Aluminum and its compounds presentation for a chemistry lesson (9th grade) on the topic. Presentation "aluminum and its compounds" famous sapphires of the English royal family

Aluminum and its compounds

I am irreplaceable metal, Much loved by the pilot, Lightweight, electrically conductive, And the character is transitional

Pliny Senior - ancient Roman writer - polymath.

There is a legend about how a stranger came to the Roman Emperor Tiberius. As a gift to the emperor, he brought a bowl he had made, made of a metal shiny like silver, but extremely light. The master said that he received this metal from “clay soil.” But the emperor, fearing that his gold and silver would depreciate, ordered the master’s head to be cut off and his workshop to be destroyed.

In the 19th century at imperial receptions -------- dishes was the most prestigious. Napoleon III once hosted a banquet at which especially honored guests were given ____ spoons and forks. The simpler guests were honored with the usual gold and silver cutlery for the imperial court. In addition, only the son of Napoleon III had an expensive ______________rattle for those times.”

D.I. Mendeleev

At the time of the discovery of this metal, it was more expensive than gold. The British, having decided to honor the great Russian chemist D.I. Mendeleev with a rich gift, presented him with chemical scales, in which one bowl was made of gold, and the other of ... A bowl made of this metal became more expensive than gold. The resulting “silver” from clay interested not only scientists, but also industrialists and even the Emperor of France

I am made of ordinary clay,

But I am extremely modern. I'm not afraid of electric shock I fly fearlessly in the air; I serve in the kitchen without a deadline - I can handle all the tasks. I am proud of my name: My name is...........

In the 1860s, every Parisian fashionista certainly had to have in her outfit at least one piece of jewelry made of aluminum - a metal valued higher than silver and gold

“This metal is destined for a great future.”

Chernyshevsky N. G.

He is important, that's for sure.

We absolutely need him.

Handsome silver, light,

Conducts current, ductile, malleable.

No wonder they call him winged,

Every person on the planet knows about him.

This metal evokes admiration,

And the unique properties are used.

Simple substance

Chemical element

Physical properties

Position in PTCE

History of discovery

Simple substance

Chemical element

Atomic structure

Chemical properties

Being in nature

Application

Receipt

2. Atomic mass (Ar)

a) serial number;

b) period number;

c) even or odd row;

d) group number;

d) subgroup.

4. Atomic structure:

a) nuclear charge;

b) core composition;

c) number of electronic layers;

d) total number of electrons (ē);

d) electronic configuration atom;

f) the number of electrons in the outer layer;

g) graphic representation of the outer layer; valence; oxidation state;

h) whether this layer is complete or not.

Aluminum - chemical element position in the periodic table and atomic structure

1. Chemical symbol (metal or non-metal)

2. Atomic mass (Ar)

3. Position of the element in the periodic table:

serial number;
period number;
even or odd row;
group number;
subgroup.

Al (metal)

Odd

A (main)

Aluminum - atomic structure

3 p

3 s

2 p

2 s

1 s

Brief email:

Aluminum

Oxidation state

Groups of elements

Restorative

Electrochemical voltage series of metals

Li, K, Ca, Na, Mg, Al , Cr, Zn, Fe, Co, Pb, H 2 ,Cu,Hg,Ag

Weakening of restorative properties

Al" width="640"

4. Atomic structure:

nuclear charge;
core composition;
number of electronic layers;
total number of electrons (ē);

electronic configuration of an atom;

number of electrons in the outer layer;

graphic representation of the outer layer; valence; oxidation state;

Whether this layer is complete or not.

5. Formulas of the higher oxide, its hydroxide, and their chemical characteristics.

6. Formulas of gaseous hydrogen compounds, if the element forms them.

7. The metallic or non-metallic properties of the element are most pronounced.

8. Comparison of the properties of a given element with the properties of neighboring elements by period and subgroup.

13p + , 14n 0

1s 2 2s 2 2p 6 3s 2 3p 1

Al 2 O 3 - amphoteric, Al (OH) 3 - amphoteric

Metal

Construction

Aluminum and its alloys are used in industrial and civil construction in the manufacture of building frames, trusses, window frames, stairs and other structures.

ALUMINUM IN ROCKET FUEL.

When aluminum burns in oxygen and fluorine, a lot of heat is released. Therefore, it is used as an additive to rocket fuel. The Saturn rocket burns 36 tons of aluminum powder during its flight. The idea of using metals as a component rocket fuel first stated by F.A. Tsander.

