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

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$B < Be < O < N$

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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?

Similar Questions

The graph shows the variation of Ionization Potential $(I.P.)$ with Atomic Number $(At. No.)$ for elements $A$ to $E$. If these elements belong to the same group in the periodic table,identify the group.

The first ionization potential $(IP)$ of $Be$ $(Z=4)$ is higher than which of the following elements?
$(a) B (Z=5)$
$(b) Mg (Z=12)$
$(c) Li (Z=3)$
$(d) Al (Z=13)$
$(e) K (Z=19)$

The energy required to remove an electron of a gaseous atom from its ground state is called

Find the incorrect comparison of second ionisation energy.

The first $I.P.$ of $Mg$ is ...... than $Al$.

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