Which of the following is the correct order o | vedclass

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(C) The second ionization energy corresponds to the energy required to remove an electron from a unipositive ion. The electronic configurations of the

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$C < N < F < O$

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(C) The second ionization energy corresponds to the energy required to remove an electron from a unipositive ion. The electronic configurations of the unipositive 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$As we move from left to right in a period,the ionization energy generally increases due to increasing effective nuclear charge.However,$O^+$ has a stable half-filled $2p^3$ configuration,which makes it harder to remove the second electron compared to $F^+$. Therefore,the second ionization energy of $O$ is higher than that of $F$.The correct order is $C < N < F < O$.

Which of the following is the correct order of increasing second ionization energy?

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