1. I. Intermolecular Forces (Ch. 6, p.189-193)
Ch Liquids & Solids
I. Intermolecular Forces (Ch. 6, p )

2. A. Definition of IMF Attractive forces between molecules.
Much weaker than chemical bonds within molecules.

3. B. Types of IMF

4. B. Types of IMF
London Dispersion Forces
View animation online.

5. B. Types of IMF
Attractive forces that arise as a result of temporary dipoles induced in atoms or molecules
ion-induced dipole interaction
dipole-induced dipole interaction
11.2

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

7. B. Types of IMF
Hydrogen Bonding

8. C. Determining IMF NCl3 polar = dispersion, dipole-dipole CH4
nonpolar = dispersion HF
H-F bond = dispersion, dipole-dipole, hydrogen bonding

9. II. Physical Properties (p. 363 - 371)
Ch Liquids & Solids
II. Physical Properties (p )

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

11. A. Liquids vs. Solids
A phase is a homogeneous part of the system in contact with other parts of the system but separated from them by a well-defined boundary.

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

13. B. Liquid Properties Capillary Action
attractive force between the surface of a liquid and the surface of a solid
water
mercury

14. B. Liquid Properties
Adhesion
Cohesion

15. Water is a Unique Substance
Maximum Density
40C
Density of Water
Water is a Unique Substance
11.3

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

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

18. C. Types of Solids Covalent Molecular Covalent Network Amorphous (H2O)
(SiO2 - quartz)
Amorphous
(SiO2 - glass)

19. C. Types of Solids
Diamond
Graphite

20. C. Types of Solids

21. III. Changes of State (p. 372 - 382)
Ch Liquids & Solids
III. Changes of State (p )

22. A. Phase Changes

23. A. Phase Changes Evaporation
molecules at the surface gain enough energy to overcome IMF
Volatility
measure of evaporation rate
depends on temp & IMF

24. Greatest
Order
Least
T2 > T1
Evaporation
Condensation

25. A. Phase Changes temp volatility IMF volatility Boltzmann Distribution
# of Particles
volatility
IMF
volatility
Kinetic Energy

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

27. A. Phase Changes Vapor Pressure
pressure of vapor above a liquid at equilibrium
depends on temp & IMF
directly related to volatility

28. A. Phase Changes
IMF
v.p.
v.p.
temp

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

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

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

32. B. Heating Curves Gas - KE  Boiling - PE  Liquid - KE 
Melting - PE 
Solid - KE 

33. B. Heating Curves Heat of Vaporization (Hvap)
energy required to boil 1 gram of a substance at its b.p.
usually larger than Hfus…why?
EX: sweating, steam burns, the drinking bird

34. B. 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

35. B. Heating Curves Phase Change change in PE (molecular arrangement)
temp remains constant
Heat of Fusion (Hfus)
energy required to melt 1 gram of a substance at its m.p.

36. C. Phase Diagrams
Show the phases of a substance at different temps and pressures.

37. C. Phase Diagrams