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HW 2F.5.

Posted: Thu Nov 21, 2019 8:17 pm
by Yazmin Bocanegra 3L
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!

Re: HW 2F.5.

Posted: Thu Nov 21, 2019 8:36 pm
by Vicki Liu 2L
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.

Re: HW 2F.5.

Posted: Thu Nov 21, 2019 10:47 pm
by Daniel Martinez 1k
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

Re: HW 2F.5.

Posted: Sun Nov 24, 2019 3:33 pm
by Camille 4I
To answer this question, do you have to write out the electron movement during transformation?