Which of the following structures of ClF_3 is | vedclass

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(C) The molecule $ClF_3$ has a central $Cl$ atom with $7$ valence electrons. It forms $3$ $Cl-F$ bonds and has $2$ lone pairs,resulting in a total of

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(C) The molecule $ClF_3$ has a central $Cl$ atom with $7$ valence electrons. It forms $3$ $Cl-F$ bonds and has $2$ lone pairs,resulting in a total of $5$ electron pairs ($sp^3d$ hybridization). According to $VSEPR$ theory,to minimize repulsion,the lone pairs prefer the equatorial positions in a trigonal bipyramidal geometry. This arrangement minimizes the $90^{\circ}$ lone pair-bond pair repulsions. Therefore,the structure with both lone pairs in the equatorial positions is the most stable.

$A$. Trigonal planar	$I$. $PCl_5$
$B$. Tetrahedral	$II$. $SF_6$
$C$. Trigonal bipyramidal	$III$. $BF_3$
$D$. Octahedral	$IV$. $CCl_4$

Which of the following structures of $ClF_3$ is the most stable?

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Match the molecular geometries in List-$I$ with their corresponding molecules in List-$II$:
$A$. Trigonal planar $I$. $PCl_5$
$B$. Tetrahedral $II$. $SF_6$
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$D$. Octahedral $IV$. $CCl_4$

The correct match for $A, B, C, D$ is:

Which of the following species is non-linear?

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