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Chapter 14
Liquids and Solids
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2. Figure 14.1: Representations of the gas, liquid, and solid states.
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Figure 14.2: Intermolecular forces exist between molecules. Bonds exist within molecules.
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Figure 14.3: (a) Interaction of two polar molecules. (b) Interaction of many dipoles in a liquid.
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5. Figure 14.4: Polar water molecules.
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6. Figure 14.4: Hydrogen bonding among water molecules.
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7. Figure 14.5: The boiling points of covalent hydrides.
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8. Figure 14.6: Atoms with spherical electron probability.
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9. 14.6: The atom on the left develops an instantaneous dipole.
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10. Figure 14.6: Instantaneous dipole on A induces a dipole on B.
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Figure 14.7: The heating/cooling curve for water heated or cooled at a constant rate.
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Figure 14.8: Both liquid water and gaseous water contain H2O molecules.
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13. Figure 14.9: Microscopic view of a liquid near its surface.
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14. Figure 14.10: Behavior of a liquid in a closed container.
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Figure 14.11: (a) Measuring vapor of a liquid by using a simple barometer (b) The water vapor pushed the mercury level down (c) Diethyl ether shows a higher vapor pressure than water.
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16. Figure 14.12: Water rapidly boiling on a stove.
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17. Figure 14.13: Bubble expands as H2O molecules enter.
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Figure 14.14: The formation of the bubble is opposed by atmospheric pressure.
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19. Figure 14.15: Sodium and chloride ions.
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20. Figure 14.17: The classes of crystalline solids.
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21. Figure 14.18: Molecular representation of diamond.
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22. Figure 14.18: Molecular representation of sodium chloride.
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23. Figure 14.18: A molecular solid.
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Figure 14.19: The packing of Cl¯ and Na+ ions in solid sodium chloride.
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Figure 14.21: A representation of part of the structure of solid phosphorus.
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26. Figure 14.22: Molecular representation of brass.
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27. Figure 14.22: Molecular representation of steel.
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