1. KINETIC THEORY AND STATES OF MATTER
Chapter 13

2. Section Gases
Use the kinetic-molecular theory to explain the behavior of gases and introduce Gas Laws
Explain how gas pressure is measured
Review Vocabulary
kinetic energy: energy due to motion

3. The Kinetic-Molecular Theory
The kinetic-molecular theory describes the behavior of matter in terms of particles in motion.

4. Section 13-1 Explaining the Behavior of Gases
Great amounts of space exist between gas particles.
Compression reduces the empty spaces between particles.
Section 13-1

5. Explaining the Behavior of Gases (cont.)
Gases easily flow past each other because there are no significant forces of attraction.
Diffusion is the movement of a material across a concentration gradient

6. The Kinetic-Molecular Theory (cont.)
Kinetic energy of a particle depends on mass and velocity.
Temperature is a measure of the average kinetic energy of the particles in a sample of matter.

7. Gas Pressure
Pressure is defined as force per unit area.
Gas particles exert pressure when they collide with the walls of their container.

8. Section 13-1 Gas Pressure (cont.)
The particles in the earth’s atmosphere exert pressure in all directions called air pressure.
There is less air pressure at high altitudes because there are fewer particles present, since the force of gravity is less.
Section 13-1

9. Gas Pressure (cont.)
The SI unit of force is the newton (N).
One Pascal (Pa) is equal to a force of one Newton per square meter or N/m2.
One atmosphere is equal to 760 mm Hg or kilopascals.

10. Gas Pressure (cont.)
Torricelli invented the barometer.
Barometers are instruments used to measure atmospheric air pressure.

11. Gas Pressure (cont.)
Section 13-1

12. Gas Pressure (cont.)
Ptotal = P1 + P2 + P3 +...Pn
Partial pressure can be used to calculate the amount of gas produced in a chemical reaction.

13. Section 13.2 Forces of Attraction
Describe intramolecular forces.
polar covalent: a type of bond that forms when electrons are not shared equally
Compare and contrast intermolecular forces.
Intermolecular forces—including dispersion forces, dipole-dipole forces, and hydrogen bonds—determine a substance’s state at a given temperature.

14. Section 13-2 Intermolecular Forces
Attractive forces between molecules cause some materials to be solids, some to be liquids, and some to be gases at the same temperature.
Section 13-2

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16. Section 13-2 Intermolecular Forces (cont.)
London Dispersion forces are weak forces that result from temporary shifts in density of electrons in electron clouds.
Section 13-2

17. Intermolecular Forces (cont.)
Dipole-dipole forces are attractions between oppositely charged regions of polar molecules.

18. Intermolecular Forces (cont.)
Hydrogen bonds are special dipole-dipole attractions that occur between molecules that contain a hydrogen atom bonded to a small, highly electronegative atom with at least one lone pair of electrons, typically fluorine, oxygen, or nitrogen.

19. Intermolecular Forces (cont.)
Section 13-2

21. Section 13-2 Section 13.2 Assessment
Which of the following molecules can form hydrogen bonds?
A. CO2
B. C2H6
C. NH3
D. H2 A B C D
Section 13-2

22. Section 13-3 Section 13.3 Liquids and Solids
Contrast the arrangement of particles in liquids and solids.
Describe the factors that affect viscosity.
Explain how the unit cell and crystal lattice are related.
meniscus: the curved surface of a column of liquid
Section 13-3

23. Section 13.3 Liquids and Solids (cont.)
unit cell
amorphous solid
viscosity
surface tension
crystalline solid
The particles in solids and liquids have a limited range of motion and are not easily compressed.

24. Liquids
Forces of attraction keep molecules closely packed in a fixed volume, but not in a fixed position.
Liquids are much denser than gases because of the stronger intermolecular forces holding the particles together.

25. Liquids (cont.)
Fluidity is the ability to flow and diffuse; liquids and gases are fluids.
Viscosity is a measure of the resistance of a liquid to flow and is determined by the type of intermolecular forces, size and shape of particles, and temperature.

