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(C) The electronic configuration of the elements are: $C (Z=6): 1s^2 2s^2 2p^2$ $N (Z=7): 1s^2 2s^2 2p^3$ $O (Z=8): 1s^2 2s^2 2p^4$ $F (Z=9): 1s^2 2s^

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Oxygen

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(C) The electronic configuration of the elements are: $C (Z=6): 1s^2 2s^2 2p^2$ $N (Z=7): 1s^2 2s^2 2p^3$ $O (Z=8): 1s^2 2s^2 2p^4$ $F (Z=9): 1s^2 2s^2 2p^5$ After the removal of the first electron,the configurations for the second ionisation are: $C^+: 1s^2 2s^2 2p^1$ $N^+: 1s^2 2s^2 2p^2$ $O^+: 1s^2 2s^2 2p^3$ $F^+: 1s^2 2s^2 2p^4$ The second ionisation potential involves removing an electron from the $2p$ orbital. Among these,$O^+$ has a half-filled $2p^3$ configuration,which is exceptionally stable. Therefore,it requires the highest energy to remove the second electron.

Which of the following elements has the highest second ionisation potential?

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