Six bonding pairs

With six bonding pairs, the electrons move to the corners of an imaginary octahedron, with the central atom in the middle:

Sulphur (VI) fluoride ['Sulphur hexafluoride']

The bond angle is 90o

Non-bonding pairs

If some electron pairs are non-bonding, the molecule adopts a similar shape, but with one or more atoms 'missing'. The 'missing' atoms are the locations of the lone pairs.

Xenon (IV) fluoride ['Xenon tetrafluoride'] has two lone pairs and four bonding pairs. The shape is square and planar - an octahedral arrangement with two atoms missing.

Introduction

One and two bonding pairs

Three bonding pairs

Four bonding pairs

Five bonding pairs

Four bonding/lone pairs