2F.7

[Fiona Latifi 1A]

How do you identify the hybrid orbitals used by an atom? I am able to figure out the hybridization of an atom (as in question 2F.5) but am having trouble with this question. Thanks.

[Adam Kramer 1A]

I believe the question is asking the same thing as in 2F.5. The question wants to know the hybridization orbitals, which is the same as the hybridization of the atom.

[Asia Yamada 2B]

Yes, I agree that it’s similar to 2F.5. You would go through the same process as you did before to find the hybridized orbitals.

[Ivy Tan 1E]

Hi!
An easy way to identify hybrid orbitals is by memorizing this:
2 bonds --> sp
3 bonds --> sp2
4 bonds --> sp3
5 bonds --> sp3d
6 bonds --> sp3d2
Since VSEPR disregards multiple bonds, a double or triple bond would still be considered one bond. For example, if a molecule has one single bond and one double bond, it would have 2 bonds with the hybridization sp. Hope this was helpful!!

[Faith St Amant 3D]

Exactly^! As we did in 2F.5, we should start by drawing out the Lewis structure of each compound, and then identify the regions of electron density, and then identify the hybridized orbitals present. So for part b, for example, AsF3 has a Lewis structure with 4 regions of electron density (and a trigonal pyramidal shape), so the hybridized orbitals present here would be sp^3 orbitals. Hope this helps :)