"Antimy" - Application. Obtaining antimony. Being in nature. Physical properties. Position in the Mendeleev PS. Antimony is known in crystalline and three amorphous forms: explosive, black and yellow. Antimony. Story. Chemical properties.

“Metal copper” - Chemical element of a secondary subgroup of group 1 – Cu (Copper). Due to its high thermal conductivity, copper is an irreplaceable material for various heat exchangers and refrigeration equipment. COPPER (Latin. The role of bronze was especially great. Sea water contains approximately 1·10-8% copper. The ingestion of copper salts into the body leads to various human diseases.

“Production of hydrogen” - Types of reactions. Production of hydrogen in industry and its application. Hydrogen production in industry. Methods of obtaining. Production mineral fertilizers. Natural gas. Application of hydrogen. Heating. Methods for producing hydrogen. Complete the chemical reactions.

“Properties of Aluminum” - Aluminum occurs in nature in the form of aluminosilicates, bauxite, corundum and cryolite. Why is aluminum so necessary for humans? Draw a conclusion about the abundance of aluminum in the earth's crust compared to other metals. Mg>Al

"Element aluminum" - Aluminum). The influence of aluminum compounds on environmental pollution. Obtaining the substance. Number. Chemical properties of the substance. Aluminum reacts: The Latin name probably goes back to the Greek “halme” - brine, salt solution. Does not dissolve in water. Aluminum oxide Al2O3: Aluminum is the most common metal in the earth's crust.

“Calcium and magnesium compounds” - Ca and Mg compounds. Composition and chemical formulas of the most important compounds of calcium and magnesium. Application of calcium hydroxide. Eliminate the extra word. Sea salt. Calcium and magnesium compounds. Karst caves and valleys. Carry out the transformation. Astringent action. Scale. Alkaline earth metals. Formation of stalactites and stalagmites.

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Slide captions:

Slide 1
Aluminum

Slide 2
13
Aluminum (lat. Aluminium)
3 8 2
26,9815
3s2 3p1
Serial number. Chemical element of group III of the main subgroup of the 3rd period.

Slide 3
Number
protons p+=13 electrons ē=13 neutrons n0=14

Slide 4
Diagram of the arrangement of electrons on energy sublevels
+13Al 1s2 2s2 2p6 3s2 3p1
1s
2s
2p
3s
3p
in compounds exhibits an oxidation state of +3

Slide 5
Al is a typical metal
Reducing properties of Al 0- 3ē Al+3 Type of chemical bond - metallic Type of crystal lattice - cubic face-centered

Slide 6
Physical properties of matter
Al is a silver-white metal, ductile, lightweight, conducts heat and electric current well, has good malleability, is easy to process, and forms light and strong alloys. =2.7 g/cm3 tmelt.=6600С

Slide 7
Features of the physical and chemical properties of aluminum, its occurrence in nature and application:
Aluminum is the most common metal in the earth's crust. Its resources are practically inexhaustible. It has high corrosion resistance and practically does not need special protection. The high chemical activity of aluminum is used in aluminothermy. Low density combined with the high strength and ductility of its alloys makes aluminum an indispensable structural material in aircraft construction and contributes to the expansion of its use in ground-based and water transport, as well as in construction. Relatively high electrical conductivity allows them to replace much more expensive copper in electrical engineering.

Slide 8
Aluminum reacts with simple substances - non-metals
4Al+3O2 = 2Al2O3 The surface is covered with an oxide film, and in a finely divided form it burns, releasing a large amount of heat.2. 2Al + 3Cl2 = 2 AlCl33. 2Al + 3S = Al2S3 - when heated4. 4Al + 3C = Al4C3 - when heated

Slide 9
Aluminum dissolves in acid solutions2Al + 6HCl = 2AlCl3 + 3H22Al + 3H2SO4 = Al2(SO4)3 + 3H2 Concentrated sulfuric and nitric acids passivate aluminum.2. Aluminum reacts with solutions of salts of less active metals2Al + 3СuCl2 = 2AlCl3 + 3Cu

Slide 10
Aluminum reacts with complex substances:
3. Aluminum at high temperatures reacts with oxides of less active metals (Aluminothermy - production of metals: Fe, Cr, Mn, Ti, W and others, by reducing them with aluminum) 8Al + 3Fe3O4 = 4Al2O3 + 9Fe

