Comment upon the statement, "Paradox of fractional oxidation numbers".

Starting with the correctly balanced half-reactions, write the overall net ionic reaction for the following:
Chloride ion is oxidised to ${\mathrm{Cl}}_2$ by $\underline{\mathrm{Mn}}{\mathrm{O}}_4^{-}$ ( in acid solution). Also, find out the change in the oxidation number of the underlined atom.

Starting with the correctly balanced half-reactions, write the overall net ionic reaction for the following change:

Nitrous acid $\left(\mathrm{H}\underline{\mathrm{N}}{\mathrm{O}}_2\right)$ reduces ${{\mathrm{MnO}}_4}^{-}$( in acid solution). Also, find out the change in the oxidation number of the underlined atom.

Starting with the correctly balanced half-reactions, write the overall net ionic reaction in the following change:

Nitrous acid $\left(\mathrm{H}\underline{\mathrm{N}}{\mathrm{O}}_2\right)$ Oxidises ${\mathrm{I}}^{-}$ to ${\mathrm{I}}_2$ (in acid solution). Also, find out the change in the oxidation number of the underlined atom.

Starting with the correctly balanced half-reactions, write the overall net ionic reaction in the following change:
Chlorate ion $\left(\underline{\mathrm{Cl}}{{\mathrm{O}}_3}^{-}\right)$ oxidises ${\mathrm{Mn}}^{2+}$to ${\mathrm{MnO}}_2$ (in acid solution). Also, find out the change in the oxidation number of the underlined atom.

Starting with the correctly balanced half-reactions, write the overall net ionic reaction in the following change:

Chromite ion $\left(\underline{\mathrm{Cr}}{{\mathrm{O}}_3}^{-}\right)$ is oxidised by ${\mathrm{H}}_2{\mathrm{O}}_2$ (in strongly basic medium). Also, find out the change in the oxidation number of the underlined atom.