1. Liquids & Solids Dr. Ron Rusay Fall 2001

2. States of Matter

4. Changes of State

5. Energy of Phase Changes

7. Heating Curve for H 2 O Calculate the heat necessary to completely boil 1.0 kg of ice that is at -5 o C. Cp ice =0.50 cal/g x o C Cp liq =1.00 cal/g x o C Cp vap =0.48 cal/g x o C  H fusion = +80.0 cal/g  H vapor = +540 cal/g +722.5 kcal = +3,023 kJ

8. Vapor Pressure vs. Temperature

9. Vapor Pressures of Liquids

10. Periodicity: Boiling Point Boiling Point: Temperature at which the vapor pressure of the liquid equals the atmospheric pressure. Higher vapor pressure : Lower boiling point. Does water boil at the same temperature in Concord and Tahoe?

11. Boiling Points of Simple Hydrogen Compounds What can explain the trends?

13. Intermolecular Hydrogen Bonds in H 2 O Besides oxygen, both nitrogen and fluorine form intermolecular hydrogen bonds. Other atoms DO NOT.

14. Views of Water 104.5 o AngleDipole Moment

15. Dissolution of NaCl in Water

16. Intermolecular Forces Ionic & Polar Interactions: + and - ;  + ----  -

17. Ion-Dipole Forces

18. Dipole-Dipole Forces FG11_004.JPG

19. Surface Forces of a Liquid Viscosity & Surface Tension of liquids are directly related to the strength of the intermolecular forces: Eg. Water versus gasoline. 1.00 vs 0.20 centipoise and 70 vs. 15 dynes/cm 2 respectively.

20. Close Packing

21. Close Packed Spheres

22. Three Types of Crystalline Solids Ionic MolecularMetallic

23. Diamond and Graphite

24. Cross Section of a Metal

25. Crystal Lattice

26. Cubic Lattices

27. Space-Filling Cubic Cells

28. Crystal Lattice of NaCl

29. Unit Cell of NaCl

30. Unit Cells

31. X-Ray Crystallography

32. Table 11.6