sp3 hybridization


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

sp3 hybridization

Postby Erin Jannusch » Tue Dec 05, 2017 11:22 pm

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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Re: sp3 hybridization

Postby Rachel Lu_dis1H » Tue Dec 05, 2017 11:39 pm

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

Postby Alexander Peter 1F » Tue Dec 05, 2017 11:40 pm

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
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Re: sp3 hybridization

Postby Steven Chau 1B » Sat Dec 09, 2017 8:48 pm

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
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Joined: Sat Jul 22, 2017 3:01 am

Re: sp3 hybridization

Postby Angel R Morales Dis1G » Sat Dec 09, 2017 9:48 pm

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

Postby Thompson W 2C » Sun Dec 10, 2017 1:06 am

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

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

Re: sp3 hybridization

Postby 905022356 » Sun Dec 10, 2017 2:07 am

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.


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