The correct order of second ionization potent | vedclass

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Question

(C) The electronic configurations of the elements are: $C (2s^2 2p^2)$,$N (2s^2 2p^3)$,$O (2s^2 2p^4)$,$F (2s^2 2p^5)$.After the removal of the first

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$O > F > N > C$

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(C) The electronic configurations of the elements are: $C (2s^2 2p^2)$,$N (2s^2 2p^3)$,$O (2s^2 2p^4)$,$F (2s^2 2p^5)$.After the removal of the first electron,the configurations become: $C^+ (2s^2 2p^1)$,$N^+ (2s^2 2p^2)$,$O^+ (2s^2 2p^3)$,$F^+ (2s^2 2p^4)$.The second ionization potential involves removing an electron from these cations.$O^+$ has a stable half-filled $2p^3$ configuration,making it the most difficult to remove an electron from.Following the periodic trend and stability,the order of second ionization potential is $O > F > N > C$.

The correct order of second ionization potential of carbon,nitrogen,oxygen and fluorine is

Similar Questions

The incorrect statement is:

Ionization potential is lowest for

The electronic configuration of elements $A, B$ and $C$ are $[He] 2s^1, [Ne] 3s^1$ and $[Ar] 4s^1$ respectively. Which one of the following orders is correct for the first ionization potentials (in $kJ \ mol^{-1}$) of $A, B$ and $C$?

Which element has the maximum first ionization potential?

Which of the following elements has the lowest ionisation potential?

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