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

I need to draw all forms of the resonance structures. It also states that although sulfur can have an expanded octet, we should not do so in these forms and we should not have double-headed arrows either. I know it is hard to draw lewis structures on the computer, so any hints that you can give will be fine.

2 Answers

  • 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.

  • S2o3 2 Lewis Structure

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