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The oxidation state +2.5 is just the average oxidation state for the #S# atom.Īccording to the structure, the symmetry suggests a #-1# on each bridging sulfur ( #color(blue)(blue)#) (just like the bridging #O# atoms in a peroxide), and a #+6# ( #color(red)(red)#) on each central sulfur (like in sulfate). Group 1A elements (alkalai metals) always have an oxidation of +1. There are a set a rules that we use to determine oxidation number. The oxidation numbers also tell us how electrons move in an oxidation reduction (redox) reaction.

You need to consider the Lewis structure of this ion. The oxidation numbers tell us how electrons are divided up or shared between atoms in a chemical compound. Why the decimal place? Because the individual partial charges of the four #S# atoms are not equal to each other. Therefore, we can rewrite the equation as Let #color (red) y# be the oxidation state of #S#. The most common oxidation state of oxygen is -2. #S_4O_6^"2-"# : overall oxidation state is -2 First we need to calculate the oxidation state of #S# atom the usual way.