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(D) The second ionisation enthalpy involves the removal of an electron from a unipositive ion $(M^+)$. The electronic configurations of the elements a

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Oxygen

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(D) The second ionisation enthalpy involves the removal of an electron from a unipositive ion $(M^+)$. The electronic configurations of the elements after the first ionisation are as follows:$O^+: 1s^2 2s^2 2p^3$ (Half-filled stable configuration)$N^+: 1s^2 2s^2 2p^2$$P^+: 1s^2 2s^2 2p^6 3s^2 3p^2$$C^+: 1s^2 2s^2 2p^1$Among these,$O^+$ has a stable half-filled $2p^3$ configuration. Removing an electron from this stable configuration requires a significantly higher amount of energy compared to the others. Therefore,oxygen has the highest second ionisation enthalpy.

Identify the element which has the highest second ionisation enthalpy.

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