Sodium silicate solution, adding ferric chloride, copper sulfate, zinc sulfate and other metal salts, you can see a colorful "tree"-like scene growing up gradually.
2. Metal replacement
For example, copper wire inserted into silver nitrate can grow a "silver tree", and iron wire inserted into the mixed solution of copper sulfate and sodium chloride can grow a "copper tree".
3. Electrolytic water
There is nothing to say. The specific operation is easy to check and the phenomenon is obviously harmless.
Which chemical experiments are suitable for primary school students to watch? Light candles to measure products.
Hydrogen peroxide produces oxygen.
"Water-fire compatibility" experiment (white phosphorus is burned after air is introduced under hot water) (especially recommended, which can arouse students' interest)
I will be very happy if the landlord adopts it. (ゝ。 ? )
What chemical experiments can middle school students do? Main experimental operations and phenomena in 80 cases
1. Magnesium rod burns in air: it gives off dazzling light and a lot of heat, and at the same time produces white smoke and a kind of white material.
Charcoal burns in oxygen: it gives off white light and heat.
3. Sulfur burns in oxygen: it gives off a bright blue-purple flame, gives off heat and produces a gas with an odor of * * *.
4. Iron wire burns in oxygen: it burns violently, sparks are everywhere, heat is released, and black solid substances are produced.
5. Heat the ammonium bicarbonate in the test tube: produce odorous gas and liquid drops on the test tube.
6. Hydrogen burns in the air: the flame is light blue.
7. Hydrogen burns in chlorine: it gives off a pale flame and generates a lot of heat.
Droplets are formed at the nozzle.
9. Copper oxide powder is reduced by carbon powder, so that the generated gas is introduced into clear limewater, black copper oxide becomes shiny metal particles, and limewater becomes turbid.
10. Carbon monoxide burns in the air: it gives off a blue flame and gives off heat.
1 1. Dropping hydrochloric acid into a test tube containing a small amount of potassium carbonate solid: generating gas.
12. Heat the copper sulfate crystal in the test tube: the blue crystal gradually turns into white powder, and droplets are formed at the mouth of the test tube.
13. Sodium burns in chlorine: violent combustion produces white solid.
14. ignite pure chlorine and cover the flame with a dry and cold beaker: a light blue flame is emitted, and droplets are generated on the inner wall of the beaker.
15. The silver nitrate solution acidified by nitric acid was dropped into the solution containing C 1- to produce white precipitate.
16. The barium chloride solution acidified with nitric acid was added dropwise to the solution containing SO ~ (42-), resulting in white precipitate.
17. Put a rusty nail into a test tube filled with dilute sulfuric acid and heat it: the rust gradually dissolves, the solution turns pale yellow, and gas is generated.
18. Drop sodium hydroxide solution into copper sulfate solution: blue flocculent precipitate is formed.
19. When Cl2 is introduced into colorless KI solution, brown substance will be produced in the solution.
20. Drop the sodium hydroxide solution into the ferric chloride solution: a reddish-brown precipitate is formed.
2 1. Add a small amount of water to the test tube filled with quicklime: the reaction is intense and a lot of heat is released.
22. Immerse clean nails in copper sulfate solution: red substances are attached to the nail surface, and the color of the solution gradually becomes lighter.
23. Insert the copper sheet into the mercury nitrate solution: silver white material is attached to the surface of the copper sheet.
24. Inject concentrated sodium carbonate solution into a test tube filled with limewater: white precipitate is generated.
25. Add water after burning thin copper wire in chlorine gas: brown smoke is generated, and green solution is generated after adding water.
26. Strong light irradiates the mixed gas of hydrogen and chlorine: the reaction is rapid and an explosion occurs.
27. Red phosphorus burns in chlorine: white smoke is produced.
28. Chlorine meets wet colored cloth strips: the color of colored cloth strips fades.
29. Heat the mixture of concentrated hydrochloric acid and manganese dioxide: produce yellow-green odor gas.
30. Heat the mixture of sodium chloride (solid) and sulfuric acid (concentrated): generate fog and odor.
3 1. Drop silver nitrate solution into sodium bromide solution, and then add dilute nitric acid: pale yellow precipitate is formed.
