The first ionisation energies (in kJ mol^{-1 | vedclass

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(B) The first ionisation energy is the energy required to remove the most loosely bound electron from an isolated gaseous atom.Nitrogen $(Z = 7)$ has

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$1402$

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(B) The first ionisation energy is the energy required to remove the most loosely bound electron from an isolated gaseous atom.Nitrogen $(Z = 7)$ has the electronic configuration $1s^2 2s^2 2p^3$.Due to the exactly half-filled $2p$-subshell, nitrogen exhibits extra stability, resulting in a higher first ionisation energy compared to its immediate neighbors, carbon $(1086 \ kJ \ mol^{-1})$ and oxygen $(1314 \ kJ \ mol^{-1})$.Among the given values, $1402 \ kJ \ mol^{-1}$ corresponds to nitrogen, while $1681 \ kJ \ mol^{-1}$ corresponds to fluorine, which has a higher effective nuclear charge.Thus, the correct value for nitrogen is $1402 \ kJ \ mol^{-1}$.

The first ionisation energies (in $kJ \ mol^{-1}$) of four consecutive elements of the second period are given in the options. The first ionisation energy of nitrogen is

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