Grow red crystals out of a potassium ferricyanide solution!
- Put on protective gloves and eyewear.
- Conduct the experiment on the plastic tray.
- Observe safety precautions when working with boiling water.
- 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
Yes, this is possible. In this case, pour the solution into a Petri dish, leaving the insoluble precipitate behind.
Wait just a little longer – you’ll get your beautiful crystals in the end!
This is possibly because they were contaminated with dust or exposed to a temperature change during their formation.
But don’t be upset! You can change that. Wait until the crystals are completely formed. Dissolve the same crystals in 10 mL of boiling water and pour them back into the Petri dish. Try to protect the solution from dust and changes in temperature.
If you want to keep your crystals nice, coat them with a colorless nail polish. After the nail polish dries, store the crystals in a closed container.
In this case, drain the solution back into the plastic cup and rinse the Petri dish with water. Carefully pour the solution back into the Petri dish, this time without the sediment.
Dissolve some potassium ferricyanide K3[Fe(CN)_6] in hot water. Potassium ferricyanide dissolves much better in hot water than in cold water, so you can obtain a saturated solution much faster using heat.
Leave your K3[Fe(CN)_6] solution to cool and evaporate.
Dispose of solid waste along with household garbage.
Hot water can usually dissolve a greater quantity of a substance than cold water. As the solution gradually cools and the water evaporates from the Petri dish, the ions become crowded in the solution and therefore can’t move around as easily as before. They bump into one another and stick to each other. As more and more ions stick together, small crystals form. With time, they become bigger and, as a result, visible!
How are the crystals formed?
The formation of a crystal is a marvelous triumph of order over chaos. Just consider the amazing regularity and the uniform precision of the many small components that make up a crystal. Then think of how these many small components are all precisely incorporated in a perfect structure that we call a crystal.
Crystals can be composed of various components such as molecules (like sugar), ions (like table salt NaCl) or atoms (like diamonds C). Crystals made of metal are particularly fascinating. Yes, metallic crystals! In a metallic crystal, the metal atoms are bound together via an electron cloud shared throughout the entire crystal. Some of these crystals consist of an endless chain of metal atoms (for example, crystals of cesium or bismuth). There also exist some complex crystals that contain both ions and molecules.
The world around us is moving all the time. Yet even in this reality of constant change, crystals demonstrate fundamental stability and permanency. How is this possible?
Crystal growth can be compared to the construction of a brick house. If the bricks are simply dumped into a pile, they’ll remain a pile of bricks. However, if each brick is carefully and patiently put into place, stable and solid walls can be built. The same applies to crystals. Under the right conditions, the principal components – the “bricks” – form a strong, precise, carefully-assembled structure. It’s important to remember that, unlike real bricks, the “bricks” that form crystals can bond to each other without any additional “mortar” or other binding material.
For example, oppositely-charged ions attract one another. Thanks to the unique interlacing arrangement of these ions in a crystal, the attraction of the oppositely charged ions outweighs the repulsion of the similarly charged ions.
That’s exactly what happens in a crystal of potassium hexacyanoferrate (III) K3[Fe(CN)6].
In the first half of the 20th century, scientists discovered new technologies that allowed them to closely examine crystalline structures. This, in turn, helped them to determine the orientation of the atoms and molecules in a crystal and helped them to precisely measure the distance between them. For example, the study of potassium hexacyanoferrate (III) crystals (which we obtained in this experiment) demonstrates that each negatively-charged ion [Fe(CN)6]3– is surrounded by six positively-charged ions K+, while K+ ions are also surrounded by three or four negatively-charged ions. These ions are bound by the electrostatic attraction which keeps the crystal from crumbling into powder. Though a crystal can be crushed into fine dust, it would require a lot of work.
Why does potassium hexacyanoferrate (III) precipitate out of the solution and form a crystalline structure?
In this experiment, potassium hexacyanoferrate (III) is dissolved in a given amount of water at an elevated temperature of almost 100 oC (212 oF). As the solution slowly cools down and the water evaporates, the ions start to feel very “crowded." Some of the ions take off and leave the solution to form a crystalline precipitate.
Is it possible to dissolve the crystals and repeat the experiment?
Yes, it is possible to dissolve the crystals and repeat the experiment. The potassium hexacyanoferrate (III) crystals are soluble in water.