32. After the silver nitrate solution is dripped into the potassium iodide solution, dilute nitric acid is added: a yellow precipitate is formed.
33.I2 meets starch and produces a blue solution.
34. Thin copper wire burns in sulfur vapor: When thin copper wire turns red, it will produce black substance.
35. Iron powder and sulfur powder are mixed and heated to red heat: the reaction continues, releasing a lot of heat and generating black substances.
36. Incomplete combustion of hydrogen sulfide gas (cover the evaporating dish on the flame): the flame is light blue (there is yellow powder at the bottom of the evaporating dish).
37. Hydrogen sulfide gas burns completely (cover a dry and cold beaker on the flame): the flame is light blue, and gas with * * * odor is generated (droplets are generated on the inner wall of the beaker).
38
Mix hydrogen sulfide and sulfur dioxide in a gas container: the inner wall of the bottle forms yellow powder.
39. Sulfur dioxide gas is heated after introducing magenta solution: the red color recedes, and the original color is restored after heating.
40. Put excess copper into a test tube filled with concentrated sulfuric acid, heat it, and after the reaction, add water to the solution after cooling: gas with * * * odor is generated, and the solution is sky blue after adding water.
4 1. Heat the test tube filled with concentrated sulfuric acid and charcoal: generate gas, which has the smell of * * *.
42. Sodium burns in the air: the flame is yellow, producing light yellow substances.
43. Sodium is thrown into the water: the reaction is fierce, and sodium floats on the water surface, releasing a lot of heat to make sodium dissolve into small balls and swim on the water surface, making a "before" sound.
44. Drop water into a test tube filled with sodium peroxide solid, and put the wooden strip with Mars into the mouth of the test tube: the wooden strip is re-ignited.
45. Heat the sodium bicarbonate solid to make the generated gas flow into the clarified limewater: the clarified limewater becomes turbid.
46. Ammonia meets hydrogen chloride: there is a lot of white smoke.
47. Heat the mixture of ammonium chloride and calcium hydroxide: produce gas with * * * odor.
48. Heat the test tube filled with solid ammonium chloride: white crystals are produced at the mouth of the test tube.
49. The concentrated nitric acid in colorless reagent bottle is exposed to the sun: the space in the bottle is brown and the nitric acid is yellow.
50. Reaction between copper sheet and concentrated nitric acid: The reaction is fierce, producing reddish-brown gas.
5 1. The copper sheet reacts with dilute nitric acid: colorless gas is produced at the lower end of the test tube, which gradually turns reddish brown when it rises.
52. Add dilute hydrochloric acid to sodium silicate solution to produce white colloidal precipitate.
53. Add magnesium sulfate solution to the iron hydroxide colloid: the colloid becomes turbid.
54. Heat the iron hydroxide colloid: the colloid becomes turbid.
55. Put the ignited magnesium bar into a gas cylinder filled with carbon dioxide: it burns violently and there is black substance attached to the inner wall of the gas cylinder.
56. Dropping ammonia water into the aluminum sulfate solution: fluffy white flocculent substances are generated.
57. Drop the sodium hydroxide solution into the ferrous sulfate solution: form a white flocculent precipitate, which immediately turns gray-green and then red-brown precipitate.
58. Drop the KSCN solution into the solution containing Fe3+: the solution is blood red.
59. Add chlorine water dropwise to the sodium sulfide aqueous solution: the solution becomes turbid. S2-+Cl2=2Cl2-+S↓
60. Add a small amount of soap to natural water: the foam gradually decreases and precipitation occurs.
6 1. ignite the methane in the air, and put the dry and cold beaker on the flame: the flame is light blue, and droplets are produced on the inner wall of the beaker.
62. Illumination of mixed gas of methane and chlorine: Yellow-green color gradually becomes shallow for a long time (droplets are formed on the inner wall of the container).
