Choose the correct statement regarding SeOCl_ | vedclass

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(C) $SeOCl_2$ has a trigonal pyramidal geometry with $sp^3$ hybridization of the central $Se$ atom.$1$. The molecule has a plane of symmetry passing t

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The lone pair has greater than $33.3\% \, s-$ character.

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(C) $SeOCl_2$ has a trigonal pyramidal geometry with $sp^3$ hybridization of the central $Se$ atom.$1$. The molecule has a plane of symmetry passing through the $Se=O$ bond and bisecting the $Cl-Se-Cl$ angle.$2$. Due to the presence of a lone pair and the double bond $(Se=O)$,the $Cl-Se-Cl$ bond angle is compressed to approximately $106^\circ$,while the $Cl-Se-O$ bond angle is approximately $108^\circ$. Thus,$Cl-Se-Cl $3$. According to Bent's rule,the lone pair occupies an orbital with higher $s-$ character. In $sp^3$ hybridization,the $s-$ character is $25\%$. The lone pair in $SeOCl_2$ has more than $25\% \, s-$ character (often cited as $> 33.3\%$ in specific theoretical models for such molecules).$4$. $Se$ does not use $d-$ orbitals for hybridization in this molecule; it is $sp^3$ hybridized.

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

Choose the correct statement regarding $SeOCl_2$ molecule.

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