1. 1 Take out CLICKERS: “GO 41 GO” -or- “CH 41 CH” and CALCULATORS NEXT LECTURE:Friday, Dec. 11; Review for FINAL EXAM HOMEWORK #15:Ch. 11: # 2, 6, 16, 26, 54, 62 Due in Recitation, Tomorrow QUIZ #16:WebCT (On-Line): Wednesday-Friday (Dec. 9-11) Chapter 11 material COURSE EVALUATIONS:On-Line (WebCT); 3 Bonus Points possible… FINAL EXAM:Monday, December 14, 7-9 PM Chemistry 177 December 9, 2009

2. 2 Structures of Solids: Metals and Ionic Salts Sphere Packings: 3D Hexagonally Closest Packed (HCP) A B A B (Mg, Sc, Ti, Zn) Cubic Closest Packed (CCP = FCC) A B C A (Al, Ca, Ni, Cu) ROTATE FCC = Face-Centered Cubic: (Unit Cell) Chapter 11: Intermolecular Forces, Liquids, and Solids

3. 3 Unit Cells: Counting Atoms # Atoms/Unit Cell = Chapter 11: Intermolecular Forces, Liquids, and Solids

4. 4 Unit Cells: Counting Atoms Face-Centered CubicBody-Centered Cubic # Atoms Inside = # Atoms on Faces = # Atoms on Edges = # Atoms on Corners = # Atoms/Cell = # Atoms Inside = # Atoms on Faces = # Atoms on Edges = # Atoms on Corners = # Atoms/Cell = Chapter 11: Intermolecular Forces, Liquids, and Solids

5. 5 Unit Cells: Counting Atoms; Density # Atoms Inside = # Atoms on Faces = # Atoms on Edges = # Atoms on Corners = # Atoms/Cell = 542.86 pm Chapter 11: Intermolecular Forces, Liquids, and Solids How many Si atoms are in the unit cell?

6. 6 Unit Cells: Counting Atoms; Density What is the density (g/cm 3 ) of Si under normal conditions (T = 298 K, p = 1 atm)? AW(Si) = 28.1 g/mol 1 pm = 10  10 cm Mass of Si Atoms: Volume of Unit Cell: Density: Chapter 11: Intermolecular Forces, Liquids, and Solids 542.86 pm

7. 7 Chapter 11: Intermolecular Forces, Liquids, and Solids Write the Balanced Chemical Equation for the following:

8. 8 Liquid SolidGas Supercritical Fluids Different Solid Phases (a)Multiple Crystalline Phases (b)Amorphous (c)Magnetic, Superconducting Phase: state of matter that is uniform throughout in both chemical constitution and physical state. Two or more phases can coexist. Chapter 11: Intermolecular Forces, Liquids, and Solids

9. 9 Phase Diagrams Graphical Representation of Equilibrium Behavior PRESSURE TEMPERATURE Variables: T, p, x 1, x 2, …, x C Mole Fractions of Components 1 Component: only T and p (x 1 = 1) Gibbs Phase Rule: Relationship between # Distinct Chemical Components (C) # Phases (P) # Independent Variables (F) Chapter 11: Intermolecular Forces, Liquids, and Solids

10. 10 Phase Diagrams (Examples) Source: http://www.cbu.edu/~mcondren/water-phase-diagram.jpg H2OH2O Chapter 11: Intermolecular Forces, Liquids, and Solids

11. 11 Source: http://www.cbu.edu/~mcondren/CO2_phase_diagram.jpg Phase Diagrams (Examples) CO 2 Chapter 11: Intermolecular Forces, Liquids, and Solids

12. 12 Source: http://www.lsbu.ac.uk/water/images/phasexp.gif Phase Diagrams (Examples) H2OH2O Rank the forms of ice from lowest to highest DENSITY: Ca. 10 4 atm (1 MPa = 9.869 atm) (2000 atm) Chapter 11: Intermolecular Forces, Liquids, and Solids

13. 13 Iron Pressure 13 GPa Temperature 1173 K1660 K1808 K Liquid 1043K Curie Temperature  -Fe: 11.78 Å 3  -Fe: 10.66 Å 3  -Fe: 12.13 Å 3  -Fe: 12.60 Å 3 Volume Decreases Volume Increases D.A. Young, Phase Diagrams of the Elements, 1976. Phase Diagrams (Examples) HCP CCP BCC Chapter 11: Intermolecular Forces, Liquids, and Solids

14. 14 Critical Points SOLID LIQUID GAS PRESSURE TEMPERATURE 300.7  C Benzene (T c = 308  C) 309.2  C SUPERCRITICAL FLUID 307.4  C Chapter 11: Intermolecular Forces, Liquids, and Solids