Carefully!!! Aluminum

Aluminum cookware, under the influence of boiling milk and boiled vegetables in microscopic doses, splits off from the container and safely penetrates into our stomach. So it is better to refrain from storing any food in aluminum appliances.

If cooking in such utensils takes place over many years, then, according to experts, a sufficient amount of aluminum accumulates in the body throughout this time, which can cause anemia, kidney, liver disease, and also provoke neurological disorders.

According to some studies, the intake of aluminum into the human body has been considered a factor in the development of the disease. Alzheimer's

Li K Ba Ca Na Mg Al Mn Cr Zn Fe Co Sn Pb H2 Cu Hg Au

Consider the electrochemical series of metals.

In what form (free or combined)

Is aluminum found in nature?

Being in nature

Aluminum is the most common element in nature; its content in the earth’s crust (8%) is in third place after oxygen and silicon.

Bauxite – Al 2 O 3 H 2 O

Nephelines – KNa 3 4

Alumina - Al 2 O 3

Ca 3 Al 2 (SiO 4) 3

Be 3 Al 2 Si 6 O 18

sapphire

ruby

AL 2 O 3

Alumina

Corundum

Bauxite

Use of sapphires and rubies

famous sapphires of the English royal family

D.I. Mendeleev

« aluminum is the most common in nature; it is enough to indicate that it is part of clay, so that the universal distribution of aluminum in the earth’s crust is clear. Aluminum or metal alum), which is why it is also called clay because it is found in clay.”

physical properties

Aluminum is a record holder in many respects. List them

Take an aluminum wire, examine it, try to change its shape. Based on observations and your life experiences, characterize the physical properties of aluminum and write them down. If you have any difficulties, place a question mark next to the corresponding property.

General physical properties:

1. state of aggregation;
2. color;
3. metallic luster;
4. smell;
5. plasticity;
6. electrical conductivity;
7. thermal conductivity;
8. solubility in water.

Individual physical properties:

9. density 2.698 g/cm 3
10. melting point 660.4 °C
11. boiling point 2466.9 °C
12.Easy to process
13. forms light and strong alloys

E T O V A G N O

The combination of these properties allows us to classify aluminum as one of the most important technical materials

Aluminum as a simple substance chemical properties

If the surface of aluminum is rubbed with mercury salt, the following reaction occurs:

2Al + 3HgCl2 = 2AlCl3 + 3Hg

The released mercury dissolves the aluminum, forming an amalgam.

Chemical properties

interaction with simple substances

loose powder

stripped of protective film

+3O 2

aluminum oxide

+3Cl 2

aluminum chloride

t 200 +3S

aluminum sulfide

t 500 +P

aluminum phosphide

t 800 +N 2

aluminum nitride

+H 2

interaction with water

If, in the absence of air, the oxide film is removed from the surface of aluminum, it reacts actively with water.

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

Chemical properties

interaction with complex substances

2. Easily interacts with diluted acids

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

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

8Al + 30HNO 3 = 8Al(NO 3 ) 3 +3N 2 O+15H 2 O

(as a product of the reduction of nitric acid

may also be nitrogen and ammonium nitrate)

3. Concentrated sulfuric and nitric acids passivate aluminum (a dense oxide film is formed), the reaction occurs when heated.

2Al + 6H 2 SO 4 = Al 2 (SO 4 ) 3 +3SO 2 + 6H 2 O

Al + 6HNO 3 = Al(NO 3 ) 3 +3NO 2 + 3H 2 O

interaction with alkalis

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

1. 2NaOH + Al 2 O 3 + 3H 2 O=2Na

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

3. NaOH + Al(OH) 3 =Na

CHEMICAL CHAMELEON

AlCl 3 +3NaOH= Al(OH) 3 +3NaCl

The sediment disappears

Reacts like an acid

Reacts as a base

Amphoteric hydroxide

As a base:

Al(OH) 3 + 3HCl ® AlCl 3 + 3H 2 O

Like acid

Al(OH) 3 + NaOH ® Na

As an insoluble hydroxide

2Al(OH) 3 – t° ® Al 2 O 3 + 3H 2 O

Gel from aluminum hydroxide is part of a medicine for the treatment of stomach diseases.

Aluminum hydroxide used for water purification because it has the ability to absorb various substances.

