Matter

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.

Properties of Matter

• All matter has characteristics, or properties

• These properties can either be:– Chemical– Physical

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

Volume and Density

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

• 1 mL = 1 cm3

Which is more dense?

Physical Properties

• States of matter:– Bose-Einstein

– Solid – Liquid– Gas– Plasma

(Newest State)

Bose-Einstein Condensate

• Exist at extremely cold temperatures (around absolute zero or -460 oF)

• Particles are super unexcited

• Particles lock or “clump” together so firmly that they move as a single unit

Solid

• Particles are tightly compact

• Particles vibrate without the ability to move freely

• Definite shape and volume

• Solid Animation

Liquid

• Particles are tightly compact, but able to move around close to each other

• No definite shape, but definite volume

• Liquid Animation

Gas

• Particles can easily spread out or move close together

• Particle move freely and with a lot of energy

• No definite shape or volume

• Gas Simulation

Plasma

• Particles broken apart and move freely with extremely high energy

• Exist at extremely high temps (several million degrees Celsius)

• Not too common on earth, but the most common form of matter in the universe

• Examples: Florescent and neon lights, lightning, fire

Why do you think this is the most common

form/state of matter in the universe?

Physical Properties

• Physical states of matter result from the amount of energy that the particles composing the matter have.

• More energy = more movement for the particles

If you were to compare an ice cube and the steam created from boiling water, which would

you think has more energy?

Types of Energy

• Potential- stored energy• Kinetic energy- energy a moving object

has• Temperature-average kinetic energy of

all atoms in a substance • Thermal energy- sum of both the

kinetic and potential energy of the atoms of a substance

Physical Properties

Taken from: http://www.chem4kids.com/files/matter_becondensate.html

What about this states of matter continuum could be considered a little misleading?

Changes in States(Physical Changes)

Melting

Vaporization

(Evaporation/Boiling)

Freezing

Condensation

All changes in state require a change in energy

Sublimation

Bose-Einstein

Solid

Liquid

Gas

PlasmaDisposition

Why do you think Bose-Einstein and plasma are not equally distanced

from the other three states of matter?

Heating Curve•The heating curve below shows how adding more thermal energy results in changes in the states of water

boiling point

melting point

Thermal Expansion

• Thermal expansion- the increase in the size of a substance when the temperature is increased.– Hot air balloons rise due to the thermal

expansion of air– Colder water will contract and sink– Density and temp– The exception of this is water because

when it becomes ice it expands and floats

Physical Properties of Fluids

• Fluid- any substance that can flow, like a liquid or gas

• Buoyancy- the ability of a fluid to exert an upward force on an object immersed in it. – Archimedes principle-the

buoyant force on an object is equal to the weight of the fluid displaced by that object

Density and Buoyancy

• Density= mass (g) volume (mL or cm3)• Because saltwater has the

additional mass of salt in the water and is more dense, things are more buoyant in saltwater than fresh

• Generally if an objectis more dense than the fluid, it will sink

• If an object is less dense it will float

Physical Properties of Fluids

• Pascals principle- pressure applied to a fluid is transmitted throughout the fluid P (Pascals)= Force (Newton)

Area (m2)where one Pascal is a N/m2

Check for Understanding

• As you sit here, atmospheric pressure from the air is pushing on you

• If the atmospheric pressure at sea level is 101 kPa (or N/m2), and the average human’s area is 1.80 m2, with how much force does the atmosphere push on the average human?

Check for Understanding

• As you sit here, atmospheric pressure from the air is pushing on you

• If the atmospheric pressure at sea level is 101 kPa (or N/m2), and the average human’s area is 1.80 m2, with how much force does the atmosphere push on the average human?

• P = F so F = PA A

• F (N) = 101 kPa X 1.80 m2 = 101,000Pa X 1.80 m2

• F (N) = 182,000 Pa m2 = 182,000 N

Physical Properties of Fluids

• Bernoulli’s principle- fluid velocity increases when the flow of the fluid is restricted

Physical Properties of Fluids

• Viscosity- the resistance of a fluid to flowing.

• Maple syrup is very viscous, even more so cold than when warm

• Water is not viscous at all

Physical Properties of Gases

• Boyle’s Law- decrease the volume of a container of gas and hold the temp constant, pressure from the gas will increase

• Conversely, increase the volume of a container of gas holding the temp constant, pressure from the gas will decrease

Boyle’s Law

• Boyle’s Law as an equation:– PiVi = PfVf where i=initial and f=final

• If a weather balloon has a volume of 100L when it is released at sea level where the pressure is 101 kPa, what will be the balloon’s volume when it reaches an altitude where the pressure is 43 kPa?– PiVi = PfVf so = PiVi = Vf

Pf

– Vf = 100L X 101,000Pa = 235L

43,000 Pa

Check for Understanding

• Boyle’s Law as an equation:

– PiVi = PfVf where i=initial and f=final

• If a balloon has a volume of 11L when it is released at sea level where the pressure is 101 kPa, what will be the balloon’s volume when it reaches an altitude where the pressure is 86 kPa?

