A-Level Chemistry Shapes of molecules

4 bonding pairs, no lone pairs

Tetrahedral

3 bonding pairs, 1 lone pair

Trigonal Pyramidal

2 bonding pairs, 2 lone pairs

Bent planar

2 bonding pairs, no lone pairs

Linear

3 bonding pairs, no lone pairs

Trigonal planar

5 bonding pairs, no lone pairs

Trigonal bipyramidal

6 bonding pairs, no lone pairs

Octahedral

Tetrahedral bond angle

109.5°

Trigonal pyramidal bond angle

Around 107°

Bent planar bond angle

Around 104.5°

Linear bond angle

180°

Trigonal planar bond angle

120°

Trigonal bipyramidal bond angles

90° and 120°

Octahedral bond angles

90°

Electron pair repulsion theory

A theory which explains the shapes of simple molecules by assuming that pairs of electrons around a central atom repel each other and thus take up positions as far away as possible from each other in space.

3 bonding pairs, 2 lone pairs

T-shaped

4 bonding pairs, 2 lone pairs

Square planar - lone pairs go in axial positions.

2 bonding pairs, 3 lone pairs

Lone pairs go in equatorial position so linear.