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3.1: Prelude to Molecular Orbital Theory

  • Page ID
    360821
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    Valence bond (VB) theory gave us a qualitative picture of chemical bonding, which was useful for predicting the shapes of molecules, bond strengths, etc. It fails to describe some bonding situations accurately because it ignores the wave nature of the electrons. Molecular orbital (MO) theory has the potential to be more quantitative. With it we can also get a picture of where the electrons are in the molecule, as shown in the image at the right. This can help us understand patterns of bonding and reactivity that are otherwise difficult to explain.

    Although MO theory in principle gives us a way to calculate the energies and wavefunctions of electrons in molecules very precisely, usually we settle for simplified models. These models do not give very accurate orbital and bond energies, but they do explain concepts such as resonance (e.g., in the ferrocene, C10H10Fe, molecule) that are hard to represent otherwise. We can get more accurate energies from MO theory using computational methods. While MO theory is more correct than VB theory and can be very accurate in predicting the properties of molecules, it is also rather complicated even for fairly simple molecules. For example, you should be able to draw the VB pictures for CO, NH3, and benzene, but we will find that these are increasingly challenging with MO theory.

     

    3.1: Prelude to Molecular Orbital Theory is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts.