Super chemistry and physics description of experiments. The most spectacular experiments with household chemicals

Who loved at school laboratory works in chemistry? It is interesting, after all, it was to mix something with something and get a new substance. True, it didn’t always work out the way it was described in the textbook, but no one suffered about this, did they? The main thing is that something happens, and we saw it right in front of us.

If in real life if you are not a chemist and do not face much more complex experiments every day at work, then these experiments that can be carried out at home will definitely amuse you, at least.

lava lamp

For experience you need:
– Transparent bottle or vase
— Water
- Sunflower oil
- Food coloring
- Several effervescent tablets "Suprastin"

Mix water with food coloring sunflower oil. You don't need to mix, and you won't be able to. When will it be visible clear line between water and oil, we throw a couple of Suprastin tablets into the container. Watching lava flows.

Since the density of oil is lower than that of water, it remains on the surface, with an effervescent tablet creating bubbles that carry water to the surface.

Elephant Toothpaste

For experience you need:
- Bottle
- small cup
— Water
- dish detergent or liquid soap
- Hydrogen peroxide
- Fast acting nutritional yeast
- Food coloring

Mix liquid soap, hydrogen peroxide and food coloring in a bottle. In a separate cup, dilute the yeast with water and pour the resulting mixture into a bottle. We look at the eruption.

Yeast releases oxygen, which reacts with hydrogen and is pushed out. Due to the soap suds, a dense mass erupts from the bottle.

Hot Ice

For experience you need:
- container for heating
- Clear glass cup
- Plate
- 200 g baking soda
— 200 ml acetic acid or 150 ml of its concentrate
- crystallized salt

We mix acetic acid and soda in a saucepan, wait until the mixture stops sizzling. We turn on the stove and evaporate excess moisture until an oily film appears on the surface. The resulting solution is poured into a clean container and cooled to room temperature. Then add a crystal of soda and watch how the water “freezes” and the container becomes hot.

Heated and mixed vinegar and soda form sodium acetate, which, when melted, becomes an aqueous solution of sodium acetate. When salt is added to it, it begins to crystallize and release heat.

rainbow in milk

For experience you need:
- Milk
- Plate
- Liquid food coloring in several colors
- cotton swab
— Detergent

Pour milk into a plate, drip dyes in several places. Wet a cotton swab in detergent, dip into a bowl of milk. Let's see the rainbow.

In the liquid part there is a suspension of droplets of fat, which, when in contact with the detergent, split and rush from the inserted stick in all directions. A regular circle is formed due to surface tension.

Smoke without fire

For experience you need:
– Hydroperite
— Analgin
- Mortar and pestle (can be replaced with a ceramic cup and spoon)

The experiment is best done in a well-ventilated area.
We grind hydroperite tablets to a powder, we do the same with analgin. We mix the resulting powders, wait a bit, see what happens.

During the reaction, hydrogen sulfide, water and oxygen are formed. This leads to partial hydrolysis with the elimination of methylamine, which interacts with hydrogen sulfide, a suspension of its small crystals which resembles smoke.

pharaoh snake

For experience you need:
- Calcium gluconate
- Dry fuel
- Matches or lighter

We put several tablets of calcium gluconate on dry fuel, set fire to it. Let's look at the snakes.

Calcium gluconate decomposes when heated, which leads to an increase in the volume of the mixture.

non-newtonian fluid

For experience you need:

- mixing bowl
- 200 g corn starch
- 400 ml of water

Gradually add water to the starch and stir. Try to make the mixture homogeneous. Now try to roll the ball out of the resulting mass and hold it.

The so-called non-Newtonian fluid during rapid interaction behaves as solid, and when slow - like a liquid.

Home chemists-scientists believe that the most useful property detergents is the content of surfactants (surfactants). Surfactants significantly reduce the electrostatic voltage between the particles of substances and break down conglomerates. This feature makes it easier to clean clothes. In this article, chemical reactions that you can repeat with household chemicals, because with the help of surfactants you can not only remove dirt, but also conduct spectacular experiments.

Experience one: a foamy volcano in a jar

It is very easy to carry out this interesting experiment at home. For him you will need:

hydroperite, or (the higher the concentration of the solution, the more intense the reaction and the more effective the eruption of the "volcano"; therefore, it is better to buy tablets at a pharmacy and dilute them in a small volume in a ratio of 1/1 immediately before use (you will get a 50% solution - this is an excellent concentration);

gel detergent for dishes (prepare approximately 50 ml of an aqueous solution);

dye.

