A metal tree grows before your very eyes!
- Put on protective gloves and eyewear.
- Conduct the experiment on the plastic tray.
- Always follow proper safety precautions when handling batteries.
- 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.
- 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.
- 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
Try using another bottle nozzle. It should fit snugly in the bottle. And, of course, you can always ask an adult for help.
Yes, of course, you can. But be sure to take a cap from a bottle meant for liquids! Otherwise, you won’t be able to close the bottle tightly enough.
Try placing the Petri dish on a horizontal surface and shaking it gently. If that doesn't help, add 1 more drop of liquid soap.
First, try lowering the clips below the Petri dish wall.
Secondly, make sure that the solution has spread out to completely cover the base of the Petri dish leaving no empty areas. If there isn’t enough solution, add 1-2 teaspoons of water.
Don’t worry! This is probably easy to fix.
· First of all, make sure that the batteries have been properly inserted into the battery holder. If everything has been set up correctly but nothing is happening, try changing the batteries.
· Make sure that the crocodile clips are clamped to the metal, not the insulation.
· Make sure that the crocodile clips are touching the solution.
· And don’t forget to check the polarity!
Yes, everything is fine. This clip is acting as an anode in this electrochemical cell. A water decomposition reaction is producing gaseous oxygen (O2), which bubbles through the solution and makes it foamy.
If you leave the electrochemical cell working for some time, one of the clips will start to dissolve. This is an ordinary electrochemical reaction, which is neither dangerous nor impeding the experiment. However, the part of the clip immersed in the solution will gradually dissolve.
How can you repeat the experiment (or do the follow-ups) if this has happened? First, disconnect the clips from the battery block and then follow one of these two options:
Option 1: Take the clip out of the solution, wash it with water, and dry with a paper towel. Now connect the “dissolved” clip to a wire from the battery block. You can now use the undissolved clip to continue your research!
Option 2: Turn the clip around, placing the dissolved part on the outside of the Petri dish. Make sure that the “undissolved” part of the clip is immersed in the solution.
We highly recommend that you use the same brand of batteries in your devices. Batteries made by different manufacturers can have different specs (voltage, amperage, etc.). If these characteristics conflict, one of the batteries can start to overheat, which can potentially result in a battery leaking and damage to the equipment.
Carefully examine your batteries to determine their polarity and location in the battery holder.
The flat end of the cylindrical batteries is their "-".
The convex end of cylindrical batteries is their "+".
And the polarity must be indicated on the battery case or label!
There is almost always a spring on the negative side of the contact in the battery holder. You need to connect "-" of the battery with "-" of the battery holder, "+" with "+". Insert the new batteries into the battery holder, keeping the polarity in mind.
After use, immediately remove one battery from the battery holder. If the batteries don’t work, and you did everything correctly, then dispose of them in accordance with the environmental standards of your region.
First, prepare the tin chloride SnCl2 solution.
The solution will not coat the surface of the Petri dish well. To make the liquid distribute evenly, we need to decrease its surface tension by adding some liquid soap.
Place the electrodes into the solution.
Connect the electrodes to their source of electric current—the batteries.
Tin ions Sn2+ near the negatively charged electrode (the black one) will transform into metal tin Sn0. The tin will gradually form long dendrite-shaped crystals throughout the solution.
A wonderful dendrite grows from a colorless salt solution.
Please refer to local regulations when disposing of chemicals. Dispose of other solid waste with household garbage. Pour leftover solutions down the sink. Wash with an excess of water.
Batteries are basically electron pumps: they suck electrons in with their "+" and pump them out from their "-" . When such a pump is connected to a solution via "electric hoses" (i. e. wires), a variety of chemical reactions can take place: by the "-" electrode some particles will capture the electrons that are pouring out, and by the "+" electrode some particles will give their electrons away.
In our experiment, tin ions Sn2+ (i. e. tin atoms with two electrons missing) will gladly accept some electrons at the "-" wire and will turn into metallic tin . Meanwhile, the "+" electrode itself , which is made of iron, will give some of its electrons to the "+" wire , leaving some iron ions floating around . This is why the red crocodile clip will eventually dissolve if you don't disconnect it.
Why does the tin dendrite grow?
By attaching the crocodile clips to the Petri dish edges we connect the tin(II) chloride (SnCl2) solution to the batteries. Once connected, the electric current starts to flow through the solution. Near to one of the clips, a tin reduction reaction takes place:
Sn2+(solution) + 2e-→ Sn(solid)
Tin is a metal that precipitates (forms a solid) as solid, elemental tin. The tin dendrite grows in the direction that the electric current flows through the solution; from one clip towards the other.
The crocodile clips are electrical conductors, known as electrodes. A variety of types of electrode is available. It is important to learn about different types that have been invented and to understand the type we use in our experiment. Electrodes may be made of metal, graphite, or polymer material. Some of them participate in chemical reactions that occur in solution (called consumable electrodes), others are chemically inert (non-consumable electrodes).
Tin forms on one of the clips as a dendrite that grows directly towards the other clip. Why does the dendrite not appear as a sort of tin "island" near the first clip? The answer is that once a bit of tin dendrite has grown on the electrode it can also conduct electricity. Consequently, it acts as part of the electrode immersed in the solution and so each new branch of dendrite grows further into the solution.
It is important to understand that dendrites made from different metal solutions grow in diverse ways because each metal forms unique crystals with unique properties. Tin has a very special crystalline structure and forms long and thin, but strong enough, crystals.
What is electrolysis?
Electrolysis is a process by which chemical reactions are induced by an electric current. Electrolysis takes place when current flows through a solution (or a fusion) of certain substances, known as electrolytes. Electrolytes are substances that can split readily into ions in solution. For example, ammonia chloride (NH4Cl) forms two ions in aqueous solution:
NH4Cl → NH4+ + Cl-
Electrolysis provides us with a way to form new substances, which evolve from substances presented in solution under the influence of an electric current. For example, metallic copper (Cu) precipitates from coper sulfate solution (CuSO4). Such products can also be formed by secondary electrode reactions, for example, oxidation of tin(II) chloride (SnCl2) to tin(IV) (Sn4+) gives oxygen (O2), which evolves as a gas from water during electrolysis.
What is electric current? It is a flow of charged particles. These particles are electrons (electronic current) or ions (ionic current).
As the electric current flows through the wires it sets up a negative charge on one of the electrodes (clips) and a positive charge on the other. This makes the ions in the solution move between the clips. The positively charged electrode is called the anode and negatively charged particles (anions) move towards this clip. The negatively charged electrode is called the cathode and positively charged particles (cations) move towards this electrode. This is how ionic current forms in solution.
In our experiment, tin deposits on the cathode and grows into a beautiful dendrite:
Cathode-: 2Sn2+(solution) + 4e-→ 2Sn(solid)
More reactions occur at the anode. The main process is the formation of oxygen (O2):
Anode+: 2H2O – 4e- → O2 + 4H+
At the same time, a secondary reaction between the evolving oxygen and tin chloride (SnCl2) takes place:
2SnCl2 + O2 + 2H2O → 2SnO2 + 4HCl
You should note that the oxygen, which interacts with the tin, is not actually an O2 molecule. It is more like atomic oxygen — a very reactive particle that participates in this reaction. It oxidizes tin(II) (Sn2+) to tin(IV) (Sn4+). A white precipitate of tin(IV) oxide (SnO2) forms.
These are not all the reactions that occur near the anode, but there is no point making our story more complicated, so let's skip them.
Why do we use SnCl2?
We have chosen tin chloride because of some specific properties of tin. Firstly, tin crystals form thin and long structures; this is because the speed of crystal growth in one direction is faster than the speed of crystal growth in other directions. Secondly, tin is a bright, glittery, silver color, which is why the dendrite looks spectacular. Tin is also a ductile and soft metal, which decreases the chances that the dendrite will break (owing to its own weight or detachment from the clip). In fact the tin dendrite floats on the surface of the liquid. Moreover, metallic tin is inert enough to oxygen and moisture from the air, so it will not decompose during the experiment. Finally, the tin reduction reaction is fast enough to be able to watch the dendrite grow.
Can dendrites be obtained from other salt solutions?
Tin is the best for this experiment. Many metals form a precipitate as an electric current flows through a solution of their salts, but only tin provides such a spectacular dendrite. Some metals, such as lead (Pb), would flake off the clip surface, layer by layer. Other metals, such as copper (Cu) or silver (Ag), would form weak porous structures that would collapse under their own weight. Each metal has unique characteristics, which results in different crystalline lattices and, consequently, crystals with unique properties.
We have prepared some ideas so that you can continue this experiment. We advise you read them all and choose the most interesting for you.
The disappearing dendrite
Be very careful to avoid shaking the table or the Petri dish during this experiment. To succeed, the dendrite should be in contact with the clip it grew on. Make sure that the crocodile clips are attached securely to the Petri dish. It is better to grow a rather small dendrite for this follow-up — about 1/3 of the Petri dish in size.
Now, swap the clips on the battery block. To do so, disconnect them both from the battery block and then reconnect them one at a time. Watch the dendrite carefully! It will start to disappear. At the same time, a new dendrite will begin to form on the opposite side.
What happens? We have changed the polarity of our cell. Now, electric current flows through the system in the opposite direction. That is why the old dendrite starts to disappear:
Snsolid – 2e- → Sn2+solution
How can I control the growth of the tin dendrite?
It is no big deal to do this! Follow the instructions at the beginning. When the dendrite starts to grow from one of the crocodile clips, disconnect the other clip from the Petri dish wall and move it along. Ensure that the clip stays immersed in the tin chloride solution! The dendrite will try to “reach” the clip you are moving by the shortest path possible. You can also take the clip off the Petri dish wall completely to move it across the dish. Again, make sure that clip stays in contact with the solution.
Hieroglyphics: a filter paper experiment
Be sure to wear protective gloves when carrying out this experiment. Take regular filter paper (a fine coffee filter or drawing paper would work). Cut a rectangular piece (4 х 8 cm or 1.5 x 3.0 inches). If the paper you use is multilayered and can easily be separated into single layers, it is better to take a single layer. Moisten the piece of paper with the tin chloride solution thoroughly (do this in a clean Petri dish). Avoid the use of too much liquid. Take the paper out of the dish and attach two crocodile clips to it on opposite ends. Watch the paper carefully: a small tin dendrite will gradually appear inside. Try to see the “hieroglyphics” by holding the filter paper up to a light source (but make sure the clips stay connected to the paper). Remember to wear protective glasses!
How will diluting the SnCl2 solution influence the experiment?
Before you start this experiment, dilute the tin chloride solution two-fold with water. Follow the instructions thereafter.
The concentration of tin ions decreases as we dilute the solution, which causes the rate of dendrite growth to slow down. Dendrite “branches” grow less frequently and align perpendicularly to each other. Finally, all branches will be much thinner.