The correct order of second I.E. of C,N,O,and | vedclass

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(D) The electronic configurations of the neutral atoms are:${}_{6}C: 1s^2 2s^2 2p^2$${}_{7}N: 1s^2 2s^2 2p^3$${}_{8}O: 1s^2 2s^2 2p^4$${}_{9}F: 1s^2 2

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$O > F > N > C$

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(D) The electronic configurations of the neutral atoms are:${}_{6}C: 1s^2 2s^2 2p^2$${}_{7}N: 1s^2 2s^2 2p^3$${}_{8}O: 1s^2 2s^2 2p^4$${}_{9}F: 1s^2 2s^2 2p^5$To find the second ionization energy $(IE_2)$,we look at the configurations of the unipositive ions $(M^+)$:$C^+: 1s^2 2s^2 2p^1$$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 provides extra stability,making its $IE_2$ the highest.Comparing the remaining ions,$F^+$ has a higher effective nuclear charge than $N^+$,and $N^+$ has a higher effective nuclear charge than $C^+$.Therefore,the correct order of second ionization enthalpy is $O > F > N > C$.

The correct order of second $I.E.$ of $C$,$N$,$O$,and $F$ is:

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