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When drawing the Lewis structure of the ClO2+ ion, there are different possible structures. One uses double bonds for both the Cl-O bonds while another uses a double bond for one of the Cl-O bonds and a single bond for the other. Both end up with the same overall formal charge of +1. If I am not mistaken, I think that the structure with the overall formal charge closest to zero is usually considered the most stable, but how do you determine the most stable structure when both possible structures have the same value for the overall formal charge such as in this case?
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