## Relation to Bond Angles

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

Samantha Man 1L
Posts: 63
Joined: Fri Sep 28, 2018 12:22 am

### Relation to Bond Angles

How is hybridization related to bond angles and how do lone pairs factor into this relationship?

Meghanhe1l
Posts: 60
Joined: Fri Sep 28, 2018 12:17 am

### Re: Relation to Bond Angles

Even though certain atomic orbitals would support the observed number of bonds in a molecule, they don’t always support the observed bond angles. For instance, in nh3, there are three unpaired electrons in nitrogen’s atomic orbitals that correctly support the three h bonds; however, these three bonds would be 90 degrees to one another, something vesper disproves because of the distortion the lone pair creates. Therefore, hybridization is necessary.

megan blatt 2B
Posts: 61
Joined: Fri Sep 28, 2018 12:28 am

### Re: Relation to Bond Angles

I had similar confusion on this topic. Can someone please explain to me why the three h bonds without hybridization would be at 90 degree angles and how hybridization changes these angles to the correct bond angles according to VESPR?

Matthew Tran 1H
Posts: 165
Joined: Fri Sep 28, 2018 12:16 am

### Re: Relation to Bond Angles

The three unpaired electrons in nitrogen are in the p orbitals, which are in the x, y, and z planes, which are 90 degrees to each other (orthogonal). Ammonia (NH3) has a tetrahedral electron density geometry, so you need 4 sp3 hybrid orbitals.