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(C) complex formed by the dative bond between a Lewis acid and a Lewis base is called a Lewis acid-base adduct.In all the given cases,the Lewis acid,$

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$H_{3}N \rightarrow BCl_{3}$

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(C) complex formed by the dative bond between a Lewis acid and a Lewis base is called a Lewis acid-base adduct.In all the given cases,the Lewis acid,$BCl_{3}$,is the same.Therefore,the stability depends on the strength of the Lewis base.Among the given options,$H_{3}N \rightarrow BCl_{3}$ forms the most stable adduct because the $N$ atom in $NH_{3}$ has a lone pair and is less electronegative compared to $O$ in $H_{2}O$.This allows $NH_{3}$ to effectively donate its lone pair into the empty $p$-orbital of $B$ in $BCl_{3}$,forming a strong $p\pi - p\pi$ dative bond.In option $(A)$,$O$ is highly electronegative,which reduces its donor ability.In options $(B)$ and $(D)$,the $d\pi - p\pi$ interaction (involving $S$ or $P$) is less effective than the $p\pi - p\pi$ interaction in $NH_{3} \rightarrow BCl_{3}$.

The most stable Lewis acid-base adduct among the following is

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