Slide 11
Aluminum reacts with complex substances:
4. Since aluminum is an amphoteric metal, it reacts with alkali solutions. In this case, sodium tetrahydroxoaluminate is formed and hydrogen is released: 2Al + 2NaOH + 6H2O = 2Na + 3H25. When the oxide film is removed from the surface of aluminum, it reacts with water to form aluminum hydroxide and hydrogen: 2Al + 6H2O = 2Al(OH)3 + 3H2

Slide 12
Aluminum production
Aluminum is produced by electrolysis of alumina solution in molten cryolite (Na3AIF6) and electrolysis of AlCl3 melt

Slide 13
Application of Al

Slide 14
Aluminum compounds In nature, aluminum is found only in the form of compounds and, in terms of prevalence in the earth's crust, ranks first among metals and third among all elements (after oxygen and silicon). The total aluminum content in the earth's crust is 8.8% by weight.

Slide 15
Aluminum oxide Al2O3:
Very hard (corundum, ruby) in a crystalline state, white powder, refractory - 20500C. Insoluble in water. Amphoteric oxide, interacts: a) with acids Al2O3 + 6H+ = 2Al3+ + 3H2Ob) with alkalis Al2O3 + 2OH- = 2AlO-2 + H2O Formed: a) during the oxidation or combustion of aluminum in air 4Al + 3O2 = 2Al2O3b) in the aluminothermic reaction 2Al + Fe2O3 = Al2O3 + 2Feв) during the thermal decomposition of aluminum hydroxide 2Al (OH)3 = Al2O3 + 3H2O

Slide 16
White powder insoluble in water. Exhibits amphoteric properties, interacts: a) with acids Al (OH)3 + 3HCl = AlCl3 + 3H2Ob) with alkalis Al (OH)3 + Na OH = NaAlO2 + 2H2O Decomposes when heated 2Al (OH)3 = Al2O3 + 3H2O Formed: a) during the interaction of solutions of aluminum salts with solutions of alkalis (without excess) Al3+ + 3OH- = Al (OH)3 b) during the interaction of aluminates with acids (without excess) AlO-2 + H+ + H2O = Al (OH )3
Aluminum hydroxide Al(OH)3:

Slide 17
Homework:
1) Using the presentation material and textbook, learn the properties of aluminum and its compounds. 2) Complete interactive tasks on the topic “Aluminium” on the lyceum website, write down the correct answers in a notebook. 3) Complete virtual practical work “Chemical properties of aluminum”, format it in a notebook.

On the topic: methodological developments, presentations and notes

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Aluminum

Teacher of chemistry and biology Egorova Yu.V.

MCOU "Secondary School No. 4"

Aluminum (lat. Aluminum)

Serial number. Chemical element of group III of the main subgroup of the 3rd period.

Number

protons p + =1 3

electrons ē=1 3

neutrons n 0 = 14

Diagram of the arrangement of electrons on energy sublevels

+ 13 Al 1s 2 2s 2 2p 6 3s 2 3p 1

At high temperatures it very rarely forms compounds with the oxidation state +1, +2.

in compounds exhibits oxidation state +3

Al – typical metal

• Restorative properties

Al 0 - 3ē Al +3

• Type of chemical bond - metal
• Type of crystal lattice – cubic face-centered

Physical properties of matter

Al – silver-white metal, ductile, lightweight, conducts heat and electricity well, has good malleability, is easy to process, and forms light and strong alloys.

 =2 ,7 g/cm 3

t pl. =660 0 WITH

Easily drawn into wire and rolled into foil up to 0.01 mm thick.

Features of the physical and chemical properties of aluminum, its occurrence in nature and application:

• Aluminum is the most common metal in the earth's crust. Its resources are practically inexhaustible.
• It has high corrosion resistance and practically does not require special protection.
• The high chemical activity of aluminum is used in aluminothermy.
• Low density, combined with the high strength and ductility of its alloys, makes aluminum an indispensable structural material in aircraft construction and contributes to the expansion of its use in land and water transport, as well as in construction.
• Relatively high electrical conductivity allows them to replace much more expensive copper in electrical engineering.

Aluminum reacts with simple substances - non-metals

• 4Al + 3O 2 = 2Al 2 O 3

The surface is covered with a film of oxide, and in a finely crushed form it burns, releasing a large amount of heat.

2. 2Al + 3Cl 2 = 2 AlCl 3

3. 2Al + 3S = Al 2 S 3 - when heated

4. 4 Al+3 WITH = Al 4 WITH 3 - when heated

When heated, aluminum burns in air. Due to the formation of a protective film, it does not react with HNO 3 and does not dissolve in H 3 PO 4. Reacts with difficulty with H 2 SO 4, slowly with solutions of HNO 3 and H 3 PO 4, faster with HCl solution, dissolves in alkali solutions: Al + 4HNO 3 = Al(NO 3) 3 + NO + 2H 2 O/

At normal temperature it reacts with Cl 2, Br 2, when heated - with F 2, I 2, S, C, N 2; does not react directly with H2.

