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(D) The second ionization enthalpy corresponds to the energy required to remove an electron from a unipositive ion $(M^+ \rightarrow M^{2+} + e^-)$.El

Vedclass · Accepted Answer

$O > F > N > C$

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(D) The second ionization enthalpy corresponds to the energy required to remove an electron from a unipositive ion $(M^+ \rightarrow M^{2+} + e^-)$.Electronic configurations of the ions are:$C^+: 1s^2 2s^2 2p^1$$N^+: 1s^2 2s^2 2p^2$$O^+: 1s^2 2s^2 2p^3$$F^+: 1s^2 2s^2 2p^4$$O^+$ has a half-filled $2p$ subshell $(2p^3)$,which is exceptionally stable.Therefore,the energy required to remove an electron from $O^+$ is higher than that for $F^+$.The general trend of ionization enthalpy increases across a period,but due to the stability of the half-filled $p$-orbital in $O^+$,the order is $O > F > N > C$.

Which of the following presents the correct order of second ionization enthalpies of $C$,$N$,$O$ and $F$?

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