Aluminum oxide in the form of corundum it is used as a forming material for processing metal products.

Aluminum oxide in the form of ruby, it is widely used in laser technology.

Aluminum oxide used as a catalyst for the separation of substances in chromatography.

Aluminum chloride AlCl3 is a catalyst in the production of organic substances.

Aluminum salts

Insoluble in water:

Soluble in water

phosphates

Decomposed by water: sulfites, sulfides

Al 2 S 3 + 6H 2 O → 2Al(OH) 3 ↓ + 3H 2 S

Salts of unstable aluminum acids - orthoaluminum N 3 AlO 3 and meta-aluminum НAlO 2 called aluminates

Natural aluminates : noble spinel And precious chrysoberyl

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

Aluminum

“He will light up like a bright star, White and light metal, In the 13th cell of the table He took a place of honor. For ease of alloys it is given, He created the power of airplanes. Ductile and plastic, excellent forging This metal is silver. Composed of crimson rubies, In the sapphire blue lights, In gray ordinary clay In the form of sandstones, I see metal everywhere In a distinct cage of lines. The age of the lightest metals is coming Our wonderful metal."

THIS IS INTERESTING:

Aluminum will also find its place in the production of new so-called "smart" clothes . Manufacturers have already created fabric coated with a thin layer of this metal, which is called aluminized fabric.

With interesting properties such as sequential warming and cooling, it can

be applied in various fields.

For example, if there are curtains made of this fabric hanging on the window, they will reflect heat rays on hot days, but will let light through. This way the room will be cool and light. In winter, the curtains can be turned with the metal side facing the room, this will return heat to the room. This fabric can be considered universal - the owner of a raincoat made from it need not fear either heat or cold. In this case, depending on the weather, the raincoat must be turned one way or another.

Which of the compounds will react with aluminum:

Cl 2

K 2 O

CuSO 4

H 2 O

BaSO 4

HCL

Fe 2 O 3

Using the diagram, write the equations for reactions 1 - 9

Al 2 (SO 4 ) 3

Al 2 O 3

Al(OH) 3

H 3 AlO 3

Aluminum – position in PTCE

Characteristic

First received in 1825 Hans Oersted.

In the Periodic Table it is located in the 3rd period,

Found in nature only in the form of connections.

IIIA-group .

Silver-white, light metal. Has high thermal and electrical conductivity.

Danish physicist Hans Oersted () He first obtained aluminum in 1825 by the action of potassium amalgam on aluminum chloride followed by distillation of mercury.

Modern production of aluminum The modern production method was developed independently of each other: by the American Charles Hall and the Frenchman Paul Héroux in 1886. It consists of dissolving aluminum oxide in molten cryolite, followed by electrolysis using consumable coke or graphite electrodes.

As a student at Oberlin College, he learned that he could become rich and gain the gratitude of humanity if he could invent a way to produce aluminum on an industrial scale. Like a man possessed, Charles experimented with producing aluminum by electrolysis of cryolite-alumina melt. On February 23, 1886, a year after graduating from college, Charles produced the first aluminum using electrolysis. Charles Hall (1863 – 1914) American chemical engineer

Paul Héroux () - French chemical engineer In 1889, he opened an aluminum plant in Front (France), becoming its director, he designed an electric arc furnace for steel smelting, named after him; he also developed an electrolytic method for obtaining aluminum alloys

Found in nature The most important aluminum mineral today is bauxite. The main chemical component of bauxite is alumina (Al 2 O 3) (%).

Physical properties soft light (with low density - 2.7 g/cm 3) with high thermal and electrical conductivity fusible (melting point 660 ° C) silver-white with a characteristic metallic luster Occupies 1st place in the earth's crust among metals The combination of these important properties allows us to classify aluminum as one of the most important technical materials E T O V A N O:

With sulfur, forming aluminum sulfide: 2Al + 3S = Al 2 S 3 with nitrogen, forming aluminum nitride: 2Al + N 2 = 2AlN with carbon, forming aluminum carbide: 4Al + 3C = Al 4 C 3 with chlorine, forming aluminum chloride: 2Al + 3Cl 2 = 2AlCl 3 Chemical properties with oxygen, forming aluminum oxide: 4Al + 3O 2 = 2Al 2 O 3 Interaction with simple substances:

