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

2. AP Chm HW Problems 7 & 9 Page 268

3. Solids

4. Molecular Solids Covalently bound molecules held together by intermolecular forces

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

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

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

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

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

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

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

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

19. Drill: Describe unit cells & crystal lattice

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

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

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

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

31. 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

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

34. Drill: List & describe the 7 crystal structures

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

36. Anhydrous Solid A crystal without water

37. Hygroscopic Crystals that absorb moisture from the air

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

39. Efflorescent Crystals that give up water to the surroundings

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

42. Isomorphous When different substances have the same crystal structure

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

68. Dipole-Dipole When two polar molecules connect

69. 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

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

72. 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

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

75. 1 atm 100 K400 K Approximate MP & BP:

76. Phase Diagrams

78. Describe conditions at each number

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

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

81. Determine the phase changes for the 3 arrows: