Question

Predict the molecular structure and the bond angles for each of the following. (See Exercises 97 and 98.)

a. XeCl₂ b. ICl₃ c. TeF₄ d. PCl₅

Short answer

XeCl₂ is linear and bond angle is 180°

ICl₃ is T-shaped and bond angle is less than 90°

TeF₄ is see-saw and bond angle isless than 108° and 90°

PCl₅ is trigonal bipyramidal and bond angle is 108° and 90°

Step-by-step solution

Explaining the structure of XeCl2

First, draw the lewis dot structure of XeCl₂in which minimum lone pair repulsion is available.

There is three lone pair on the Xe atom at the axial position and canceling out each other affects.Therefore, it is linear in structure.

Explaining the structure of ICl3

First, draw the lewis dot structure of ICl₃in which minimum lone pair repulsion is available. There is two lone pair available on iodine atom which creates repulsion.Therefore, it is T-shaped.

 Step 3: Explaining the structure of TeF4

First, draw the lewis dot structure of TeF₄in which minimum lone pair repulsion is available. There is a lone pair available on Te which creates repulsion. Therefore, it is a see-saw.

Explaining the structure of PCl5

First, draw the lewis dot structure of PCl₅in which minimum lone pair repulsion is available. It is perfect trigonal pyramidal because there is no lone pair on central atom.