Orbitals and Covalent bonding.

The shared pair of electrons can be thought of as 2 overlapping orbitals with the maximum probability of finding the electron pair in the middle.

 Eg for 2 s-orbitals.

These types of bonds involving 2 electrons, one from each atom are called sigma ( or s) bonds. Otherwise known as single bonds.

If orbitals can overlap (i.e. they can occupy the same space), a bond can be formed.

E.g. a p orbital with a p orbital

or a p with an s orbital

So we can draw a 3-D representation of ethane (C₂H₆) using orbitals.

A double bond (or p bond) is caused by sideways overlap of p-orbitals.

These are met in C-C double bonds

Sometimes known as banana bonds because of their shape.

These are weaker than s-bonds and quite easy to break open.