## Ammonia

$sp, sp^{2}, sp^{3}, dsp^{3}, d^{2}sp^{3}$

Siddiq 1E
Posts: 106
Joined: Fri Aug 09, 2019 12:15 am

### Ammonia

So I know electrons prefer to occupy unhybridized orbitals rather than spin pair in a hybridized orbital, so I'm confused as to why NH3 is hybridized sp3 when it has 5 electrons? It has a lone pair but I don't understand how that plays into it.

Ashley Osorio
Posts: 54
Joined: Thu Jul 11, 2019 12:17 am

### Re: Ammonia

NH3 has 4 areas of electron density- three bonded regions and one region with a lone pair. Therefore, the hybridization is sp3.

Siddiq 1E
Posts: 106
Joined: Fri Aug 09, 2019 12:15 am

### Re: Ammonia

Perhaps I wasn't clear. I know why it has sp3 hybridized orbitals but my question has to do with the amount of electrons in the sp3 orbital.

charleejohnson1L
Posts: 99
Joined: Fri Aug 30, 2019 12:17 am

### Re: Ammonia

Since there are 5 valence electrons, when you hybridize the orbitals to get sp3, there will be one valence with a lone pair and three orbitals with one electron in it (that's the five valence electrons you're asking about). I hope this answers your question! :)

Siddiq 1E
Posts: 106
Joined: Fri Aug 09, 2019 12:15 am

### Re: Ammonia

charleejohnson3L wrote:Since there are 5 valence electrons, when you hybridize the orbitals to get sp3, there will be one valence with a lone pair and three orbitals with one electron in it (that's the five valence electrons you're asking about). I hope this answers your question! :)

It does thank you so much!! Does this mean that any time there's a lone pair in hybridized orbitals it'll be a spin pair?