Now you need to get an effective catalyst - ammonia. Carefully and drop by drop add the ammonia liquid until completely dissolved.

copper sulfate crystals

Consider the formula:

CuSO₄ + 6NH₃ + 2H₂O = (OH)₂ (copper ammonia) + (NH₄)₂SO₄

Peroxide decomposition reaction:

2H₂O₂ → 2H₂O + O₂

We make a volcano: mix ammonia with a washing solution in a jar or wide-necked flask. Then quickly pour in the hydroperite solution. The "eruption" can be very strong - for safety reasons, it is better to substitute some kind of container under the volcano flask.

Experience two: the reaction of acid and sodium salts

Perhaps this is the most familiar connection that is in every home - this is baking soda. It reacts with acid, and the result is new salt, water and carbon dioxide. The latter can be detected by hissing and bubbles at the reaction site.

Experience three: "floating" soap bubbles

This is a very simple experience with baking soda. You will need:

• aquarium with a wide bottom;
• baking soda (150-200 grams);
• (6-9% solution);
• soap bubbles (to make your own, mix water, dish soap and glycerin)

On the bottom of the aquarium you need to evenly sprinkle soda and pour it with acetic acid. The result is carbon dioxide. It is heavier than air and therefore settles at the bottom of the glass box. To determine if there is CO₂ there, lower a lit match to the bottom - it will instantly go out in carbon dioxide.

NaHCO₃ + CH₃COOH → CH₃COONa + H₂O + CO₂

Now you need to blow bubbles into the container. They will slowly move along a horizontal line (the boundary of contact between carbon dioxide and air invisible to the eye, as if swimming in an aquarium).

Experience four: the reaction of soda and acid 2.0

For experience you will need:

• different types of non-hygroscopic food products(e.g. gummies).
• a glass of diluted baking soda (one tablespoon);
• a glass with a solution of acetic or any other available acid (malic,).

Cut pieces of marmalade with a sharp knife into strips 1-3 cm long and place for processing in a glass with soda solution. Wait 10 minutes and then transfer the pieces to another beaker (with an acid solution).

Ribbons will be overgrown with bubbles of the resulting carbon dioxide and float to the top. On the surface, the bubbles will disappear, the lifting force of the gas will disappear, and the marmalade ribbons will sink, again overgrown with bubbles, and so on until the reagents in the container run out.

Experience five: properties of alkali and litmus paper

Most detergents contain sodium hydroxide, the most common alkali. It is possible to reveal its presence in a solution of a detergent in this elementary experiment. At home, a young enthusiast can easily conduct it on his own:

• take a strip of litmus paper;
• dissolve some liquid soap in water;
• dip the litmus into the soapy liquid;
• wait for the indicator to color Blue colour, which will indicate alkaline reaction solution.

Click to find out what other experiments to determine the acidity of the environment can be carried out from improvised substances.

Experience six: colored explosions-stains in milk

The experience is based on the properties of the interaction of fats and surfactants. Fat molecules have a special, dual, structure: hydrophilic (interacting, dissociating with water) and hydrophobic (water-insoluble "tail" of a polyatomic compound) end of the molecule.

1. Pour milk into a wide container of small depth (“canvas”, on which a color explosion will be visible). Milk is a suspension, a suspension of fatty molecules in water.
2. With a pipette, add a few drops of water-soluble liquid dye to the milk container. You can add different dyes to different places of the container and make a multi-color explosion.
3. Then you need to moisten a cotton swab in liquid detergent and touch the surface of the milk. The white "canvas" of milk turns into a moving palette with paints that move in the liquid like spirals and twist into bizarre curves.

This phenomenon is based on the ability of surfactants to fragment (divide into sections) a film of fat molecules on the surface of a liquid. Fat molecules, repelled by their hydrophobic "tails", migrate in the milk suspension, and with them the partially undissolved paint.

