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I know at the review session, the UAs explained that oxygen has a lower ionization energy than nitrogen because nitrogen has a symmetrical arrangement while oxygen does not. Are there any other cases that differ from the general trend of ionization energy increasing to the right and up the table like this one?
Online it says that the two primary exceptions are that 1) N has an ionization energy greater than O and 2) Be has an ionization energy greater than B. Those are probably the most important to remember since they are located in the first three periods of the periodic table.
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