Hybridization

[Morgan Micallef 1A]

Hi! I'm pretty confused about how you determine the type of hybridization that is occurring, could someone explain?

[kiara chan]

to figure out what hybridization is occuring, you first need to figure out the shape. Once you do that, count how many electron density regions there are and that will allow you to find out the number of hybrid orbitals. Then all you need to do is match the # of hybrid orbitals to see what one(sp, sp2, sp3, dsp3, d2sp3) it is
sp = 2 e- regions
sp2 = 3 e- regions
sp3 = 4 e- regions
dsp3 = 5 e- regions
(for me to remember, i just count the # of letters to find out how many regions there are)

For example NH3 has a geometry of AX3E1 (tetrahedral) so there are 4 e- regions (since there are 3 electron pairs and 1 lone pair bonded to the central atom). Therefore, NH3 = sp3 since sp3 as seen above, has 4 e- regions.

Hope this helps!

[Ruben Adamov 1E]

The hybridization is dependent on the regions of electron density (both bonding and lone pair alike).
For example both NH3 (3 bonding and 1 lone pair) and CH4 (4 bonding pairs) have 4 regions of electron density, therefore both will have a sp3 hybridization.
Hope this helps!!!

[205769933]

Hey!

A pretty easy way of understanding hybridization is to look at the shape, as as each shape corresponds to a specific hybridized orbital as mentioned before hand. A really good practice problem to work on that attacks this in depth would be 2.45 in the textbook--it's a pretty hard problem, but with the answer sheet hopefully you'll understand why the molecule is hybridized the way it is.

[Jaipal Virdi 2I]

To determine the hybridization of a molecule, just count the areas of density. Below I have included a table to help:

Regions and their respective hybrid orbital
2 -> sp
3 -> sp2
4 -> sp3
In lecture, I don't think we went any further than this.

[Esther Kim]

You count the regions of electron densities (bonds and valence electrons) in the lewis structure to determine hybridization.
sp = 2 e- regions
sp2 = 3 e- regions
sp3 = 4 e- regions
dsp3 = 5 e- regions

[Polo Morales 3C]

You first need to count the regions of electron density (lone pairs + atoms attached). From this, one can keep in mind that 2 regions -> sp , 3 -> sp2, 4 -> sp3, etc. One must also make sure to conserve the total amount of orbitals.

[Palig Kechichian 3F]

First, count the regions of electron density, and then you have to make sure your total regains of e- density equals to total number of hybridized orbitals.