1. Chapter 3 – States of Matter

2. I. Solids, Liquids, and Gases

3. A. Describing the states of matter.
I. Solids, Liquids, and Gases
3.1 Solids, Liquids, and Gases
A. Describing the states of matter.
What are the three most common states of matter?
Solid
Liquid
Gas
How would you describe what these states are to someone who didn’t know?

4. A. Describing the states of matter. 1. Solids
3.1 Solids, Liquids, and Gases
I. Solids, Liquids, and Gases
A. Describing the states of matter.
1. Solids
- definite shape
- definite volume
Atoms in a solid are packed close together in an orderly arrangement

5. A. Describing the states of matter. 2. Liquids
I. Solids, Liquids, and Gases
A. Describing the states of matter.
2. Liquids
- variable shape (takes shape of container)
- definite volume
Atoms in a liquid are free to move around one another

6. A. Describing the states of matter. 3. Gases
I. Solids, Liquids, and Gases
A. Describing the states of matter.
3. Gases
- variable shape (takes shape of container)
- variable volume (fill container)
Atoms in a gas are far apart from one another and free to move around

7. A. Describing the states of matter. 4. Other states of matter
I. Solids, Liquids, and Gases
A. Describing the states of matter.
4. Other states of matter
Plasmas
Bose-Einstein Condensate (BEC)

8. kinetic energy (KE) – energy an object has due to its motion
I. Solids, Liquids, and Gases
B. Kinetic Theory
kinetic energy (KE) – energy an object has due to its motion
the faster an object moves the more kinetic energy it has
all particles of matter in constant motion
the particles in all matter are attracted to one another

9. I. Solids, Liquids, and Gases
Kinetic Theory

10. C. Explaining the Behavior of Gases
I. Solids, Liquids, and Gases
C. Explaining the Behavior of Gases
gas particles have a great deal of kinetic energy
constant motion allows a gas to fill its container
the particles are moving too fast for attractions to have any effect
variable volume
variable shape

11. D. Explaining the Behavior of Liquids
I. Solids, Liquids, and Gases
D. Explaining the Behavior of Liquids
liquid particles have less KE than gas particles
liquid particles are more closely packed compared to a gas
there is a tug-of-war between particle motion and particle attraction
definite volume
variable shape

12. E. Explaining the Behavior of Solids
I. Solids, Liquids, and Gases
E. Explaining the Behavior of Solids
solid particles have the least KE
solid particles very closely packed
solid particles only vibrate around fixed positions
definite volume
definite shape

13. I. Solids, Liquids, and Gases

14. - force distributed over an area
II. The Gas Laws
3.2 The Gas Laws
A. Pressure
- force distributed over an area
- measured in Pascals (N/m2)

15. The atmosphere’s pressure is measured using a barometer.
3.2 The Gas Laws
II. The Gas Laws
The atmosphere’s pressure is measured using a barometer.

16. II. The Gas Laws
3.2 The Gas Laws

17. Collisions of gas particles with container walls cause pressure
3.2 The Gas Laws
II. The Gas Laws
Collisions of gas particles with container walls cause pressure

18. B. Factors affecting gas pressure (there are 3)
II. The Gas Laws
3.2 The Gas Laws
B. Factors affecting gas pressure (there are 3)
Basketball goes flat after using it for awhile in the cold weather, until you warm it up
1. Temperature
- higher T, greater pressure
- increased temperature increases KE of particles
- particles move faster, collide with walls more

19. 3 factors affecting gas pressure
3.2 The Gas Laws
II. The Gas Laws
3 factors affecting gas pressure
2. Volume
As the volume is decreased the air pressure inside is increased
- lower V, greater pressure
- decrease volume, particles collide with walls more often

20. 3 factors affecting gas pressure
3.2 The Gas Laws
II. The Gas Laws
3 factors affecting gas pressure
As more particles are added the pressure increases
3. Number of particles
- more particles, greater pressure
- more particles to collide with walls more often

21. - as temperature increases, volume increases
3.2 The Gas Laws
II. The Gas Laws
C. Charles’s Law – The volume of a gas is directly proportional to its temperature in Kelvins
- as temperature increases, volume increases

