Hybridization molecular orbitals and

I believe essentially all of the material in the first five chapters is accessible to the advanced general chemistry students at most universities. The final three chapters are written at a somewhat higher level on the whole. Chapter 6 introduces Schrodinger s equation and rationalizes more advanced concepts, such as hybridization, molecular orbitals, and multielectron atoms. It does the one-dimensional particle-in-a-box very thoroughly (including, for example, calculating momentum and discussing nonstation-ary states) in order to develop qualitative principles for more complex problems. 

Mixing atomic orbitals forms hybrid molecular orbitals, and the number of s- and p-orbitals used to form the hybrid determines the hybridization (sp , for example). 

In hybridization, molecular orbital, and valence bond theory, not only is energy conserved, but also the number of orbitals is conserved. For example, for an sp hybridized atom, there is still one p orbital left over and for an sp hybridized atom, there are two unhybridized p orbitals left over. Carbon readily uses the leftover p orbitals to form TT bonds (see page 482). In contrast, silicon, the element one below carbon, does not use the p orbitals as readily to form tt bonds. As we will see in Section 11-4, the formation of a 77 bond involves the side-to-side overlap of unhybridized p orbitals. An unhybridized 3p orbital of silicon does not project out far enough to form 77 bonds. 

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