(Polar molecules, Non-polar molecules, etc.)

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Sophie Krylova 2J
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Joined: Fri Sep 29, 2017 7:06 am


Postby Sophie Krylova 2J » Mon Nov 13, 2017 8:59 pm

In the solution of part a) there is a single bond between O and Sb, rather than a double. I understand that O is more electronegative and more likely to pull electrons to itself, rather than share, but based on the formal charge calculation double bond would be more stable. Same thing with S and O in part b). Why is that?

Sarah Rutzick 1L
Posts: 50
Joined: Tue Oct 10, 2017 7:13 am

Re: 4.23

Postby Sarah Rutzick 1L » Mon Nov 13, 2017 10:10 pm

In the answer book, there is a not with this problem that says that other Lewis structures are possible and more stable, like the ones you are talking about, but that they don't change the shape of the molecule. You're right about the double bonded structures being more stable, but I think for the sake of looking at shape in these problems, single bonds can be used.

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