6th Edition 12.15

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Tam To 1B
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Joined: Fri Sep 28, 2018 12:25 am

6th Edition 12.15

Postby Tam To 1B » Sun Dec 02, 2018 1:14 pm


Question 12.15 in the 6th edition asks to write the Lewis structure of each reactant, identify the Lewis acid and the Lewis base, and then write the Lewis structure of the product for the following acid-base reaction:
(b) Cl- + SO2 -->

I'm a little confused on this one, because I thought SO2 had two double bonds with a pair of lone electrons on S, however, when I check my answer in the textbook, it shows SO2 having one double bond and one single bond. Is this supposed to be right? How would the product look?

Thanks in advance. :)

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Re: 6th Edition 12.15

Postby Chem_Mod » Sun Dec 02, 2018 1:52 pm

Both you and the textbook are partially correct because both are one of the contributors for SO2. It is true that your structure would look more stable because there are no non-zero formal charges, but electrons on SO2 are actually resonating and thus diffused across the entire molecule

Refer to this YouTube video for a full explanation:

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