Question

Total number of planar molecule in which $d-$ orbital(s) is/are use in their bonding.
$S{O}_2,S{O}_3,Xe{F}_2,Xe{F}_4,Xe{F}_6,P{H}_3,IC{I}_4^{\ominus },PC{l}_5,I_3^{\ominus }$

Answer 1

Answer: 4

. $S{O}_2$ contains two sigma bond and one lone pair, due to which it has bent shape structure with $s{p}^2$ hybridisation.

$S{O}_3$ contains three sigma bonds and zero lone pair, due to which it has trigonal planar shape. with $s{p}^2$ hybridisation.

$Xe{F}_2$ contains two sigma bonds and three lone pair, due to which it has linear shape with $s{p}^3{d}^2$ hybridisation

$Xe{F}_4$ contains four sigma bonds and two lone pair, due to which it has square planar shape with $s{p}^3{d}^2$ hybridisation.

$Xe{F}_6$ contains six sigma bonds and one lone pair, due to which it has distorted octahedral shape with $s{p}^3{d}^3$ hybrdisation.

$P{H}_3$ contains no hybridisation but it has non-planar structure

$IC{l}_4^{-}$ contains four sigma bonds and two lone pair, due to which it has square planar shape with $s{p}^3{d}^2$ hybridisation.

$PC{l}_5$ contains five sigma bonds which means it has trigonal bipyramidal shape with $s{p}^{3}d$ hybrdisation.

$I_3^{-}$ contains two sigma bonds and three lone pairs which means it has linear shape with $s{p}^{3}d$ hybridisation.