Chemical experience of bromine with aluminum

If a few milliliters of bromine are placed in a test tube made of heat-resistant glass and a piece of aluminum foil is carefully lowered into it, then after a while (necessary for bromine to penetrate through the oxide film), a violent reaction will begin. From the heat released, aluminum melts and, in the form of a small fireball, rolls over the surface of bromine (the density of liquid aluminum is less than the density of bromine), rapidly decreasing in size. The test tube is filled with bromine vapor and white smoke, consisting of the smallest crystals of aluminum bromide:

2Al+3Br 2 → 2AlBr 3 .

It is also interesting to observe the reaction of aluminum with iodine. Mix in a porcelain cup a small amount of powdered iodine with aluminum powder. While the reaction is not noticeable: in the absence of water, it proceeds extremely slowly. Using a long pipette, drop a few drops of water on the mixture, which plays the role of an initiator, and the reaction will proceed vigorously - with the formation of a flame and the release of purple vapors of iodine.

Chemical experiments with gunpowder: how gunpowder explodes!

Gunpowder

Smoky, or black, gunpowder is a mixture of potassium nitrate (potassium nitrate - KNO 3), sulfur (S) and coal (C). It ignites at a temperature of about 300 °C. Gunpowder can also explode on impact. It consists of an oxidizing agent (nitrate) and a reducing agent (charcoal). Sulfur is also a reducing agent, but its main function is to bind potassium into a strong compound. During the combustion of gunpowder, the following reaction occurs:

2KNO 3 + ЗС + S → K 2 S + N 2 + 3СО 2,
- as a result of which a large volume is released gaseous substances. The use of gunpowder in military affairs is connected with this: the gases formed during the explosion and expanding from the heat of the reaction push the bullet out of the gun barrel. It is easy to verify the formation of potassium sulfide by smelling the barrel of a gun. It smells of hydrogen sulfide - a product of the hydrolysis of potassium sulfide.

Chemical experiments with saltpeter: fiery inscription

Spectacular chemical experience can be done with potassium nitrate. Let me remind you that nitrates are complex substances - salts of nitric acid. AT this case we need potassium nitrate. Its chemical formula is KNO 3 . On a sheet of paper, draw a contour, a drawing (for greater effect, let the lines do not intersect!). Prepare a concentrated solution of potassium nitrate. For information: in 15 ml hot water 20 g of KNO 3 are dissolved. Then, using a brush, we impregnate the paper along the drawn contour, while leaving no gaps or gaps. let the paper dry. Now you need to touch a burning splinter to some point on the contour. Immediately a "spark" will appear, which will slowly move along the contour of the picture until it closes it completely. Here's what happens: Potassium nitrate decomposes according to the equation:

2KNO 3 → 2 KNO 2 + O 2 .

Here KNO 2 +O 2 is a salt of nitrous acid. From the released oxygen, the paper chars and burns. For greater effect, the experiment can be carried out in a dark room.

Chemical experience of dissolving glass in hydrofluoric acid

Glass dissolves
in hydrofluoric acid

Indeed, glass dissolves easily. Glass is a very viscous liquid. The fact that glass can dissolve can be verified by performing the following chemical reaction. Hydrofluoric acid is an acid formed by dissolving hydrogen fluoride (HF) in water. It is also called hydrofluoric acid. For greater clarity, let's take a thin speckle, on which we attach a weight. We lower the glass with a weight into the solution hydrofluoric acid. When the glass dissolves in the acid, the weight will fall to the bottom of the flask.

Chemical experiments with smoke emission

Chemical reactions with
smoke emission
(ammonium chloride)

Let's do a beautiful experiment to get thick white smoke. To do this, we need to prepare a mixture of potash (potassium carbonate K 2 CO 3) with an ammonia solution (ammonia). Mix the reagents: potash and ammonia. Add a solution of hydrochloric acid to the resulting mixture. The reaction will begin already at the moment when the flask with hydrochloric acid is brought close to the flask containing ammonia. Carefully add hydrochloric acid to the ammonia solution and observe the formation of a thick white vapor of ammonium chloride, the chemical formula of which is NH 4 Cl. The chemical reaction between ammonia and hydrochloric acid proceeds as follows:

HCl + NH 3 → NH 4 Cl

Chemical experiments: the glow of solutions

Glow reaction solution

As noted above, the glow of solutions is a sign chemical reaction. Let's conduct another spectacular experiment, in which our solution will glow. For the reaction, we need a solution of luminol, a solution of hydrogen peroxide H 2 O 2 and crystals of red blood salt K 3. Luminol- a complex organic substance, the formula of which is C 8 H 7 N 3 O 2. Luminol is highly soluble in some organic solvents while not soluble in water. The glow occurs when luminol reacts with some oxidizing agents in an alkaline medium.

