2. KINETIC THEORY AND STATES OF MATTER Chapter 13

3. Section 13.1 Gases Use the kinetic-molecular theory to explain the behavior of gases and introduce Gas Laws Review Vocabulary kinetic energy: energy due to motion Explain how gas pressure is measured

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

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

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

7. 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

8. Gas Pressure Pressure is defined as force per unit area. Gas particles exert pressure when they collide with the walls of their container. https://www.youtube.com/watch?v=t-Iz414g-ro https://www.youtube.com/watch?v=kkUvU-elGtw

9. 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.

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

11. 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/m 2. One atmosphere is equal to 760 mm Hg or 101.3 kilopascals. https://www.youtube.com/watch?v=GRxglLS1YWI

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

13. Daltons Law of Partial Pressure states that the total pressure of a mixture of gases is equal to the sum of the pressures of all the gases of the mixture. The partial pressure of a gas depends on the number of moles, size of the container, and temperature and is independent of the type of gas.

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

15. Section 13-2 Section 13.2 Forces of Attraction Describe intramolecular forces. polar covalent: a type of bond that forms when electrons are not shared equally dispersion force dipole-dipole force hydrogen bond 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.

16. 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.

17. https://www.youtube.com/watch?v=XHV9Lz CH2KAhttps://www.youtube.com/watch?v= eVv3TpaQ2-Ahttps://www.youtube.com/watch?v=XHV9Lz CH2KAhttps://www.youtube.com/watch?v= eVv3TpaQ2-A

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

19. Section 13-2 Intermolecular Forces (cont.) Dipole-dipole forces are attractions between oppositely charged regions of polar molecules.Dipole-dipole forces

20. Section 13-2 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.Hydrogen bonds

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

22. A.A B.B C.C D.D Section 13-2 Section 13.2 Assessment A hydrogen bond is a type of ____. A.dispersion force B.ionic bond C.covalent bond D.dipole-dipole force

23. A.A B.B C.C D.D Section 13-2 Section 13.2 Assessment Which of the following molecules can form hydrogen bonds? A.CO 2 B.C 2 H 6 C.NH 3 D.H 2

24. End of Section 13-2

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

26. Section 13-3 Section 13.3 Liquids and Solids (cont.) viscosity surface tension surfactant crystalline solid The particles in solids and liquids have a limited range of motion and are not easily compressed. unit cell allotrope amorphous solid

27. Section 13-3 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. Large amounts of pressure must be applied to compress liquids to very small amounts.

28. Section 13-3 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.Viscosity

29. Section 13-3 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 increases viscosity because the added energy allows the molecules to overcome intermolecular forces and flow more freely.

30. Section 13-3 Liquids (cont.) Surface tension is the energy required to increase the surface area of a liquid by a given amount.Surface tension Surfactants are compounds that lower the surface tension of water.Surfactants

31. Section 13-3 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.

32. Section 13-3 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.

33. Section 13-3 Solids (cont.) Crystalline solids are solids with atoms, ions, or molecules arranged in an orderly, geometric shape.Crystalline solids

34. Section 13-3 Solids (cont.) A unit cell is the smallest arrangement of atoms in a crystal lattice that has the same symmetry as the whole crystal.unit cell

35. Section 13-3 Solids (cont.)

36. Section 13-3 Solids (cont.)

37. Section 13-3 Solids (cont.) Amorphous solids are solids in which the particles are not arranged in a regular, repeating pattern.Amorphous solids Amorphous solids form when molten material cools quickly.

38. A.A B.B C.C D.D 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

39. A.A B.B C.C D.D 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

40. End of Section 13-3

41. 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.

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

43. Section 13-4 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.

44. Section 13-4 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.melting point

45. Section 13-4 Phase Changes That Require Energy (cont.) Particles with enough energy escape from the liquid and enter the gas phase.

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

47. Section 13-4 Phase Changes That Require Energy (cont.) In a closed container, the pressure exerted by a vapor over a liquid is called vapor pressure.vapor pressure

48. Section 13-4 Phase Changes That Require Energy (cont.) The boiling point is the temperature at which the vapor pressure of a liquid equals the atmospheric pressure.boiling point

49. Section 13-4 Phase Changes That Require Energy (cont.) Sublimation is the process by which a solid changes into a gas without becoming a liquid.

50. Section 13-4 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.freezing point

51. Section 13-4 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.condensation Deposition is the process by which a gas or vapor changes directly to a solid, and is the reverse of sublimation.Deposition

52. 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.phase diagram

53. Section 13-4 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.triple point

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

55. A.A B.B C.C D.D 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

56. A.A B.B C.C D.D 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

57. End of Section 13-4

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

59. 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.

60. 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.

61. 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.

62. 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.

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

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

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

66. A.A B.B C.C D.D Chapter Assessment 4 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

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

68. A.A B.B C.C D.D STP 1 What do effusion rates depend on? A.temperature of the gas B.temperature and pressure of the gas C.molar mass of the gas D.molar mass and temperature of the gas

69. A.A B.B C.C D.D STP 2 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

70. A.A B.B C.C D.D 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

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

72. A.A B.B C.C D.D STP 5 How many atoms of oxygen are present in 3.5 mol of water? A.2.1 x 10 24 B.3.5 x 10 23 C.6.02 x 10 23 D.4.2 x 10 24

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94. CIM Table 13.4Unit Cells Table 13.5Types of Crystalline Solids Figure 13.30Phase Diagrams

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