## Hibridization

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

Valeria Viera 1B
Posts: 60
Joined: Fri Apr 06, 2018 11:05 am

### Hibridization

Can someone explain to me how to determine hybridization? What are some key things to remember?

KateCaldwell 1A
Posts: 43
Joined: Fri Apr 06, 2018 11:02 am

### Re: Hibridization

Hybridization is the mixing of orbitals into new orbitals to accommodate electrons to form new chemical bonds of the valence-bond theory. To solve for hybridization, look at the amount of electrons/atoms bonded to the central atom. For linear, there is 2 atomic orbitals as well as two hybrid orbitals, so the hybridization is sp. There’s a full table on page 125 showing all the hybridization of atoms.

Johanna Caprietta 1E
Posts: 30
Joined: Fri Apr 06, 2018 11:02 am

### Re: Hibridization

I would say for the final we need to know how to identify how many electron bonds a molecule has and memorizing what the hybridization would be.

404975170
Posts: 68
Joined: Thu Jul 27, 2017 3:00 am

### Re: Hibridization

To find hybridization you must determine the number of regions of electron density present.

A region of electron density is either a pair of lone pair electrons or a bond (every single, double and triple bonds just counts as one region). The number of regions correspond to a hybrid orbital (s, sp, sp2 etc.)
1 region - s
2 regions- sp
3 regions- sp2
4 regions- sp3
5 regions- sp3d
6 regions-sp3d2

Count the number of regions of electron density around the particular atom you are focusing on and then it’s hybridization is shown above which should be memorized.