1. 11.5 Vapor Pressure
Explaining Vapor Pressure on the Molecular Level, Volatility,
Vapor Pressure, and Temperature;
Vapor Pressure and Boiling Point
11.6 Phase Diagrams
The Phase Diagrams of H2O and CO2
11.7 Structures of Solids
Unit Cells
The Crystal Structure of Sodium Chloride
Close Packing of Spheres
11.8 Bonding in Solids
Molecular Solids
Covalent-Network Solids
Ionic Solids
Metallic Solids
Chapter 13 Properties of Solutions
13.1 The Solution Process
Energy Changes and Solution Formation
Solution Formation, Spontaneity, and Disorder
Solution Formation and Chemical Reactions

2. The observation of Vapor Pressure:

3. And, at higher temperatures, the vp is higher.

4. The same
picture is
useful to
rationalize
Vapor
Pressure

5. With the beaker covered, equilibrium is
soon established.

6. Contrast that with an uncovered beaker!

9. ← Temp. increases But, recall, we always prefer straight lines!
(Add slide of C-C eq and plot.)
← Temp. increases

10. The slope! Using the Clausius-Clapeyron Equation:
Tabulate P in atm and T in K; Calculate lnP and 1/T
Plot lnP vs 1/T
The slope is = - ΔHvap /R
The slope!

14. First Midquarter Exam Monday, Jan 31 6:30-7:48 pm Rooms TBA
The quiz next week will be given during
your recitation.
It will cover material starting with section
11.5.
First Midquarter Exam
Monday, Jan 31
6:30-7:48 pm
Rooms TBA
Chaps 10, 11, 13

16. 11.51 The normal melting and boiling points of xenon are
-112 oC and -107 oC, respectively. Its triple point is at
-121 oC and 282 torr, and its critical point is a 16.6 oC
and 57.6 atm.
(a) Sketch the phase diagram of Xe, showing the four
points given above and indicating the area in which each
phase is stable.
(b) Which is more dense, solid or liquid Xe?
(c) If Xe gas is cooled under an external pressure of 100
torr, will it undergo condensation or deposition?

17. 11.7 Structures of Solids
Unit Cells
The Crystal Structure of NaCl
Close Packing of Spheres
11.8 Bonding in Solids
Molecular Solids
Covalent-Network Solids
Ionic Solids
Metallic Solids

18. Sulfur Crystals

19. Millerite Crystals (a nickel ore)

21. These are the ones we’ll be
interested in. ↓

28. Figure: 11-35
The ‘NaCl’ Structure

30. Figure: 11-36

35. fact
Cubic
close
packing
(ABCABC..)
Hexagonal
close
packing
(ABABAB…)

37. 11.7 Structures of Solids
Unit Cells
The Crystal Structure of NaCl
Close Packing of Spheres
11.8 Bonding in Solids
Molecular Solids
Covalent-Network Solids
Ionic Solids
Metallic Solids

38. Figure: 11-T07

39. Contrast the MPs and BPs of some materials which are
Molecular Solids:
C6H6 C6H5-CH3 C6H5-OH MP BP

43. Figure: 11-41

44. 11.59 Aluminum metal crystallizes in a cubic close-packed
structure (face-centered cubic cell).
(a) How many aluminum atoms are in a unit cell?
(b) What is the coordination number of each aluminum atom?
(c) Assume that the aluminum catoms can be represented as
spheres. If each Al atom has a radius of 1.43 Å, what is the
length of a side of the unit cell?
(d) Calculate the density of Al metal.

45. 11.67 A certain form of AgI adopts the zinc blende structure.
The density of the salt is 5.69 g/cm3.
(a) Calculate the length of a side of the unit cell.
(b) Calculate the distance between the Ag+ and I- ions in
the structure.
At wt Ag = I = 126.9
No = 6.02 x 1023 amu/g 1 Å = 10-8 cm

49. 11.32 The heat of vaporization of CCl2F2 (a CFC) is 289 J/g.
What mass of this substance must evaporate in order to
freeze 100 g of water initially at 18 oC?
(The heat of fusion of water is 334 J/g and the specific
heat of liquid water is 4.18 J/g-K)