This document is a chapter from a general chemistry textbook titled "General Chemistry: Principles and Modern Applications" by Petrucci, Harwood, and Herring. The chapter is titled "Liquids, Solids and Intermolecular Forces" and covers topics such as the properties of liquids and solids, intermolecular forces like hydrogen bonding and van der Waals forces, phase diagrams, crystal structures of solids, and energy changes during phase changes. It includes diagrams to illustrate concepts like vapor pressure curves, phase diagrams, and crystal unit cells.

1. General Chemistry
Principles and Modern Applications
Petrucci • Harwood • Herring
8th Edition
Chapter 13: Liquids, Solids and
Intermolecular Forces
Philip Dutton
University of Windsor, Canada
N9B 3P4
Prentice-Hall © 2002

2. Contents
13-1 Intermolecular Forces and some Properties of Liquids
13-2 Vaporization of Liquids: Vapor Pressure
13-3 Some Properties of Solids
13-4 Phase Diagrams
13-5 Van der Waals Forces
13-6 Hydrogen Bonding
13-7 Chemical Bonds as Intermolecular Forces
13-8 Crystal structures
13-8 Energy Changes in the Formation of Ionic Crystals
Focus on Liquid Crystals
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3. 13-1 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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5. Intermolecular Forces
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6. 13-2 Vaporization of Liquids:
Vapor Pressure
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7. Enthalpy of Vaporization
ΔHvap = Hvapor – Hliquid = - ΔHcondensation
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8. Boiling Point
Mercury Vapor Pvap Pvap Pvap
manometer pressure independent independent dependent on
of liquid of Vliq of Vgas T
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9. Vapor Pressure and Boiling Point
(e) (d) (c) (b) (a)
1
Ln P = -A ( )+B
T
ΔHvap
A=
R
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10. Clausius-Clapeyron Equation
1
Ln P = -A ( )+B
T
P2 ΔHvap 1 1
Ln =- ( - )
P1 R T1 T2
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11. 13-3 Some Properties of Solids
Freezing Point Melting Point
ΔHfus(H2O) = +6.01 kJ/mol
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12. Sublimation
ΔHsub = ΔHfus + ΔHvap
= -ΔHdeposition
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13. 13-4 Phase Diagrams
Iodine
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14. Phase Diagrams
Carbon dioxide
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15. Supercritical Fluids
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16. The Critical Point
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17. Critical Temperatures and Pressures
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18. Water
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19. 13-5 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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20. Phenomenon of Induction
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21. Instantaneous and Induced Dipoles
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22. Dipole Dipole Interactions
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23. 13-6 Hydrogen Bonding
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24. Hydrogen Bonding in HF(g)
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25. Hydrogen Bonding in Water
around a molecule in the solid in the liquid
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26. Other examples of H-Bonds
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27. 13-7 Chemical Bonds as
Intermolecular Forces
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28. Other Carbon Allotropes
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29. Interionic Forces
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30. 13-8 Crystal Structures
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31. Unit Cells in the Cubic Crystal System
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32. Holes in Crystals
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33. Hexagonal Close Packed (hcp)
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34. Coordination Number
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35. Counting Cell Occupancy
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36. X-Ray Diffraction
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37. X-Ray Diffraction
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38. Cesium Chloride
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39. Atomic Radii from Crystal Structures
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40. Sodium Chloride
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41. Holes in Crystals
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42. Prentice-Hall General Chemistry: ChapterSlide 42 of 35
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43. 13-9 Energy Changes in the Formation of
Ionic Crystals
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44. Chapter 13 Questions
1, 3, 4, 13, 24, 26, 31,
45, 52, 61, 94, 107
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