2. The States of Matter

4. States of Matter u There are 4 states of matter. u A solid is a form of matter that has its own definite shape and volume.

5. Solids u A solid cannot flow. u The particles can vibrate but cannot move around. u The particles of matter in a solid are very tightly packed; when heated, a solid expands, but only slightly.

6. Liquids u A liquid is a form of matter that flows, has constant (definite) volume, and takes the shape of its container.

7. Liquids u The particles in a liquid are not rigidly held in place and are less closely packed than are the particles in a solid; liquid particles are able to move past each other.

8. Liquids u A liquid is not very compressible. u Like solids, liquids tend to expand when heated.

9. Gases u A gas is a form of matter that flows to conform to the shape of its container and fills the entire volume of its container.

10. Gases u Compared to solids and liquids, the particles of gases are very far apart. u Because of the significant amount of space between particles, gases are easily compressed.

12. States of Matter u Plasma is composed of electrons and positive ions at temperatures greater than 5000 °C. The sun and other stars are examples of plasma.

13. Solid Liquid Gas Definite Volume? YES NO Definite Shape? YES NO Expansion with heat? Small Expans. Large Expans. Com- pressible? NO YES

14. Question Identify the following as a property of a solid, liquid or gas. The answer may include more that one state of matter. 1. flows and takes the shape of a container liquid, gas

15. Question Identify the following as a property of a solid, liquid, or gas. The answer may include more that one state of matter. 2. compressible gas

16. Question Identify the following as a property of a solid, liquid, or gas. The answer may include more that one state of matter. 3. made of particles held in a specific arrangement solid

17. Question Identify the following as a property of a solid, liquid, or gas. The answer may include more that one state of matter. 4. has definite volume solid, liquid

18. Question Identify the following as a property of a solid, liquid, or gas. The answer may include more that one state of matter. 5. always occupies the entire space of its container gas

19. Question Identify the following as a property of a solid, liquid, or gas. The answer may include more that one state of matter. 6. has a definite volume but flows liquid

20. States of Matter u The word vapor refers to the gaseous state of a substance that is a solid or a liquid at room temperature. u For example, steam is a vapor because at room temperature water exists as a liquid.

21. Matter u Some substances are described as volatile, which means that they change to a gas easily at room temperature. u Alcohol and gasoline are more volatile than water.

22. Liquids u Kinetic-molecular theory predicts the constant motion of the liquid particles. u Individual liquid molecules do not have fixed positions in the liquid.

23. Liquids u However, forces of attraction between liquid particles limit their range of motion so that the particles remain closely packed in a fixed volume. u These attractive forces are called intermolecular forces. Inter = between Molecular = molecules

24. Liquids u A liquid diffuses more slowly than a gas at the same temperature, however, because intermolecular attractions interfere with the flow.

25. Liquids u Viscosity is a measure of the resistance of a liquid to flow. u Viscosity decreases with increasing temperature.

26. Liquids u Particles in the middle of the liquid can be attracted to particles above them, below them, and to either side. u For particles at the surface of the liquid, there are no attractions from above to balance the attractions from below.

27. Liquids u Thus, there is a net attractive force pulling down on particles at the surface. u Surface tension is a measure of the inward pull by particles in the interior.

28. Liquids

29. u Soaps and detergents decrease the surface tension of water by disrupting the hydrogen bonds between water molecules.

30. Solids u For a substance to be a solid rather than a liquid at a given temperature, there must be strong attractive forces acting between particles in the solid.

31. Solids u These forces limit the motion of the particles to vibrations around fixed locations in the solid. Thus, there is more order in a solid than in a liquid. u The particles can only vibrate and revolve in place.

32. Solids u Because of this order, solids are much less fluid than liquids and gases. In fact, solids are not classified as fluids. u Most solids are more dense than most liquids.

33. Crystalline Solids u A crystalline solid is a solid whose atoms, ions, or molecules are arranged in an orderly, geometric, three-dimensional structure. u Most solids are crystals.

34. Amorphous Solids u Amorphous solids lack an orderly internal structure. u Think of them as supercooled liquids. u Examples of amorphous solids include rubber and glass.

35. Solid Liquid Gas Melting Vaporization Condensation Freezing Sublimation Deposition

36. Heating Curve for Water Section A: Ice is being heated to the melting to the meltingpoint. Section B: The ice is melting. Section C: Water is being heated to the boiling to the boilingpoint. Section E: Steam is being heated. Section D: Water is Boiling.

37. PHASE CHANGES

38. Liquid Vaporization Solid Gas ???? Condensation

39. Vaporization u If a substance is usually a liquid at room temperature (as water is), the gas phase is called a vapor. u Vaporization is the process by which a liquid changes into a gas or vapor. u Vaporization is an endothermic process - it requires heat.

