Opening the book…
- 13.4: Sigma Bonding with p Orbitals
- In our qualitative examination of bonding in main group diatomics, we will take the approach used in Lewis structures and just look at the valence electrons. A quantitative molecular orbital calculation with a computer would not take this shortcut, but would include all of the electrons in the atoms that are bonding together.
- 13.7: Experimental Evidence for Molecular Orbital Results
- The molecular orbital picture of dioxygen differs from the Lewis picture. Both models predict an oxygen-oxygen double bond, but one model suggests unpaired electrons whereas the other indicates an electron-paired system. Often, there is experimental evidence available to check the reliability of predictions about structure. These data include measurements of bond lengths and bond strengths as well as magnetic properties.
- 13.8: Symmetry and Mixing
- At first, we approximated and said that only orbitals of the same kind can interact with each other: s orbitals with s orbitals, p orbitals with p orbitals, and so on. One of the qualitative differences between a real MO calculation and our scrap-paper approach is that mixing does occur between different kinds of orbitals. However, restrictions still apply. Orbital interactions are governed by symmetry.
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