MatterPhysical and Chemical

Properties

1

Matter vs. Energy

• The universe is made up of matter and energy.

• Matter:– Has mass and takes up space (volume)– Is usually a “thing”

• Energy:– Does not have mass or take up space– Energy moves matter!!!!!!

• ** Energy is the ability to make things move. Light, heat, sound, motion, and electricity are all forms of energy.

2

Properties of Matter• Property -characteristic that

distinguishes one type of matter from another– Chemical– Physical

• Specific property – a property that allows for the ID of matter

• For 2 separate samples of matter to be the same kind of matter, they have to have all the same specific properties

3

Extensive/Intensive

Intensive – Does not depend on the amount of material

Examples: temperature, density, boiling point

Extensive – Depends on the amount of material

Examples: mass and volume

4

Physical Properties

• Physical property- any property of matter that can be observed or measured without changing the identity of the matter

• Examplescolor shapetaste

densitystate/phasemalleability

D = M V

5

Volume and Density

• Volume= length X width X height• Density= mass (g) volume (mL or cm3)

• 1 mL = 1 cm3

Which is more dense?6

Physical Properties• States of matter:

– Bose-Einstein

– Solid – Liquid– Gas– Plasma

(Newest State)

7

States of Matter

Solid - fixed shape and volume and particles close together so rigid structure - particles vibrate only – no movement

Liquid - fixed volume & takes shape of container - particles farther apart than solid - little order - particles can move around

Gas - takes volume and shape of container - particles are far apart - random motion of particles

Physical Properties of Fluids

• Viscosity- the resistance of a fluid to flowing.

• Viscousmaple syrup (cold especially!)

• Not viscouswater

9

Physical Properties of Solids

• Malleable- able to be hammered or pressed out of shape without breaking

• This is a property of many metals

10

Chemical Properties

• Chemical property- property of matter that describes a substance based on its ability to change into a new substance

• Examplesflammability

reactivity with vinegarreactivity with oxygenreactivity with water

Iron + Oxygen Iron oxide (rust)

2Fe + 3O2 Fe2O311

Let’s Do It!!! Label your paper 1-5Chemical or Physical Property?Chemical vs. Physical Property

video1. Paper is white

2. Boiling point of H2O is 100oC

3. Zinc reacts with hydrochloric acid and creates hydrogen gas

4. Nitrogen does not burn

5. Sulfur smells like rotten eggs

Physical Property

Physical Property

Physical Property

Chemical Property

Chemical Property

12

Reference-Comparing Physical and Chemical

PropertiesSubstance/Matter Physical Property Chemical Property

Helium Less dense than air Nonflammable

Wood Grainy texture Flammable

Baking soda White powder Reacts with vinegar to produce bubbles

Powdered sugar White powder Does not react with vinegar

Rubbing alcohol Clear liquid Flammable

Red food coloring Red color Reacts with bleach and loses color

Iron Malleable Reacts with oxygen

13

Changes in Matter

• Matter is constantly changing• There are two types of changes in

matter:– Chemical– Physical

14

Physical Changes

• Physical change- a change in shape, size, color, or state a change without a change in chemical composition– Examples

tearing paper cutting your hair change in state

• Some mixtures can be separated based on their physical properties

Physical changes are

not indicative of a chemical reaction

15

Let’s Do It!!!

• Get with a partner• Google “Harcourt Mixtures Lab”

and click on the link for “The Mixtures Lab” and read the info on the left.

• Draw the chart from the lab in your notes. You have 15 minutes

• The Mixtures Lab• Online stopwatch 16

Chemical Changes• Chemical change- a change in which a

substance becomes another substance having different properties– A change that is not reversible using

ordinary physical means – Changes that usually cause, heat, sound,

light, odor, fizzing/foaming, color changes– Examples

mixing vinegar & baking sodaburning a piece of wood

soured milk

A chemical analysis is the only 100% way to know a

chemical change has occurred.

17

Chemical Changes

• Chemical reaction- the process by which a chemical change occurs

• Types of chemical reactions– Synthesis (creating)– Decomposition (separating)– Combustion (burning)– Displacement/Replacement

(switching of atoms)

18

Chemical Changes• During chemical

changes, atoms are rearranged, and chemical bonds are broken and reformed

• One or more substances change to produce one or more different substances

O2H2

What does H2 & O2 gas

create?

19

Let’s Do It!!!!Label your paper 1-5

Chemical or Physical Change?1. Bending a Paper Clip

2. Baking a cake

3. The sublimation of carbon dioxide

4. Crushing an aluminum can

5. Vinegar and baking soda combining to create salt and water

Physical Change

Chemical Change

Chemical Change

Physical Change

Physical Change

20

Changes are either…. Endothermic – absorbing

energy • ex. boiling water

• Exothermic - releasing energy

ex. burning a candle

21

Nuclear Changes/Reactions

• A new substance is formed by changes in the atoms themselves - not just by rearranging the atoms.

22

Nuclear Reactions

• The TOTAL of mass plus energy is conserved.

• Mass + Energy of reactants =Mass + Energy of products

• Matter can change into energy and energy can change into matter.