Check for Understanding• Boyle’s Law as an equation:

– PiVi = PfVf where i=initial and f=final

• If a balloon has a volume of 11L when it is released at sea level where the pressure is 101 kPa, what will be the balloon’s volume when it reaches an altitude where the pressure is 86 kPa?– PiVi = PfVf so = PiVi = Vf

Pf

– Vf = 11L X 101,000Pa = 12.9L

86,000 Pa

Physical Properties of Gases

• Charles’s Law- the volume of a gas increases with increasing temperature as long as the pressure on the gas is constant

Charles’s Law• Charles’s Law as an equation:

– Vi = Vf where i=initial and f=final

Ti Tf

and temperature must be measured in Kelvin• K = oC + 273• Remember:

– 0K is absolute zero– 273K is the freezing point of water– 373K is the boiling point of water

Charles’s Law

• A 2L balloon at room temperature (20.0oC) is placed in a refrigerator at 3.0oC. What will be the balloon’s volume be after it cools?

• K = oC + 273• So Ti = 293K and Tf = 276K Vi = Vf so Vi X Tf = Vf

Ti Tf Ti

Vf = 2L X 276K = 1.89 L (it shrinks!) 293K

Check for Understanding

• What would be the final volume if the balloon was put in a -18oC freezer?

Check for Understanding• What would be the final volume if the

balloon was put in a -18oC freezer?

• K = oC + 273• So Ti = 293K and Tf = 255K

Vi = Vf so Vi X Tf = Vf

Ti Tf Ti

Vf = 2L X 255K = 1.7 L (it shrinks smaller!) 293K

Physical Properties of Solids

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

• This is a property of many metals

Composition of Matter• All matter has a composition, what it’s made of• Different kinds of composition are:

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

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

MATTER

PURE SUBSTANCES(non-mixtures)

MIXTURES

ELEMENTS COMPOUNDS SOLUTIONS

MECHANICAL MIXTURES

COLLOIDS

HOMOGENEOUS

HETEROGENEOUS

SUSPENSIONS

Pure Substances

• Element- made up of one kind of atom that can’t be broken down into simpler substances by physical or chemical means

• 90 occur naturally on Earth

• 25 were synthesized (made) by scientists

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

Pure Substances

• Compound- substance composed of two or more different elements (atoms) that are chemically combined

Examples:H2O, CO2,CO, NO2,

Mixtures

• Mixtures- combination of 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?

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

Heterogeneous Mixtures

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

Heterogeneous Mixtures• Colloids- heterogeneous mixture with

particles that never settle– Milk and paint– Have a foggy appearance because its

particles are large enough to scatter light, unlike a solution

Homogeneous Mixtures

• “Homo” = same • Has the same uniform appearance and

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

• Commonly referred to as solutions• Example:

Salt WaterNotice theuniform

appearance

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?

Solutes Change Solvents• The amount of solute in a solution determines

how much the physical properties of the solvent are changed

• Examples:

Lowering the Freezing Point

The freezing point of a liquid solvent decreases when a solute is dissolved in it.

Ex. Pure water freezes at 320F (00C), but when salt is dissolved in it, the freezing point is lowered.

This is why people use salt to melt ice.

Raising the Boiling Point

The boiling point of a solution is higher than the boiling point of the solvent.

Therefore, a solution can remain a liquid at a higher temperature than its pure solvent.

Ex. The boiling point of pure water is 2120F (1000C), but when salt is dissolved in it, the boiling

point is higher. This is why it takes salt water longer to boil than fresh water.

Concentration

• Concentration- the amount of solute dissolved in a solvent at a given temperature•Described as dilute if it has a low concentration of solute

•Described as saturated if it has a high concentration of solute

•Described as supersaturated if contains more dissolved solute than normally possible

Solubility

• The amount of solute that dissolves in a certain amount of a solvent at a given temperature and pressure to produce a saturated solution

• Influenced by:Temperature Pressure

Solids increased temperature causes them to be more soluble and vice versa

Gases increased temperature causes them to be less soluble and vice versa

Ex. Iced Coffee

Solids increased pressure has no effect on solubility

Gases increased pressure causes them to be more soluble and vice versa

Ex. Soda, “The Bends”

What do we call things that are not soluble?

Chemical Properties

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

• Examplesflammability

reactivity with vinegarreactivity with oxygen

Iron + Oxygen Iron oxide (rust)2Fe + 3O2 Fe2O3

Chemical or Physical Property?

1. 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

Comparing Physical and Chemical Properties

Substance/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

Changes in Matter

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

matter:– Chemical– Physical

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

• The Mixtures Lab

Physical changes are

not indicative of a chemical reaction

Changes in States(Physical Changes)

Melting

Vaporization

(Evaporation/Boiling)

Freezing

Condensation

All changes in state require a change in energy

Sublimation

Bose-Einstein

Solid

Liquid

Gas

PlasmaDisposition

Why do you think Bose-Einstein and plasma are not equally distanced

from the other three states of matter?

Physical ChangesSimulation 1

Simulation 2

• Chemistry of Chocolate

This is what happens when energy is added and taken away

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.

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)

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?

Out of the four types of reactions, which would describe the

chemical reaction taking place to the right?

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

Law of Conservation of Mass

• Proposed by Antoine Lavoisier• In a chemical reaction, atoms are neither created

nor destroyed• All atoms present in the reactants are also present

in the products• Chemical equations must be balanced to show the

conservation of mass

H2 + O2 H2O

In its present form, does this chemical equation show a conservation of mass?

How would you balance this equation to

show the conservation of mass?

2 2Reactants

H 2O 2

Products

42

H 2O 1

42