Both nitrogen and oxygen have electrons in th | vedclass

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(B) In oxygen $(Z=8)$,the electronic configuration is $1s^2 2s^2 2p^4$. In nitrogen $(Z=7)$,the electronic configuration is $1s^2 2s^2 2p^3$. In oxyge

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Oxygen; lower ionization enthalpy

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(B) In oxygen $(Z=8)$,the electronic configuration is $1s^2 2s^2 2p^4$. In nitrogen $(Z=7)$,the electronic configuration is $1s^2 2s^2 2p^3$. In oxygen,the $2p^4$ configuration results in greater electron-electron repulsion due to the pairing of electrons in one of the $2p$ orbitals. This increased repulsion makes it easier to remove an electron from oxygen compared to nitrogen,resulting in a lower first ionization enthalpy for oxygen compared to nitrogen.

Both nitrogen and oxygen have electrons in the $2p$ orbital. In which of these is the electron-electron repulsion greater,and what is its effect?

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