26. Liquids (cont.)
The stronger the intermolecular attractive forces, the higher the viscosity.
Larger molecules create greater viscosity.
Long chains of molecules result in a higher viscosity.
Increasing the temperature decreases viscosity because the added energy allows the molecules to overcome intermolecular forces and flow more freely.

27. Liquids (cont.)
Surface tension tendency of liquids which makes it acquire the least surface area possible.

28. Liquids (cont.)
Cohesion is the force of attraction between identical molecules.
Adhesion is the force of attraction between molecules that are different.
Capillary action is the upward movement of liquid into a narrow cylinder, or capillary tube.

29. Vaporization is the process by which a liquid changes to a gas or vapor.
Evaporation is vaporization only at the surface of a liquid.

30. Solids
Solids contain particles with strong attractive intermolecular forces.
Particles in a solid vibrate in a fixed position.
Most solids are more dense than liquids.
Ice is not more dense than water.

31. Solids (cont.)
Crystalline solids are solids with atoms, ions, or molecules (or unit cells) arranged in an orderly, geometric shape.

32. Solids (cont.)
Section 13-3

33. Solids (cont.)
Amorphous solids are solids in which the particles are not arranged in a regular, repeating pattern.

34. Section 13-3 Section 13.3 Assessment
The smallest arrangement of atoms in a crystal that has the same pattern as the crystal is called ____.
A. crystal lattice
B. unit cell
C. crystalline
D. geometric cell A B C D
Section 13-3

35. Section 13-3 Section 13.3 Assessment
The viscosity of a liquid will increase as:
A. particle size decreases
B. temperature decreases
C. intermolecular forces decrease
D. particle size increases A B C D
Section 13-3

36. Section 13-4 Section 13.4 Phase Changes
Explain how the addition and removal of energy can cause a phase change.
phase change: a change from one state of matter to another
Interpret a phase diagram.
Section 13-4

37. Section 13-4 Section 13.4 Phase Changes (cont.) melting point
vaporization
evaporation
vapor pressure
boiling point
freezing point
condensation
deposition
phase diagram
triple point
Section 13-4
Matter changes phase when energy is added or removed.

38. Phase Changes That Require Energy
Melting occurs when heat flows into a solid object.
Heat is the transfer of energy from an object at a higher temperature to an object at a lower temperature.

39. Phase Changes That Require Energy (cont.)
When ice is heated, the ice eventually absorbs enough energy to break the hydrogen bonds that hold the water molecules together.
When the bonds break, the particles move apart and ice melts into water.
The melting point of a crystalline solid is the temperature at which the forces holding the crystal lattice together are broken and it becomes a liquid.

40. Section 13-4 Phase Changes That Require Energy (cont.)
Vaporization is the process by which a liquid changes to a gas or vapor.
Evaporation is vaporization only at the surface of a liquid.
Section 13-4

41. Phase Changes That Require Energy (cont.)
In a closed container, the pressure exerted by a vapor over a liquid is called vapor pressure.

42. Phase Changes That Require Energy (cont.)
The boiling point is the temperature at which the vapor pressure of a liquid equals the atmospheric pressure.  At that temperature, the vapor pressure of the liquid becomes sufficient to overcome atmospheric pressure and allow bubbles of vapor to form inside the bulk of the liquid.

43. Phase Changes That Require Energy (cont.)
Sublimation is the process by which a solid changes into a gas without becoming a liquid.

44. Phase Changes That Release Energy
As heat flows from water to the surroundings, the particles lose energy.
The freezing point is the temperature at which a liquid is converted into a crystalline solid.

45. Phase Changes That Release Energy (cont.)
As energy flows from water vapor, the velocity decreases.
The process by which a gas or vapor becomes a liquid is called condensation.
Deposition is the process by which a gas or vapor changes directly to a solid, and is the reverse of sublimation.

46. Section 13-4 Phase Diagrams
A phase diagram is a graph of pressure versus temperature that shows in which phase a substance will exist under different conditions of temperature and pressure.
Section 13-4

47. Phase Diagrams (cont.)
The triple point is the point on a phase diagram that represents the temperature and pressure at which all three phases of a substance can coexist.

