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Unformatted text preview: the first ionization energy increases as you go left to right, but each element varies. The reason borons first ionization energy is lower than berylliums is because the outermost electron of boron is in the 2p orbital. The reason the first ionization energy of oxygen is lower than that of nitrogen is because the electrons in nitrogen are all spinning the same direction. However, oxygen has one electron in the 2p level that is paired with another. It is repelling the electron that it is paired with more than the three outer electrons in nitrogen are, so the paired electron in oxygen is easier to remove. All of the other elements follow the normal trend of first ionization energies....
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- Fall '07