The correct order of the first ionization ent | vedclass

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Question

(A) The ionization enthalpy generally increases across a period from left to right due to an increase in effective nuclear charge. For the elements $L

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$Li < B < Be < N$

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(A) The ionization enthalpy generally increases across a period from left to right due to an increase in effective nuclear charge. For the elements $Li$,$Be$,$B$,and $N$ in the second period,the expected order is $Li However,$Be$ $(1s^2 2s^2)$ has a fully filled $2s$ orbital,and $N$ $(1s^2 2s^2 2p^3)$ has a half-filled $2p$ subshell,both of which are exceptionally stable. Due to this,$Be$ has a higher ionization enthalpy than $B$. Therefore,the correct order is $Li < B < Be < N$.

The correct order of the first ionization enthalpies of the following elements is:

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Given below are two statements:
Statement $(I)$: The first ionisation enthalpy of the elements $Na$, $Mg$, $Cl$ and $Ar$ follows the order $Na > Mg > Cl > Ar$.
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The correct order of ionisation energy of $C$,$N$,$O$,and $F$ is

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