Question

What will happen when copper metal is put in zinc nitrate solution? Write the chemical reaction involved.

Answer 1

Hint: For the displacement reaction to occur, the reduction potential of the metal is considered. As the metal with lower potential will displace the metal with higher potential in accordance with the reactivity series.

Complete answer:
When copper metal is placed in the zinc nitrate solution, for the reaction to take place with the displacement of the zinc ion, $Z{{n}^{2+}}$ by the $C{{u}^{2+}}$ion, the reduction potential of the ions will be considered. The reduction potential is the tendency of the ion to accept electrons and get reduced to its metallic state.
In the zinc atom, having a stable fully-filled configuration, that is, $\left[ Ar \right]3{{d}^{10}}4{{s}^{2}}$ , its valence electrons have lower potential energy due to more shielding effect from the filled d-orbital. So, it can easily lose its electrons, getting oxidised. Thus, acting as a better reducing agent, with a negative reduction potential (-0.76 V).
Whereas, in the copper, it has lower tendency to form ions and with its ion having greater attraction for the electrons. It has a positive reduction potential (0.34 V) and acts as a better oxidising agent.
Then in the given reaction, the copper having higher reduction potential than the zinc, is less reactive and will remain in its reduced metallic state. So, no reaction will take place, as only the metal with lower reduction potential can displace the metal with higher reduction potential.

Note:
The species with negative reduction potential has tendency to get oxidised, whereas the species with positive reduction potential tends to get reduced easily, in the reactivity series.