1. CHAPTER 13 Intermolecular Forces, Liquids and solids

2. Kinetic Molecular Theory of Matter

3. Intermolecular Forces

4. Real gases: van der Waals Equation of State

5. Empirical correction factors

6. Ion-Dipole Interactions

7. Shape and Polarity

8. Permanent Dipole Moments

9. Measuring Dipole Moments

10. Dipole - Dipole interactions Non-polarPolar M (g/mol) bp (  C) M (g/mol) bp (  C) N2N2 28-196CO28-192 SiH 4 32-112PH 3 34-88 GeH 4 77-90AsH 3 78-62 Br 2 16059ICl16297 attractive repulsive

11. Boiling Points in Hydrogen compounds ?

12. 151617 N7N7 O8O8 F9F9 P 15 S 16 Cl 17 As 33 Se 34 Br 35 The Hydrogen Bond A Exceptionally strong DP-DP Force ++ 

13. H bonding: examples Double H-bonds in acetic acidBoiling points of two isomers: EtOH and DME 78.3  C -24.8  C

14. H Bonding in Water

15. H bonding and the Structure of DNA

16. DP – non-DP Forces (dispersion forces)

19. DP – non-DP and non DP – non DP forces (dispersion forces)

20. Example of DP – non-DP and non DP – non DP Forces (dispersion forces)

22. Summary of Intermolecular Forces Increase with A.M H Bonding Increasing Polarity

23. Energy required for a molecule to leave the liquid phase. Properties of Liquids

24. Equilibrium Vapour Pressure

25. Vapour Pressure Curves

26. The Molar Enthalpy of Vaporization

27. Example – Vapor Pressure

28. Critical Temperature and Pressure H2OH2O Triple point

29. Critical Temperature Data

30. Importance to common trade gases

31. Surface tension, viscosity and capillary action

32. EXERCISE

33. Solids and Phase Diagrams

34. Amorphous Solids

35. Crystalline Solids

36. X-ray Diffraction

37. Crystalline solids: Metals

38. EXERCISE

39. Sodium Chloride (Rock Salt) Structure Type ohis is based on the face-centred cubic unit cell, insofar as the (large) Cl – ions occupy all the sites of the fcc lattice Ionic Crystals

40. Physical Properties of Solids

41. Semicrystalline Materials

42. Example: Polyvinylidenedifluoride

43. Electrical Properties of Semicrystalline Materials

44. Phase Diagrams: H 2 O

45. Phase Diagrams: CO 2

46. Important Concepts from Chapter 13 Kinetic-molecular theory of matter Intermolecular forces (four categories, hydrogen bonding) Properties of liquids Vapour pressure Boiling vs. evaporation Enthalpy of vaporization - Clausius-Clapeyron equation Surface tension, capillary action & viscosity Properties of solids Six different types of solids Enthalpy of fusion Enthalpy of sublimation Phase diagrams Predicting changes of state under different conditions Critical point & supercritical fluids Triple point