Aluminum - general characteristics of the element, chemical properties. Adapter plates MA and AP for connecting aluminum buses to copper leads of electrical devices

II. LITERATURE REVIEW.

§ 1. DOUBLE SYSTEMS OF ELEMENTS IV - V GROUPS

WITH ALUMINUM.

1.1. Vehicle state diagram - A1.

1.2. The structure of the bx - A1 and NG - A1 binary systems.

1.3. The structure of the state diagram of the double system Lb - A1.

§ 2. THE STRUCTURE OF BINARY SYSTEMS M - N (M = A1, TC, bx, w, bb).

2.1. State diagram A1 - N.

2.2. Vehicle state diagram - N.

2.3. State diagrams of binary systems bx - N and NG - N.

2.4. State diagram Lb - N.

2.5. Physico- Chemical properties and methods for the synthesis of nitrides.

§ 3. STRUCTURE OF TRIPLE STATE DIAGRAMS M - A1 - N

M = TC, bx, H £ bh).

3.1. Vehicle state diagram - A1 - N.

3.2. State diagrams bx - A1 - N and NG - A1 - N.

3.3. State diagram N1) - A1 - N.

III. EXPERIMENTAL PART

§ 1. TECHNIQUE FOR PREPARING SAMPLES.

§2. SAMPLE RESEARCH TECHNIQUE.

2.1. Electron Probe Microanalysis (EZMA).

2.2. Scanning Electron Microscopy (SEM).

2.3. Optical microscopy.

2.4. X-ray phase analysis.

§ 3 DEVELOPMENT OF A METHOD FOR STUDYING PHASE DIAGRAMS

WITH NITROGEN PARTICIPATION.

IV. RESULTS AND DISCUSSION.

§ 1. PHASE BALANCES IN THE T1 - A1 - N SYSTEM.

§ 2. CONDITIONS FOR EQUILIBRIUM OF THE PHASES IN THE SYSTEM bx - A1 - N.

§ 3. STRUCTURE OF THE STATE DIAGRAM OF THE SYSTEM Ш - А1 - N. dd

§ 4. PHASE BALANCES IN THE L - A1 - N SYSTEM.

Recommended list of dissertations

Interaction of alloys based on iron, nickel and elements of IV-VI groups with nitrogen at increased partial pressure 1999, candidate of chemical sciences Abramycheva, Natalia Leonidovna
Phase equilibria in M-M "-N systems at elevated pressure 2001, candidate of chemical sciences Vyunitskiy, Ivan Viktorovich
Decomposition of carbide zirconium-niobium solid solutions and segregation of the ZrC phase in the ternary system Zr - Nb - C 2002, candidate of physical and mathematical sciences Rempel, Svetlana Vasilievna
Modeling the processes of internal nitriding of heat-resistant steels and alloys 2001, Doctor of Technical Sciences Petrova, Larisa Georgievna
Interaction of elements in compositions of refractory metals with heat-resistant alloys based on nickel and iron 1999, candidate of chemical sciences Kerimov, Elshat Yusifovich

Dissertation introduction (part of the abstract) on the topic "Phase equilibria in nitrogen-aluminum-transition metal systems of IV-V groups"

Ceramic materials based on double aluminum nitrides and Group IV elements are widely used in different areas industry and technology. In microelectronics, it is generally accepted to use substrates made of aluminum nitride, which has a unique combination of high parameters: heat resistance, electrical resistance, and thermal conductivity. Due to its resistance to metallic melts, titanium nitride is promising for metallurgy. Zirconium nitride is an essential component of nitride nuclear fuel in fast breeder reactors.

At present, considerable interest is being paid to the development of various composite materials based on aluminum nitride in combination with nitrides of transition metals of groups IV - V. In particular, an important role in the development of microelectronics is assigned to a multilayer material consisting of A1N and NbN layers. No less promising for the creation of wear-resistant and protective coatings, diffusion barriers in microelectronics, high-temperature ceramic, cermet, composite materials are Ti - Al - N and Zr - Al - N alloys. Determination of the phase composition of this kind of materials showed the presence of only double nitride phases. Nevertheless, recent, thorough studies of M - Al - N alloys (hereinafter M = Ti, Zr, Hf, Nb) have revealed the existence of complex nitrides: Ti3AlN, TÎ2A1N, Ti3Al2N2; Zr3AlN, ZrsAbNj.x; Hf3AlN, Hf5Al3N; Nb3Al2N. Their properties are practically unexplored, although there is good reason to believe that they may be unique. This is evidenced by the fact that composite materials based on a combination of A1 and M double nitrides have the maximum level of physical characteristics precisely in the regions of ternary phase compositions. For example, the abrasive properties of the Ti - Al - N ternary compounds are two times higher than that of corundum and even than that of tungsten carbide.

