1. Bellwork -State Changes
Water exists on Earth as a liquid, a solid, and a vapor.
As water cycles through the atmosphere, the oceans,
and Earth’s crust, it undergoes repeated changes of
state. You will learn what conditions can control the
state of a substance.
BELLWORK-name the
following phase changes:
a)Solid to liquid b) liquid to solid
c)Liquid to gas d) gas to liquid
e) Solid to gas

2. Melting - solid to liquid
Freezing- liquid to solid
Vaporization- liquid to gas
Vapor- a gas that is usually a liquid at room temp
Condensation- changing from a gas to a liquid

3. Chapter 13- States of Matter
Intro to Gases
The skunk releases its spray! Within seconds
you smell that all-too-familiar foul odor.
You will discover some
general characteristics of
gases that help explain
how odors travel through
the air, even on a
windless day.

4. 13.1
The Kinetic Molecular Theory explains
the behavior of gases.

6. The word kinetic refers to motion.

7. The word kinetic refers to motion.
•The energy an object has
because of its motion is called
kinetic energy.

8. The word kinetic refers to motion.
•The energy an object has
because of its motion is called
kinetic energy.
• According to the
kinetic theory,
all matter consists
of tiny particles that
are in constant
motion.

9. Kinetic Molecular Theory: GASES

10. Kinetic Molecular Theory: GASES
• The particles in a gas are small,
hard spheres with an
insignificant volume.

11. Kinetic Molecular Theory: GASES
• The particles in a gas are small,
hard spheres with an
insignificant volume.
• The motion of gas particles is
rapid, constant, and random.

12. Kinetic Molecular Theory: GASES
• The particles in a gas are small,
hard spheres with an
insignificant volume.
• The motion of gas particles is
rapid, constant, and random.
• All collisions between gas
particles are perfectly elastic
(no energy lost).

13. 13.1
Gas particles are in rapid, constant motion.

14. 13.1
Gas particles travel in straight-line paths.
Gas particles move randomly.

15. 13.1
A gas fills its container.

16. 13.1
Kinetic theory explains gas pressure.

17. 13.1
Pressure = Force/Area
A force is a push or a pull.
Same
force
more less
area area
more
pressure!

19. Which would you prefer? Why?

20. 13.1
Kinetic theory explains gas pressure.

21. 13.1
Kinetic theory explains gas pressure.
Gas pressure
is the force
exerted by gas
particles
hitting the
surface of an
object.

22. 13.1
Kinetic theory explains gas pressure.
Gas pressure can KILL!

24. An empty space with no particles
and no pressure is called a vacuum.

25. Atmospheric pressure is the pressure
created by the earth’s gravitational
pull on the gases in our atmosphere.

26. Gas pressure is exerted in all
directions.

27. A barometer is a device that is used
to measure atmospheric pressure.

28. Pressure Poem
An empty water bottle,
closed tightly at high elevation,
will be crushed by the atmosphere
at sea level.

29. 13.1
Units of Pressure
• The SI unit of pressure is the pascal (Pa).
• One standard atmosphere (atm) is the
atmospheric pressure at sea level.

30. 13.1

31. 13.1
450 kPa x

32. 13.1
450 kPa x kPa

33. 13.1
atm
450 kPa x kPa

34. 13.1
1 atm
450 kPa x
101.3 kPa

35. 13.1
1 atm
450 kPa x = 4.4 atm
101.3 kPa

36. 13.1
1 atm
450 kPa x = 4.4 atm
101.3 kPa
450 kPa x

37. 13.1
1 atm
450 kPa x = 4.4 atm
101.3 kPa
450 kPa x
kPa

38. 13.1
1 atm
450 kPa x = 4.4 atm
101.3 kPa
mm Hg
450 kPa x
kPa

39. 13.1
1 atm
450 kPa x = 4.4 atm
101.3 kPa
760 mm Hg
450 kPa x 101.3
kPa

40. 13.1
1 atm
450 kPa x = 4.4 atm
101.3 kPa
760 mm Hg = 3400mm Hg
450 kPa x 101.3
kPa

41. for Sample Problem 13.1

42. Particles at a given temperature have a
wide range of kinetic energies.
Most of the particles have kinetic
energies in the middle of this range.

43. Particles at a given temperature have a
wide range of kinetic energies.
Most of the particles have kinetic
energies in the middle of this range.

44. Particles at a given temperature have a
wide range of kinetic energies.
Most of the particles have kinetic
energies in the middle of this range.
Temperature
measures
Average
Kinetic
Energy

45. 13.1
The Kelvin temperature of a
substance is directly proportional
to average kinetic energy.

46. 13.1
The Kelvin temperature of a
substance is directly proportional
to average kinetic energy.
The higher the kinetic energy, the higher
the temperature.

47. 13.1
Two substances with the same average
kinetic energy are at the same
temperature.
Two substances at the same
temperature have the same
average kinetic energy.

48. 13.1
Absolute zero (0 K, or –273.15°C)
is the temperature at which the
motion of particles theoretically
stops.

49. 13.1
Absolute zero (0 K, or –273.15°C)
is the temperature at which the
motion of particles theoretically
stops.
•Particles would have no kinetic
energy at absolute zero.

50. 13.1
Absolute zero (0 K, or –273.15°C)
is the temperature at which the
motion of particles theoretically
stops.
•Particles would have no kinetic
energy at absolute zero.
• Absolute zero has never been produced
in the laboratory (and not for lack of
trying!).

51. Bellwork- Kinetic Energy
•What is kinetic energy?
•How is average kinetic energy
related to temperature?
•Which has higher kinetic energy,
an olympic size pool of water or a
cup of hot coffee?

