$3{\mathrm{Cl}}_2+6\mathrm{NaOH}\to 5\mathrm{NaCl}+{\mathrm{NaClO}}_3+3{\mathrm{H}}_2\mathrm{O}$, chlorine gets 

From ${\mathrm{Cl}}_2\to \mathrm{NaCl}$, chlorine's oxidation number changes from $0\left({Cl}_2\right)$ to $-1\left(\mathrm{NaCl}\right)$ i.e., it gets reduced. Whereas, from ${\mathrm{Cl}}_2\to {\mathrm{NaClO}}_3$ chlorine gets oxidized. The oxidation number changes from $0\left({\mathrm{Cl}}_2\right)$ to $+1\left({\mathrm{NaClO}}_3\right)$. Hence, chlorine gets oxidized as well as reduced in the given reaction.