Compounds of A1 and elements of groups IV-V with nitrogen play an equally important role in the design and production of a wide range of steel grades and alloys, especially with an increased nitrogen content. Naturally, the physical, physicochemical, and mechanical properties of the listed materials are directly related to the type and amount of nitrogen-containing phases formed. Accurate data on the composition and conditions of existence of complex compounds are also of fundamental theoretical importance for understanding the nature of chemical bonds and other key characteristics that determine the degree of their stability. To predict the synthesis conditions and stability of nitrides, reliable information on phase equilibria is required. The construction of multicomponent phase diagrams with the participation of nitrogen is a very difficult task due to the low thermodynamic stimuli for the formation of mixed compounds from binary phases adjacent in the phase diagram, low diffusion rates of components in them, as well as the complexity and low accuracy of determining the true nitrogen content. Therefore, the currently available information is fragmentary and extremely contradictory both in the composition of ternary nitrides and in the position of the phase equilibrium lines. It was mainly obtained by one group of researchers by the method of annealing of powder-like compacts, in which it is difficult to achieve an equilibrium state of the alloy.

GOAL OF THE WORK:

Development of a new approach to the study of state diagrams of multicomponent nitride systems, based on the use of a complex of modern experimental techniques of physicochemical analysis, methods of thermodynamic analysis and calculation, which makes it possible to determine with high accuracy the conditions for the coexistence of phases and obtain comprehensive evidence of their correspondence to equilibrium. Study of phase equilibria in the solid-phase region of ternary systems aluminum - nitrogen - metal of IV - V groups at a temperature of 1273 K.

SCIENTIFIC NOVELTY:

Methods of thermodynamic analysis and calculation have shown the inconsistency of the available experimental data on the conditions of phase equilibrium in the systems T1-A1-Nyrr-A1-K;

A method for studying the phase diagrams of nitride systems has been developed, which is based on a complex of modern methods of physicochemical analysis and the implementation of different ways to achieve the same final state of the alloy, which makes it possible to obtain exhaustive evidence of compliance with its equilibrium;

Thermodynamic modeling, analysis and calculation of phase equilibria in the systems bx - A1 - N and NG - A1 - N have been carried out. For the first time, the thermodynamic functions of ternary compounds formed in these systems have been found;

Solid-phase regions of the state diagrams of the P - A1 - N systems are constructed.

A1-N and NG-A1-N at 1273 K; The character of phase equilibria in the Lb - A1 - N system at a temperature of 1273 K.

SCIENTIFIC AND PRACTICAL IMPORTANCE OF THE WORK:

The obtained information on the equilibrium conditions and thermodynamic functions of the phases in the M - A1 - N systems (M = T1, bx, H £ Lb) are the fundamental scientific basis for the development of coatings, ceramic and cermet, composite materials important for microelectronics, power engineering, mechanical engineering. ... They make it possible to determine the technological parameters for the production and processing of such materials, and are also of fundamental importance for predicting the phase composition and properties of a wide range of steels and alloys with an increased nitrogen content.

RELIABILITY AND JUSTIFICATION:

Data obtained by different methods of physicochemical analysis on samples of alloys synthesized different ways(nitriding of binary alloys, prolonged homogenizing annealing, diffusion vapors), using modern experimental approaches and equipment, such as electron probe microanalysis, scanning electron microscopy, X-ray phase analysis, in all cases were in excellent agreement both with each other and with the results of thermodynamic calculation.

THE FOLLOWING PROVISIONS ARE MADE TO PROTECT:

1. A technique for constructing state diagrams of multicomponent nitride systems based on a combination of a complex of modern methods of physicochemical analysis with different ways to achieve the same equilibria, thermodynamic modeling and calculation of phase equilibria.

2. The structure of the solid-phase region of the isothermal section of the A - A1 - N phase diagram at a temperature of 1273 K.