22. Absolute zero – 0 Kelvin (can’t get any colder)
3.2 The Gas Laws
II. The Gas Laws
Absolute zero – 0 Kelvin (can’t get any colder)
Charles’s Law

23. - as volume decreases, pressure increases
3.2 The Gas Laws
II. The Gas Laws
D. Boyle’s Law – The volume of a gas is inversely proportional to its pressure
- as volume decreases, pressure increases

24. 3.2 The Gas Laws
II. The Gas Laws
Boyle’s Law

25. Algebra Practice AB = XY Solve for X 4B = X-Y Solve for X
2AB = XY Solve for A
A = X Solve for A
B Y
A = X Solve for X

26. Algebra Practice AB = XY Solve for X 4B = X-Y Solve for X
2AB = XY Solve for A
A = X Solve for A
B Y
A = X Solve for X
= AB / Y
= 4B + Y
= XY / 2B
= BX / Y
= AY / B

27. P1V1 = P2V2 T1 T2 E. Combined Gas Law
3.2 The Gas Laws
II. The Gas Laws
E. Combined Gas Law
- a combination of Charles’ and Boyle’ Laws
P1V1 = P2V2
T T2

28. Units Pressure: Pascals (Pa) OR atmosphere (atm)
Volume: Liters (L) OR meters cubed (m3)
Temperature: Celsius (C) OR Kelvin (K)

29. The Gas Laws V1 = V2 T1 T2 P1 V1 = P2 V2 P1 V1 = P2 V2 T1 T2
Charles’s Law
Boyle’s Law
Combined Gas Law

30. Solving Gas Law Problems
Write the name of the law that applies.
Write a description what is happening in the problem.
Write the equation of the law that applies.
Plug in all known values into the equation
Solve the equation

31. Solving Gas Law Problems
Write the name of the law that applies.
Write a description what is happening in the problem.
Write the equation of the law that applies.
Plug in all known values into the equation
Solve the equation
Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!)

32. Solving Gas Law Problems
Write the name of the law that applies.
Write a description what is happening in the problem.
Write the equation of the law that applies.
Plug in all known values into the equation
Solve the equation
Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!)
Charles’s Law (relates T and V)
Boyle’s Law (relates P and V)

33. Solving Gas Law Problems
Write the name of the law that applies.
Write a description what is happening in the problem.
Write the equation of the law that applies.
Plug in all known values into the equation
Solve the equation
Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!)
Charles’s Law (relates T and V)

34. Solving Gas Law Problems
Write the name of the law that applies.
Write a description what is happening in the problem.
Write the equation of the law that applies.
Plug in all known values into the equation
Solve the equation
Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!)
Volume getting bigger, temperature changing

35. Solving Gas Law Problems
Write the name of the law that applies.
Write a description what is happening in the problem.
Write the equation of the law that applies.
Plug in all known values into the equation
Solve the equation
Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!)
V1 = V2
T T2
P1 V1 = P2 V2

36. Solving Gas Law Problems
Write the name of the law that applies.
Write a description what is happening in the problem.
Write the equation of the law that applies.
Plug in all known values into the equation
Solve the equation
Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!)
V1 = V2
T T2

37. Solving Gas Law Problems
Write the name of the law that applies.
Write a description what is happening in the problem.
Write the equation of the law that applies.
Plug in all known values into the equation
Solve the equation
Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!)
3.00 = 5.00 T2

38. Solving Gas Law Problems
Write the name of the law that applies.
Write a description what is happening in the problem.
Write the equation of the law that applies.
Plug in all known values into the equation
Solve the equation
Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!)
3.00 = 5.00 T2
T2 = 300(5.00)
3.00
3.00(T2) = 300(5.00)

39. Solving Gas Law Problems
Write the name of the law that applies.
Write a description what is happening in the problem.
Write the equation of the law that applies.
Plug in all known values into the equation
Solve the equation
Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!)
T2 = 500

