Question

Total number of planar molecule in which $d-$ orbital(s) is/are use in their bonding.
$SO_{2},SO_{3}, \, XeF_{2}, \, XeF_{4},XeF_{6},PH_{3},ICI_{4}^{\ominus},PCl_{5},I_{3}^{\ominus}$

Answer 1

. $SO_{2}$ contains two sigma bond and one lone pair, due to which it has bent shape structure with $sp^{2}$ hybridisation.

$SO_{3}$ contains three sigma bonds and zero lone pair, due to which it has trigonal planar shape. with $sp^{2}$ hybridisation.

$XeF_{2}$ contains two sigma bonds and three lone pair, due to which it has linear shape with $sp^{3}d^{2}$ hybridisation

$XeF_{4}$ contains four sigma bonds and two lone pair, due to which it has square planar shape with $sp^{3}d^{2}$ hybridisation.

$XeF_{6}$ contains six sigma bonds and one lone pair, due to which it has distorted octahedral shape with $sp^{3}d^{3}$ hybrdisation.

$PH_{3}$ contains no hybridisation but it has non-planar structure

$ICl_{4}^{-}$ contains four sigma bonds and two lone pair, due to which it has square planar shape with $sp^{3}d^{2}$ hybridisation.

$PCl_{5}$ contains five sigma bonds which means it has trigonal bipyramidal shape with $sp^{3}d$ hybrdisation.

$I_{3}^{-}$ contains two sigma bonds and three lone pairs which means it has linear shape with $sp^{3}d$ hybridisation.