Which one of the following orders is correct | vedclass

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(C) The first ionisation energy $(IE)$ generally increases across a period from left to right. For the second period elements,the expected order is $L

Vedclass · Accepted Answer

$B < Be < O < N$

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(C) The first ionisation energy $(IE)$ generally increases across a period from left to right. For the second period elements,the expected order is $Li However,due to the stability of fully-filled and half-filled orbitals,the actual order for $B, Be, N,$ and $O$ is $B The lower $IE$ of $B$ $(1s^2, 2s^2 2p^1)$ compared to $Be$ $(1s^2, 2s^2)$ is because the electron is removed from a $2p$ orbital in $B$,which is easier than removing an electron from the stable,fully-filled $2s$ orbital in $Be$. The lower $IE$ of $O$ $(1s^2, 2s^2 2p^4)$ compared to $N$ $(1s^2, 2s^2 2p^3)$ is because $N$ has a stable,half-filled $2p$ subshell,making it harder to remove an electron compared to $O$.

Which one of the following orders is correct for the first ionisation energies of the elements?

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