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(C) The electronic configuration of the elements are: $C (Z=6): 1s^2 2s^2 2p^2$ $N (Z=7): 1s^2 2s^2 2p^3$ $O (Z=8): 1s^2 2s^2 2p^4$ $F (Z=9): 1s^2 2s^

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Oxygen

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(C) The electronic configuration of the elements are: $C (Z=6): 1s^2 2s^2 2p^2$ $N (Z=7): 1s^2 2s^2 2p^3$ $O (Z=8): 1s^2 2s^2 2p^4$ $F (Z=9): 1s^2 2s^2 2p^5$ After the removal of the first electron,the configurations for the second ionisation are: $C^+: 1s^2 2s^2 2p^1$ $N^+: 1s^2 2s^2 2p^2$ $O^+: 1s^2 2s^2 2p^3$ $F^+: 1s^2 2s^2 2p^4$ The second ionisation potential involves removing an electron from the $2p$ orbital. Among these,$O^+$ has a half-filled $2p^3$ configuration,which is exceptionally stable. Therefore,it requires the highest energy to remove the second electron.

Which of the following elements has the highest second ionisation potential?

Similar Questions

Which one of the following is the correct order of the second ionisation potential of $Na$,$Ne$,$Mg$,and $Al$?

The incorrect statement is:

Which of the following processes requires the largest amount of energy?

The first ionization enthalpy of $Al$ is lower than that of $Mg$ because .......................

The first ionization enthalpy of the following elements are in the order:

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