So, let's start: add a solution of hydrogen peroxide to luminol, then add a handful of red blood salt crystals to the resulting solution. For greater effect, try experimenting with dark room! As soon as the blood red salt crystals touch the solution, a cold blue glow will immediately be noticeable, which indicates the course of the reaction. The glow in a chemical reaction is called chemiluminescence

Another chemical experience with luminous solutions:

For it, we need: hydroquinone (formerly used in photographic equipment), potassium carbonate K 2 CO 3 (also known as "potash"), pharmacy solution of formalin (formaldehyde) and hydrogen peroxide. Dissolve 1 g of hydroquinone and 5 g of potassium carbonate K 2 CO 3 in 40 ml of pharmacy formalin (formaldehyde aqueous solution). Pour this reaction mixture into a large flask or bottle with a capacity of at least one liter. In a small vessel, prepare 15 ml of concentrated hydrogen peroxide solution. You can use hydroperite tablets - a combination of hydrogen peroxide with urea (urea will not interfere with the experiment). For more effect go to dark room Once your eyes have adjusted to the dark, pour the hydrogen peroxide solution into a large vessel of hydroquinone. The mixture will begin to foam (hence the need for a large vessel) and a distinct orange glow will appear!

The chemical reactions in which the glow appears do not occur only during oxidation. Sometimes the glow occurs during crystallization. The easiest way to observe it is table salt. Dissolve table salt in water, and take enough salt so that undissolved crystals remain at the bottom of the glass. Pour the resulting saturated solution into another glass and add concentrated hydrochloric acid to this solution drop by drop. The salt will begin to crystallize, and sparks will fly through the solution. It is most beautiful if the experience is set in the dark!

Chemical experiments with chromium and its compounds

Multicolored chrome!... The color of chromium salts can easily change from purple to green and vice versa. Let's carry out the reaction: let's dissolve in water a few purple crystals of chromium chloride CrCl 3 6H 2 O. When boiled, the purple solution of this salt turns green. When the green solution is evaporated, a green powder of the same composition as the original salt is formed. And if you saturate a green solution of chromium chloride cooled to 0 ° C with hydrogen chloride (HCl), its color will turn purple again. How to explain the observed phenomenon? It's rare in inorganic chemistry an example of isomerism - the existence of substances that have the same composition, but different structure and properties. In the violet salt, the chromium atom is bonded to six water molecules, and the chlorine atoms are counterions: Cl 3, and in green chromium chloride they change places: Cl 2H 2 O. In an acidic environment, dichromates are strong oxidizing agents. Their recovery products are Cr3+ ions:

K 2 Cr 2 O 7 + 4H 2 SO 4 + 3K 2 SO 3 → Cr 2 (SO 4) 3 + 4K 2 SO 4 + 4H 2 O.

Potassium chromate (yellow)
dichromate - (red)

At a low temperature, violet crystals of potassium chromium alum KCr (SO 4) 2 12H 2 O can be isolated from the resulting solution. The dark red solution obtained by adding concentrated sulfuric acid to a saturated aqueous solution of potassium dichromate is called “chromic peak”. In laboratories, it is used for washing and degreasing chemical glassware. The dishes are carefully rinsed with chromic, which is not poured into the sink, but is used repeatedly. In the end, the mixture becomes green - all the chromium in such a solution has already passed into the Cr 3+ form. Especially strong oxidizing agent- chromium oxide (VI) СrО 3 . With it, you can light an alcohol lamp without matches: just touch the wick moistened with alcohol with a stick with several crystals of this substance. When CrO 3 is decomposed, dark brown chromium (IV) oxide powder CrO 2 can be obtained. It has ferromagnetic properties and is used in the magnetic tapes of some types of audio cassettes. The body of an adult contains only about 6 mg of chromium. Many compounds of this element (especially chromates and dichromates) are toxic, and some of them are carcinogens, i.e. capable of causing cancer.

