1. Chapter 12: Liquids, Solids and Intermolecular Forces
Chemistry 140 Fall 2002
General Chemistry
Principles and Modern Applications
Petrucci • Harwood • Herring
8th Edition
Chapter 12: Liquids, Solids and Intermolecular Forces
Philip Dutton
University of Windsor, Canada
N9B 3P4
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2. General Chemistry: Chapter 13
Chemistry 140 Fall 2002
Contents
12-1 Intermolecular Forces and some Properties of Liquids
12-2 Vaporization of Liquids: Vapor Pressure
12-3 Some Properties of Solids
12-4 Phase Diagrams
12-5 Van der Waals Forces
12-6 Hydrogen Bonding
12-7 Chemical Bonds as Intermolecular Forces
12-8 Crystal structures
12-8 Energy Changes in the Formation of Ionic Crystals
Focus on Liquid Crystals
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General Chemistry: Chapter 13

3. 12-1 Intermolecular Forces and Some Properties of Liquids
Cohesive Forces
Intermolecular forces between like molecules.
Adhesive Forces
Intermolecular forces between unlike molecules.
Surface Tension
Energy or work required to increase the surface area of a liquid.
Viscosity
A liquids resistance to flow
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4. Intermolecular Forces
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General Chemistry: Chapter 13

5. Intermolecular Forces
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6. 12-2 Vaporization of Liquids: Vapor Pressure
Chemistry 140 Fall 2002
12-2 Vaporization of Liquids: Vapor Pressure
Bonding atomic orbitals are shown in grey.
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7. Enthalpy of Vaporization
ΔHvap = Hvapor – Hliquid = - ΔHcondensation
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8. Boiling Point Mercury manometer Vapor pressure of liquid
Pvap independent of Vliq
Pvap independent of Vgas
Pvap dependent on T
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9. Vapor Pressure and Boiling Point
(e) (d) (c) (b) (a)
Ln P = -A ( ) + B 1 T
A =
ΔHvap R
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10. Clausius-Clapeyron Equation
Ln P = -A ( ) + B 1 T
Ln = ( ) P2 P1 1 T2 T1
ΔHvap R
Example 12-1:
The vapor pressure is  5.08 kPa at 18.1 °C, the vaporization enthalpy is  41.9 kJ/mol. What is the vapor pressure at 61.1 °C?
Example 12-2:
A compound has a kPa vapor pressure at °C. At °C it has kPa vapor pressure.  What is the molar enthalpy of vaporization in J mol-1 of this compound?
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11. 12-3 Some Properties of Solids
Freezing Point
Melting Point
ΔHfus(H2O) = kJ/mol
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12. General Chemistry: Chapter 13
Sublimation
ΔHsub = ΔHfus + ΔHvap
= -ΔHdeposition
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General Chemistry: Chapter 13

13. General Chemistry: Chapter 13
Chemistry 140 Fall 2002
12-4 Phase Diagrams
Iodine
OD represents the FUSION CURVE. There is little effect of pressure on melting point.
O is the triple point. A unique temperature and pressure at which three states of matter coexist in equilibrium.
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General Chemistry: Chapter 13

14. General Chemistry: Chapter 13
Chemistry 140 Fall 2002
Phase Diagrams
Carbon dioxide
Triple point is greater than one atmosphere, so we do not form liquid. Sublimation occurs.
Liquid present in fire extinguishers (P > 5.1 atm)
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General Chemistry: Chapter 13

15. General Chemistry: Chapter 13
Supercritical Fluids
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General Chemistry: Chapter 13

16. General Chemistry: Chapter 13
Chemistry 140 Fall 2002
Phase Diagram of Water
Fusion curve (OD) has a negative slope. Unusual behavior. Ice skating.
Polymorphysm, the existence of a solid substance in more than one form. This is common.
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General Chemistry: Chapter 13

17. General Chemistry: Chapter 13
The Critical Point
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18. Critical Temperatures and Pressures
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19. 3 dimension p-V-T surface
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20. Water 3 dimension p-V-T surface

21. Van der Waals Constants
The Van der Waals constants can be obtained from the critical data:
a = 3pc Vc and b = Vc/3
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22. General Chemistry: Chapter 13
12-5 Van der Waals Forces
Instantaneous dipoles.
Electrons move in an orbital to cause a polarization.
Induced dipoles.
Electrons move in response to an outside force.
Dispersion or London forces.
Instaneous dipole – induced dipole attraction.
Related to polarizability.
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23. Phenomenon of Induction
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24. Instantaneous and Induced Dipoles
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25. London dispersion in hydrocarbons
C5H C15H C18H38

26. Dipole Dipole Interactions
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27. The water molecule (dipole moment)
Dipole moment:  = Debye
Polarizability: α = x cm3 δ- δ+
General Chemistry: Chapter 13

28. General Chemistry: Chapter 13
12-6 Hydrogen Bonding
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29. Hydrogen Bonding in HF(g)
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30. Hydrogen Bonding in Water
Chemistry 140 Fall 2002
Hydrogen Bonding in Water
Solid ice has lower density than liquid water. H-bonding holds the ice in a rigid but open structure.
Maximum density of water at 3.98 C.
around a molecule in the solid in the liquid
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31. Other examples of H-Bonds
Chemistry 140 Fall 2002
Other examples of H-Bonds
Viscosity
Units centipoise (cP). Water at 20 C 1 cP.
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32. 12-7 Chemical Bonds as Intermolecular Forces
Chemistry 140 Fall 2002
12-7 Chemical Bonds as Intermolecular Forces
Network covalent solids. C allotropes: Diamond and Graphite
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33. Other Carbon Allotropes
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34. General Chemistry: Chapter 13
Interionic Forces
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35. General Chemistry: Chapter 13
12-8 Crystal Structures
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36. Unit Cells in the Cubic Crystal System
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37. General Chemistry: Chapter 13
Holes in Crystals
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38. Hexagonal Close Packed (hcp)
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39. General Chemistry: Chapter 13
Coordination Number
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40. Counting Cell Occupancy
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41. General Chemistry: Chapter 13
X-Ray Diffraction
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42. General Chemistry: Chapter 13
X-Ray Diffraction
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43. General Chemistry: Chapter 13
Cesium Chloride
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General Chemistry: Chapter 13

44. Atomic Radii from Crystal Structures
Chemistry 140 Fall 2002
Atomic Radii from Crystal Structures
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45. General Chemistry: Chapter 13
Sodium Chloride
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46. General Chemistry: Chapter 13
Holes in Crystals
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47. General Chemistry: Chapter 13
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General Chemistry: Chapter 13

48. 12-9 Energy Changes in the Formation of Ionic Crystals
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49. General Chemistry: Chapter 13
Chapter 13 Questions
1, 3, 4, 13, 24, 26, 31, 45, 52, 61, 94, 107
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General Chemistry: Chapter 13