Disproportionation reaction: In this type of reaction, same elemental species gets oxidised as well as reduced.

 $\stackrel{+1}{\text{Na}}\stackrel{-1}{\text{Br}}+\stackrel{0}{{\text{Cl}}_2}\to 2\stackrel{+1}{\text{Na}}\stackrel{-1}{\text{Cl}}+\stackrel{0}{{\text{Br}}_2}-$not disproportionate,

$\left[2\mathrm{K}\stackrel{+7}{\mathrm{M}\mathrm{n}}{\mathrm{O}}_4\to {\mathrm{K}}_2\stackrel{+6}{\mathrm{Mn}}{\mathrm{O}}_4+\stackrel{+4}{\mathrm{M}\mathrm{n}}{\mathrm{O}}_2+{\mathrm{O}}_2\right]-$not disproportionate,

$2\stackrel{+7}{\mathrm{M}\mathrm{n}}{\mathrm{O}}_4^{-}+10{\mathrm{J}}^{-}+16{\mathrm{H}}^{+}\to 2\stackrel{+2}{\mathrm{M}\mathrm{n}}+\mathrm{S}{\mathrm{I}}_2+8{\mathrm{H}}_2\mathrm{O}-$not disproportionate
 

-It is disproportionate.