2. Network Solids To play movie you must be in Slide Show Mode
PC Users: Please wait for content to load, then click to play
Mac Users: CLICK HERE
Copyright © Cengage Learning. All rights reserved

3. The Structures of Diamond and Graphite
Copyright © Cengage Learning. All rights reserved

4. Partial Representation of the Molecular Orbital Energies in a) Diamond b) a Typical Metal
Copyright © Cengage Learning. All rights reserved

5. The p Orbitals and Pi-system in Graphite
Copyright © Cengage Learning. All rights reserved

6. Ceramics
Typically made from clays (which contain silicates) and hardened by firing at high temperatures.
Nonmetallic materials that are strong, brittle, and resistant to heat and attack by chemicals.
Copyright © Cengage Learning. All rights reserved

7. Semiconductors
n-type semiconductor – substance whose conductivity is increased by doping it with atoms having more valence electrons than the atoms in the host crystal.
p-type semiconductor – substance whose conductivity is increased by doping it with atoms having fewer valence electrons than the atoms of the host crystal.
Copyright © Cengage Learning. All rights reserved

8. Energy Level Diagrams for (a) an n-type Semiconductor (b) a p-type Semiconductor
Copyright © Cengage Learning. All rights reserved

9. Silicon Crystal Doped with (a) Arsenic and (b) Boron

10. To play movie you must be in Slide Show Mode
PC Users: Please wait for content to load, then click to play
Mac Users: CLICK HERE
Copyright © Cengage Learning. All rights reserved

11. To play movie you must be in Slide Show Mode
PC Users: Please wait for content to load, then click to play
Mac Users: CLICK HERE
Copyright © Cengage Learning. All rights reserved

12. Ionic Solids
Ionic solids are stable, high melting substances held together by the strong electrostatic forces that exist between oppositely charged ions.
Copyright © Cengage Learning. All rights reserved

13. Three Types of Holes in Closest Packed Structures
Trigonal holes are formed by three spheres in the same layer.
Copyright © Cengage Learning. All rights reserved

14. Three Types of Holes in Closest Packed Structures
Tetrahedral holes are formed when a sphere sits in the dimple of three spheres in an adjacent layer.
Copyright © Cengage Learning. All rights reserved

15. Three Types of Holes in Closest Packed Structures
Octahedral holes are formed between two sets of three spheres in adjoining layers of the closest packed structures.
Copyright © Cengage Learning. All rights reserved

16. trigonal < tetrahedral < octahedral
For spheres of a given diameter, the holes increase in size in the order:
trigonal < tetrahedral < octahedral
Copyright © Cengage Learning. All rights reserved

17. Types and Properties of Solids
Copyright © Cengage Learning. All rights reserved

18. Behavior of a Liquid in a Closed Container a) Initially b) at Equilibrium
Copyright © Cengage Learning. All rights reserved

19. The Rates of Condensation and Evaporation
Copyright © Cengage Learning. All rights reserved

20. Vapor Pressure Pressure of the vapor present at equilibrium.
The system is at equilibrium when no net change occurs in the amount of liquid or vapor because the two opposite processes exactly balance each other.
Copyright © Cengage Learning. All rights reserved

21. What is the vapor pressure of water at 100°C? How do you know? 1 atm
The vapor pressure of water at 100oC is 1 atm. You know this because atmospheric pressure is 1 atm and this is the temperature at which we observe water to boil.
Copyright © Cengage Learning. All rights reserved

22. Vapor Pressure
Copyright © Cengage Learning. All rights reserved

23. Vapor Pressure
Liquids in which the intermolecular forces are large have relatively low vapor pressures.
Vapor pressure increases significantly with temperature.
Copyright © Cengage Learning. All rights reserved

24. Vapor Pressure vs. Temperature
Copyright © Cengage Learning. All rights reserved

25. Clausius–Clapeyron Equation
Pvap = vapor pressure ΔHvap = enthalpy of vaporization R = J/K·mol T = temperature (in kelvin)
Copyright © Cengage Learning. All rights reserved

26. The vapor pressure of water at 25°C is 23
The vapor pressure of water at 25°C is 23.8 torr, and the heat of vaporization of water at 25°C is 43.9 kJ/mol. Calculate the vapor pressure of water at 65°C. 194 torr
ln(23.8 torr/Pvap,T2) = [(43900 J/mol)/( J/K·mol)][(1/338 K) – (1/298)]
Pvap,T2 = 194 torr
Copyright © Cengage Learning. All rights reserved

27. Changes of State To play movie you must be in Slide Show Mode
PC Users: Please wait for content to load, then click to play
Mac Users: CLICK HERE
Copyright © Cengage Learning. All rights reserved

28. Heating Curve for Water
Copyright © Cengage Learning. All rights reserved

29. CONCEPT CHECK!
Which would you predict should be larger for a given substance: ΔHvap or ΔHfus? Explain why.
ΔHvap should be larger because it will take a lot more energy to break the intermolecular forces between the liquid molecules to completely break apart to form a gas.
Copyright © Cengage Learning. All rights reserved

30. Phase equilibrium lines
A convenient way of representing the phases of a substance as a function of temperature and pressure:
Triple point
Critical point
Phase equilibrium lines
Copyright © Cengage Learning. All rights reserved

31. Phase Diagram for Carbon Dioxide
Copyright © Cengage Learning. All rights reserved

32. Phase Diagram for Water
Copyright © Cengage Learning. All rights reserved

33. CONCEPT CHECK!
As intermolecular forces increase, what happens to each of the following? Why?
Boiling point
Viscosity
Surface tension
Enthalpy of fusion
Freezing point
Vapor pressure
Heat of vaporization
Boiling point increases
Viscosity increases
Surface tension increases
Enthalpy of fusion increases
Freezing point increases
Vapor pressure decreases
Heat of vaporization increases