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This is because oxygen has one more electron than a half-full orbital as in nitrogen with 3 of 6 p filled. So the energy needed to remove that outlier electron on oxygen will be lower despite the normal trend of ionization energy increasing down a period.
From what I gather, it has to do with the electron configuration. Since N has half of its 2p shell filled with electrons it is more stable, whereas Oxygen has an extra electron there so it is more likely to want to lose the electron to become more stable.
This is due to an electron being added to an already half full orbital in oxygen, which results in electron-electron repulsion, which will lower the ionization energy. The 2p sublevel for N has one electron in each orbital. O has two electrons in the first orbital and one in each of the other two orbitals. There is greater electronic repulsion in the 2p sublevel for O than N. Therefore, it is easier to remove an electron from the O than the N, and the ionization energy of O is lower than N. Also N is more stable due to half-filled shells
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