Relation to Bond Angles


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

Relation to Bond Angles

Postby Samantha Man 1L » Mon Nov 19, 2018 6:30 pm

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

Postby Meghanhe1l » Mon Nov 19, 2018 6:48 pm

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

Postby megan blatt 2B » Mon Nov 19, 2018 7:41 pm

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

Postby Matthew Tran 1H » Mon Nov 19, 2018 8:06 pm

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.


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