3. Results of thermodynamic analysis and calculation of phase equilibria in the T - A1 - N system at 1273 and 1573 K.

4. The structure of the solid-phase regions of the state diagrams of the systems Zr - A1 - N. NG - A1 - N. N1) - A1 - N at 1273 K.

II. LITERATURE REVIEW

Similar dissertations in the specialty "Physics of Condensed Matter", 01.04.07 code VAK

Phase equilibria and directional synthesis of solid solutions in ternary semiconductor systems with two volatile components 1998, Doctor of Chemistry Semenova, Galina Vladimirovna
Quasicrystalline phases in the systems Al-Mn-Si, Al-Cu-Fe, Al-Cu-Co: conditions of existence, structure, properties 2012, candidate of chemical sciences Kazyonnov, Nikita Vladimirovich
Calculation of multicomponent phase diagrams and their use for the development of alloys and improvement of their processing technology 2001, Doctor of Technical Sciences Smagulov, Dauletkhan Uyalovich
Synthesis of nitrides of elements of III-VI groups and composite materials based on them by nitriding of ferroalloys in combustion mode 2009, Doctor of Technical Sciences Chukhlomina, Lyudmila Nikolaevna
Thermodynamics of phase equilibria in metal alloys containing carbon 2001, candidate of chemical sciences Kachurina, Olga Ivanovna

Conclusion of the thesis on the topic "Physics of Condensed Matter", Han Yu Xing

Vi. conclusions.

1. A technique has been developed for studying the phase diagrams of multicomponent nitride systems based on a combination of methods for nitriding binary alloys, prolonged homogenizing annealing of three-component compositions, diffusion pairs, thermodynamic calculation and modeling of phase equilibria. It allows you to implement different ways to achieve the same final state of the alloy and to obtain comprehensive evidence of compliance with its equilibrium. It was found that when studying the regions of phase diagrams with high nitrogen concentrations, the most reliable and informative method is the nitriding of binary alloys. At low nitrogen concentrations, the diffusion vapor method gives the best results.

2.Using modern approaches For thermodynamic calculation and modeling of phase equilibrium conditions, the analysis of the existing data on the state diagrams of the M-A1-I systems is carried out. Their inconsistency is revealed and the ways of optimal formulation of experimental research are determined.

3. Using a complex of modern methods of physicochemical analysis, the regularities of the interaction of elements in 85 samples of binary and ternary alloys of the M-A1-N systems have been studied.

4. A solid-phase diagram of the state of the T1-A1-K system at 1273 K was constructed. It was found that aluminum nitride is in equilibrium with the phases IA1s, NrAS and TO ^. * a (P) and The crystal lattice parameters of the ternary phases T12ASh (a = 2.986 (9) A, c = 13.622 (5) A), T1sASh (a = 4.1127 (17) A), and the Gibbs energy of their formation modifications of elements stable at this temperature: -360.0 kJ / mol and -323.3 kJ / mol, respectively.

5. Phase equilibria in crystalline alloys at 1273 K have been investigated. The position of all regions of three-phase equilibria has been reliably established. Aluminum nitride is in equilibrium with the 2rA1s, ZtA \ 2 and ZrN phases. The triple phase yszAN forms fields of three-phase equilibria with phases

ZrsAbNi.x and a (Zr) based solid solution. The lattice parameters of the complex nitride Z ^ AIN are q = 3.366 (6) A, "= 11.472 (10) A, c = 8.966 (9) A, the Gibbs energy of formation is A / 3 = -380.0 kJ / mol.

6. It was found that in solid compositions of the Hf-Al-N system at 1273K, practically all binary phases of the Hf-Al system are in equilibrium with hafnium nitride HfN. The ternary compound Hf ^ AlN forms regions of three-phase equilibria with the phases HfsAh, HfN and a solid solution based on a (Hf). Double phases Hf2Al, ^ N2 are realized only in limited regions of compositions of the ternary system. Aluminum nitride is in equilibrium with H £ A13 and HfN.

7. For the first time, the isothermal T = 1273 K cross-section of the solid-phase part of the state diagram of the Nb-Al-N system was constructed. The ternary compound Nl ^ AhN is in equilibrium with the phases AIN, NbAb, NbAb and Nb2N. The Nb3Al-based phase and the niobium-based solid solution form a three-phase field with Nb2N. Niobium nitride NbN is in equilibrium with aluminum nitride and Nb2N.