23

Einstein’s Equation

• E = mc2

• Einstein is saying that matter and energy are different forms of the same thing!• c =(3.00 x 1010 cm/sec)2

24

How much energy can be obtained by completely converting 1.00g of

matter into energy?• E = mc2

• E = (1.00g) (3.00 x 1010 cm/sec)2

(after adjusting units)

• E = 21,500,000,000,000 calories

25

This means……

• SMALL amounts of matter convert to

LARGE amounts of energy

26

Reaction Laws

• Law of Conservation of Energy – in chemical and physical reactions, energy is conserved(not created or destroyed)

• Law of Conservation of Mass – in chemical and physical reactions, mass is conserved (not created or destroyed)

27

Law of Conservation of Mass

Chemical EquationH + O H2OReactants Products

Mass of Reactants = Mass of Products

Example: H + O H2O 5.0g + 5.0g = ?

10.0g28

ReviewChemical vs. Physical Changes

video 7 min• Number your paper from 1-5 and

answer the following questions• Which of these is a metric unit?

– A. pounds– B. cups– C. liters– D. inches

29

Review

• C• 2. Which of these is the symbol for

the metric unit micro?– A. M– B. m– C. ρ– D. μ

30

Review

• D• 3. Which of these is a physical

property?– A. density– B. reaction to water– C. combustibility

31

Review

• A• 4. Which of the following is a

chemical property? – A. reaction to acid– B. odor– C. temperature– D. color

32

Review

• A• 5. If 59 g of NaCl is produced in a

creaction, how much Cl was combined with 23 g of Na? Na + Cl NaCl– A. 36– B. 36 g– C. 79 g– D. 23 g 33

Review

• B

34

Composition of Matter• All matter has a composition, what it’s

made of• Different kinds of composition are:

– Pure substances- matter with a fixed composition that can’t be separated physically• Element • Compound

– Mixture- can be separated physically • Solutions• Colloids• Mechanical mixture 35

Classification is based on physical and chemical properties-Reference

Matter

Mixture Pure substance

Homogeneous(Solution)

Heterogeneous Element Compound

Metal Metalloid Nonmetal

Pure Substances• Element- made up of one

kind of atom and can’t be broken down intosimpler substancesby physical or chemical means

• 90 occur naturally on Earth 29 were synthesized (made) by scientists

• C, N, O, Na, H, Au (gold), etc.

118

Uuo117

Uus116Uuh(292)

115

Uup(288)

114

Uuq(289)

113

Uut(284)

112Uub(285)

111

Rg(272)

110

Ds(269)

109

Mt(268)

108

Hs(269)

107

Bh(264)

106

Sg(266)

105

Db(262)

104

Rf(261)

103

Lr(262)

88

Ra(226)

87

Fr(223)

86

Rn(222)

85

At(210)

84

Po(209)

83

Bi208.980

82

Pb207.2

81

Tl204.383

80

Hg200.59

79

Au196.967

78

Pt195.078

77

I r192.217

76

Os190.23

75

Re186.207

74

W183.84

73

Ta180.95

72

Hf178.49

71

Lu174.967

56

Ba137.327

55

Cs132.905

54

Xe131.29

53

I126.904

52

Te127.60

51

Sb121.760

50

Sn118.710

49

I n114.818

48

Cd112.4

47

Ag107.868

46

Pd106.42

45

Rh102.906

44

Ru101.07

43

Tc(98)

42

Mo95.94

41

Nb92.906

40

Zr91.224

39

Y88.906

38

Sr87.62

37

Rb85.468

36

Kr83.80

35

Br79.904

34

Se78.96

33

As74.922

32

Ge72.61

31

Ga69.723

30

Zn65.39

29

Cu63.546

28

Ni58.69

27

Co58.933

26

Fe55.845

25

Mn54.938

24

Cr51.996

23

V50.942

22

Ti47.87

21

Sc44.956

20

Ca40.078

19

K39.098

118

Uuo117

Uus116Uuh(292)

115

Uup(288)

114

Uuq(289)

113

Uut(284)

112Uub(285)

111

Rg(272)

110

Ds(269)

109

Mt(268)

108

Hs(269)

107

Bh(264)

106

Sg(266)

105

Db(262)

104

Rf(261)

103

Lr(262)

88

Ra(226)

87

Fr(223)

86

Rn(222)

85

At(210)

84

Po(209)

83

Bi208.980

82

Pb207.2

81

Tl204.383

80

Hg200.59

79

Au196.967

78

Pt195.078

77

I r192.217

76

Os190.23

75

Re186.207

74

W183.84

73

Ta180.95

72

Hf178.49

71

Lu174.967

56

Ba137.327

55

Cs132.905

54

Xe131.29

53

I126.904

52

Te127.60

51

Sb121.760

50

Sn118.710

49

I n114.818

48

Cd112.4

47

Ag107.868

46

Pd106.42

45

Rh102.906

44

Ru101.07

43

Tc(98)

