Question

Question #28bb4

Answer 1

It is always useful to draw the Lewis structure when trying to determine if a molecule has single, double, or triple bonds.

So, ammonia (`NH_3`) has a total of `8` valence electrons, `5` from `N` and `1` from each `H` atom.

Each `H` atom bonds with the `N` in a single bond - 2 electrons shared. The 3 single bonds between `N` and the `H` atoms make up for `6` of the valence electrons, the remaining `2` being set as a lone pair around the `N` atom.

A quick way to determine the type of bonds formed is to take into account the fact that `H` can only form single bonds, since it only has one orbital filled with one electron; therefore, it only requires one electron more to form a stable doublet configuration.