For an element to undergo disproportionation reactions atleast how many nuumber of oxidant states should the elements exhbit?

Explanation

When an element undergoes disproportionation reactions ,oxidation state the element changes in the following way -
`underset("oxidation state")(Intermediate)tounderset(state)("Higher oxidation")+underset(state)("Lower oxidation")`
Example : The reaction of `CI_(2)` with cold and dilute NaOH is a disproportionation reaction.
`underset("Intermediate oxidation state")(Coverset(0)(l)_(2))+2NaOH(aq)to underset("Higher oxidation state")(NaOoverset(+1)(Cl)(aq))+underset("Lower oxidation state")(Naoverset(-1)(Cl)(aq))+H_(2)O(l)`
So an, element will be able to undergoe disproportionation reaction if ot exhibits at least oxidation states.