Which of the following orders for ionization | vedclass

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Question

(B) The correct order for ionization energy is $B < Be < C < O < N$.
On moving from left to right in a period,with an increase in the ato

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$B < Be < C < O < N$

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(B) The correct order for ionization energy is $B < Be < C < O < N$.
On moving from left to right in a period,with an increase in the atomic number,the ionization enthalpy generally increases.
However,there are two main exceptions due to electronic configuration:
$(1)$ Ionization energy of $B < $ ionization energy of $Be$. This is because $Be$ $(1s^2 2s^2)$ has a fully filled $2s$ subshell,which is more stable than the $2p^1$ electron in $B$ $(1s^2 2s^2 2p^1)$.
$(2)$ Ionization energy of $O < $ ionization energy of $N$. Nitrogen $(1s^2 2s^2 2p^3)$ has a half-filled $2p$ subshell,which is extra stable. Therefore,more energy is required to remove an electron from $N$ compared to $O$ $(1s^2 2s^2 2p^4)$.

Which of the following orders for ionization energy is correct?

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