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In the 2p orbital, all nitrogen's are half-filled with electrons whereas oxygen has one full orbital and two half-filled orbitals. This first full orbital in oxygen has greater electron repulsion than the first half-full orbital in nitrogen, which makes it easier to remove an electron
The half-filled p orbital is more stable than the p orbital of oxygen. It is easier for an oxygen atom to lose/gain an electron to fill up the remaining unpaired shells as it is in a more unstable form.
If you look at the electron configuration for nitrogen N, the p orbital is half filled with electrons. This is actually a more stable orbital compared to the oxygen O orbital. Therefore, N has a higher ionization energy because it will take more energy to remove an electron from a more stable orbital.
So then when it comes to ionization energy is the only exemptions nitrogen and oxygen? Are the rest of the elements still increasing in ionization energy going up and across to the right of the periodic table which is the same trend as electronegativity on the periodic table?
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