The correct order of first ionization enthalp | vedclass

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Question

(C) The electronic configurations of the elements are as follows: $C (Z=6): 1s^2 2s^2 2p^2$ $N (Z=7): 1s^2 2s^2 2p^3$ $O (Z=8): 1s^2 2s^2 2p^4$ $F (Z=

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$C < O < N < F$

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(C) The electronic configurations of the elements are as follows: $C (Z=6): 1s^2 2s^2 2p^2$ $N (Z=7): 1s^2 2s^2 2p^3$ $O (Z=8): 1s^2 2s^2 2p^4$ $F (Z=9): 1s^2 2s^2 2p^5$ Across a period,ionization enthalpy generally increases due to increasing effective nuclear charge. However,nitrogen $(N)$ has a stable half-filled $2p^3$ configuration,which makes its ionization enthalpy higher than that of oxygen $(O)$. Therefore,the correct order is $C < O < N < F$.

The correct order of first ionization enthalpy for the given four elements is:

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