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(A) To determine the shape of the molecules,we look at their hybridization and the presence of lone pairs:$1$. $SO_2$: The sulfur atom has $sp^2$ hybr

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$SO_2$

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(A) To determine the shape of the molecules,we look at their hybridization and the presence of lone pairs:$1$. $SO_2$: The sulfur atom has $sp^2$ hybridization with one lone pair. Due to the lone pair-bond pair repulsion,the molecule adopts a bent (or angular) shape.$2$. $BeBr_2$: The beryllium atom has $sp$ hybridization with no lone pairs,resulting in a linear shape.$3$. $CO_2$: The carbon atom has $sp$ hybridization with no lone pairs,resulting in a linear shape.$4$. $BF_3$: The boron atom has $sp^2$ hybridization with no lone pairs,resulting in a trigonal planar shape.Therefore,$SO_2$ is the molecule with a bent shape.

List-$I$	List-$II$
$A$. $H_3O^+$	$I$. Tetrahedral
$B$. Acetylide anion	$II$. Linear
$C$. $NH_4^+$	$III$. Pyramidal
$D$. $ClO_2^-$	$IV$. Bent

Identify a molecule having a bent shape from the following.

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Match List-$I$ with List-$II$ :

List-$I$ List-$II$

$A$. $H_3O^+$ $I$. Tetrahedral

$B$. Acetylide anion $II$. Linear

$C$. $NH_4^+$ $III$. Pyramidal

$D$. $ClO_2^-$ $IV$. Bent

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