1. Calculate  H o,  G o, &  S o for N 2 O 5 + H 2 OHNO 3 Cpd N 2 O 5 H 2 O HNO 3  H f o -11.3 -285.8 -174.1  G f o -10.4 -237.2 -151.5 Drill:

2. AP Chm HW Problems 7 & 9 Page 268

3. Solids

4. Molecular Solids Covalently bound molecules held together by intermolecular forces (asphalt or ice)

5. Molecular Solids Non-conductors Insoluble in water mostly Low MP & BP Held by intermolecular F

6. Intermolecular Forces Instantaneous weak forces that hold one molecule to another or to another part of itself

8. Intermolecular Forces H-bond Dipole-dipole Dipole-induced dipole London dispersion

10. Importance of H-bonding Hydrogen bonding will have a profound effect on the strength of the bond; thus, will cause a tremendous increase of the BP or MP.

12. Network Molecular Solids or Macromolecules Bound by a continuous network of covalent bonds High MP, insoluble, non- conductor

13. Ionic Solids Ions or ionic compounds held together by electrostatic charge F attraction = Kq 1 q 2 /d 2

14. Ionic Solids Non-conductors as solids Conductors in solution Soluble in water mostly Very high MP & BP Brittle

15. Metallic Solids Conductors, insoluble in water mostly, high MP & BP, held by gravitational type force F attraction = Gm 1 m 2 /d 2

16. Crystal Solid Any substance that has a well defined crystal structure

17. Crystal Lattice The three dimensional arrangement of unit cells in a crystal structure

18. Unit Cell The smallest repeating unit that a crystal structure can be divided into

20. Crystal Structures CubicMonoclinic TetragonalTriclinic Orthorhombic Hexagonal Rhombohedral

21. Cubic All angles = 90 o All sides are = All faces are squares

22. Tetragonal All angles = 90 o 2 side sets are =, third  1 set of opposing squares 2 sets opposing rectangles

23. Orthorhombic All angles = 90 o all 3 side sets are  3 unequal sets opposing rectangles

24. Hexagonal All angles = 90 o or 120 o 1 set of opposing hexagons 3 sets opposing rectangles

25. Monoclinic 2 sets of angles = 90 o third set  90 o 1 set of opposing parallel 2 sets opposing rectangles

26. Triclinic No angles = 90 o 3 unequal sets of opposing parallelograms

28. Rhombohedral No angles = 90 o All sides = 3 sets of opposing congruent rhombuses

30. Drill: Describe unit cells & crystal lattice

31. AP CHM HW Work problem 8 on page 268.

32. Simple Cube Unit cell with one atom at each vertex 1 atom/cell

34. http://departments.kings. edu/chemlab/animation/i ndex.html Great website

35. Body Centered Cube BCC Unit cell with one atom at each vertex & one atom in the center of the cube 2 atoms/cell

37. Face Centered Cube FCC or CCP Unit cell with one atom at each vertex & one atom on each face of the cube 4 atoms/cell

41. The density of iron in its normal state of BCC is 7.86 g/mL. Calculate its density in the FCC state

42. A B C A A B 2 = A 2 + A 2 = 2A 2 C 2 = A 2 + B 2 = 3A 2

44. Hydrated Crystal A solid with water in the crystal CuSO 4 *5H 2 O

45. Anhydrous Solid A crystal without water

46. Hygroscopic Crystals that absorb moisture from the air

47. Deliquescent Crystals that absorb enough moisture from the air to liquify

48. Efflorescent Crystals that give up water to the surroundings

49. Polymorphous When a single substance can have multiple crystal structures

51. Isomorphous When different substances have the same crystal structure

52. Amorphous Solid A solid w/o a well defined crystal structure Super-cooled liquid

53. Liquid Crystals Part solid & part liquid Has a well defined crystal structure in 1 or 2 but not all 3 dimensions

54. Smectic Liquid crystal that have a well defined crystal structure in 2 dimensions

55. Nematic Liquid crystals that have a well defined crystal structure in only 1 dimension

57. Drill: List & describe the 7 crystal structures

58. Liquid A substance that holds together loosely, but has no structure in any dimension

59. Solid Definite size & shape Particles vibrate about fixed points

60. Liquid Definite size but no shape Particles vibrate about moving points

61. Gas No definite size or shape Particles move at random

63. Drill: Name & describe each of the 7 crystal structures

64. Melting Point Temperature at which the solid phase & liquid phase are at equilibrium MP & FP are equal

65. Melting Point Temperature at which the vapor pressure of a solid = the vapor pressure of its liquid phase

66. Boiling Point Temperature at which the liquid phase & gaseous phase are at equilibrium

67. Boiling Point Temperature at which the vapor pressure of a liquid = the vapor pressure of its gaseous phase or atmospheric P

68. Adhesion The attraction of particles from different substances to each other

69. Cohesion The attraction of particles of the same substance towards each other

70. Capillarity The movement of a liquid up a thin tube due to adhesion & cohesion

71. Surface Tension Pressure on the surface of a liquid caused by the uneven forces acting on the surface molecules

73. Vapor Pressure The pressure caused by the evaporated particles in the vapor above a liquid

74. Intermolecular Forces Weak temporary attractions between atoms from one molecule to another or another part of a larger molecule

76. Intermolecular Forces Hydrogen-bond Dipole-dipole Dipole-induced dipole London dispersion forces

77. Hydrogen Bond Strongest of the intermolecular forces Occurs when H is bound to one highly EN element & connects to another

78. Dipole-Dipole When two polar molecules connect

79. Dipole-Dipole + + + - + - + - - - - - - + - + - + + +

80. Dipole-Induced Dipole When a polar molecule gets near a non-polar one, it induces the non-polar one to become polar; thus, they connect

81. Dipole-Induced Dipole + + + - + + - - + - - - - + - + - + + - + - + -

82. London Dispersion Instantaneous attraction for fractions of seconds in which non-polar molecules connect Very weak force

84. Predict & explain the MP trends of: 1) Li, Na, K, & Rb 2) F 2, Cl 2, Br 2, & I 2 3) LiF, NaCl, KBr, & RbI

85. Phase Diagram Graphic representation of all the phases of a substance with respect to temperature & pressure

87. 1 atm 100 K400 K Approximate MP & BP:

88. Phase Diagrams

90. Describe conditions at each number

91. AP Chm HW Problems: 27, 51, & 53 Pages 269 & 270

92. Define solids, liquids, gases, melting & Boiling points

93. Determine the phase changes for the 3 arrows: