7th Edition 2E.23

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

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Henry Krasner 1C
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Joined: Fri Sep 28, 2018 12:15 am

7th Edition 2E.23

Postby Henry Krasner 1C » Thu Nov 15, 2018 2:00 pm

Why in this question when we do the Lewis Structure for these molecules, before determining the shape, are the Oxygen atoms NOT double bonded to the central atom? Is this not blatantly disregarding the formal charge?

Aurbal Popal
Posts: 63
Joined: Fri Sep 28, 2018 12:27 am

Re: 7th Edition 2E.23

Postby Aurbal Popal » Thu Nov 15, 2018 2:45 pm

According to the solutions manual, having a double bonded oxygen is acceptable as it is more stable than having a single bonded oxygen.

The formal charges with the single bonded oxygens are not disregarded though; the oxygen will have a formal charge of -1, but Sb would have a formal charge of +1, S will have +2 (it is bonded with two oxygens) , and I will have +1 charge (this is also bonded with two oxygens, but the charge of the overall molecule is -1)

This would make the molecule to have the appropriate formal charges as it will equal 0 (or -1 for c). It is just not as stable or ideal.

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