Problem 2.81

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Problem 2.81

Postby Palmquist_Sierra_2N » Wed Oct 19, 2016 10:25 pm

Ionization energies usually increase on going from left to right across the periodic table. The ionization energy for oxygen, however, is lower than that of either nitrogen or fluorine. Explain this anomaly.

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Re: Problem 2.81

Postby Jamie_Lin_3I » Thu Oct 20, 2016 9:23 am

You can find a detailed explanation for this question in section 2.10 of the textbook
If you write out the electron configuration and draw out the orbitals for oxygen, nitrogen and fluorine, you can see that nitrogen has a half-filled 2p orbital and typically a half-filled orbital or a filled orbital is more stable. You could think that oxygen would be more readily to remove the electron in the 2px orbital in order to achieve a half-filled orbital. Also, the paired electrons in oxygen actually repel each other because of their charge, giving that orbital a higher energy and hence easier to remove the electron.

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