Question

If two atoms have the same number of bonds, why would a compound with a lone pair of electrons on the central atom have smaller bond angles than a compound without a lone pair?

Lone electron pairs cause greater repulsion than bonding pairs; therefore, angles between bonding pairs are increased.
Both compounds would have the same bond angles because they have the same number of bonding electrons.
Bonding pairs of electrons cause greater repulsion than lone pairs; therefore, angles between the bonding pairs are increased.
Lone electron pairs cause greater repulsion than bonding pairs; therefore, angles between the bonding pairs are reduced.

Answer 1

For molecules that have lone pairs, the real bond angle is less than the model bond angle.

Lone pairs tend to take up more space around a central atom than bonding pairs.

Step-by-step explanation:

For molecules that have lone pairs, the real bond angle is less than the model bond angle. For molecules with no lone pairs, the real bond angle is the same as the model bond angle. This implies that lone pairs take up more space around the central atom than bonding pairs do. So, the presence of lone pairs decreases the bond angles in a molecule.

Answer 2

The correct answer is lone electron pairs causes greater repulsion than bonding pairs therefore angles between the bonding pairs are reduced.

Step-by-step explanation:

We all know that lone pair lone pair repulsion>lone pair bond pair repulsion>bond pair bond pair repulsion.

lone pair of electrons present in central atom has greater magnitude of repulsion than that without lone pair.

As a result presence of lone pair of electrons reduces the bond angle between the bonding pairs.