3. Chapter Menu States of Matter Section 12.1Section 12.1Gases Section 12.2Section 12.2 Forces of Attraction Section 12.3Section 12.3 Liquids and Solids Section 12.4Section 12.4 Phase Changes Exit Click a hyperlink or folder tab to view the corresponding slides.

4. Section 12-4 Section 12.4 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.

5. Section 12-4 Section 12.4 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

6. Section 12-4 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.

7. Section 12-4 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

8. Section 12-4 Phase Changes That Require Energy (cont.) Particles with enough energy escape from the liquid and enter the gas phase.

9. Section 12-4 Phase Changes That Require Energy (cont.) Vaporization is the general process by which a liquid changes to a gas or vapor.Vaporization Evaporation is vaporization only at the surface of a liquid.Evaporation Sublimation is the process by which a solid changes into a gas without becoming a liquid. Boiling is vaporization throughout the volume of the liquid.

10. Section 12-4 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

11. Section 12-4 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

12. Section 12-4 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

13. Section 12-4 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

14. Section 12-4 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

15. Section 12-4 Phase Diagrams (cont.)

16. Section 12-4 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

17. Section 12-4 Phase Diagrams (cont.) The phase diagram for different substances are different from water.

18. A.A B.B C.C D.D Section 12-4 Section 12.4 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

19. A.A B.B C.C D.D Section 12-4 Section 12.4 Assessment The transfer of energy from one object to another at a lower temperature is ____. A.heat B.degrees C.conductivity D.electricity

20. End of Section 12-4

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

22. Study Guide 1 Section 12.1 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.

23. Study Guide 2 Section 12.2 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.

24. Study Guide 3 Section 12.3 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.

25. Study Guide 4 Section 12.4 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.

26. 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

27. 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

28. 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

29. 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

30. 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

31. 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

32. 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

33. 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

34. 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

35. 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

36. IB Menu Click on an image to enlarge.

37. IB 1

38. IB 2

39. IB 3

40. IB 4

41. IB 5

42. IB 6

43. IB 7

44. IB 8

45. IB 9

46. IB 10

47. IB 11

48. IB 12

49. IB 13

50. IB 14

51. IB 15

52. IB 16

53. IB 17

54. IB 18

55. IB 19

56. IB 20

57. CIM Table 12.4Unit Cells Table 12.5Types of Crystalline Solids Figure 12.30Phase Diagrams

58. Help Click any of the background top tabs to display the respective folder. Within the Chapter Outline, clicking a section tab on the right side of the screen will bring you to the first slide in each respective section. Simple navigation buttons will allow you to progress to the next slide or the previous slide. The “Return” button will allow you to return to the slide that you were viewing when you clicked either the Resources or Help tab. The Chapter Resources Menu will allow you to access chapter specific resources from the Chapter Menu or any Chapter Outline slide. From within any feature, click the Resources tab to return to this slide. To exit the presentation, click the Exit button on the Chapter Menu slide or hit Escape [Esc] on your keyboards while viewing any Chapter Outline slide.

59. End of Custom Shows This slide is intentionally blank.