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(C) The first ionization enthalpy $(IE_1)$ generally increases across a period from left to right.For the given elements ($Al$,$Si$,$C$,$N$),they belo

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$N$

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(C) The first ionization enthalpy $(IE_1)$ generally increases across a period from left to right.For the given elements ($Al$,$Si$,$C$,$N$),they belong to the $2^{nd}$ and $3^{rd}$ periods.$Al$ and $Si$ are in the $3^{rd}$ period,while $C$ and $N$ are in the $2^{nd}$ period.Elements in the $2^{nd}$ period have higher ionization enthalpies than those in the $3^{rd}$ period due to smaller atomic size.Comparing $C$ and $N$ in the $2^{nd}$ period,$N$ has a higher $IE_1$ than $C$ because of its stable half-filled $p$-orbital configuration $(2s^2 2p^3)$.Therefore,the order of $IE_1$ is $Al < Si < C < N$.

List-$I$ (Electronic configuration of neutral atom where $n=2$)	List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$	$I. 2080$
$B. ns^2np^1$	$II. 899$
$C. ns^2np^3$	$III. 800$
$D. ns^2np^6$	$IV. 1402$

The element having the highest first ionization enthalpy is

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Match List-$I$ with List-$II$:
List-$I$ (Electronic configuration of neutral atom where $n=2$) List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$ $I. 2080$
$B. ns^2np^1$ $II. 899$
$C. ns^2np^3$ $III. 800$
$D. ns^2np^6$ $IV. 1402$

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