Chemical experiments: the reducing properties of iron

Ferric chloride III

This type chemical reaction refers to redox reactions. To carry out the reaction, we need diluted (5%) aqueous solutions iron(III) chloride FeCl 3 and the same solution of potassium iodide KI. So, a solution of iron (III) chloride is poured into one flask. Then add a few drops of potassium iodide solution to it. Observe the color change of the solution. The liquid will take on a reddish-brown color. The following chemical reactions will take place in the solution:

2FeCl 3 + 2KI → 2FeCl 2 + 2KCl + I 2

KI + I 2 → K

Ferric chloride II

Another chemical experiment with iron compounds. For it, we need dilute (10–15%) aqueous solutions of iron (II) sulfate FeSO 4 and ammonium thiocyanate NH 4 NCS, bromine water Br 2. Let's start. Pour a solution of iron(II) sulfate into one flask. 3-5 drops of ammonium thiocyanate solution are also added there. We notice that there are no signs of chemical reactions. Of course, iron(II) cations do not form colored complexes with thiocyanate ions. Now add bromine water to this flask. But now the iron ions "given themselves out" and colored the solution in a blood-red color. this is how the (III) ion of valence iron reacts to thiocyanate ions. Here's what happened in the flask:

Fe(H 2 O) 6 ] 3+ + n NCS– (n–3) – + n H 2 O

Chemical experiment on the dehydration of sugar with sulfuric acid

Sugar dehydration
sulfuric acid

concentrated sulphuric acid dehydrates sugar. Sugar is a complex organic substance whose formula is C 12 H 22 O 11. Here's how it goes. Powdered sugar is placed in a tall glass beaker, slightly moistened with water. Then a little concentrated sulfuric acid is added to the wet sugar. mix gently and quickly with a glass rod. The stick is left in the middle of the glass with the mixture. After 1 - 2 minutes, the sugar begins to turn black, swell and rise in the form of a voluminous, loose black mass, taking the glass rod with it. The mixture in the glass gets very hot and smokes a little. In this chemical reaction, sulfuric acid not only removes water from sugar, but also partially turns it into coal.

C 12 H 22 O 11 + 2H 2 SO 4 (conc.) → 11C + CO 2 + 13H 2 O + 2SO 2

The released water during such a chemical reaction is mainly absorbed by sulfuric acid (sulfuric acid "greedily" absorbs water) with the formation of hydrates, hence the strong release of heat. And carbon dioxide CO 2, which is obtained during the oxidation of sugar, and sulfur dioxide SO 2 raise the charring mixture up.

Chemical experiment with the disappearance of an aluminum spoon

Mercury nitrate solution

Let's carry out another funny chemical reaction: for this we need an aluminum spoon and mercury nitrate (Hg (NO 3) 2). So, let's take a spoon, clean it with a fine-grained sandpaper then degrease with acetone. Dip a spoon for a few seconds in a solution of mercury nitrate (Hg (NO 3) 2). (remember that mercury compounds are poisonous!). As soon as the surface of the aluminum spoon in the mercury solution becomes gray color, the spoon must be removed, washed boiled water dry (wetting, but not wiping). After a few seconds, the metal spoon will turn into fluffy white flakes, and soon only a grayish pile of ash will be left of it. This is what happened:

Al + 3 Hg(NO 3) 2 → 3 Hg + 2 Al(NO 3) 3 .

In the solution, at the beginning of the reaction, a thin layer of aluminum amalgam (an alloy of aluminum and mercury) appears on the surface of the spoon. The amalgam then turns into fluffy white flakes of aluminum hydroxide (Al(OH) 3). The metal consumed in the reaction is replenished with new portions of aluminum dissolved in mercury. And, finally, instead of a shiny spoon, white Al (OH) 3 powder and tiny droplets of mercury remain on the paper. If, after a solution of mercury nitrate (Hg (NO 3) 2), an aluminum spoon is immediately immersed in distilled water, then gas bubbles and flakes will appear on its surface white color(hydrogen and aluminum hydroxide will be released).

A chemist is a very interesting and multifaceted profession, uniting many different specialists: chemical scientists, chemical technologists, analytical chemists, petrochemists, chemistry teachers, pharmacists and many others. We decided to celebrate the upcoming Chemist's Day 2017 together with them, so we chose some interesting and impressive experiments in the field under consideration, which even those who are as far from the profession of a chemist as far as possible can repeat. Best chemical experiments at home - read, watch and memorize!

