* Electron Configuration: Zinc has an electron configuration of [Ar] 3d¹⁰ 4s², while copper has an electron configuration of [Ar] 3d¹⁰ 4s¹. This means that zinc has two valence electrons in its outermost shell, making it easier to lose them and form positive ions. Copper, with only one valence electron, requires more energy to lose an electron.

* Electrochemical Series: The electrochemical series ranks metals based on their tendency to lose electrons and form cations. Zinc has a more negative standard electrode potential (-0.76 V) compared to copper (+0.34 V). This indicates that zinc has a greater tendency to lose electrons and is therefore more reactive.

Practical Example:

* If you put a piece of zinc metal into a solution of copper sulfate, the zinc will displace the copper ions from the solution, forming zinc sulfate and depositing copper metal on the zinc surface. This is a clear demonstration of zinc's higher reactivity.

In Summary:

Zinc's greater reactivity stems from its electron configuration, which allows it to readily lose electrons, and its more negative standard electrode potential, indicating a stronger tendency to form positive ions.