I need help with the resonance structures of S2O2 and S2O3?

Question

I need assistance with the resonance structures of S2O2 and S2O3. Specifically, I would like to draw all possible resonance forms. It is mentioned that while sulfur can have an expanded octet, we should avoid doing so in these cases, and we should not use double-headed arrows. I understand that drawing Lewis structures on a computer can be challenging, so any tips or hints you can provide would be greatly appreciated.

Haylee Bradtke · Accepted Answer

Are you taking CHE131 in Stony Brook? Looks like one of my homework questions lol.

For S2O2 there are 3 structures, some are not stable at all but that’s what the question wants anyway:

1. O=S-S-O

2. O-S=S-O

3. O-S-S=O

I’m sure you have no problem filling in the electrons. No formal charge is needed for this question.

For S2O3 you can write the structure in many shapes, I chose to use an inverse-T, with 1 O on the top, 2 O’s on the sides and 2 S in the middle(1 S on top of another S, it forms an accurate looking inverse-T). All you have to do is to rotate the double bonds around so that every space between the atoms gets a chance to have double bond at least once.(Since the total bonds needed are 5, there must be a double bond somewhere) There are total of 4 resonance forms.

Hopefully it helps, I don’t know how to draw out the whole thing by using this typing system so this is the best I can do. Let me see if I can draw it here…

___O

___ll

___S

___l

O–S–O

___O

___l

___S

___ll

O–S–O

___O

___l

___S

___l

O=S–O

___O

___l

___S

___l

O–S=O

Don’t forget to fill in the electrons, no formal charge is needed.

I got 100 from the SmartWork HW#16 so they are the answers Stony Brook chemistry class is looking for.

Anonymous · Answer

S2o3 2 Lewis Structure

Owen Reinger III

I need help with the resonance structures of S2O2 and S2O3?

2 Answers

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