# How do you find hybridization orbitals?

The nitrogen is bonded to each hydrogen via an $s {p}^{3}$ hybridized molecular orbital. What this means is that the $2 s$ valence atomic orbital of nitrogen increases in energy level until it is degenerate (same energy) with the $2 {p}_{x}$, $2 {p}_{y}$, and $2 {p}_{z}$ valence atomic orbitals of nitrogen, and these four orbitals mix together to produce a hybridized molecular orbital.
Since there was one $2 s$ and three $2 p$ atomic orbitals, the hybridized molecular orbital is called $s {p}^{3}$. The reason why it has to hybridize its orbitals is that it has five valence electrons, two of which are in the $2 s$ orbital, while there is one valence electron in each $2 p$ orbital.
To make the three single bonds, nitrogen needs to contribute three electrons (the three hydrogens each contribute one), and so it uses two originally from the $2 s$ and one originally from one of the $2 p$ orbitals. The remaining two become the lone electron pair.