Consider the following species: (i) ClO ^- (ii) ClO ₂^- (iii) ClO ₃^- (iv) ClO ₄^- Among them, the species that undergoes(undergo) disproportionation reactions is(are):

Step-by-step solution

The oxidation states of chlorine in the given species are: (i) ClO ^- : +1 (ii) ClO ₂^- : +3 (iii) ClO ₃^- : +5 (iv) ClO ₄^- : +7 For a species to undergo disproportionation, the element must be present in an intermediate oxidation state so that it can be simultaneously oxidized and reduced. Chlorine exhibits oxidation states ranging from -1 to +7 . Since chlorine in ClO ₄^- is in its maximum oxidation state of +7 , it cannot be further oxidized and thus does not undergo disproportionation. The species ClO ^- , ClO