

4Be

12Mg

20Ca

38Sr

56Ba

88Ra

21Sc

39Y

57La*

89Ac†

22Ti

40Zr

72Hf

104Unq

23V

41Nb

73Ta

105Unp

24Cr

42Mo

74W

106Unh

25Mn

43Tc

75Re

107Uns

26Fe

44Ru

76Os

108Uno

27Co

45Rh

77Ir

109Une

110Uun

111Uuu

28Ni

46Pd

78Pt

29Cu

47Ag

79Au

30Zn

3 4 5 6 7 8 9 10 11 12

48Cd

80Hg

31Ga

49In

81Tl

5B

13Al

32Ge

50Sn

82Pb

6C

14Si

33As

51Sb

83Bi

7N

15P

34Se

52Te

84Po

8O

16S

9F

17Cl

35Br

53I

85At

10Ne

18Ar

36Kr

54Xe

86Rn

2He

58Ce

90Th

59Pr

91Pa

60Nd

92U

61Pm

93Np

62Sm

94Pu

63Eu

95Am

64Gd

96Cm

65Tb

97Bk

66Dy

98Cf

67Ho

99Es

68Er

100Fm

69Tm

101Md

70Yb

102No

71Lu

103Lr

1A

2A

Transition metals

3A 4A 5A 6A 7A

8A1

2 13 14 15 16 17

18A

lkali

me

tals

Alkalineearth metals Halogens

Noblegases

*Lanthanides

† Actinides

PERIODIC TABLE OF THE ELEMENTS

COMPOUND

• - a substance with constant composition that can be broken into elements by chemical processes.

• Compounds include:– water - sodium chloride– ethanol - ammonia– sugar - carbon dioxide– potassium nitrate - sodium hydroxide

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HomogeneousHomogeneous Physical Change HeterogeneousHeterogeneous


ElementElement CompoundCompoundChemical Change

HETEROGENEOUS MATTER

• - has different properties throughout -- a mixture.– Salt and pepper– soil– granite– sea water– spaghetti & meat balls

Pure Substances vs. Mixtures• Pure Substances

– All samples have the same physical and chemical properties

– Constant Composition all samples have the same composition

– Homogeneous

– Separate into components based on chemical properties

• All mixtures are made of pure substances

Pure Substances vs. Mixtures• Mixtures

– Different samples may show different properties

– Variable composition

– Homogeneous or Heterogeneous

– Separate into components based on physical properties

• All mixtures are made of pure substances

Figure 3.5: Sand and water do not mix to form a uniform mixture

SEPARATION OF MIXTURES

- mixtures can be separated by physical means. – distillation– filtration– centrifuging– magnet– evaporation– chromatography

Separation of Mixtures• Separate mixtures based on different

physical properties of the components– Physical change

EvaporationVolatility

ChromatographyAdherence to a Surface

FiltrationState of Matter (solid/liquid/gas)

DistillationBoiling Point

TechniqueDifferent Physical Property

Figure 3.6: Distillation of a solution consisting of salt dissolved in water

Figure 3.8: Filtration separates a liquid from a solid

CENTRIFUGE

Paper Chromatography

Chromatography has two phases of matter: a stationaryphase (the paper) and a mobile phase ( the liquid).



Electron ShellsElectron Shells NucleusNucleus

Chemical Change

HOMOGENEOUS MATTER

• - a substance with the same properties throughout -- a pure substance.

• Elements and compounds are pure substances (homogeneous matter).

SOLUTION

• - is a homogeneous mixture.

• - has a variable composition...

• - can be separated by physical means.

• - no evidence of a chemical change when a solution is formed.

