When a reactive metal pushes a less reactive metal out of a solution, a chemical reaction happens. This type of reaction is called a displacement reaction.

This process relies on something called the reactivity series, which is a list that shows how metals can lose electrons and become positive ions.

Reactivity Series Example

• More Reactive Metal: Zinc (Zn)
• Less Reactive Metal: Copper (Cu)

For example, if we put zinc into a solution of copper(II) sulfate ($\text{CuSO}_4$), here’s what happens:

$\text{Zn (s)} + \text{CuSO}_4 (aq) \rightarrow \text{ZnSO}_4 (aq) + \text{Cu (s)}$

Observations

1. Color Change: The blue color of copper(II) sulfate disappears as copper ions are pushed out.
2. Solid Formation: We see a reddish-brown coating of copper forming.

Explanation

Zinc, being the more reactive metal, pushes out copper because it can lose electrons more easily. This creates zinc sulfate and solid copper from the reaction.

This idea is important to understand why we use certain metals in things like galvanization (a way to protect metals from rust) and metal extraction.

So, when a more reactive metal is involved, you can expect some interesting chemical changes!