1. Chapter 11 Properties of Liquids and Solids Formula  Lewis Structure  Electron Geometry  Molecular Geometry  Polarity  Intermolecular Forces  Properties

2. What happens when water boils. Draw pictures. Bonding vs. Intermolecular Forces (IMFs): Where do IMFs come from?

3. Types of forces between molecules: Intermolecular Forces (IMFs)

4. Enthalpy of hydration: Trends: Ion-Dipole Forces: Between dissolved ions and polar molecules

5. Dipole-Dipole Forces: Between polar molecules Trends:

6. Dipole-Induced Dipole Forces: Between polar and nonpolar molecules Trends:

7. Induced Dipole-Induced Dipole Forces: Between nonpolar molecules Trends:

8. Hydrogen Bonding: Molecules with F-H, O-H, or N-H bonds

10. Hydrogen Bonding: Properties of water

12. More on Boiling Points and Hydrogen Bonding

13. Identifying IMFs

14. Relative Contributions of Different IMFs

15. Properties of Liquids Vapor Pressure (volatility) Boiling Point Enthalpy of Vaporization Viscosity Surface Tension

16. Molecular interpretation of vapor pressure and boiling. Enthalpy of vaporization:

21. Clausius-Clapyron Equation: Vapor Pressure,  H vap, and T

22. Graphical Method of Determining Enthalpy of Vaporization

25. Example 2. What is the mass of water in the air in this lecture hall? 14 m x 5 m x 17 m T = 22 o C Humidity = 43%

26. Example 3. A 1-L flask of air is at 30 o C and relative humidity of 68%. The flask is put in a freezer and the temperature decreases to 5 o C. What happens?

27. Surface Tension

28. Types of Solids: Ionic Molecular Network: crystalline amorphous Metallic

29. More Network Solids diamond Quartz: SiO 2

33. Counting Atoms in Unit Cells: Inside: 1 Face:½ Edge:¼ Corner:1/8

36. Unit Cells, Dimensions and Measurements: Ca metal: Face centered cubic unit cell Density = 1.54 g/cm 3 What is the radius of a Ca atom?

38. What fraction of a simple cubic unit cell is filled with atoms? What fraction of a face-centered cubic unit cell is filled with atoms?

43. Supercritical Fluids