A copper coin turns "silver," then "gold!”

40 minutes



  • Put on protective gloves and eyewear.
  • Conduct the experiment on the plastic tray.
  • Keep a bowl of water nearby during the experiment.
  • Remove protective gloves before lighting the candles.
General safety rules
  • Do not allow chemicals to come into contact with the eyes or mouth.
  • Keep young children, animals and those not wearing eye protection away from the experimental area.
  • Store this experimental set out of reach of children under 12 years of age.
  • Clean all equipment after use.
  • Make sure that all containers are fully closed and properly stored after use.
  • Ensure that all empty containers are disposed of properly.
  • Do not use any equipment which has not been supplied with the set or recommended in the instructions for use.
  • Do not replace foodstuffs in original container. Dispose of immediately.
General first aid information
  • In case of eye contact: Wash out eye with plenty of water, holding eye open if necessary. Seek immediate medical advice.
  • If swallowed: Wash out mouth with water, drink some fresh water. Do not induce vomiting. Seek immediate medical advice.
  • In case of inhalation: Remove person to fresh air.
  • In case of skin contact and burns: Wash affected area with plenty of water for at least 10 minutes.
  • In case of doubt, seek medical advice without delay. Take the chemical and its container with you.
  • In case of injury always seek medical advice.
Advice for supervising adults
  • The incorrect use of chemicals can cause injury and damage to health. Only carry out those experiments which are listed in the instructions.
  • This experimental set is for use only by children over 12 years.
  • Because children’s abilities vary so much, even within age groups, supervising adults should exercise discretion as to which experiments are suitable and safe for them. The instructions should enable supervisors to assess any experiment to establish its suitability for a particular child.
  • The supervising adult should discuss the warnings and safety information with the child or children before commencing the experiments. Particular attention should be paid to the safe handling of acids, alkalis and flammable liquids.
  • The area surrounding the experiment should be kept clear of any obstructions and away from the storage of food. It should be well lit and ventilated and close to a water supply. A solid table with a heat resistant top should be provided
  • Substances in non-reclosable packaging should be used up (completely) during the course of one experiment, i.e. after opening the package.

FAQ and troubleshooting

The coin didn’t become silvery. What should I do?

Wait a little longer. Double-check to make sure that the coin is resting on the zinc wire. This experiment requires direct contact between the zinc in the rod and the copper in the coin!

I poured one bottle of ZnSO4 into the candle holder, and it turned cloudy.

This can happen, but it won’t interfere with the experiment! Your coin will still turn silver.

What should I do if the zinc coating on the coin isn’t great?

Whatever you do, don’t touch the coin and the rod without gloves. There may be some pollutants on the surface of the coin. Try carefully cleaning the coin again, or just use another coin.

I left the silver coin on top of the stove for more than 10 minutes, but nothing happened.

If the coin has not changed colors at all, gently move the coin closer to the area above the flames and wait 5–15 more minutes.

The coin should turn golden after it is cooled and washed.

When removing the coin from the stove, I melted the tweezers...

Don’t worry! Just continue the experiment.

Step-by-step instructions

Put a copper Cu coin on a piece of zinc Zn wire.


Cover both metals with zinc sulfate ZnSO4 solution.


When the solution is heated, charged zinc particles—Zn2+ ions begin rapidly jumping off the wire and settling back down. Since the zinc and copper are connected, the zinc ions from ZnSO4 occasionally settle on the copper instead of the zinc. As a result, the copper coin is slowly covered with a layer of silvery metallic zinc.


If you heat the coin, the zinc and copper atoms start jiggling around and get all mixed up, producing a yellowish alloy called brass.


When you clean the coin, it almost looks like it's made of gold!


Wash the brush to repeat the experiment.


Dispose of solid waste along with household garbage. Pour solutions down the sink. Wash with an excess of water.

Scientific description

Why does the coin turn silvery?

In this experiment, we create the specific conditions that allow zinc to transition from its bound form – zinc sulfate ZnSO4 in the solution – onto the surface of the copper coin. The copper coin is completely covered by newly-formed metallic zinc Zn, causing the coin’s surface to turn silvery.

Learn more

It is well known that most metals conduct electricity well. In fact, electrical current is a flow of charged particles. The term ‘electrical conductivity’ is used to define matter’s ability to pass electrical current through itself. The electrical conductivity of metals is directly related to their atomic structure. Metals’ thermal conductivity, ductility (the ability to easily change shape while preserving integrity), and even metallic luster all result from their structural features, as does electrical conductivity.

A piece of metal can be thought of as a green field filled with fresh, dense grass and populated with ambling sheep. The sheep represent electrons, and the field represents positively-charged metal ions arranged in a certain order inside this piece of metal. However, all metals are different. For instance, compare copper’s and zinc’s crystal lattices (i.e. the order that their ions are arranged in). From the “sheep’s” (or electrons’) perspective, copper is a more pleasant “field” than zinc because the grass there is greener, tastier, and denser. Analogically, electrons are more attracted to copper ions than zinc ions. This explains an amazing phenomenon that happens when the two metals come in contact with each other: some electrons from zinc transfer into copper. No wonder: the grass is juicier there!

