The first ionisation energy of oxygen is less | vedclass

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(C) The electronic configuration of nitrogen $(N)$ is $1s^2 2s^2 2p^3$,which is a stable half-filled $p$-orbital configuration.Oxygen $(O)$ has the co

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Greater inter-electron repulsion between two electrons in the same $p$-orbital counter balances the increase in effective nuclear charge on moving from nitrogen to oxygen

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(C) The electronic configuration of nitrogen $(N)$ is $1s^2 2s^2 2p^3$,which is a stable half-filled $p$-orbital configuration.Oxygen $(O)$ has the configuration $1s^2 2s^2 2p^4$.Although oxygen has a higher effective nuclear charge than nitrogen,the $2p^4$ configuration of oxygen experiences greater inter-electron repulsion between two electrons in the same $p$-orbital.This repulsion makes it easier to remove an electron from oxygen compared to the stable half-filled configuration of nitrogen,thus resulting in a lower first ionisation energy for oxygen.

The first ionisation energy of oxygen is less than that of nitrogen. Which of the following is the correct reason for this observation?

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