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Fiona Latifi 1A
Posts: 102
Joined: Sat Sep 14, 2019 12:16 am


Postby Fiona Latifi 1A » Sat Nov 23, 2019 7:30 pm

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
Posts: 103
Joined: Sat Aug 24, 2019 12:15 am

Re: 2F.7

Postby Adam Kramer 1A » Sat Nov 23, 2019 8:21 pm

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
Posts: 97
Joined: Wed Sep 30, 2020 9:36 pm

Re: 2F.7

Postby Asia Yamada 2B » Tue Dec 01, 2020 2:22 am

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
Posts: 95
Joined: Wed Sep 30, 2020 10:09 pm
Been upvoted: 2 times

Re: 2F.7

Postby Ivy Tan 1E » Thu Dec 03, 2020 11:21 am

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
Posts: 110
Joined: Wed Sep 30, 2020 9:54 pm
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Re: 2F.7

Postby Faith St Amant 3D » Fri Dec 04, 2020 11:31 am

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 :)

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