What are some of the chemistry experiments that amaze you?

Fill half a glass of water in a glass, put a dozen potassium chlorate crystals on the bottom of the water, and then use tweezers to pick up a few small grains of yellow phosphorus and put them into the potassium chlorate crystals. Then use a glass pipette to absorb a small amount of concentrated sulfuric acid and transfer it into a mixture of potassium chlorate and yellow phosphorus, at which point there is a fire in the water. Isn't fire in water "fire and water compatible"?

Concentrated hydrochloric acid and concentrated ammonia are pre-dripping at different locations on the paper, both of which are extremely volatile, and when they meet in the air, they also form ammonium chloride, creating a smog effect. It's like you've gone to the fairy mirror.

Cut the lemon and squeeze the lemon juice into a glass. Add an appropriate amount of water, pour in another tablespoon of baking soda, shake gently to dissolve the baking soda well, and add some more sugar. The bottle was full of steam.

The solid lead iodide melts, puts it into the bottle and shakes it simply, and it can form "** rain"! A bottle full of golden substance, you don't have any other ideas than to take it home, **ah!

Potassium permanganate is mixed with glycerol and reacts violently to release a large amount of heat, which causes the solid residue formed by the decomposition of ammonium dichromate to be ejected with the generated gas. This soon formed an erupting volcano.

Throw the sodium metal into the water.

Five classical chemistry experiments.

First, oxygen is produced in the laboratory.

1.With H2O2 (hydrogen peroxide).

2h2o2=mno2=2h2o+o2↑

Devices: test tubes, catheters, sinks, gas collection cylinders.

Pyrolysis. 2kclo3=△=2kcl+o2

Installation: alcohol lamp, test tube, catheter, sink, gas collection cylinder, iron frame potassium permanganate) pyrolysis.

2kmNO4= =K2MNO4+MNO2+O2 Device: alcohol lamp, test tube, catheter, sink, gas collection cylinder, iron frame 2, laboratory CO2

CaCO3CaCO3+2HCl=CaCl2+H2O+CO2 Test tubes, catheters, gas collector cylinders.

Third, acid-base neutralization reaction.

Fourth, the reaction of substitution, Fe, Mg, Cu and hydrochloric acid, sulfuric acid Five, hydrogen reduction of copper oxide.

A whole bunch of them, like Lavoisier's combustion test, Liebig's analytical experiment.

Volcanic eruptions.

Raw material: Ammonium dichromate, as long as you light it with a lighter, it will decompose, and sparks and ash will emerge, much like a volcanic eruption. It's not dangerous, he's just on fire, and he won't **.

Elephant toothpaste. 30% hydrogen peroxide, potassium iodide (this one is a bit expensive, it is not recommended) or potassium permanganate, detergent, spread a small spoonful of potassium permanganate on the bottom of the graduated cylinder, mix hydrogen peroxide and detergent and pour it in, and there will be a stream of foam washed out.

Blank paper. Use a glass stick dipped in dilute sulfuric acid to write on the printer paper and then air dry, you can't see the appearance of the words, and then bake it on the fire for a while (don't bake it) and black words will come out (dilute sulfuric acid becomes concentrated sulfuric acid, so it's best not to touch those words).

That's all, simple.

Thermite reaction, I feel that the fire is amazing! ~

Jumping small charcoal. When the small charcoal was first put into the test tube, the temperature of the potassium nitrate in the test tube was low, and it had not yet been able to make the charcoal burn, so the small charcoal was still lying there. After continuing to heat the test tube, the temperature rises, so that the small charcoal reaches the ignition point, and then it has a fierce chemical reaction with potassium nitrate, and releases a large amount of heat, so that the small charcoal immediately burns and glows.

Because potassium nitrate decomposes at high temperatures and releases oxygen, this oxygen immediately reacts with the small charcoal to form carbon dioxide gas, which suddenly lifts the small charcoal. After the charcoal jumps, it is out of contact with the potassium nitrate liquid below, the reaction is interrupted, and the carbon dioxide gas no longer occurs, and when the small charcoal falls back to the potassium nitrate due to the action of gravity, the reaction occurs again, and the small charcoal jumps up for the second time. This cycle repeated, and the little charcoal kept jumping up and down.

White sugar turns black charcoal. White sugar and concentrated sulfuric acid undergo a chemical reaction called "dehydration". Concentrated sulfuric acid has a particularly strange hobby, that is, its desire to combine with water is particularly strong, it makes full use of the moisture in the air, even the moisture in other substances It does not let go, as long as it meets, it has to take the water over.

White sugar is a carbohydrate (C12H22O11), and when it encounters concentrated sulfuric acid, the water in the white sugar molecule is immediately taken away by it, and the poor white sugar is left with charcoal and turns black. After the concentrated sulfuric acid took the water for itself, it was not satisfied, and it exerted another skill, it oxidized part of the charcoal left in the sugar, and generated carbon dioxide gas.

c+2h2so4=2h2o+2so2+co2

As the carbon dioxide and sulfur dioxide gas produced after the reaction escapes, the volume becomes larger and larger, and finally it becomes fluffy "black snow". In the "battle" of concentrated sulfuric acid to seize water, it is an exothermic process, so it makes a snorting sound and provides heat for the concentrated sulfuric acid to continue the process of carbon oxidation.

Light bulbs that do not use electricity. This bulb contains magnesium strips and concentrated sulfuric acid, which undergo a violent chemical reaction inside the bulb, causing exothermic luminescence. As we all know, concentrated sulfuric acid has strong oxidizing properties, especially when it meets some metals, it can show its oxidation ability.

Magnesium metal is a particularly easy to be oxidized substance, so they are born "the right match", as long as they meet, they will immediately detach the chemical reaction: mg 2h2SO4 (concentrated) MGSO4 SO2 2H20 in the reaction process releases a lot of heat, so that the temperature in the light bulb rises sharply, quickly make the magnesium strip reach the ignition point, in the case of concentrated sulfuric acid full supply of oxygen, the magnesium strip burns more vigorously, like a flare.