40. Solving Gas Law Problems
Write the name of the law that applies.
Write a description what is happening in the problem.
Write the equation of the law that applies.
Plug in all known values into the equation
Solve the equation
Jack’s balloon has a volume of 3.00 L at 300 K (about room temperature). His balloon can expand to 5.00 L before it will pop. If Jack puts his balloon into the oven, at what temperature will his balloon burst? (MAKE SURE YOUR ANSWER HAS THE CORRECT UNITS!!)
T2 = 500 K

41. P1V1 = P2V2 T1 T2 E. Combined Gas Law 3.2 The Gas Laws
II. The Gas Laws
E. Combined Gas Law
P1V1 = P2V2
T T2

42. Section 3.2

43. Section 3.2

44. Section 3.2

45. Section 3.2

46. Section 3.2

47. Section 3.2

48. Section 3.2

49. Section 3.2

50. Riding on Air II. The Gas Laws 3.2 The Gas Laws
What gases have been used in balloons that carry passengers?
Why do the particles of a gas inside a balloon fill the entire balloon?
What causes a hot-air balloon to lift off and rise from a surface?
Why did Piccard design the balloon so that it could become airborne when it was only partially filled?
Why must the air pressure inside the cabin be controlled?

51. A. Characteristics of Phase Changes
III. Phase Changes
A. Characteristics of Phase Changes
Phase Change – substance changes from one state to another (it is a reversible physical change)

52. III. Phase Changes

53. 1. Temperature and Phase Changes:
III. Phase Changes
1. Temperature and Phase Changes:
We can use temperature as a way to determine when a phase change is taking place
The temperature of a substance does not change during a phase change

54. III. Phase Changes
Figure 16

55. The temperature of a substance does not change during a phase change.
III. Phase Changes
The temperature of a substance does not change during a phase change.
Instead the energy added is used to overcome the attractions between molecules

56. The temperature of a substance does not change during a phase change
III. Phase Changes
The temperature of a substance does not change during a phase change
Time (minutes)
Temperature (ºC)
boiling (100 ºC)
melting (0 ºC)

57. III. Phase Changes
Time (minutes)
Temperature (ºC)

58. III. Phase Changes
2. Energy and Phase Changes + =
SOLID
LIQUID

59. III. Phase Changes
2. Energy and Phase Changes + =
LIQUID
GAS

60. 2. Energy and Phase Changes
III. Phase Changes
2. Energy and Phase Changes
Energy is absorbed or released during a phase change
Endothermic change
- energy absorbed by a substance
Melting is an example of an endothermic change

61. Energy is absorbed or released during a phase change
III. Phase Changes
Energy is absorbed or released during a phase change
Exothermic change
- energy is released by a substance
Freezing is an example of an exothermic change

62. III. Phase Changes
B. Melting and Freezing
The arrangement of molecules in water becomes less orderly as water melts and more orderly as water freezes.

63. The arrangement of molecules becomes LESS orderly
III. Phase Changes
1. Melting
melting
(Endothermic)
The arrangement of molecules becomes LESS orderly

64. The arrangement of molecules becomes MORE orderly
III. Phase Changes
2. Freezing
freezing
(Exothermic)
melting
The arrangement of molecules becomes MORE orderly

65. Attractions between particles have an effect
III. Phase Changes
Freezing
Attractions between particles have an effect

66. C. Vaporization and Condensation
III. Phase Changes
C. Vaporization and Condensation
Vaporization - change from liquid to a gas
- two types of vaporization
Condensation – change from gas to liquid

67. Molecular arrangement less orderly
III. Phase Changes
Vaporization
vaporization
(Endothermic)
melting
freezing
Molecular arrangement less orderly

68. Two Types of Vaporization
III. Phase Changes
Two Types of Vaporization
1. Evaporation – takes place at the surface of liquid

69. Two Types of Vaporization
III. Phase Changes
Two Types of Vaporization
1. Evaporation – takes place at the surface of liquid

70. Two Types of Vaporization
III. Phase Changes
Two Types of Vaporization
Evaporation
- takes place at the surface of liquid
- can occur at temperatures below boiling.
Vapor pressure – pressure exerted by the vapor above a liquid

71. Two Types of Vaporization
III. Phase Changes
Two Types of Vaporization
2. Boiling – bubbles form within the liquid when the vapor pressure equals atmospheric pressure

