In what form occurs copper in copper(II) sulfate?
$Cu^{2+}$ ion (blue).
What happens with this ion?
It is reduced to metallic $Cu$.
What happens with metallic $Fe$?
It is oxidised to $Fe^{2+}$ ion (light green).
What role does $Cu^{2+}$ play?
It is the oxidant, because it takes electrons.
What role does $Fe$ play?
It is the reductant because it gives electrons away.
Write the partial equations representing the half reactions of oxidation and reduction, followed by the complete redox reaction!
$Cu^{2+}$ $+$ $2e^-$ $\longrightarrow$ $Cu$
$Fe$ $-$ $2e^-$ $\longrightarrow$ $ Fe^{2+}$
$Cu^{2+}$ $+$ $Fe$ $\longrightarrow$ $Cu$ $+$ $Fe^{2+}$
Complete for the ions which are not involved et annotate!
$Cu^{2+}$ $+$ $SO_4^{2-}$ $+$ $Fe$ $\longrightarrow$ $Cu$ $+$ $Fe^{2+}$ $+$ $SO_4^{2-}$ Copper(II) sulfate solution and iron produce copper and iron(II) sulfate solution.