When an iron nail is placed in a solution of copper sulfate, a single displacement reaction occurs. Iron displaces copper from the solution, forming iron(II) sulfate and depositing reddish-brown copper metal on the nail while the solution’s blue color fades.

1. Fill a small beaker with copper sulfate solution.
2. Place a clean iron nail into the solution.
3. Leave the nail in the solution for several minutes.
4. Observe the reddish-brown copper coating forming on the nail (it probably won't be smooth, but copper will form).
5. Note the gradual fading of the blue color in the solution as Cu²⁺ ions are replaced by Fe²⁺ ions.

Redox Single Displacement Reaction of Copper 2 Sulfate & Iron in RamZland - RamZland:

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• Use steel wool or different forms of iron instead of an iron nail.
• Compare the displacement reactions of different metals (e.g., zinc or magnesium in copper sulfate solution).
• Measure the mass of the iron nail before and after to quantify copper deposition.

• Avoid contact of copper sulfate with eyes and wash hands after the experiment.
• Dispose of the copper sulfate solution according to local regulations; do not pour down the drain.

• Why does copper coat the iron nail? (Iron is more reactive than copper and displaces it from solution.)
• What evidence shows a chemical reaction has taken place? (Deposition of copper, fading of blue solution, formation of Fe²⁺ ions.)
• How is this reaction an example of redox? (Iron undergoes oxidation to Fe²⁺, while Cu²⁺ undergoes reduction to copper metal.)
• What role does the reactivity series play in predicting whether displacement will occur? (A more reactive metal will displace a less reactive one from its compound.)