Final answer:
The correct option is c.
The reaction of copper metal in silver nitrate solution is an oxidation-reduction (redox) reaction, where copper is oxidized to copper ions and silver ions are reduced to silver metal.
Step-by-step explanation:
When copper metal is placed in a solution of silver nitrate, an oxidation-reduction or redox reaction occurs. This reaction can be written succinctly as:
Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s)
The silver ions (Ag+) in the solution are reduced to elemental silver (Ag), and the copper metal (Cu) is oxidized to copper ions (Cu2+). The half-reactions are:
oxidation: Cu(s) → Cu2+(aq) + 2e−
reduction: 2 × (Ag+(aq) + e− → Ag(s))
Removing the spectator ions, the nitrate ions (NO3−), gives the net ionic equation:
Cu(s) + 2 Ag+ (aq) → Cu2+ (aq) + 2 Ag(s)
This transformation of copper metal into copper ions and silver ions into silver metal is a clear indication of an oxidation-reduction reaction, where one species is being oxidized and the other reduced. The blue coloration of the solution is due to the presence of copper ions, confirming their formation during the reaction.
The complete question is given below:
copper metal is placed in a solution of silver nitrate the following reaction occurs 2AgNO3+Cu Cu(NO3)+2Ag
a. decomposition
b. neutralization
c. oxidation-reduction