The shape of the SF_2Cl_2 molecule is .... | vedclass

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(B) To determine the shape of $SF_2Cl_2$,we calculate the steric number using the formula: $Steric \ Number = \frac{1}{2} [V + M - C + A]$,where $V$ i

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Seesaw

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(B) To determine the shape of $SF_2Cl_2$,we calculate the steric number using the formula: $Steric \ Number = \frac{1}{2} [V + M - C + A]$,where $V$ is the number of valence electrons of the central atom $(S = 6)$,$M$ is the number of monovalent atoms ($F = 2, Cl = 2$,so $M = 4$),$C$ is the cationic charge $(0)$,and $A$ is the anionic charge $(0)$.$Steric \ Number = \frac{1}{2} [6 + 4] = 5$.$A$ steric number of $5$ corresponds to $sp^3d$ hybridization with a trigonal bipyramidal electron geometry.In $SF_2Cl_2$,the central sulfur atom has $5$ electron pairs ($4$ bonding pairs and $1$ lone pair).According to $VSEPR$ theory,the lone pair occupies an equatorial position to minimize repulsion.This arrangement results in a seesaw shape.

The shape of the $SF_2Cl_2$ molecule is $...$.

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