When is Chemist's Day celebrated?

Before we begin to consider our chemical experiments, let us clarify that the Chemist's Day is traditionally celebrated on the territory of the states of the post-Soviet space at the very end of spring, namely, on the last Sunday of May. This means that the date is not fixed: for example, in 2017 Chemist's Day is celebrated on May 28th. And if you work in the field chemical industry, or you study a specialty from this area, or are otherwise directly related to chemistry on duty, which means that you have every right to join the celebration on this day.

Chemical experiments at home

And now let's get down to the main thing, and we begin to perform interesting chemical experiments: it is best to do this together with young children, who will definitely perceive what is happening as a magic trick. Moreover, we tried to select such chemical experiments, the reagents for which can be easily obtained at a pharmacy or a store.

Experience No. 1 - Chemical traffic light

Let's start with a very simple and beautiful experiment, which received such a name by no means in vain, because the liquid participating in the experiment will change its color just to the colors of the traffic light - red, yellow and green.

You will need:

• indigo carmine;
• glucose;
• caustic soda;
• water;
• 2 clear glass containers.

Don't let the names of some of the ingredients scare you - you can easily buy glucose in tablets at a pharmacy, indigo carmine is sold in stores as a food coloring, and you can find caustic soda in hardware store. It is better to take containers tall, with a wide base and a narrower neck, for example, flasks, so that it is more convenient to shake them.

But what is interesting about chemical experiments - there is an explanation for everything:

• By mixing glucose with caustic soda, i.e. sodium hydroxide, we obtained an alkaline solution of glucose. Then, mixing it with a solution of indigo carmine, we oxidize the liquid with oxygen, with which it was saturated during the transfusion from the flask - this is the reason for the appearance of green color. Further, glucose begins to work as a reducing agent, gradually changing color to yellow. But by shaking the flask, we again saturate the liquid with oxygen, allowing the chemical reaction to go through this circle again.

How interesting it looks live, you will get an idea from this short video:

Experience No. 2 - A universal indicator of acidity from cabbage

Children love interesting chemical experiments with colorful liquids, it's no secret. But we, as adults, responsibly declare that such chemical experiments look very spectacular and curious. Therefore, we advise you to conduct another "color" experience at home - a demonstration of amazing properties red cabbage. It, like many other vegetables and fruits, contains anthocyanins - natural dyes-indicators that change their color depending on the pH level - i.e. the degree of acidity of the environment. This property of cabbage is useful to us in order to obtain further multi-colored solutions.

What we need:

• 1/4 red cabbage;
• lemon juice;
• baking soda solution;
• vinegar;
• sugar solution;
• drink type "Sprite";
• disinfectant;
• bleach;
• water;
• 8 flasks or glasses.

Many substances on this list are quite dangerous, so be careful when doing simple chemistry experiments at home, wear gloves, goggles if possible. And do not let children get too close - they can knock over the reagents or the final contents of the colored cones, even want to try them, which should not be allowed.

Let's get started:

And how do these chemical experiments explain the color changes?

• The fact is that light falls on all objects that we see - and it contains all the colors of the rainbow. Moreover, each color in the spectrum beam has its own wavelength, and the molecules different shapes, in turn, reflect and absorb these waves. The wave that is reflected from the molecule is the one that we see, and this determines what color we perceive - because other waves are simply absorbed. And depending on what substance we add to the indicator, it begins to reflect only rays of a certain color. Nothing complicated!

A slightly different version of this chemical experiment, with fewer reagents, see the video:

Experience number 3 - Dancing jelly worms

We continue to do chemical experiments at home - and we will conduct the third experiment on all our favorite jelly sweets in the form of worms. Even adults will find it funny, and children will be completely delighted.

Take the following ingredients:

• a handful of jelly worms;
• vinegar essence;
• ordinary water;
• baking soda;
• glasses - 2 pcs.

When choosing the right candies, opt for smooth gooey worms, without sugar sprinkles. So that they are not heavy and move more easily, cut each candy lengthwise into two halves. So, we begin interesting chemical experiments:

1. Make a solution of warm water and 3 tablespoons of baking soda in one glass.
2. Put the worms in there and hold them there for about fifteen minutes.
3. Fill another deep glass with essence. Now you can slowly throw the jelly into the vinegar, watching how they begin to move up and down, which in some ways looks like a dance:

Why is this happening?

