Hybrid orbitals in oxygen and nitrogen

Hybridization concepts can also be applied to atoms other than carbon. Here, we look at how we can understand the properties of oxygen and nitrogen compounds by considering hybrid orbitals for these atoms. 

These orbital pictures tend to get a little confusing, in that we really need to put in the elemental symbol to distinguish it from carbon, and we usually wish to show the lone pair electrons. We accordingly use a compromise representation that employs the cleaner line drawings for part of the structure and shows the all-important orbital with its lone pair of electrons. These are duly shown for ammonia and water. 

The tetrahedral geometry resultant from these sp -hybridized nitrogen and oxygen atoms is found to exist in both ammonia and water. Bond angles in 

Lone pair electrons may be used in bonding. Since they already have a complement of two electrons, bonds will need to be made to an atom that is electron deficient, e.g. a proton. Thus, the ammonium cation and the hydronium cation also share tetrahedral geometry, and each possesses a a bond formed from lone pair electrons. 

The hydronium cation still possesses a lone pair of electrons. It does not bond to a second proton for the simple reason that the cation would then be required to take on an unfavourable double positive charge. 

---