## HW 2F.5.

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

Yazmin Bocanegra 3L
Posts: 51
Joined: Thu Jul 25, 2019 12:17 am

### HW 2F.5.

2F.5. State the hybridization of the atom in boldface red type in each of the following molecules and ions:
a) BeCl2
b) BH3
c) BH4-
d) SiF4

How do you find the hybridization? Thank you!

Vicki Liu 2L
Posts: 101
Joined: Sat Aug 24, 2019 12:15 am

### Re: HW 2F.5.

To find the hybridization, use the fact that the number of regions of electron density around the central atom corresponds to the number of hybridized orbitals. So draw out the Lewis structures for each molecule, count the number of bonding and lone pairs, and then write out the hybridization.

For example, for BeCl2, the Lewis structure shows that there are two regions of electron density around Be. Thus, there needs to be two hybrid orbitals which corresponds to sp.

Daniel Martinez 1k
Posts: 50
Joined: Wed Sep 18, 2019 12:16 am

### Re: HW 2F.5.

In order to find hybridization, you have to count the number of regions of electron density around the central atom. It can be useful to draw out the lewis structure to see the regions of e- density. After that, you would simply write out the hybridization:

s- 1 region of electron density
sp- 2 regions of electron density
sp^3- 4 regions of electron density
sp^3d^2- 6 regions of electron density

Camille 4I
Posts: 57
Joined: Sat Aug 24, 2019 12:18 am

### Re: HW 2F.5.

To answer this question, do you have to write out the electron movement during transformation?