Which of the following orders is correct for | vedclass

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(B) The second ionisation energy $(IE_{2})$ is the energy required to remove an electron from a monovalent cation. The electronic configurations of th

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$C < N < F < O$ $(2^{nd} \ I.E.)$

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(B) The second ionisation energy $(IE_{2})$ is the energy required to remove an electron from a monovalent cation. The electronic configurations of the corresponding cations are:$C^{+} (2s^{2} 2p^{1})$$N^{+} (2s^{2} 2p^{2})$$O^{+} (2s^{2} 2p^{3})$$F^{+} (2s^{2} 2p^{4})$Due to the stable half-filled $2p^{3}$ configuration of $O^{+}$,it has a higher $IE_{2}$ than $F^{+}$. The correct order of $IE_{2}$ is $C K (19) > Cl (17) > S (16)$,the $IE$ order should be $Ca^{2+} > K^{+} > Cl^{-} > S^{2-}$. Thus,option $A$ is incorrect. Re-evaluating $B$: $C^{+} (2s^{2} 2p^{1})$,$N^{+} (2s^{2} 2p^{2})$,$F^{+} (2s^{2} 2p^{4})$,$O^{+} (2s^{2} 2p^{3})$. $O^{+}$ is more stable than $F^{+}$,so $IE_{2}$ of $O > F$. The correct order is $C < N < F < O$.

Which of the following orders is correct for the property mentioned in brackets?

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The correct order of $IE_2$ (second ionization enthalpy) is:

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