Molecule Geometry

2 Electron Domains (Pairs of Electrons)

1. If you have 2 bonds and 0 lone pairs of electrons: The shape is Linear with an angle of 180°

3 Electron Domains (Pairs of Electrons)

2. If you have 3 bonds and 0 lone pairs of electrons: The shape is Trigonal Planar with an angle of 120°

3. If you have 2 bonds and 1 lone pair of electrons: The shape is Bent with an approximate angle of ~118°

4 Electron Domains (Pairs of Electrons)

4. If you have 4 bonds and 0 lone pairs of electrons: The shape is Tetrahedral with an angle of 109.5°

5. If you have 3 bonds and 1 lone pair of electrons: The shape is Trigonal Pyramidal with an approximate angle of ~107°

6. If you have 2 bonds and 2 lone pairs of electrons: The shape is Bent with an approximate angle of ~104.5°

5 Electron Domains (Pairs of Electrons)

7. If you have 5 bonds and 0 lone pairs of electrons: The shape is Trigonal Bipyramidal with angles of 90° and 120°

8. If you have 4 bonds and 1 lone pair of electrons: The shape is See-saw

9. If you have 3 bonds and 2 lone pairs of electrons: The shape is T-shaped

10. If you have 2 bonds and 3 lone pairs of electrons: The shape is Linear

6 Electron Domains (Pairs of Electrons)

11. If you have 6 bonds and 0 lone pairs of electrons: The shape is Octahedral with an angle of 90°

12. If you have 5 bonds and 1 lone pair of electrons: The shape is Square Pyramidal

13. If you have 4 bonds and 2 lone pairs of electrons: The shape is Square Planar