Which of the following is the correct order o | vedclass

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(B) In a period,the ionization energy generally increases from left to right due to an increase in effective nuclear charge. For the elements $B$ (ato

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$N > C > B$

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(B) In a period,the ionization energy generally increases from left to right due to an increase in effective nuclear charge. For the elements $B$ (atomic number $5$),$C$ (atomic number $6$),and $N$ (atomic number $7$),the electronic configurations are: $B: [He] 2s^2 2p^1$ $C: [He] 2s^2 2p^2$ $N: [He] 2s^2 2p^3$ Since $N$ has a stable half-filled $2p$ subshell,it has a higher ionization energy than $C$. Thus,the correct order of first ionization energy is $N > C > B$.

Which of the following is the correct order of the first ionization energy for $B$,$C$,and $N$?

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