40. Vaporization u When vaporization occurs only at the surface of an uncontained liquid (no lid on the container), the process is called evaporation.

41. Evaporation u Molecules at the surface break away and become gas. u Only those with enough kinetic energy (KE) escape. u Evaporation is a cooling process. u It requires heat, which is endothermic.

42. Vapor Pressure u Vapor pressure is the pressure exerted by a vapor over a liquid. u As temperature increases, water molecules gain kinetic energy and vapor pressure increases.

43. Boiling u When the vapor pressure of a liquid equals atmospheric pressure, the liquid has reached its boiling point, which is 100°C for water at sea level. u Recall that standard atmospheric pressure equals 1 atm.

44. Boiling u At this point, molecules throughout the liquid have the energy to enter the gas or vapor phase. u The temperature of a liquid can never rise above its boiling point.

45. Boiling u Boiling is an endothermic process. u It requires the addition of heat.

46. Changing the Boiling Point u As you go up into the mountains (increase in elevation), atmospheric pressure decreases. u Lower external pressure requires lower vapor pressure.

47. Changing the Boiling Point u Lower vapor pressure means lower boiling point. u As a result, spaghetti cooks slower in the mountains than at the beach.

48. u When you use a pressure cooker to can vegetables, the external pressure around the mason jars rises. Changing the Boiling Point

49. u This raises the vapor pressure needed in order for water to boil. u In turn, the boiling point is raised so the food cooks faster. Changing the Boiling Point

50. u Some phase changes release energy into their surroundings. u For example, when a vapor loses energy, it may change into a liquid. Condensation

51. u Condensation is the process by which a gas or vapor becomes a liquid. It is the reverse of vaporization. Condensation

52. u In a closed system, the rate of vaporization can equal the rate of condensation. Dynamic Equilibrium

53. u When first sealed, the molecules gradually escape the surface of the liquid. u As the molecules build up above the liquid, some condense back to a liquid. Dynamic Equilibrium

54. u Equilibrium is reached when Rate of Vaporization = Rate of Condensation Dynamic Equilibrium

55. u Molecules are constantly changing phase - “Dynamic”  The total amount of liquid and vapor remains constant - “Equilibrium” Dynamic Equilibrium

56. Liquid Melting Solid Gas ???? Freezing

57. u The melting point of a solid is the temperature at which the forces holding the particles together are broken and the solid becomes a liquid. u When heated the particles vibrate more rapidly until they shake themselves free of each other. Melting

58. u The freezing point is the temperature at which a liquid becomes a crystalline solid. u The freezing point is the same as the melting point. Freezing

59. Liquid Sublimation Solid Gas ???? Deposition

60. u The process by which a solid changes directly into a gas without first becoming a liquid is called sublimation. u Solid air fresheners and dry ice are examples of solids that sublime. Sublimation

61. u When a substance changes from a gas or vapor directly into a solid without first becoming a liquid, the process is called deposition. u Deposition is the reverse of sublimation. u Frost is an example of water deposition. Deposition

62. Question Classify the following phase change. 1. dry ice (solid carbon dioxide) to carbon dioxide gas sublimation

63. Question Classify the following phase change. 2. ice to liquid water melting

64. Question Classify the following phase change. 3. liquid water to ice freezing

65. Question Classify the following phase change. 4. water vapor to liquid water condensation

66. PHASE DIAGRAMS

67. u Temperature and pressure control the phase of a substance. u A phase diagram is a graph of pressure versus temperature that shows in which phase a substance exists under different conditions of temperature and pressure. Phase Diagrams

68. u A phase diagram typically has three regions, each representing a different phase and three curves that separate each phase. Phase Diagrams

70. u The points on the curves (the red, blue and yellow lines) indicate conditions under which two phases coexist. Phase Diagrams

71. u The critical point indicates the critical pressure and the critical temperature above which a substance cannot exist as a liquid. Phase Diagrams

72. u The triple point is the point on a phase diagram that represents the temperature and pressure at which three phases of a substance can coexist. Phase Diagrams

73. u The negative slope of the solid-liquid line in the phase diagram for water indicates the the solid floats on its liquid. Phase Diagrams

74. Question What happens to solid carbon dioxide at -100 ºC and 1 atm pressure as it is heated to room temperature? (The dry ice sublimes to CO 2 gas.)

75. Question What happens to water at 1 atm as the temperature rises from -15°C to 60°C? (It melts.)

76. Question What state of matter is water at 50°C and 20 atm? (liquid)

77. Question At what temperature does the triple point occur for water? (0.0098 ° C) 0.0098

78. Question At what temperature does the critical point occur for carbon dioxide? (31 ° C)

79. Question At standard pressure and -78°C, what phase changes can occur for carbon dioxide? (sublimation and deposition)

80. Question What state of matter is carbon dioxide at -80°C and 2 atm? (solid)