1. Intermolecular Forces Forces Between Molecules

2. Why are intermolecular forces important? They determine the phase of a substance at room temperature.

3. 3 Types of Intermolecular Forces Dispersion or Van der Waals Dipole-dipole Hydrogen Bonds

4. Strongest Intermolecular Force Hydrogen Bonds

5. When do Hydrogen bonds occur? Between molecules containing F, O, N bonded to a H atom

6. Strongest hydrogen bonds? Between molecules containing F-H bonds

7. Weakest hydrogen bonds? Between molecules containing N-H bonds

8. What effect does H-bonding have on the properties of the substance? Hydrogen bonding leads to substantial increases in the expected boiling point.

9. Weakest Intermolecular Force Dispersion or Van der Waals forces

10. When do dispersion forces occur? Between nonpolar molecules

11. Nonpolar No Poles! The molecule is symmetric! Cannot tell 1 end from the other.

12. 2 Easy categories of Nonpolar Molecules Monatomic Gases (Column 18) & Diatomic Elements

13. What are the diatomic elements? H 2, N 2, O 2, F 2, Br 2, Cl 2, & I 2

14. 3rd category of Nonpolar Molecules Larger molecules with a very symmetric shape

15. What can you say about dispersion forces as a function of molecular size? The larger the molecules the stronger the dispersion forces!

16. When do dipole-dipole forces occur? Between polar molecules.

17. Polar Has Poles! The molecule is NOT symmetric! Can tell 1 end from the other.

18. Vapor Gas phase of a substance that is normally a liquid at room temperature.

19. Vapor Pressure The partial pressure of a vapor above its liquid.

20. What does vapor pressure depend on? (Hint: see Table H) Vapor pressure depends on the temperature of the liquid.

21. What happens to the vapor pressure as the temperature of the liquid is increased? The vapor pressure always increases with temperature.

22. Does the vapor pressure depend on the amount of liquid present? No. A thimbleful is as good as an ocean.

23. What are some differences between evaporation & boiling? Evaporation occurs at all temperatures. Boiling occurs at a definite temperature. Evaporation occurs at the surface. Boiling occurs throughout the liquid.

24. Heat of fusion Amount of energy required to convert 1 gram of a pure solid to the liquid phase at its melting point.

25. Heat of vaporization Amount of energy required to convert 1 gram of a pure liquid to the gas phase at its boiling point.

26. What happens to the boiling point as the intermolecular forces increase? The stronger the intermolecular forces, the higher the boiling point.

27. What happens to the melting point as the intermolecular forces increase? The stronger the intermolecular forces, the higher the melting point.

28. What happens to the heat of fusion as the intermolecular forces increase? The stronger the intermolecular forces, the higher the heat of fusion.

29. What happens to the heat of vaporization as the intermolecular forces increase? The stronger the intermolecular forces, the higher the heat of vaporization.

30. What happens to the evaporation rate as the intermolecular forces increase? The stronger the intermolecular forces, the lower the evaporation rate.

31. What happens to the vapor pressure as the intermolecular forces increase? The stronger the intermolecular forces, the lower the vapor pressure.

32. Boiling Point Temperature at which the vapor pressure of a liquid is equal to the external pressure.

33. Normal Boiling Point Temperature at which the vapor pressure of a liquid is equal to 1 atm or 101.3 kPa or 760 torr.

34. What happens to the boiling point when the external pressure is reduced? The boiling point is reduced.

35. Sublimation Solid to gas

36. Deposition Gas to solid

37. Vaporization Liquid to Gas

38. Condensation Gas to liquid

39. Fusion Solid to liquid Or Melting

40. Freezing Liquid to solid Crystallization Solidification

41. Which phase changes are endothermic? Solid to liquid Liquid to Gas Solid to Gas GLSGLS

42. Which phase changes are exothermic? Gas to Liquid Liquid to Solid Gas to Solid G L S