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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.

List-$I$ (Electronic configuration of neutral atom where $n=2$)	List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$	$I. 2080$
$B. ns^2np^1$	$II. 899$
$C. ns^2np^3$	$III. 800$
$D. ns^2np^6$	$IV. 1402$

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

Similar Questions

Which of the following elements has the lowest ionization energy?

Ionisation energy in group $I$ elements varies in the decreasing order as:

Which of the following electronic configurations will have the highest tendency to form a univalent gaseous cation?

Match List-$I$ with List-$II$:
List-$I$ (Electronic configuration of neutral atom where $n=2$) List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$ $I. 2080$
$B. ns^2np^1$ $II. 899$
$C. ns^2np^3$ $III. 800$
$D. ns^2np^6$ $IV. 1402$

Discuss the trend of the first ionisation enthalpy in the same period and explain why it occurs.

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