• It's simple: baking soda, in which the worms are soaked for a quarter of an hour, is sodium bicarbonate, and the essence is an 80% solution of acetic acid. When they react, water, carbon dioxide in the form of small bubbles, and the sodium salt of acetic acid are formed. It is carbon dioxide in the form of bubbles that surrounds the worm, rises up, and then falls when they burst. But the process is still going on, causing the candy to rise on the resulting bubbles and descend until it is complete.

And if you are seriously interested in chemistry, and want Chemist's Day to become yours in the future professional holiday, then you will probably be curious to watch the following video, which tells in detail about the typical everyday life of chemistry students and their exciting educational and scientific activities:

Take it, tell your friends!

Read also on our website:

show more

Entertaining physics in our presentation, he will tell you why in nature there cannot be two identical snowflakes and why the driver of an electric locomotive backs up before setting off, where the largest reserves of water are located and what invention of Pythagoras helps fight alcoholism.

Evening of entertaining chemistry

When preparing a chemical evening, careful preparation of the teacher for conducting experiments is required.

The evening should be preceded by long, careful work with students, and one student should not be assigned more than two experiments.

The purpose of the chemistry evening- repeat the knowledge gained, deepen students' interest in chemistry and instill in them practical skills in developing and implementing experiments.

Description of the main stages of the evening of entertaining chemistry

I. Introductory speech of the teacher on the topic "The role of chemistry in the life of society."

II. Entertaining experiences in chemistry.

Leading (the role of the leader is performed by one of the students of the 10-11th grade):

Today we are having an evening of entertaining chemistry. Your task is to carefully follow the chemical experiments and try to explain them. And so, we begin! Experience No. 1: "Volcano".

Experience number 1. Description:

A participant in the evening pours powdered ammonium dichromate (in the form of a slide) onto an asbestos net, on upper part Gorki puts several heads of matches and sets them on fire with a splinter.

Note: The volcano will look even more spectacular if you add a little powdered magnesium to the ammonium dichromate. Mix the components of the mixture immediately, because. magnesium burns vigorously and being in one place causes the scattering of hot particles.

The essence of the experiment is the exothermic decomposition of ammonium dichromate under local heating.

There is no smoke without fire, says an old Russian proverb. It turns out that with the help of chemistry you can get smoke without fire. And so, attention!

Experience number 2. Description:

The participant of the evening takes two glass rods, on which a little cotton wool is wound, and wets them: one in concentrated nitric (or hydrochloric) acid, the other in an aqueous 25% ammonia solution. Sticks should be brought to each other. White smoke rises from the sticks.

The essence of the experience is the formation of nitrate (chloride) ammonium.

And now we present to your attention the following experience - “Shooting Paper”.

Experience number 3. Description:

The participant of the evening takes out pieces of paper on a sheet of plywood, touches them with a glass rod. When you touch each leaf, a shot is heard.

Note: narrow strips of filter paper are cut in advance and moistened in a solution of iodine in ammonia. After that, the strips are laid out on a sheet of plywood and left to dry until the evening. The shot is the stronger, the better the paper is impregnated with the solution and the more concentrated the solution of nitrogen iodide was.

The essence of the experiment is the exothermic decomposition of the fragile compound NI3*NH3.

I have an egg. Which one of you guys will peel it without breaking the shells?

Experience number 4. Description:

The participant of the evening places the egg in a crystallizer with a solution of hydrochloric (or acetic) acid. After a while, it pulls out an egg covered only with a shell membrane.

The essence of the experience is that the composition of the shell mainly includes calcium carbonate. In hydrochloric (acetic) acid, it turns into soluble calcium chloride (calcium acetate).

Guys, I have a figure of a man made of zinc in my hands. Let's dress him up.

Experience number 5. Description:

The participant of the evening lowers the figurine into a 10% lead acetate solution. The figurine is covered with a fluffy layer of lead crystals, reminiscent of fur clothes.

The essence of the experiment is that a more active metal displaces a less active metal from salt solutions.

Guys, is it possible to burn sugar without the help of fire? Let's check!

Experience number 6. Description:

The participant of the evening pours icing sugar (30 g) into a glass placed on a saucer, pours 26 ml of concentrated sulfuric acid into the same place and stirs the mixture with a glass rod. After 1-1.5 minutes, the mixture in the glass darkens, swells and rises above the edges of the glass in the form of a loose mass.

