Which of the following behave as Lewis acids: | vedclass

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(D) Lewis acid is defined as an electron-pair acceptor.$BF_3$ has an incomplete octet (only $6$ electrons around $B$),so it acts as a Lewis acid.$SnCl

Vedclass · Accepted Answer

$BF_3, SnCl_2, SnCl_4$

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(D) Lewis acid is defined as an electron-pair acceptor.$BF_3$ has an incomplete octet (only $6$ electrons around $B$),so it acts as a Lewis acid.$SnCl_4$ has an empty $d$-orbital and the central atom $Sn$ is in a high oxidation state $(+4)$,allowing it to accept electron pairs,thus acting as a Lewis acid.$SnCl_2$ has a lone pair on $Sn$,but it also has an empty $d$-orbital and can accept electron pairs to expand its coordination sphere,acting as a Lewis acid.Therefore,all three species $BF_3, SnCl_2,$ and $SnCl_4$ behave as Lewis acids.

Column $I$ (Molecules)	Column $II$ (Number of lone pairs on central atom)
$A. \ NH_3$	$1. \ \text{Two}$
$B. \ H_2O$	$2. \ \text{Three}$
$C. \ XeF_2$	$3. \ \text{Zero}$
$D. \ CH_4$	$4. \ \text{Four}$
	$5. \ \text{One}$

Which of the following behave as Lewis acids: $BF_3, SnCl_2, SnCl_4$?

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