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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: