The pair of compounds having identical shapes | vedclass

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(A) To determine the shape,we use the $VSEPR$ theory based on hybridization and lone pairs:$1$. $BeCl_2$ ($sp$ hybridization,$0$ lone pairs) is linear

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$BeCl_2, CO_2$

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(A) To determine the shape,we use the $VSEPR$ theory based on hybridization and lone pairs:$1$. $BeCl_2$ ($sp$ hybridization,$0$ lone pairs) is linear.$2$. $CO_2$ ($sp$ hybridization,$0$ lone pairs) is linear.$3$. $XeF_2$ ($sp^3d$ hybridization,$3$ lone pairs) is linear.$4$. $ICl_2^-$ ($sp^3d$ hybridization,$3$ lone pairs) is linear.Both pairs $(BeCl_2, CO_2)$ and $(XeF_2, ICl_2^-)$ have identical linear shapes. Given the standard options provided in typical chemistry problems of this type,$BeCl_2$ and $CO_2$ are the most common examples of linear molecules.

List-$I$ (Molecule)	List-$II$ (Shape)
$A. SF_4$	$I. T\text{-shaped}$
$B. ClF_3$	$II. \text{Square planar}$
$C. BrF_5$	$III. \text{See-saw}$
$D. XeF_4$	$IV. \text{Square pyramidal}$

The pair of compounds having identical shapes for their molecules is

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List-$I$ (Molecule) List-$II$ (Shape)
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