Chemical properties 1. with water (after removing the protective oxide film) 2Al + 6H 2 O = 2Al(OH) 3 + 3H 2 2. with alkali solutions (with the formation of tetrahydroxoaluminate) 2Al + 2NaOH + 6H 2 O = 2Na + 3H 2 3 . with hydrochloric and dilute sulfuric acids: 2Al + 6HCl = 2AlCl 3 + 3H 2 2Al + 3H 2 SO 4 (diluted) = Al 2 (SO 4) 3 + 3H 2 4. with oxides of less active metals (aluminothermy) 8Al + 3Fe 3 O 4 = 4Al 2 O 3 + 9Fe 2Al + Cr 2 O 3 = Al 2 O 3 + 2Cr Interaction with complex substances:

Fill in the missing words in the text: Test yourself: Aluminum is a metal whose compounds have equal oxidation states. In nature it occurs in the form. +3 aluminum oxide Aluminum can react with to form aluminum hydroxide, which has. amphoteric water Aluminum reacts to reduce less active metals from their aluminothermic oxides
Links to sources of information and images: G.E. Rudzitis, F.G. Feldman - Chemistry 9th grade

Continue to form ideas about the chemical element and simple substance aluminum, its occurrence in nature; atomic structure, physical and chemical properties, use of aluminum and its alloys. Improve the ability to write equations of chemical reactions that characterize the chemical properties of aluminum, the features of its interaction with alkalis. Continue developing ideas about amphotericity using the example of aluminum oxide and hydroxide and the use of aluminum compounds. Develop and improve the ability to write equations in molecular, full and abbreviated ionic forms. Improve experimental skills using the example of proving the amphoteric nature of aluminum hydroxide.

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"Presentation for the lesson "Aluminum and its compounds""

Aluminum and its connections

Position in the Periodic Table

Aluminum is located in period 3, in group IIIA.
Element serial number – 13
Relative atomic mass – 27
Aluminum is a metal whose compounds have amphoteric properties.

Structure of the aluminum atom

Charge of the nucleus of an aluminum atom +13
There are 3 energy levels in an atom
The electron shell of the aluminum atom contains

s- and p-electrons

On the outside electronic level 3 electrons (2 – paired s-electrons and 1 – unpaired p-electron)

Being in nature

In terms of abundance in the earth's crust, aluminum ranks 3rd after oxygen and silicon among all atoms and 1st among metals. Found only in compounds.

Aluminum production

Aluminum was first obtained by the Danish physicist Hans Oersted in 1825 by the action of potassium amalgam on aluminum chloride followed by distillation of mercury. The name of the element is derived from Lat. aluminis - alum .

AlCl 3 + 3K = 3KCl + Al

Currently, aluminum is produced by electrolysis of the oxide:

2Al 2 O 3 = 4Al + 3O 2 – 3352 kJ

Physical properties

density (at 20°C) 2698.9 kg/m3;
t pl 660.24°C;
boiling point about 2500°C;

Aluminum combines a very valuable set of properties: low density, high thermal and electrical conductivity, high ductility and good corrosion resistance, and has high reflectivity, close to silver (it reflects up to 90% of incident light energy).

Chemical properties

Oxidizes in air :

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

3 O 2 0 + 4ē → 2O -2 reduction, oxidizing agent

Displaces hydrogen from water

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

4 Al 0 - 3 ē → Al +3 oxidation, reducing agent

3 2H +1 + 2ē → H 2 0 reduction, oxidizing agent

Chemical properties

Interacts with acids:

2Al + 6HCl = 2AlCl3 + 3H2

2Al + 6H + + 6Cl - = 2Al 3+ + 6Cl - + 3H 2

2Al + 6H + = 2Al 3+ + 3H 2

Interacts with alkalis:

2Al + 2H 2 O + 2NaOH = 2NaAlO 2 + 3H 2

2Al + 2H 2 O + 2Na + + 2OH - = 2Na + + 2AlO 2 - + 3H 2

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

Chemical properties

Displaces metals from their oxides

(aluminothermy):

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

8 Al 0 - 3 ē → Al +3 – oxidation, reducing agent

3 24 Fe +2 + 2ē → Fe 0 – reduction, ok

3 2Fe +3 + 6ē → 2Fe 0 – reduction, ok

Aluminum connections. Oxide

Very hard white powder.
Formed:

a) during the oxidation or combustion of aluminum:

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

b) in the aluminothermic reaction:

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

c) during thermal decomposition of hydroxide:

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

Chemical properties aluminum oxide

Al 2 O 3 is an amphoteric oxide in nature.

