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One exception is for the ionization energy of group 15 and 16 elements. Although it typically increases across a row, the ionization energy of group 16 elements is actually less than group 15 elements because the half-filled orbital is more stable, and harder to remove an electron.
There is an exception to the ionization trend with Nitrogen and Oxygen. Based on periodic trends, one would think O has a higher ionization energy than N, however, due to the electron configuration of N this is not the case. N's electron configuration presents a half filled 2p orbital which is actually more stable than O's electron configuration. Since it is more stable, N will have a higher ionization energy than O because it is harder to remove an electron.
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