63. Heat the mixture of ethanol and concentrated sulfuric acid (170℃), and introduce the generated gas into bromine water and acidic potassium permanganate solution: when the gas is generated, the bromine water fades and the purple gradually becomes lighter.
64. Ignite the ethylene in the air: the flame is bright, producing black smoke and releasing heat.
65. Ignite acetylene in the air: the flame is bright, producing smoke and releasing heat.
66. There is benzene in the air
Burning in the air: bright flame with black smoke.
67. Ethanol burns in the air: the flame is light blue.
68. Introduce acetylene into bromine water: bromine water fades.
69. Introduce acetylene into acidic potassium permanganate solution: purple gradually becomes lighter until it fades.
Benzene reacts with bromine in the presence of iron powder as catalyst: white mist is produced and the product is oily brown.
7 1. Pour a small amount of toluene into a proper amount of potassium permanganate solution and shake well: purple fades.
72. Put sodium metal into a test tube filled with ethanol: the gas is released.
73. Drop excessive concentrated bromine water into a test tube containing a small amount of phenol: form a white precipitate.
74. Drop a few drops of ferric chloride solution into a test tube containing phenol and shake well: the solution turns purple.
75. Acetaldehyde reacts with silver ammonia solution in the test tube: the inner wall of the clean test tube is attached with a layer of bright as a mirror.
When heated to boiling, acetaldehyde reacts with newly formed copper hydroxide: a red precipitate is formed.
77. Under suitable conditions, ethanol reacts with acetic acid to form a transparent oily liquid with fragrance.
78. protein encountered a concentrated nitric acid solution: it turned yellow.
79. The purple litmus test solution turns blue when it meets alkali.
80. Colorless phenolphthalein test solution turns red when it meets alkali.
What are the interesting chemistry experiments (suitable for junior high school students)? It is safe to add acetic acid to eggs, which can let junior high school students know what eggs are and is also very interesting.
What handicrafts are suitable for primary school students? In the case of safety first, use branches, leaves, paper and pens to create through modeling, drawing and folding. Children's eyes can see features that adults can't. Educational is better. For example, if you know the color of winter, you can draw a picture with it as the theme. You can also roll the paper into balls to represent planets of different sizes and simulate the solar system.
What biochemical experiments are there in the university? I am a preventive medicine major, and the experimental guidance is arranged like this.
1 and folin phenol reagent for the determination of protein
2. Serum protein cellulose acetate membrane electrophoresis.
3. Serum protein polyacrylamide gel electrophoresis.
4. Determination of molecular weight of protein -SDS- polyacrylamide gel electrophoresis.
5. Factors affecting enzyme activity
6. Competitive inhibition of succinate dehydrogenase
7, the nature of the enzyme-the specificity of the enzyme
8. Determination of Km value of alkaline phosphatase
9. Determination of lactate dehydrogenase isoenzymes by agarose electrophoresis.
10, determination of blood sugar content
1 1, serum lipoprotein electrophoresis
12, amino conversion
13, determination of serum alanine aminotransferase activity
14, zeolite column chromatography
15, Determination of Vitamin C in Food
16, polymerase chain reaction and product identification (PCR)
17, extraction and content determination of animal tissue accounting
18, Rapid Extraction and Content Determination of Plasmid DNA
19, Extraction and Electrophoresis Detection of Genomic DNA
20. Separation and purification of serum gamma globulin.
Too much sweat. The experimental class will start next week. Pretty scary. ..
Chapter 1 Experimental Techniques of Biochemistry and Molecular Biology Chapter 2 Quantitative Analysis Techniques of protein Chapter 3 Enzyme Separation and Analysis Techniques Chapter 4 Nucleic Acid Separation and Analysis Techniques Chapter 5 Study on Substance Metabolism and Regulation Chapter 6 Chromatographic Techniques Chapter 7 Electrophoresis Techniques Chapter 8 Molecular Imprinting Techniques Chapter 9 Gene Cloning and Related Technical Appendices.
Chemical experiments in universities include inorganic chemistry, organic chemistry, analytical chemistry, physical chemistry, structural chemistry and many other experiments.