Question

Which one of the following compounds is having maximum 'lone pair-lone pair' electron repulsions?

• A. ClF\(_3\)
• B. IF\(_5\)
• C. SF\(_4\)
• D. XeF\(_2\)

Hint:

Lone pair-lone pair repulsion is strongest when lone pairs are in positions where they are not spread out, such as the axial positions in square pyramidal or linear geometries.

Answer 1

The Correct Option is D

Step 1: {Understanding Lone Pair-Lone Pair Repulsions}
Lone pairs on a central atom repel each other. Maximum repulsion is achieved by positioning lone pairs to minimize mutual interaction. Lone pair-lone pair repulsion intensifies with an increased number of lone pairs and specific spatial arrangements.Step 2: {Analysis of Compounds}
ClF\(_3\) exhibits 3 lone pairs and 2 bonding pairs on chlorine, resulting in a T-shaped geometry.
IF\(_5\) has 2 lone pairs and 5 bonding pairs on iodine, leading to a square pyramidal geometry.
SF\(_4\) contains 1 lone pair and 4 bonding pairs on sulfur, yielding a seesaw geometry.
XeF\(_2\) possesses 3 lone pairs and 2 bonding pairs on xenon, resulting in a linear geometry.
XeF\(_2\), with the highest number of lone pairs (3), experiences the greatest lone pair-lone pair repulsions, and thus, the maximum repulsion.Therefore, the correct answer is (D).