1. Covalent Bonding: Orbitals (cont’d)
Chapter 10 (c)
Covalent Bonding: Orbitals (cont’d)

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3. Figure 10. 22: The structures of diamond and graphite
Figure 10.22: The structures of diamond and graphite. In each case only a small part of the entire structure is shown.

4. Figure 10.23: Partial representation of the molecular orbital energies in (a) diamond and (b) a typical metal.
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5. Figure 10.24: The p orbitals (a) perpendicular to the plane of the carbon ring system in graphite can combine to form (b) an extensive π-bonding network.
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6. Figure 10.25: Graphite consists of layers of carbon atoms.
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7. Computer-generated model of silica.
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8. Figure 10. 26: (top) The structure of quartz (empirical formula SiO2)
Figure 10.26: (top) The structure of quartz (empirical formula SiO2). Quartz contains chains of SiO4 tetrahedra (bottom) that share oxygen atoms.

9. Figure 10.27: Examples of silicate anions, all of which are based on SiO44- tetrahedra.
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10. Figure 10.28: Two-dimensional representations of (a) a quartz crystal and (b) a quartz glass.

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12. Figure 10.29: (a) A silicon crystal doped with arsenic, which has one more valence electron than silicon. (b) A silicon crystal doped with boron, which has one less electron than silicon.