## Problem 4.33

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

Jane Burgan 1C
Posts: 73
Joined: Fri Sep 28, 2018 12:15 am

### Problem 4.33

State the hybridization of the atom in boldface type in each
of the following molecules: (a) BeCl2 (Be boldface); (b) BH3 (B boldface); (c) BH4 (B boldface); (d) SiF4 (Si boldface).

How do you do this problem?

105114680
Posts: 60
Joined: Fri Sep 28, 2018 12:23 am

### Re: Problem 4.33

To solve problems such as this one, draw the lewis structure of the compounds and then from there you can deduce how many regions of electron density surround the atom in boldface. The total number of regions of electron density will be the hybridization of the atom. For example if there are 5 regions of electron density around the atom in boldface, the hybridization of the atom is sp3d (1 s-orbital would be used, 3 p-orbitals would be used and 1 d-orbital would be used for a total of 5). Hope this was helpful!