Amongst the following,which one will have max | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) To determine the maximum 'lone pair - lone pair' (lp-lp) repulsions,we analyze the number of lone pairs on the central atom for each molecule:$1$.

Vedclass · Accepted Answer

$XeF_{2}$

Vedclass · Answer

(C) To determine the maximum 'lone pair - lone pair' (lp-lp) repulsions,we analyze the number of lone pairs on the central atom for each molecule:$1$. $IF_{5}$: Iodine has $7$ valence electrons. It forms $5$ bonds with $F$ atoms,leaving $1$ lone pair. Number of lp-lp repulsions = $0$.$2$. $SF_{4}$: Sulfur has $6$ valence electrons. It forms $4$ bonds with $F$ atoms,leaving $1$ lone pair. Number of lp-lp repulsions = $0$.$3$. $XeF_{2}$: Xenon has $8$ valence electrons. It forms $2$ bonds with $F$ atoms,leaving $3$ lone pairs. These $3$ lone pairs occupy the equatorial positions of the trigonal bipyramidal geometry,resulting in $3$ lp-lp repulsions at $90^\circ$ angles.$4$. $ClF_{3}$: Chlorine has $7$ valence electrons. It forms $3$ bonds with $F$ atoms,leaving $2$ lone pairs. Number of lp-lp repulsions = $1$.Comparing these,$XeF_{2}$ has the maximum number of lone pair - lone pair repulsions.

Amongst the following,which one will have maximum 'lone pair - lone pair' electron repulsions?

Similar Questions

Which of the following species contains three bond pairs and one lone pair around the central atom?

Amongst $ClF_3$,$BF_3$ and $NH_3$ molecules,the one with non-planar geometry is:

The bond angle $H-X-H$ is the greatest in the compound

The number of lone pairs of electrons on the central atom of $BrF_5, XeO_3, SO_2$ respectively are

Explain why $PCl_5$ is trigonal bipyramidal whereas $IF_5$ is square pyramidal.

Vedclass Test Series

Exam Paper Generator

Online Exam Module