Of the elements N, O, and F, O has the highest and N the lowest second ionizatio

Question

Of the elements N, O, and F, O has the highest and N the lowest second ionization energy. Explain. more filled larger less smaller half-filled O would have the highest second ionization energy because the electron configuration of O^+ has a p orbital which is stable and therefore it would require energy to remove the second electron. N would have the lowest second ionization energy because the size of N^+ would be than the radius of the F^+, so the attraction between the outer electron and the nucleus would be in N^+ than in F^+ making it easier to remove the electron.

Explanation / Answer

O would have the highest second ionization energy because the electron configuration of O+ has a half-filled p orbital which is stable and therefore it would required more energy to remove the second electron. N would have lowest second ionization energy because the size of N+ would be larger than the radius of F+, so the attraction between the outer electron and the nucleus would be less in N+ than in F+ making it easier to remove the electron.

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