In this demonstration, a steel nail or other metallic object is coated with a thin layer of copper using an electric current. The copper ions in solution are attracted to the polarized nail, which acts as the cathode, resulting in a visible copper coating.

1. Prepare a copper sulfate solution by dissolving copper sulfate crystals in water.
2. Place a copper strip (anode) into the solution.
3. Connect the copper strip to the positive terminal of a power supply or battery.
4. Attach a clean steel nail (cathode) or other piece of metal to the negative terminal.
5. Immerse the nail into the solution without letting it touch the copper strip.
6. Allow electricity to flow for several minutes.
7. Remove the nail and observe the copper coating that has formed on its surface.

Copper Electroplating - The Sci Guys:

Copper Electroplating Experiment - Faraday's Law of Electrolysis (Chemistry) - BeardedScienceGuy:

• Try using different metals (such as a coin or key) instead of a nail.
• Experiment with different voltages to see how plating speed and quality change.

• Wear safety goggles and gloves when handling copper sulfate solution.
• Do not ingest or touch the solution with bare skin.
• Keep electrical equipment away from water spills.
• Dispose of copper sulfate solution properly as it is toxic to the environment.

• Why does the copper deposit onto the nail instead of staying in solution? (The negatively charged nail attracts positively charged copper ions, which are reduced to solid copper.)
• What role does the copper strip play in the experiment? (It serves as the source of copper ions, gradually dissolving into the solution.)
• How does increasing the voltage affect the plating process? (It speeds up plating but may cause uneven or poor-quality coatings.)
• Why is electroplating used in jewelry and industry? (To improve appearance, provide corrosion resistance, and reduce costs by using thin coatings of valuable metals.)