Which is the best description of the behaviour of bromine in the reaction given below? $$ \mathrm{H}_2 \mathrm{O}+\mathrm{Br}_2 \rightarrow \mathrm{HOBr}+\mathrm{HBr} $$

In the given reaction, the oxidation number of bromine increases from 0 to +1 and decreases from 0 to -1 . Due to this reason bromine is both oxidised as well as reduced. $$ : \mathrm{H}_2 \mathrm{O}+\stackrel{0}{\mathrm{Br}_2} \longrightarrow \mathrm{HOBr}+\mathrm{HBr}^{-1} $$ Caution Some students understood that the given reaction is redox reaction, but confuse with fact that redox reaction is the reaction in both oxidation and reduction occurs.