In what form occurs silver in silver nitrate?
$Ag^+$ ion (colourless).
What happens with that ion?
It is reduced to metallic $Ag$.
What happens with metallic $Cu$ ?
It is oxidised to $Cu^{2+}$ ion (blue).
What role does $Ag^+$ play?
It is the oxidant, because it takes electrons.
What role does $Cu$ 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!
$2Ag^+$ $+$ $2e^-$ $\longrightarrow$ $2Ag$
$Cu$ $-$ $2e^-$ $\longrightarrow$ $Cu^{2+}$
$2Ag^+$ $+$ $Cu$ $\longrightarrow$ $2Ag$ $+$ $Cu^{2+}$
Complete for the ions which are not involved et annotate!
$2Ag^+$ $+$ $2NO_3^-$ $+$ $Cu$ $\longrightarrow$ $2Ag$ $+$ $Cu^{2+}$ $+$ $2NO_3^-$ Silver nitrate solution and copper produce silver and copper(II) nitrate solution.