The essence of the experiment is that sulfuric acid removes water from sugar molecules, oxidizes carbon into carbon dioxide, and at the same time sulfur dioxide is formed. The released gases push the mass out of the glass.

What methods of making fire do you know?

Examples are given from the audience.

Let's try to do without these funds.

Experience number 7. Description:

A participant in the evening pours potassium permanganate (6 g) ground into powder on a piece of tin (or a tile) and drops glycerin on it from a pipette. After a while, a fire appears.

The essence of the experiment is that as a result of the reaction, atomic oxygen is released and glycerol ignites.

Other participant of the evening:

I will also get fire without matches, only in a different way.

Experience number 8. Description:

A participant in the evening sprinkles a small amount of potassium permanganate crystals on a brick and drips concentrated sulfuric acid on it. Around this mixture, he folds thin chips in the form of a fire, but so that they do not touch the mixture. Then he wets a small piece of cotton wool with alcohol and, holding his hand over the fire, squeezes a few drops of alcohol out of the cotton so that they fall on the mixture. The fire instantly lights up.

The essence of the experience is the vigorous oxidation of alcohol by oxygen, which is released during the interaction of sulfuric acid with potassium permanganate. The heat released during this reaction ignites the fire.

And now amazing lights!

Experience number 9. Description:

The participant of the evening puts cotton swabs moistened with ethyl alcohol into porcelain cups. On the surface of the tampons, he pours the following salts: sodium chloride, strontium nitrate (or lithium nitrate), potassium chloride, barium nitrate (or boric acid). On a piece of glass, the participant prepares a mixture (slurry) of potassium permanganate and concentrated sulfuric acid. He takes some of this mass with a glass rod and touches the surface of the tampons. Tampons flash and burn different colors: yellow, red, purple, green.

The essence of the experience is that alkali and alkaline earth metal ions color the flame in different colors.

Dear children, I am so tired and hungry that I ask you to allow me to eat a little.

Experience number 10. Description:

The host addresses the participant of the evening:

Give me some tea and biscuits, please.

The participant of the evening gives the host a glass of tea and a white cracker.

The host moistens the cracker in tea - the cracker turns blue.

Leading :

Disgrace, you almost poisoned me!

Participant of the evening:

Excuse me, I must have mixed up the glasses.

The essence of the experiment - in the glass was a solution of iodine. The starch in the bread turned blue.

Guys, I received a letter, but there was a blank sheet of paper in the envelope. Who can help me find out what's wrong?

Experience number 11. Description:

A student from the audience (prepared in advance) touches a smoldering splinter to a pencil mark on a sheet of paper. The paper along the line of the drawing slowly burns out and the light, moving along the contour of the image, outlines it (the drawing can be arbitrary).

The essence of the experience is that the paper burns due to the oxygen of the saltpeter crystallized in its thickness.

Note: a drawing is pre-applied on a sheet of paper with a strong solution potassium nitrate. It must be applied in one continuous line without intersections. From the outline of the drawing with the same solution, draw a line to the edge of the paper, marking its end with a pencil. When the paper dries, the pattern will become invisible.

Well, now, guys, let's move on to the second part of our evening. Chemical games!

III. Team games.

Participants of the evening are invited to break into groups. Each group takes part in the proposed game.

Game number 1. Chemical lotto.

Formulas are written on cards, graphed as in a regular loto. chemical substances, and on cardboard squares - the names of these substances. The group members are given cards, and one of them pulls out the squares and names the substances. The winner is the member of the group who first closes all the fields of the card.

Game number 2. Chemical quiz.

A rope is stretched between the backs of two chairs. Sweets are tied to it on strings, to which pieces of paper with questions are attached. Group members take turns cutting candy with scissors. The player becomes the owner of the candy after answering the question attached to it.

The group members form a circle. They have chemical symbols and numbers in their hands. Two of the players are in the middle of the circle. On command, they make up the chemical formula of substances from the signs and numbers held by the other players. The participant who completes the formula the fastest wins.

The group members are divided into two teams. They are given cards with chemical formulas and numbers. They must write a chemical equation. The team that completes the equation first wins.

The evening ends with the presentation of prizes to the most active participants.