Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers, and students in the field of chemistry. It only takes a minute to sign up.
Sign up to join this community
In $\ce{AB5E}$-type molecules, why are the lone pairs in axial bonds?
If the lone pair is present in axial bonds it repels four other bonds. On the other hand if the lone pair is in equatorial bonds, it repels only two other bonds.
So what is the reason behind this?
Why? Because there is no other choice. Starting from the AB6 octahedral configuration, all six vertices of the octahedron are symmetric, so it doesn't matter whichever one you “choose” to replace by the lone pair. All will yield the same final configuration.