V. CONCLUSION.

A general regularity in the structure of the state diagrams of the studied M - Al - N systems is a decrease in the number and stability of complex nitride phases with an increase in the difference between the thermodynamic stability of the double phases MN and A1N, which is characterized by the Gibbs energy of formation Zl / 7 (A1N) = - 180.0 kJ / mol, Zl / 7 (TiN) = - 217.8 kJ / mol, 4G (ZrN) = - 246.4 kJ / mol, ZlyG (HfN) -251.0 kJ / mol, zl / 7 (NbN) = -110.7 kJ / mol. So in the systems Ti - Al - N and Zr - Al - N at 1273 K there are two complex nitrides TijAIN, Ti2AlN and Z ^ AIN, ZrsAbNi-x, respectively. Moreover, at high temperatures in Ti - Al - N alloys, the TÎ4A1N3.X phase is stable, and the ZrsAbNi- * compound cannot be considered ternary, since it is isostructural to the ZrsAb intermetallic compound. On the phase diagrams of Hf - Al - N and Nb - Al - N, there is only one complex compound Hf3AlN and Nb3Al2N, respectively.

In the Ti - Al - N and Nb - Al - N systems, aluminum nitride is in equilibrium with the corresponding complex nitride, titanium or niobium nitrides and titanium or niobium aluminides with the maximum aluminum concentration. In systems with zirconium and hafnium, the AIN - M3AIN equilibrium disappears. This is caused by an increase in the thermodynamic stability of the double nitride phases ZrN and HfN. Thus, the prediction of the possibility of obtaining three-component nitride phases, including in steels and alloys, can be carried out by comparing the values of the Gibbs energies of formation of A1N and MN.

The performed studies allowed to develop a technique for the adequate construction of state diagrams of multicomponent nitrogen-containing systems and to establish the following regularities. At high concentrations of nitrogen and aluminum, the most informative is the method of nitriding powders of double metal alloys at an increased nitrogen pressure. It was found that the optimal pressure is several tens of atmospheres.

In alloys based on transition metals and with a low nitrogen content, the best results are obtained by methods of prolonged homogenizing annealing and diffusion pairs. A distinctive feature of the latter is the ability to obtain a large array of data on the conditions of phase equilibrium in the study of one sample. The commonly used method of annealing powder compacts requires a long isothermal holding and at temperatures below 1473 - 1573 K, in many cases, does not allow reaching an equilibrium state of the alloy.

Experimental research phase equilibria in alloys with a low nitrogen content in many cases is difficult or even impossible due to the low accuracy of determining its concentration by existing methods. For such sections of state diagrams, it is effective to use the methods of thermodynamic modeling and calculation of phase equilibria. They, based on the data on the conditions of phase equilibrium found for the more experimentally accessible sections of the phase diagram and the available information on thermodynamic functions, make it possible to unambiguously establish the missing information. When solving the problem, the corresponding system of equations, as a rule, turns out to be overdetermined; therefore, the calculation not only makes it possible to establish the position of the equilibrium lines, but also to obtain comprehensive evidence of the adequacy of the solution. So, when carrying out thermodynamic calculations for all studied systems, the result did not depend on which experimentally found phase fields were used as initial data.

Another important direction in the use of thermodynamic modeling and calculation is to predict the conditions of the experiment and the choice of the initial compositions of the samples in such a way as to achieve the same final state of the alloy in different ways and to prove its compliance with equilibrium.

In the present work, using a complex of modern methods of physicochemical analysis, four isothermal sections of the state diagrams of the T1 - A1 - N ternary systems are constructed. an approach based on the implementation of different paths to achieve the same final state of the alloy is consistently applied. The data found using various techniques are in good agreement both with each other and with the results of thermodynamic analysis; therefore, they can be recommended for predicting phase equilibria in these systems and compositions based on them.

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200. Khan Yu.S., Kalmykov K.B., Zaitsev A.I., Dunaev S.F. Phase equilibria in the Zr-Al-N system at 1273 K. // Metals. 2004. Vol. 5, p. 54-63.

201. Khan Yu Sin, Kalmykov K.B., Dunaev S.F. Interaction of aluminum nitride with group IV B elements. // International conference of students and graduate students on fundamental sciences "Lomonosov-2003". April 15-18, 2003 section Chemistry. Vol.2, p.244.

