Question

Draw the Lewis structure for .Which of the compounds exhibit at least one bond angle that is approximately 120 degrees? Which of the compounds exhibits hybridization? Which of the compound have a square planar molecular structure? Which of the compounds are polar?

Short answer

Lewis structure of the molecules are as follows

TeCl₄

ICI₅

PCl₅

KrCl₄

XeCl₂

The compounds which have hybridization d²sp³are $TeC{l}_4,IC{l}_5,KrC{l}_4$and the bond angle is 120 degrees in$PC{l}_5,KrC{l}_4$

$PC{l}_5,KrC{l}_4$have square planner structure.

The compounds which are polar is $PC{l}_5,IC{l}_5$.

Step-by-step solution

Lewis Structure

Lewis structure of the molecules are as follows

TeCl₄

ICI₅

PCl₅

KrCl₄

XeCl₂

Type of the compounds

To find the hybridization we need to find the number of bonds formed by central with every other atom and add the lone pairs to it.

The compounds which have hybridization $d^{2}s{p}^3$are$TeC{l}_4,IC{l}_5,KrC{l}_4$and the bond angle is 120 degrees in$PC{l}_5,KrC{l}_4$

The square planar structure is for compounds having$d^{2}s{p}^3$hybridization and two lone pairs of electrons. Hence$PC{l}_5,KrC{l}_4$ have square planner structure.

The compounds which are polar is $PC{l}_5,IC{l}_5$as in others the bond moments cancel each other and hence make them non-polar.