Figure 3.9: Separation of a sand-saltwater mixture

Identity Each of the following as a Pure Substance, Homogeneous Mixture or

Heterogeneous Mixture

Gasoline

A stream with gravel on the bottom

Copper metal

Identity Each of the following as a Pure Substance, Homogeneous Mixture or

Heterogeneous Mixture

Gasoline – a homogenous mixture

A stream with gravel on the bottom– a heterogeneous mixture

Copper metal– A pure substance (all elements are pure substances)

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Electron LevelsElectron Levels NucleusNucleus



Electron ShellsElectron Shells NucleusNucleus

Chemical Change

ElectronsElectrons ProtonsProtons NeutronsNeutrons

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MatterMatterEnergyEnergy




Electron LevelsElectron LevelsNucleusNucleus


EnergyEnergy

Potential Energy

Potential Energy

Kinetic EnergyKinetic Energy

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Potential Energy

Potential Energy

Kinetic Energy

Kinetic Energy

Potential EnergyPotential Energy

PositionPosition CompositionComposition

UniverseUniverse







Potential Energy

Potential Energy

Kinetic Energy

Kinetic Energy

PositionPositionCompositionComposition

PositionPosition

GravitationalGravitational ElectrostaticElectrostatic

UniverseUniverse







Potential Energy

Potential Energy

Kinetic Energy

Kinetic Energy



CompositionComposition

NuclearNuclear ChemicalChemical

Energy and Energy Changes

• Capacity to do work– chemical, mechanical, thermal, electrical,

radiant, sound, nuclear

• Energy may affect matter– e.g. raise its temperature, eventually causing a

state change– All physical changes and chemical changes

involve energy changes

Energy and the Temperature of Matter

• The amount the temperature of an object increases depends on the amount of heat added (Q).– If you double the added heat energy the

temperature will increase twice as much.

• The amount the temperature of an object increases depends on its mass– If you double the mass it will take twice as

much heat energy to raise the temperature the same amount.

Units of Energy

• One calorie is the amount of energy needed to raise the temperature of one gram of water by 1°C

kcal = energy needed to raise the temperature of 1000 g of water 1°C

• joule

4.184 J = 1 cal 4.184 kJ = 1 kcal• In nutrition, calories are capitalized

1 Cal = 1 kcal

Converting Calories to Joules

251J)cal 1

J 4.184(60.1cal)(

joules 4.184 cal 1

Convert 60.1 cal to joules

Specific Heat Capacity

• Specific Heat (s) is the amount of energy required to raise the temperature of one gram of a substance by one Celsius degree

• Specific heat is a characteristic or identifying property of matter.

C gJ

4.184 is water ofheat specific the,definitionBy

ENERGY CALCULATIONS

• Heat (Q) -- J

• mass (m) -- g

• specific heat (s) -- J/gCo

• “change” in temperature (t) -- Co

• Q = m s t

Calculate the amount of heat energy (in joules) needed to raise the temperature of

7.40 g of water from 29.0°C to 46.0°C

C 29.0 - C46.0 T

J 526 Q C g

J 4.184 s

C)0.17)(C g

J184(7.40g)(4. Q g 7.40 m

t s m Q ? Q

A 1.6 g sample of metal that appears to be gold requires 5.8 J to raise the temperature from 23°C

to 41°C. Is the metal pure gold?

C g

J0.20s C 23 - C41 T

C)18 g)( (1.6

J 5.8 s ? s

t)(m)(

Q s g 1.6 m

t s m Q J 5.8 Q

Table 3.2 lists the specific heat of gold as 0.13Therefore the metal cannot be pure gold.

C gJ

UniverseUniverse






ElectronsElectronsProtonsProtons NeutronsNeutrons

Potential Energy

Potential Energy

Kinetic Energy

Kinetic Energy



NuclearNuclear

ChemicalChemical

Nuclear Change

Chemical Change

“TO BUILD FROM MATTER IS SUBLIMELY GREAT, BUT GODS AND POETS ONLY CAN CREATE.”

Pitt

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Matter & Energy Chapter 3 Universe Matter Universe Classified Matter is the part of the universe that has mass and volume Energy is the part of the