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    If the first ionization energy of Sulfur is lower than Phosphorus due to the repulsion of a pair of electron within the same, second 3p orbital. Why isn't it so for Aluminum and Silicon? Wouldn't the pair of electrons within the 3p orbital of Silicon cause it to require less energy to remove the first electron than that of Aluminum?

    In Si the e- are arranged singly in different orbitals, so there is little repulsion between them. In S, two e- are required to share an orbital, meaning much more repulsion between them.
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Updated: February 14, 2018
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