42

Mo95.94

41

Nb92.906

40

Zr91.224

39

Y88.906

38

Sr87.62

37

Rb85.468

36

Kr83.80

35

Br79.904

34

Se78.96

33

As74.922

32

Ge72.61

31

Ga69.723

30

Zn65.39

29

Cu63.546

28

Ni58.69

27

Co58.933

26

Fe55.845

25

Mn54.938

24

Cr51.996

23

V50.942

22

Ti47.87

21

Sc44.956

20

Ca40.078

19

K39.098

102

No(259)

101

Md(258)

100

Fm(257)

99

Es(252)

98

Cf(251)

97

Bk(247)

96

Cm(247)

95

Am(243)

94

Pu(244)

93

Np(237)

92

U238.029

91

Pa231.036

90

Th232.038

89

Ac(227)

70

Yb173.04

69

Tm168.934

68

Er167.26

67

Ho164.930

66

Dy162.50

65

Tb158.925

64

Gd157.25

63

Eu151.964

62

Sm150.36

61

Pm(145)

60

Nd144.24

59

Pr140.908

58

Ce140.116

57

La138.906

102

No(259)

101

Md(258)

100

Fm(257)

99

Es(252)

98

Cf(251)

97

Bk(247)

96

Cm(247)

95

Am(243)

94

Pu(244)

93

Np(237)

92

U238.029

91

Pa231.036

90

Th232.038

89

Ac(227)

70

Yb173.04

69

Tm168.934

68

Er167.26

67

Ho164.930

66

Dy162.50

65

Tb158.925

64

Gd157.25

63

Eu151.964

62

Sm150.36

61

Pm(145)

60

Nd144.24

59

Pr140.908

58

Ce140.116

57

La138.906

12

Mg24.305

11

Na22.990

4

Be9.012

3

Li6.941

12

Mg24.305

11

Na22.990

4

Be9.012

3

Li6.941

1

H1.008

1

H1.008

2

He4.003

2

He4.003

18

Ar39.948

17

Cl35.453

16

S32.066

15

P30.974

14

Si28.086

13

Al26.982

18

Ar39.948

17

Cl35.453

16

S32.066

15

P30.974

14

Si28.086

13

Al26.982

10

Ne20.180

9

F18.998

8

O15.999

7

N14.007

6

C12.001

5

B10.811

10

Ne20.180

9

F18.998

8

O15.999

7

N14.007

6

C12.001

5

B10.811

1

2

3

4

5

6

7

1

2

3 4 5 6 7 8 9 10 11 12

13 14 15 16 17

18

Lanthanides

Actinides

37

• Metal- properties: luster, reflects heat and light, good conductors of heat and electricity, malleable, ductile, all are solids except mercury (liquid)

• Nonmetal-properties: poor conductors of heat and electricity, brittle, not malleable or ductile, are solids, liquids and gases

• Metalloid- has some properties of metals and some properties of nonmetals

Elements

38

Pure Substances

• Compound- composed of two or more different elements

• The atoms are chemically combined so that the elements take on new identities and lose their original properties

Examples:H2O, CO2,CO, NO2,

39

Mixtures

• Mixtures- two or more substances that do not combine chemically, but remain the same individual substances; – Can be separated by physical means– Two types:

• Heterogeneous• Homogeneous

Based on the prefixes“hetero” and “homo,” what do you think are characteristics of thesetwo types of mixtures?

40

Heterogeneous Mixtures

• “Hetero” = different• Consists of visibly different substances

or phases (solid, liquid, gas) • Mechanical mixture- visibly not wholly

one• Example:

Trail Mix

Notice the visibly differentsubstances in these mechanical

mixtures

Pizza

41

Heterogeneous Mixtures

• Suspension- special type of heterogeneous mixture of larger particles that eventually settle

42

Heterogeneous Mixtures• Colloids- heterogeneous mixture with

particles that never settle– Milk and paint– Foggy appearance because its particles are

large enough to scatter light, unlike a solution

43

Homogeneous Mixtures

• “Homo” = same • Same uniform appearance and

composition throughout; maintain one phase (solid, liquid, gas)

• Commonly referred to as solutions• Example:

Salt WaterNotice the

uniformappearance

44

Homogeneous Mixtures• Solution- a mixture of two or more

substances that is identical throughout– Can be physically separated– Composed of solutes and solvents

the substance in the smallest amount and the one that dissolves in the solvent

the substance in the larger

amount that dissolves the solute

Colloids (milk, fog, jello) are considered solutions

Iced Tea Mix(solute)

Water(solvent)

Iced Tea(solution)

Salt water is considered a

solution. How

can it be physically separated?

45

ReviewSeparating Mixtures video

8min• Number your paper from 1-5 and

answer the following questions• Which of these is a metric unit?

– A. centiliters– B. cups– C. pounds– D. inches

46

Review

• A• 2. Which of these is a chemical

property?– A. density– B. reaction with water– C. color– D. length

47

Review

• B• 3. Which of these is a pure

substance?– A. pizza– B. tap water– C. aluminum

48

Review

• C• 4. Which of the following is a

homogenous mixture? – A. air– B. trail mix– C. soil– D. air with dust particles

49

Review• A Liquefy and then distill to

separate• 5. Which of these is a compound?

– A. – B. – C. – D.

A B C D50

Review

• D

51