Bonding: General Concepts

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

Quartz grows in beautiful, regular crystals. Copyright © Houghton Mifflin Company. All rights reserved.

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. Copyright © Houghton Mifflin Company. All rights reserved.

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. Copyright © Houghton Mifflin Company. All rights reserved.

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. Copyright © Houghton Mifflin Company. All rights reserved.

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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. Copyright © Houghton Mifflin Company. All rights reserved.

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. Copyright © Houghton Mifflin Company. All rights reserved.

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. Copyright © Houghton Mifflin Company. All rights reserved.

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Figure 8.7: Sizes of ions related to positions of the elements on the periodic table. Copyright © Houghton Mifflin Company. All rights reserved.