48. Section 13-4 Phase Diagrams (cont.)
The phase diagram for different substances are different from water.
Section 13-4

49. Section 13-4 Section 13.4 Assessment
The addition of energy to water molecules will cause them to ____.
A. freeze
B. change to water vapor
C. form a crystal lattice
D. move closer together A B C D
Section 13-4

50. Section 13-4 Section 13.4 Assessment
The transfer of energy from one object to another at a lower temperature is ____.
A. heat
B. degrees
C. conductivity
D. electricity A B C D
Section 13-4

51. End of Section 13-4

52. Resources Menu Chemistry Online Study Guide Chapter Assessment
Standardized Test Practice
Image Bank
Concepts in Motion
Resources Menu

53. Study Guide 1 Section 13.1 Gases Key Concepts
The kinetic-molecular theory explains the properties of gases in terms of the size, motion, and energy of their particles.
Dalton’s law of partial pressures is used to determine the pressures of individual gases in gas mixtures.
Graham’s law is used to compare the diffusion rates of two gases.
Study Guide 1

54. Study Guide 2 Section 13.2 Forces of Attraction Key Concepts
Intramolecular forces are stronger than intermolecular forces.
Dispersion forces are intermolecular forces between temporary dipoles.
Dipole-dipole forces occur between polar molecules.
Study Guide 2

55. Study Guide 3 Section 13.3 Liquids and Solids Key Concepts
The kinetic-molecular theory explains the behavior of solids and liquids.
Intermolecular forces in liquids affect viscosity, surface tension, cohesion, and adhesion.
Crystalline solids can be classified by their shape and composition.
Study Guide 3

56. Study Guide 4 Section 13.4 Phase Changes Key Concepts
States of a substance are referred to as phases when they coexist as physically distinct parts of a mixture.
Energy changes occur during phase changes.
Phase diagrams show how different temperatures and pressures affect the phase of a substance.
Study Guide 4

57. Chapter Assessment 1 760 mm Hg is equal to ____. A. 1 Torr B. 1 pascal
C. 1 kilopascal
D. 1 atmosphere A B C D
Chapter Assessment 1

58. A collision in which no kinetic energy is lost is a(n) ____ collision.
A. net-zero
B. elastic
C. inelastic
D. conserved A B C D
Chapter Assessment 2

59. Chapter Assessment 3 Solids with no repeating pattern are ____.
A. ionic
B. crystalline
C. liquids
D. amorphous A B C D
Chapter Assessment 3

60. What is the point at which all six phase changes can occur?
A. the melting point
B. the boiling point
C. the critical point
D. the triple point A B C D
Chapter Assessment 4

61. What are the forces that determine a substance’s physical properties?
A. intermolecular forces
B. intramolecular forces
C. internal forces
D. dispersal forces A B C D
Chapter Assessment 5

62. A sealed flask contains helium, argon, and nitrogen gas
A sealed flask contains helium, argon, and nitrogen gas. If the total pressure is 7.5 atm, the partial pressure of helium is 2.4 atm and the partial pressure of nitrogen is 3.7 atm, what is the partial pressure of argon?
A. 1.3 atm
B. 6.1 atm
C. 1.4 atm
D. 7.5 atm A B C D
STP 2

63. STP 3 Adding energy to a liquid will:
A. cause it to form crystal lattice
B. decrease the viscosity
C. compress the particles closer together
D. increase the velocity of the particles A B C D
STP 3

64. STP 4 Hydrogen bonds are a special type of ____. A. ionic bond
B. covalent bond
C. dipole-dipole force
D. dispersion force A B C D
STP 4

65. STP 5 How many atoms of oxygen are present in 3.5 mol of water?
A. 2.1 x 1024
B. 3.5 x 1023
C x 1023
D. 4.2 x 1024 A B C D
STP 5

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71. IB 5

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73. IB 7

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78. IB 13

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80. IB 14

81. IB 15

82. IB 16

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84. IB 18

85. IB 19

86. IB 20

87. CIM Table 13.4 Unit Cells Table 13.5 Types of Crystalline Solids
Figure Phase Diagrams
CIM

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