## sp3 hybridization

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

Erin Jannusch
Posts: 14
Joined: Fri Sep 29, 2017 7:07 am

### sp3 hybridization

The book says that whenever an atom in a molecule has a tetrahedral electron arrangement, it is sp3 hybridized. How do lone pairs affect this hybridization? For example would a molecule with the trigonal planar or seesaw shape also be sp3 hybridized?

Rachel Lu_dis1H
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Joined: Fri Sep 29, 2017 7:06 am
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### Re: sp3 hybridization

It's based on how many areas of electron density there are. So since trigonal planar are 3 areas of electron density it would be sp2, seesaw has 5 areas of electron density and would be sp3d

Alexander Peter 1F
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Joined: Wed Jun 28, 2017 3:00 am

### Re: sp3 hybridization

To my knowledge, having lone pairs does not change the sp3 hybridization as long as the intended shape is still tetrahedral. H2O, for example, is in a bent shape but has the electron pairs needed to attempt a tetrahedral shape, and it is sp3 hybridized.

Steven Chau 1B
Posts: 21
Joined: Fri Sep 29, 2017 7:07 am

### Re: sp3 hybridization

Lone pairs count as a region of electron density, so for the case of a seesaw structure there would be 5 region of electron density due to the 2 lone pairs and the 3 other bonds. Radicals would also count as a region of electron density!

Angel R Morales Dis1G
Posts: 50
Joined: Sat Jul 22, 2017 3:01 am

### Re: sp3 hybridization

Bonds, even if they are single/double/triple, will count as one area of electron density. Lone pairs will also count as an area of electron density. So in this case, sp3 means that the atom has 4 areas of electron density.

Thompson W 2C
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### Re: sp3 hybridization

Lone pairs do count as one area of electron density. Trigonal planar would be sp2 hybridized. Seesaw would be sp3d hybridized.

905022356
Posts: 48
Joined: Mon Oct 02, 2017 7:19 am

### Re: sp3 hybridization

Lone pairs count as an area of electron density in such way that, when hybrid orbitals are formed, each lone pain occupies one of these new orbitals. In H2O, the lone pairs each occupy one sp3 orbital. The two other sp3 orbitals form covalent bonds with the two hydrogens. This results in four sp3 orbitals for the four regions of electron density.