Total number of species from the following which can undergo...

The compounds or ions or elements in which central atom has intermediate oxidation state undergo a disproportionation reaction.

Disproportionation reactions are the reactions in which the same element/compound gets oxidised and reduced simultaneously.

1)${Cu}^{+} \to {Cu}^{2 +} + Cu$

2) $2{H}_{2}\overset{- 1}{O}2\overset{}{\to}{H}_{2}\overset{- 2}{O} + \overset{0}{O}2$

$3 ) 3{Cl}_{2} + 6{OH}^{-} \to 5{Cl}^{-} + {{ClO}_{3}}^{-} + 3{H}_{2}O$

$4 ) 2{NO}_{2} ( g ) + 2{OH}^{-} ( aq ) \to {{NO}_{2}}^{-} ( aq ) + {H}_{2}O ( l ) + {{NO}_{3}}^{-}$

$5 ) {P}_{4} + 3{OH}^{-} + 3{H}_{2}O \to {PH}_{3} + 3{H}_{2}{{PO}_{2}}^{-}$

Here, the chlorine reactant is in oxidation state $0$, and if we look at the products, the chlorine in the Cl⁻ ion has an oxidation number of $- 1$, where it has undergone reduction. Meanwhile, the oxidation number of the chlorine in the ${{ClO}_{3}}^{-}$ ion is $+ 5$, which means it has been oxidised.

Hence, ${H}_{2}{O}_{2}, {Cu}^{+}, {Cl}_{2}, {ClO}_{3}, {P}_{4}, {NO}_{2}$ shows disproportionation reaction.