In all examples of disproportionation I have seen, there is one particular atom whose oxidation state is both increasing and decreasing to give rise to different products
For example, on heating phosphorous acid
$$\ce{4 H3PO3 -> 3 H3PO4 + PH3}$$
the oxidation state of phosphorous changes from +3 to +5 and -3.
However, in the case of heating $\ce{KClO3}$
$$\ce{2 KClO3 -> 2 KCl + 3 O2}$$
the oxidation state of oxygen changes from -2 to 0, while that of chlorine changes from +5 to -1. So, will such a reaction be called a disproportionation since its the same molecule giving rise to two products, or will it be simply a redox reaction?