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    Sunday, July 18, 2010



    Orbital Theory

    In chemistry, molecular orbital theory (MO theory) is a method for determining molecular structure in which electrons are not assigned to individual bonds between atoms, but are treated as moving under the influence of the nuclei in the whole molecule.In this theory, each molecule has a set of molecular orbitals.

    Molecular orbital (MO) theory uses a     linear combination of atomic orbitals (LCAO) to form molecular orbitals which cover the whole molecule. These are often divided into bonding orbitals, anti-bonding orbitals, and non-bonding orbitals.

    A molecular orbital is merely a Schrödinger orbital which includes several, but often only two nuclei.

    If this orbital is of type in which the electron(s) in the orbital have a     higher probability of being between nuclei than elsewhere, the orbital will be a bonding orbital, and will tend to hold the nuclei together.

    If the electrons tend to be present in a molecular orbital in which they spend more time elsewhere than between the nuclei, the orbital will function as an anti-bonding orbital and will actually weaken the bond.

    Electrons in     non-bonding orbitals tend to be in deep orbitals (nearly atomic orbitals) associated almost entirely with one nucleus or the other, and thus they spend equal time between nuclei or not. These electrons neither contribute nor detract from bond strength.

    Molecular orbitals are further divided according to the types of atomic orbitals combining to form a bond. These orbitals are results of electron-nucleus interactions that are caused by the fundamental force of electromagnetism.

    Chemical substances will form a bond if their orbitals become lower in energy when they interact with each other. Different chemical bonds are distinguished that differ by electron cloud shape and by energy levels.

    MO theory provides a     global, delocalized perspective on chemical bonding.

    Search engines: http://en.wikipedia.org/wiki/Molecular_orbital_theory

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