Interacts:

A) with acids:

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

Al 2 O 3 + 6H + + 3SO 4 2- = 2Al 3+ + 3SO 4 2- + 3H 2 O

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

b) with alkalis:

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

Al 2 O 3 + 6Na + + 6OH - = 6Na + + 2AlO 3 3- + 3H 2 O

Al 2 O 3 + 6OH - = 2AlO 3 3- + 3H 2 O

Aluminum hydroxide

White water-insoluble powder
Exhibits amphoteric properties.
Interacts:

A) with acids:

Al(OH) 3 + 3HNO 3 = Al(NO 3) 3 + 3H 2 O

Al(OH) 3 + 3H + + 3NO 3 - = Al 3+ + 3NO 3 - + 3H 2 O

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

b) with alkalis:

Al(OH) 3 + 3KOH = K 3 AlO 3 + 3H 2 O

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

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

Using the diagram, write the equations for reactions 1 - 9

Al 2 (SO 4 ) 3

Al 2 O 3

Al(OH) 3

H 3 AlO 3

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Slide captions:

Slide 1
Aluminum

Slide 2
13
Aluminum (lat. Aluminum)
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 well and electric current, 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 “Aluminum” on the lyceum website, write down the correct answers in a notebook.3) Complete a virtual practical work“Chemical properties of aluminum”, write it in a notebook.

On the topic: methodological developments, presentations and notes

This article is used in chemistry lessons when studying the topic “Metals”, it will broaden the horizons of students, and has a professional orientation....

...

These materials can be used by the student for independent study of the topic "Aluminum" and for organizing self-control....

1 slide

2 slide

General characteristics Aluminum is a lightweight and ductile white metal. Refers to III group periodic table, denoted by the symbol Al, has an atomic number of 13 and an atomic mass of 27. Its melting point is 660°. Aluminum is extremely common in nature: according to this parameter, it ranks 3rd among all elements and first among metals (8.8% of the mass of the earth’s crust), but is not found in its pure form.

3 slide

The most important aluminum mineral today is bauxite. The main chemical component of bauxite is alumina (Al2O3) (28-80%) In terms of abundance in the Earth's crust, it ranks 1st among metals and 3rd among elements, second only to oxygen and silicon. Mass concentration aluminum in the earth's crust, according to various researchers, is estimated from 7.45 to 8.14%

4 slide

Physical properties soft light (low density - 2.7 g/cm3) with high thermal and electrical conductivity fusible (melting point 660°C) silver-white with a characteristic metallic luster

5 slide

Aluminum restores all the elements to the right of it in the electrochemical voltage series of metals; simple substances are non-metals. From complex compounds, aluminum reduces hydrogen ions and ions of less active metals. However, at room temperature in air, aluminum does not change, since its surface is covered with a protective oxide film.

6 slide

with sulfur, forming aluminum sulfide: 2Al + 3S = Al2S3 with nitrogen, forming aluminum nitride: 2Al + N2 = 2AlN with carbon, forming aluminum carbide: 4Al + 3C = Al4C3 with chlorine, forming aluminum chloride: 2Al + 3Cl2 = 2AlCl3 Chemical properties with oxygen, forming aluminum oxide: 4Al + 3O2 = 2Al2O3 Interaction with simple substances:

7 slide

8 slide

He first obtained aluminum in 1825 by the action of potassium amalgam on aluminum chloride followed by distillation of mercury. Danish physicist Hans Oersted (1777-1851) From the history of the discovery: During the discovery of aluminum, the metal was more expensive than gold. The British wanted to honor the great Russian chemist D.I. Mendeleev with a rich gift; they gave him chemical scales, in which one cup was made of gold, the other of aluminum. An aluminum cup has become more expensive than a gold one. The resulting “silver from clay” interested not only scientists, but also industrialists and even the Emperor of France.

Slide 9

Modern method The modern production method involves dissolving aluminum oxide in molten cryolite, followed by electrolysis using consumable coke or graphite electrodes.

Aluminum and its compounds presentation for a chemistry lesson (9th grade) on the topic. Presentation "aluminum and its compounds" famous sapphires of the English royal family

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On the topic: methodological developments, presentations and notes

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"Presentation for the lesson "Aluminum and its compounds""