$$Mg_{(s)} + CuSO_{4(aq)} → MgSO_{4(aq)} + Cu_{(s)}$$

Explanation:

This reaction is a single-displacement reaction, also known as a replacement reaction. In this type of reaction, a more reactive metal replaces a less reactive metal in a compound. In this case, magnesium (Mg) is more reactive than copper (Cu), so it replaces copper in copper sulfate (CuSO4) to form magnesium sulfate (MgSO4) and copper metal (Cu).

The reaction occurs because magnesium is more easily oxidized than copper. This means that magnesium atoms are more likely to lose electrons and become positively charged ions (Mg2+). Copper ions (Cu2+), on the other hand, are more likely to gain electrons and become neutral copper atoms (Cu).

The reaction can be summarized as follows:

* Magnesium atoms lose two electrons to become magnesium ions (Mg2+).

* Copper ions gain two electrons to become copper atoms (Cu).

* Magnesium ions combine with sulfate ions (SO42-) to form magnesium sulfate (MgSO4).

The overall effect of the reaction is that magnesium replaces copper in copper sulfate, resulting in the formation of magnesium sulfate and copper metal.