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/ Copper-aluminum adapter plate MA

Copper-aluminum transition plates GOST 19357-81 are used to connect aluminum buses to copper leads of electrical devices and copper buses. The connection with aluminum busbars is welded, the connection with copper leads of electrical devices and copper busbars is either collapsible (bolted) or welded.

Type of climatic modification of the MA plate - UHL1 and T1 in accordance with GOST 19357-81... The connection of the aluminum part of the MA plate with the copper one is performed by cold pressure welding.

We will make MA adapter plates in any quantity and in the shortest possible time

An example of a conventional designation of a transitional copper-aluminum plate of the UHL1 version:

Transitional plate MA 40х4 UHL1 GOST 19357-81
Transitional plate MA 50x6 UHL1 GOST 19357-81
Transitional plate MA 60x8 UHL1 GOST 19357-81
Transitional plate MA 80x8 UHL1 GOST 19357-81
Transitional plate MA 100x10 UHL1 GOST 19357-81
Transitional plate MA 120x10 UHL1 GOST 19357-81

Plates are made in accordance with the requirements of this standard according to working drawings, approved in the prescribed manner. The surface of MA platinum has no burrs, cracks, scuffs, metal flaking and other mechanical damage. Checking the quality of the weld, the surface of the MA plate is carried out visually.

Specifications - copper-aluminum adapter plate MA

plates MA 40x4, MA 50x6, M 60x8, M 80x8, MA100x10, MA120x10

Plate type	MA plate dimensions, mm			Weight, no more, kg
Plate type		copper part, I	thickness, S	Weight, no more, kg
Transitional plate MA 40 x 4
Adapter plate MA 50 x 6
Transitional plate MA 60 x 8
Adapter plate MA 80 x 8
Adapter plate MA 100 x 10
Adapter plate MA 120 x 10

Copper-aluminum adapter plates are designed for connecting aluminum busbars to copper leads of various electrical devices, as well as to copper busbars.

Copper-aluminum transition plates have welded joints with an aluminum bus, as well as collapsible (bolted) with copper leads. The plates themselves are made by the method of the so-called resistance welding or cold pressure welding.

Copper-aluminum transition plates are normalized in full compliance with the state standard, namely standard 19357-81. According to him, such plates are divided into the following types:

with equal section with welded joint for CIP tires;
clad and of equal size in terms of their electrical conductivity for collapsible tires.

As for the connecting seam of the adapter plate, which takes place when the copper plate is connected to the aluminum one, it must be cleaned of sludge and burr. Moreover, it should be performed without any cracks or fistulas. Transitional copper-aluminum plates should not have any mechanical damage on their surface, for example, burrs, scuffs, peeling, cracks.

In accordance with the state standard, namely standard 10434-82, protective metal coatings are required on the copper area of the plate. Although, if the transition plates are made in accordance with certain climatic conditions according to the state standard 15150-69 execution "T", then they just do not have such coatings.

According to special technical requirements, the copper-aluminum transition plates must be aligned to their original position when bent at eighteen degrees. As for the welded joint of the adapter plate, it must fully comply with state standard 10434-82. The service life of such a product as copper-aluminum transition plates can in no way be less than similar indicators for the entire electrical device where they are used.

Checking of such plates for compliance with the state standard 19357-81 is carried out upon acceptance by the manufacturer, delivery, as well as in accordance with type and periodic tests. Such tests are carried out on a random sample. If the test results are unsatisfactory, take twice the number of plates from the same batch and test again. If the result is repeated, then the entire batch is usually deemed unsuitable.

Lesson objectives: consider the distribution of aluminum in nature, its physical and chemical properties, as well as the properties of the compounds formed by it.

Progress

2. Learning new material. Aluminum

Main subgroup III group of the periodic table are boron (B), aluminum (Al), gallium (Ga), indium (In) and thallium (Tl).

As can be seen from the data presented, all these elements were discovered in the 19th century.

Discovery of metals of the main subgroup III group


1806 g.	1825 g.	1875 g.	1863 g.	1861 g.
G. Lussac,	G.H. Oersted	L. de Boisbaudran	F. Reich,	W. Crookes
L. Thenar	(Denmark)	(France)	I. Richter	(England)
(France)			(Germany)

Boron is a non-metal. Aluminum is a transition metal, while gallium, indium and thallium are high grade metals. Thus, with an increase in the radii of atoms of elements of each group of the periodic table, the metallic properties of simple substances increase.

In this lecture, we will take a closer look at the properties of aluminum.

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MUNICIPAL BUDGETARY EDUCATIONAL INSTITUTION

GENERAL EDUCATIONAL SCHOOL number 81

Aluminum. The position of aluminum in the periodic table and the structure of its atom. Being in nature. Physical and chemical properties of aluminum.

chemistry teacher

MBOU OSH №81

2013

Lesson topic: Aluminum. The position of aluminum in the periodic table and the structure of its atom. Being in nature. Physical and chemical properties of aluminum.

Lesson objectives: consider the distribution of aluminum in nature, its physical and chemical properties, as well as the properties of the compounds formed by it.

Progress

1. Organizational moment of the lesson.

2. Learning new material. Aluminum

The main subgroup of group III of the periodic system is boron (B),aluminum (Al), gallium (Ga), indium (In) and thallium (Tl).

As can be seen from the data presented, all these elements were discovered in the 19th century.

Discovery of metals of the main subgroup of group III


1806 g.	1825 g.	1875 g.	1863 g.	1861 g.
G. Lussac,	G.H. Oersted	L. de Boisbaudran	F. Reich,	W. Crookes
L. Thenar	(Denmark)	(France)	I. Richter	(England)
(France)			(Germany)

In this lecture, we will take a closer look at the properties of aluminum.

1. The position of aluminum in the table of D. I. Mendeleev. Atomic structure, exhibited oxidation states.

The element aluminum is located in the III group, the main "A" subgroup, the 3rd period of the periodic system, serial number 13, relative atomic mass Ar (Al) = 27. Its neighbor on the left in the table is magnesium - a typical metal, and on the right - silicon - already a non-metal ... Consequently, aluminum must exhibit properties of some intermediate character and its compounds are amphoteric.

Al +13) 2) 8) 3, p - element,

Ground state

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

Excited state

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

Aluminum exhibits an oxidation state of +3 in compounds:

Al 0 - 3 e - → Al +3

2. Physical properties

Free aluminum is a silvery-white metal with high thermal and electrical conductivity. Melting point 650 O C. Aluminum has a low density (2.7 g / cm 3 ) - about three times less than that of iron or copper, and at the same time it is a strong metal.

3. Being in nature

In terms of prevalence in nature, it occupies1st among metals and 3rd among elements, second only to oxygen and silicon. The percentage of aluminum in earth crust according to various researchers it is from 7.45 to 8.14% of the mass of the earth's crust.

In nature, aluminum is found only in compounds(minerals).

Some of them:

Bauxite - Al 2 O 3 H 2 O (with admixtures of SiO 2, Fe 2 O 3, CaCO 3)

Nepheline - KNa 3 4

Alunites - KAl (SO 4) 2 2Al (OH) 3

Alumina (mixtures of kaolin with sand SiO 2, limestone CaCO 3, magnesite MgCO 3)

Corundum - Al 2 O 3

Feldspar (orthoclase) - K 2 O × Al 2 O 3 × 6SiO 2

Kaolinite - Al 2 O 3 × 2SiO 2 × 2H 2 O

Alunite - (Na, K) 2 SO 4 × Al 2 (SO 4) 3 × 4Al (OH) 3

Beryl - 3ВеО Al 2 О 3 6SiO 2

Bauxite
Al 2 O 3	Corundum
	Ruby
	Sapphire

4. Chemical properties of aluminum and its compounds

Aluminum easily interacts with oxygen under normal conditions and is covered with an oxide film (it gives a matte look).

Its thickness is 0.00001 mm, but thanks to it, aluminum does not corrode. To study the chemical properties of aluminum, the oxide film is removed. (Using sandpaper, or chemically: first, dipping into an alkali solution to remove the oxide film, and then into a solution of mercury salts to form an alloy of aluminum with mercury - amalgam).

I. Interaction with simple substances

Already at room temperature, aluminum actively reacts with all halogens, forming halides. When heated, it interacts with sulfur (200 ° C), nitrogen (800 ° C), phosphorus (500 ° C) and carbon (2000 ° C), with iodine in the presence of a catalyst - water:

2Аl + 3S = Аl 2 S 3 (aluminum sulfide),

2Аl + N 2 = 2АlN (aluminum nitride),

Al + P = AlP (aluminum phosphide),

4Аl + 3С = Аl 4 С 3 (aluminum carbide).

