The correct order of first ionization enthalp | vedclass

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(B) The first ionization enthalpy $(IE_1)$ generally increases across a period from left to right due to an increase in effective nuclear charge.Howev

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$E < C < A < B < D$

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(B) The first ionization enthalpy $(IE_1)$ generally increases across a period from left to right due to an increase in effective nuclear charge.However, there are exceptions due to stable electronic configurations.For the given elements in the second period, the order is:$B (2s^2 2p^1) Note that $Be$ has a higher $IE_1$ than $B$ due to a fully filled $s$-orbital, and $N$ has a higher $IE_1$ than $O$ due to a half-filled $p$-orbital.Mapping the elements to their labels: $A=O, B=N, C=Be, D=F, E=B$.The order is $B < Be < O < N < F$, which corresponds to $E < C < A < B < D$.

The correct order of first ionization enthalpy values of the following elements is:
$A. O$, $B. N$, $C. Be$, $D. F$, $E. B$
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The correct order of first ionization enthalpy values of the following elements is:$A. O$, $B. N$, $C. Be$, $D. F$, $E. B$Choose the correct answer from the options given below: