1. Bonding: General Concepts
Chapter 8(a)
Bonding: General Concepts

2. Quartz grows in beautiful, regular crystals.
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3. Figure 8. 1: (a) The interaction of two hydrogen atoms
Figure 8.1: (a) The interaction of two hydrogen atoms. (b) Energy profile as a function of the distance between the nuclei of the hydrogen atoms.
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4. Figure 8.2: The effect of an electric field on hydrogen fluoride molecules. (a) When no electric field is present, the molecules are randomly oriented. (b) When the field is turned on, the molecules tend to line up with their negative ends toward the positive pole and their positive ends toward the negative pole.
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5. Figure 8. 3: The Pauling electronegativity values
Figure 8.3: The Pauling electronegativity values. Electronegativity generally increases across a period and decreases down a group.
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7. Figure 8. 4: (a) The charge distribution in the water molecule
Figure 8.4: (a) The charge distribution in the water molecule. (b) The water molecule in an electric field.
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8. Figure 8.5: (a) The structure and charge distribution of the ammonia molecule. The polarity of the N—H bonds occurs because nitrogen has a greater electronegativity than hydrogen. (b) The dipole moment of the ammonia molecule oriented in an electric field.
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9. Figure 8. 6: (a) The carbon dioxide molecule
Figure 8.6: (a) The carbon dioxide molecule. (b) The opposed bond polarities cancel out, and the carbon dioxide has no dipole moment.
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12. Figure 8.7: Sizes of ions related to positions of the elements on the periodic table.
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