1. I. Kinetic Molecular Theory KMT

2. Assumptions of KMT All matter is composed of tiny particles These particles are in constant, random motion. Some particles are moving fast, some are moving slowly. Temperature is a measure of the average Kinetic Energy and is proportional to the average speed of the molecules.

3. KMT Model  http://preparatorychemistry.com/Bish op_KMT_frames.htm http://preparatorychemistry.com/Bish op_KMT_frames.htm  Click on the link above to see how particles of matter behave according to the KMT.

4. Liquids & Solids II. Intermolecular Forces

5. A. Definition of IMF  Attractive forces between molecules.  Much weaker than chemical bonds within molecules.  a.k.a. van der Waals forces

6. B. Types of IMF

7.  London Dispersion Forces View animation online.animation

8. B. Types of IMF  Dipole-Dipole Forces + + - - View animation online.animation

9. B. Types of IMF  Hydrogen Bonding

10. C. Determining IMF  NCl 3 polar = dispersion, dipole-dipole  CH 4 nonpolar = dispersion  HF H-F bond = dispersion, dipole- dipole, hydrogen bonding

11. III. Physical Properties Liquids & Solids

12. A. Liquids vs. Solids LIQUIDS Stronger than in gases Y high N slower than in gases SOLIDS Very strong N high N extremely slow IMF Strength Fluid Density Compressible Diffusion

13. B. Liquid Properties  Surface Tension attractive force between particles in a liquid that minimizes surface area

14. B. Liquid Properties  Capillary Action attractive force between the surface of a liquid and the surface of a solid watermercury

15. C. Types of Solids  Crystalline - repeating geometric pattern covalent network metallic ionic covalent molecular  Amorphous - no geometric pattern decreasing m.p.

16. C. Types of Solids Ionic (NaCl) Metallic

17. C. Types of Solids Covalent Molecular (H 2 O) Covalent Network (SiO 2 - quartz) Amorphous (SiO 2 - glass)

18. Liquids & Solids IV. Changes of State

19. A. Phase Changes

20.  Evaporation molecules at the surface gain enough energy to overcome IMF  Volatility measure of evaporation rate depends on temp & IMF

21. A. Phase Changes Kinetic Energy # of Particles p. 477 Boltzmann Distribution tempvolatilityIMFvolatility

22. A. Phase Changes  Equilibrium trapped molecules reach a balance between evaporation & condensation

23. A. Phase Changes  Vapor Pressure pressure of vapor above a liquid at equilibrium IMFv.p.tempv.p. depends on temp & IMF directly related to volatility p.478 temp v.p.

24. A. Phase Changes  Boiling Point temp at which v.p. of liquid equals external pressure IMFb.p.P atm b.p. depends on P atm & IMF Normal B.P. - b.p. at 1 atm

25.  Which has a higher m.p.? polar or nonpolar? covalent or ionic? A. Phase Changes  Melting Point equal to freezing point polar ionic IMFm.p.

26. A. Phase Changes  Sublimation solid  gas v.p. of solid equals external pressure  EX: dry ice, mothballs, solid air fresheners

27. A. Phase Changes Energy RequiredEnergy Released Solid  Liquid Melting or fusion Liquid  Solid freezing Liquid  Gas Vaporization, evaporation or boiling Gas  Liquid condensation Solid  Gas sublimation Gas  Solid deposition

28. Heating Curves

29. A. Heating Curves Kinetic Energy Changes – Heat Energy speeds up the molecules. Potential Energy Changes – Heat energy separates the molecules from solid to liquid, liquid to gas.

30. A. Heating Curves  Temperature Change change in KE (molecular motion) depends on heat capacity  Heat Capacity energy required to raise the temp of 1 gram of a substance by 1°C

31. A. Heating Curves  Phase Change change in PE (molecular arrangement) temp remains constant Phase Change Diagrams Show the phases of a substance at different temperatures and pressures.

32.  The energy involved in a phase change is calculated using:  Heat of Fusion (  H fus )  Heat of Vaporization (  H vap )

33. Heat of Fusion  Heat of Fusion is the energy required to change 1 gram of a substance from the solid to the liquid state without changing its temperature.  This energy breaks down the solid bonds, but it leaves a significant amount of energy associated with the intermolecular forces of the liquid state. Heat of Fusion is used for calculations involving the phase changes of solid  liquid or liquid  solid

34. A. Heating Curves  Heat of Vaporization (  H vap ) energy required to boil 1 gram of a substance at its b.p.  EX: sweating, steam burns, the drinking bird