52. 13.2
Substances that can flow are referred to as
fluids. Both liquids and gases are fluids.

53. 13.2
The intermolecular attractions
(IMFs) are counteracted by
motion of molecules.
Together they determine the physical
properties of liquids.
High IMFs promote a solid state
High temps (motion) promote a gas state.

54. 13.2
If the liquid
is not
boiling
it is called
evaporation.

55. 13.2
When a liquid converts
to a gas it is called
vaporization.
If the liquid
is not
boiling
it is called
evaporation.

56. 13.2
When a liquid converts
to a gas it is called
vaporization.
If the liquid
is not
boiling
it is called
evaporation.

57. 13.2
When a liquid converts
to a gas it is called
vaporization.
If the liquid
is not
boiling
it is called
evaporation.

58. 13.2
In a closed container, evaporated
molecules collect as a vapor
above any liquid.
Vapor pressure is the force
exerted by a gas
above a liquid.

59. During evaporation, only molecules
with a certain minimum kinetic
energy can escape from the surface
of the liquid.

60. During evaporation, only molecules
with a certain minimum kinetic
energy can escape from the surface
of the liquid.

61. During evaporation, only molecules
with a certain minimum kinetic
energy can escape from the surface
of the liquid.
Evaporation is
a cooling
process
because the
molecules with
the highest
kinetic energy
escape.

62. 13.2
In an open container,
molecules that evaporate can
escape from the container.

63. Some evaporated molecules will
condense back into a liquid.

64. Some evaporated molecules will
condense back into a liquid.

65. Some evaporated molecules will
condense back into a liquid.
A dynamic equilibrium exists between the
vapor and the liquid.
The system is in equilibrium when
the rate of evaporation equals the
rate of condensation.

67. DYNAMIC
EQUILIBRIUM

68. DYNAMIC
EQUILIBRIUM
For each
molecule that
evaporates a
different
molecule
returns to the
liquid.

69. DYNAMIC
EQUILIBRIUM
For each
molecule that
evaporates a
different
molecule
returns to the
liquid.
SAME
RATES!!

71. DYNAMIC
EQUILIBRIUM

72. DYNAMIC
EQUILIBRIUM
Equilibrium-
The amount
of liquid and
vapor do not
change.

73. DYNAMIC
EQUILIBRIUM
Equilibrium-
The amount
of liquid and
vapor do not
change.
Dynamic-
There is a
constant
turnover of
particles.

74. 13.2
Vapor pressure increases with
Temperature.

76. The particles have increased kinetic energy,
so more particles will have the minimum
energy needed to escape the liquid.

77. When a liquid is heated to a temperature at
which particles throughout the liquid have
enough kinetic energy to vaporize, the
liquid begins to boil.

78. Liquids boil when their vapor
pressure exceeds the pressure
pushing down on the liquid (usually
atmospheric pressure).

79. 13.2

81. Boiling Point and Pressure Changes

82. Boiling Point and Pressure Changes
Because a liquid boils when its vapor
pressure is equal to the external pressure,
liquids don’t always boil at the same
temperature.

83. Boiling Point and Pressure Changes
Because a liquid boils when its vapor
pressure is equal to the external pressure,
liquids don’t always boil at the same
temperature.
• At high altitudes, atmospheric
pressure is low, so water boils cooler
and food needs longer to cook.

84. Boiling Point and Pressure Changes
Because a liquid boils when its vapor
pressure is equal to the external pressure,
liquids don’t always boil at the same
temperature.
• At high altitudes, atmospheric
pressure is low, so water boils cooler
and food needs longer to cook.
• A pressure cooker increases the
boiling point so food cooks fast.

85. Altitude and Boiling Point

86. The normal boiling point is the
boiling point of a liquid at
atmospheric pressure
(1 atm or 101.3 kPa)

88. Section 13.3- Solids

89. Solids keep their shape because
their particles are in fixed positions.

90. In a crystalline solid, the
particles are in an orderly,
repeating, three-dimensional
pattern called a crystal lattice.
ionic compound elemental metal

91. 13.3
When an element can make more
than one structure, the different
forms are called allotropes.

92. 13.3
When an element can make more
than one structure, the different
forms are called allotropes.
•Allotropes have different properties
because their structures are
different.

93. 13.3
When an element can make more
than one structure, the different
forms are called allotropes.
•Allotropes have different properties
because their structures are
different.
• Only a few elements have allotropes.

94. 13.3
Carbon’s allotropes are diamond and graphite

95. Non-Crystalline Solids
An amorphous solid lacks an
ordered internal structure.
• Rubber, plastic, asphalt, and glass are
amorphous solids.

96. Non-Crystalline Solids
An amorphous solid lacks an
ordered internal structure.
• Rubber, plastic, asphalt, and glass are
amorphous solids.

97. Quartz is crystallized SiO2 Glass is amorphous SiO2

98. Non-Crystalline Solids
Quartz is crystallized SiO2 Glass is amorphous SiO2

99. Non-Crystalline Solids
An amorphous solid lacks an ordered
internal structure.
Quartz is crystallized SiO2 Glass is amorphous SiO2

100. Non-Crystalline Solids
An amorphous solid lacks an ordered
internal structure.
•A glass has cooled to a rigid state
without crystallizing.
Quartz is crystallized SiO2 Glass is amorphous SiO2

101. 13.4

102. 13.4
The change of a substance from a solid
to a vapor without passing through the
liquid state is called sublimation.
Sublimation occurs in solids with
vapor pressures that exceed
atmospheric pressure at or near
room temperature.

103. 13.4
The change of a substance from a solid
to a vapor without passing through the
liquid state is called sublimation.
Sublimation occurs in solids with
vapor pressures that exceed
atmospheric pressure at or near
room temperature.