72. III. Phase Changes
Vaporization

73. Molecular arrangement more orderly
III. Phase Changes
3. Condensation
condensation
(Exothermic)
melting
freezing
vaporization
Molecular arrangement more orderly

74. C. Sublimation and Deposition
III. Phase Changes
C. Sublimation and Deposition
Sublimation – change from solid to a gas
Deposition – change from a gas to a solid

75. Molecular arrangement less orderly
III. Phase Changes
Sublimation
sublimation
(Endothermic)
melting
freezing
vaporization
condensation
Molecular arrangement less orderly

76. Molecular arrangement more orderly
III. Phase Changes
Deposition
deposition
(Exothermic)
melting
freezing
vaporization
condensation
sublimation
Molecular arrangement more orderly

77. Sublimation and Deposition
III. Phase Changes
Sublimation and Deposition

78. III. Phase Changes
1. Why would Earth’s weather be much different without water?
2. When water freezes, it behaves differently than other substances. How so?
3. Why does water behave as you explained in the previous question?
4. If water didn’t behave this way when it froze, what would happen to all the aquatic life in a pond during the wintertime?
5. Is it possible that some very deep ponds and lakes would never completely thaw out?
6. What is a popcorn hull?
7. Why does popcorn pop?
8. Does the method by which popcorn pops remind you of any particular gas law? It should!! Which one?
9. What prevents some popcorn kernels from popping?
Does the popping of a corn kernel require an exothermic or endothermic change of water?

79. III. Phase Changes
liquid
Charles’s law
condensation
exothermic
solid
absolute zero
endothermic
vapor pressure
deposition
pressure
Boyle’s law
kinetic energy
evaporation
phase change
vaporization
gas
sublimation

80. Chapter 3 Vocabulary
liquid
Charles’s law
exothermic
solid
absolute zero
endothermic
vapor pressure
deposition
pressure
Boyle’s law
kinetic energy
evaporation
phase change
vaporization
gas
sublimation

81. Chapter 3 Vocabulary
liquid
Charles’s law
exothermic
absolute zero
endothermic
vapor pressure
deposition
pressure
Boyle’s law
kinetic energy
evaporation
phase change
vaporization
gas
sublimation

82. Chapter 3 Vocabulary
liquid
Charles’s law
exothermic
absolute zero
endothermic
vapor pressure
deposition
pressure
Boyle’s law
evaporation
phase change
vaporization
gas
sublimation

83. Chapter 3 Vocabulary
liquid
Charles’s law
exothermic
absolute zero
endothermic
vapor pressure
pressure
Boyle’s law
evaporation
phase change
vaporization
gas
sublimation

84. Chapter 3 Vocabulary
liquid
Charles’s law
absolute zero
endothermic
vapor pressure
pressure
Boyle’s law
evaporation
phase change
vaporization
gas
sublimation

85. Chapter 3 Vocabulary
liquid
Charles’s law
absolute zero
endothermic
vapor pressure
pressure
Boyle’s law
evaporation
vaporization
gas
sublimation

86. Chapter 3 Vocabulary
liquid
Charles’s law
absolute zero
endothermic
vapor pressure
Boyle’s law
evaporation
vaporization
gas
sublimation

87. Chapter 3 Vocabulary
liquid
Charles’s law
endothermic
vapor pressure
Boyle’s law
evaporation
vaporization
gas
sublimation

88. Chapter 3 Vocabulary
liquid
Charles’s law
endothermic
vapor pressure
evaporation
vaporization
gas
sublimation

89. Chapter 3 Vocabulary
liquid
Charles’s law
vapor pressure
evaporation
vaporization
gas
sublimation

90. Chapter 3 Vocabulary
Charles’s law
vapor pressure
evaporation
vaporization
gas
sublimation

91. Chapter 3 Vocabulary
Charles’s law
vapor pressure
evaporation
gas
sublimation

92. Chapter 3 Vocabulary
Charles’s law
vapor pressure
gas
sublimation

93. Chapter 3 Vocabulary
Charles’s law
gas
sublimation

94. Chapter 3 Vocabulary
Charles’s law
sublimation

95. Chapter 3 Vocabulary
sublimation