In our experiment, the electron transfer from zinc to copper leads to the zinc pellets acquiring a positive charge and the copper coin acquiring a negative charge. When heated, the fraction of electrons that “defect” to the copper coin only increases. However, both the copper coin and the zinc pellets are surrounded by the zinc salt ZnSO4 solution, not just by water. In the solution, this salt dissociates into ions:

ZnSO4 ↔ Zn2+ + SO42-

Now let's consider the situation from the perspective of positively-charged zinc ions. We have both the positively-charged zinc pellets and the negatively-charged copper coin. Naturally, a positively-charged object is attracted to a negatively-charged one. Therefore, the ions are happy to settle on the coin’s surface and accept the excess of electrons.


This forms additional “free lush meadows” on the coin, making the electrons from the zinc pellets even more attracted to the coin. And at a certain point, there are no longer enough electrons for all zinc atoms in the pellets, so the atoms on the surface finally turn into ions Zn2+. They may then leave to enter the solution.

Therefore, as a result of heating, the zinc atoms move from the pellets onto the coin “traveling light”: they pass through the solution in the form of ions Zn2+, and their “electronic luggage” delivers itself separately, through the metals’ surfaces.

Gradually, the zinc atoms cover the coin completely, and the coin’s color becomes exactly the same as that of the zinc pellets – all we can see on the coin’s surface is zinc!


The same result is obtained if zinc powder is dissolved in a solution of sodium hydroxide. Due to zinc’s amphoteric nature, it can react with both acids and bases. The reaction is:

Zn + 2NaOH → Na2ZnO2 + H2

As you can see from the following video, zinc plating from such a solution also works well.

Why does the coin turn from silvery to golden when heated?

Any atoms in a metal crystal lattice vibrate slightly from side to side. Under normal conditions, these vibrations do not break any bonds. The oscillation speed of metal atoms varies depending on temperature.

When heated, the atoms in any object begin to move faster. In our experiment, this manifests by the zinc atoms on the copper’s surface beginning to “sink” into the copper. These zinc atoms actually dissolve in the copper, resulting in a surface made of a mixture of copper and zinc atoms. When the coin’s surface is composed of this combination, its color becomes a blend of silvery (zinc) and reddish brown (copper), which makes it look golden.


Learn more

Let's take a roundabout approach to the subject. What is temperature? This property seems obvious enough in terms of our everyday experience: we can easily determine whether an object is cold or hot to the touch. Actually, temperature is an important parameter that reflects the speed of atoms and molecules. Particles begin to move faster when a substance is heated, and slow down when a compound is cooled.

The same thing happens with the coin in the experiment. When heated, the zinc atoms on its surface and copper atoms inside it begin to move actively. As a result, the zinc “sinks” into copper and thus permeates into the coin. Eventually, the coin’s surface comes to consist of a combination of zinc and copper atoms. When the atoms of the different metals alternate within one crystal lattice, an alloy is formed, in which one metal is dissolved in another. One such example is an alloy of copper and zinc, which is called brass.

Now, recall the structure of any metal. In our alloy, ions of zinc and copper are surrounded by a common “flock” of electrons. Thus, the color of the resulting alloy is a blend of silvery and reddish-brown, i.e. golden.

Can the coin be returned to its initial color? Or be made silvery again?

As we learned from previous discussions, the coin’s golden color is the result of a zinc-copper alloy that forms on its surface. In order to restore the original color of the coin, we need to remove the zinc atoms, leaving only copper atoms (i.e. we should clean the surface of the coin).

With a lot of effort, we could use sandpaper to remove every trace of zinc, but this would also leave many scratches. Science offers a much easier and more elegant method. Unlike copper, zinc can be easily dissolved in acids. Hence, to return the copper coin its original color, we can immerse it in hydrochloric acid HCl or vinegar, which is also acidic. This will dissolve all the zinc, leaving only copper with its redness.

However, some people prefer the intermediary silvery color over the original reddish-brown or final golden color. Unfortunately, there is no simple way to turn the coin’s color back from golden to silvery. From a chemical point of view, we would need to ensure the coin surface consists solely of silvery metal (in this case, zinc). The golden coin already has zinc on its surface; however, it would be very difficult to remove the integrated copper without affecting the zinc. Nor can we make the zinc atoms reverse and “float” back to the surface – there are no known forces that could pull them back out. However, the easiest way to turn the coin silvery is to immerse it in the zinc sulfate solution once more, along with the zinc pellets. Thus, we can use both the original and the golden coin to successfully deposit zinc atoms on the surface.