00:02
Hi there.
00:03
In this question, we have an ammonia molecule, which is nh3.
00:08
And the question is about the orbitals that overlap to form an n to h bond.
00:16
Well, to answer this question, i want to first sketch out the lewis structure for ammonia.
00:23
Nitrogen is in group 5a, so it has five valence electrons, and then each hydrogen comes in, bringing one valence electron to form three single covalent bonds.
00:38
All right, so that would be our lewis structure for nh3.
00:41
Well, looking at the nitrogen first, the nitrogen has three atoms bonded to it, and it has one lone pair, giving us a total of four electron domains, or a need for four equal energy orbitals.
01:17
To form four equal energy orbitals, or four hybrid orbitals, the nitrogen is going to have to be s -p -3 hybridized because it blends 1 -s and 3 -p -p orbitals together to give a total of four equal energy orbitals.
01:45
So nitrogen has sp3 hybridization.
01:54
Hydrogen only has one electron.
01:56
It only has that 1 -s orbital...