Step-by-step explanation:
Reaction of zinc metal in copper sulfate solution.
![\begin{array}{ll}\text { Oxidation : } & \mathrm{Zn}(s) \rightarrow \mathrm{Zn}^(2+)(a q)+2 e^(-)\\\text {Reduction : } & \mathrm{Cu}^(2+)(a q)+2 e^(-) \rightarrow \mathrm{Cu}(s) \\\hline \text { Full Reaction : } & \mathrm{Zn}(s)+\mathrm{Cu}^(2+)(a q) \rightarrow \mathrm{Zn}^(2+)(a q)+\mathrm{Cu}(s)\end{array}]()
Zinc is listed above copper on the activity series, this means that zinc is more easily oxidized than copper. That is why copper(II) ions can act as an oxidizing agent when put into contact with zinc metal. Ions of any metal that is below zinc, such as lead or silver, would oxidize the zinc in a similar reaction.