• Aluminum dissolves in acid solutions

2Al + 6HCl = 2AlCl 3 + 3H 2

2Al + 3H 2 SO 4 = Al 2 (SO 4 ) 3 + 3H 2

Concentrated sulfur And nitrogen acids passivate aluminum.

2 . Aluminum reacts with solutions of salts of less active metals

2Al + 3СuCl 2 = 2AlCl 3 + 3Cu

Aluminum reacts with complex substances:

• 3. Aluminum at high temperatures reacts with oxides of less active metals (Aluminothermy - production of metals: Fe, Cr, Mn, Ti, W and others, by reducing them with aluminum)

8Al + 3Fe 3 O 4 = 4Al 2 O 3 + 9Fe

Aluminum reacts with complex substances:

4. Since aluminum is an amphoteric metal, it reacts with alkali solutions.

In this case, sodium tetrahydroxoaluminate is formed and hydrogen is released:

2Al + 2NaOH + 6H 2 O = 2Na + 3H 2

5. When the oxide film is removed from the surface of aluminum, it reacts with water to form aluminum hydroxide and hydrogen:

2Al + 6H 2 O = 2Al(OH) 3 +3H 2

Aluminum production

Aluminum is produced by electrolysis of a solution of alumina in molten cryolite (Na 3 AIF 6 ) And

electrolysis of AlCl melt 3

Aluminum is produced by electric decomposition of a solution of its oxide in molten cryolite (Na 3 AIF 6):

2Al 2 O 3 = 4 Al + 3O 2 – 3352 kJ

Due to the high chemical bond energy in the oxide, the process of its decomposition is extremely energy-intensive, which limits the use of aluminum.

Application Al

The main properties of using aluminum and its alloys:

• Shipbuilding;
• Construction;
• Aircraft manufacturing;
• In chemical engineering;
• Automotive industry;
• Production of tableware;
• Production of aluminized fabrics;
• Manufacturing of equipment for the food industry;
• Wires for power lines;
• Preparation of metals from their oxides by “aluminothermy”;
• Rocket Science;
• Chemical engineering;
• Packaging material;
• Production of aluminum foam ρ = 0.19 g/cm 3

Aluminum connections In nature, aluminum is found only in the form of compounds and, in terms of abundance in the earth’s crust, ranks first among metals and third among all elements (after oxygen and silicon). The total aluminum content in the earth's crust is 8.8% by mass.

Aluminum oxide Al 2 ABOUT 3 :

Very hard (corundum, ruby) in a crystalline state, white powder, refractory - 2050 0 C.

Does not dissolve in water.

Amphoteric oxide , interacts :

A) with acids Al 2 O 3 + 6H + = 2Al 3+ + 3H 2 O

b) with alkalis Al 2 O 3 + 2OH - = 2AlO - 2 + H 2 O

Formed:

a) during the oxidation or combustion of aluminum in air

4 Al + 3O 2 = 2Al 2 O 3

b) in the aluminothermic reaction

2 Al + Fe 2 O 3 = Al 2 O 3 + 2Fe

c) during the thermal decomposition of aluminum hydroxide 2 Al (OH) 3 = Al 2 O 3 + 3H 2 O

Aluminum hydroxide Al(OH) 3 :

White, water-insoluble powder.

Shows amphoteric properties , interacts :

A) with acids Al (OH) 3 + 3HCl = AlCl 3 + 3H 2 O

b) with alkalis Al (OH) 3 + Na OH = NaAlO 2 + 2H 2 O

Decomposes when heated 2Al (OH) 3 = Al 2 O 3 + 3H 2 O

Formed:

a) during the interaction of solutions of aluminum salts with solutions of alkalis (without excess)

Al 3+ + 3OH - = Al (OH) 3

b) when aluminates interact with acids (without excess)

AlO - 2 + H + + H 2 O = Al (OH) 3

Homework:

• 1) Using the presentation material and textbook, learn the properties of aluminum and its compounds.
• 2) Complete interactive tasks on the topic “Aluminium” on the lyceum website, write down the correct answers in your notebook.
• 3) Complete virtual practical work “Chemical properties of aluminum”, write it in a notebook.