Solids :

1. Gases: Dimensionless particles in constant straight line motion colliding with their container walls 100 % elastically to create pressure

2. Liquids: Condensed state in which the particles are clustered (100-1000 particles). Order is found within the clusters but not from cluster to cluster. Attractive forces significant to make clusters but not significant enough to keep clusters from moving pasteach other.

3. Solids: with attractive forces between the particles Structural units strong enough to make a rigid structure. (i.e. particles held in fixed positions by chemical bonds)

4. Solids: Structural units with attractive forces between the particles strong enough to make a rigid structure. With An Order Without An Order (amorphous) (crystalline)

5. Scanning Tunneling Micrograph of the surface of Platinum

6. Scanning Tunneling Micrograph of the surface of graphite.

7. Solids: Structural units with attractive forces between the particles strong enough to make a rigid structure. With An Order Without An Order (amorphous) (crystalline) Simplest Repeating Pattern in 3-D Unit Cell… Eight points of a crystal lattice. (many types) A box A parallelopiped… A polyhedron with six faces, all of which are parallelograms

8. Octahedral Coordination Coordination # = 6 1 Particle per Unit Cell Simple Cubic Polonium

9. Coordination # = 8 2 Particles per Unit Cell Body-Centered Cubic Sodium

10. Coordination # = 12 4 Particles per Unit Cell Face-Centered Cubic Copper

11. ABC…ABC…ABC Stacking

12. A C B X X X A X X

13. Example Problem…Unit Cell Calculations: If nickel is cubic close packed and an edge of the unit cell is 352.4 pm, calculate the density of nickel.

14. Example Problem…Unit Cell Calculations: If nickel is cubic close packed and an edge of the unit cell is 352.4 pm, calculate the density of nickel. =8.94 g/cm3 D= m/V = 3.90x10-22 g/(3.52 x10-8cm)3 V = [(352.4 pm)(1 cm/1010 pm)]3 V = (3.52 x 10-8 cm)3 m = (4 atoms)(58.7 g/6.02x1023atoms) m = 3.90x10-22 g

16. q q d C A B sin q = AB/d 2dsin q = nl dsin q = AB Bragg’s Equation

17. In diffraction experiments involving silver crystals, info shows that constructive interference of the first order occurs when the angle of the incident x-ray is equal to 14.21° if the wavelength of the radiation is 0.7093 angstroms. What is the inter-atomic spacing of such a crystal (in cm)?

18. In diffraction experiments involving silver crystals, info shows that constructive interference of the first order occurs when the angle of the incident x-ray is equal to 14.21° if the wavelength of the radiation is 0.7093 angstroms. What is the inter-atomic spacing of such a crystal (in cm)? 2dsinq = nl d = nl/2sinq d = 7.093 x10-9 cm/0.4910 d = 1.44 x10-8 cm

19. The Seven Crystal Systems 1. Cubic (isometric) a = b= c a = b = g = 90°

21. The Seven Crystal Systems 1. Cubic (isometric) a = b= c a = b = g = 90° Examples: polonium, sodium

22. The Seven Crystal Systems 2. Tetragonal a = b= c a = b = g = 90° Examples: SnO2, BaSO4• 4H2O

23. The Seven Crystal Systems 3. Orthorhombic a = b= c a = b = g = 90° Examples: KNO3, FeSO4• 7H2O

24. The Seven Crystal Systems 4. Monoclinic a = b= c a = g = 90°b = 90° Examples: Sugar, CuSO4• 5H2O

25. The Seven Crystal Systems 5. Triclinic a = b= c a = b = g = 90° Examples: CuSO4• 5H2O, K2Cr2O7

26. The Seven Crystal Systems 6. Hexagonal a = b= c a = b = 90° g = 120° Examples: Mg, graphite

27. The Seven Crystal Systems 7. Rhombohedral (trigonal) a = b= c a = b = g = 90° Examples: AgNO3, CaCO3

28. 4 ions of each type per unit cell NaCl Coordination # of 6 for each ion

29. 2 ⅓ ions of each type per unit cell ZnS Coordination # of 4 for each ion

30. 4 ions of each type per unit cell ZnS Coordination # of 4 for each ion

31. 8 atoms per unit cell Diamond Coordination # of 4 for each atom