2 Al + 3 I 2 = 2 AlI 3 (aluminum iodide)

All these compounds are completely hydrolyzed to form aluminum hydroxide and, accordingly, hydrogen sulfide, ammonia, phosphine and methane:

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

Al 4 C 3 + 12H 2 O = 4Al (OH) 3 + 3CH 4

In the form of shavings or powder, it burns brightly in air, giving off a large amount of heat:

4Аl + 3O 2 = 2Аl 2 О 3 + 1676 kJ.

II. Interaction with complex substances

Interaction with water:

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

without oxide film

Interaction with metal oxides:

Aluminum is a good reducing agent, as it is one of the active metals. It is in the line of activity right after the alkaline earth metals. That's whyrestores metals from their oxides... Such a reaction - alumothermy - is used to obtain pure rare metals, such as tungsten, vanadium, etc.

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

Termite mixture Fe 3 O 4 and Al (powder) is also used in thermite welding.

Cr 2 O 3 + 2Al = 2Cr + Al 2 O 3

5interaction with acids:

With sulfuric acid solution: 2 Al + 3 H 2 SO 4 = Al 2 (SO 4) 3 + 3 H 2

Does not react with cold concentrated sulfuric and nitrogenous (passivates). Therefore, nitric acid is transported in aluminum tanks. When heated, aluminum is able to reduce these acids without the evolution of hydrogen:

2Аl + 6Н 2 SO 4 (conc) = Аl 2 (SO 4) 3 + 3SO 2 + 6Н 2 О,

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

Interaction with alkalis.

2 Al + 2 NaOH + 6 H 2 O = 2 NaAl (OH) 4 + 3 H 2

Na [Al (OH) 4] - sodium tetrahydroxoaluminate

At the suggestion of the chemist Gorbov, during the Russo-Japanese War, this reaction was used to produce hydrogen for balloons.

With salt solutions:

2Al + 3CuSO 4 = Al 2 (SO 4) 3 + 3Cu

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

2Al + 3HgCl 2 = 2AlCl 3 + 3Hg

The released mercury dissolves the aluminum to form an amalgam.

5. Application of aluminum and its compounds

The physical and chemical properties of aluminum have led to its widespread use in technology.The aviation industry is a large consumer of aluminum.: the plane is 2/3 composed of aluminum and its alloys. An airplane made of steel would be too heavy to carry far fewer passengers.Therefore, aluminum is called a winged metal.Cables and wires are made from aluminum: with the same electrical conductivity, their mass is 2 times less than that of the corresponding copper products.

Given the corrosion resistance of aluminum,make parts for devices and containers for nitric acid... Aluminum powder is the basis for the manufacture of silvery paint to protect iron products from corrosion, as well as to reflect heat rays with this paint they cover oil storage tanks and firefighters' suits.

Aluminum oxide is used to produce aluminum and also as a refractory material.

Aluminum hydroxide is the main component of the well-known drugs Maalox, Almagel, which lower the acidity of gastric juice.

Aluminum salts are highly hydrolyzed. This property is used in the process of water purification. Aluminum sulfate and a small amount of slaked lime are added to the water to be treated to neutralize the resulting acid. As a result, a bulk precipitate of aluminum hydroxide is released, which, when settling, carries away suspended particles of turbidity and bacteria.

Thus, aluminum sulfate is a coagulant.

6. Obtaining aluminum

1) The modern, cost-effective method of producing aluminum was invented by the American Hall and the Frenchman Eroux in 1886. It consists in the electrolysis of a solution of aluminum oxide in molten cryolite. Molten cryolite Na 3 AlF 6 dissolves Al 2 O 3, how water dissolves sugar. The electrolysis of the “solution” of alumina in molten cryolite occurs as if cryolite was only a solvent, and alumina was an electrolyte.

2Al 2 O 3 electric → 4Al + 3O 2

In the English Encyclopedia for Boys and Girls, an article about aluminum begins with the following words: “On February 23, 1886, a new metal age began in the history of civilization - the age of aluminum. On that day, Charles Hall, a 22-year-old chemist, came to his first teacher's laboratory with a dozen small balls of silvery-white aluminum in his hand and with the news that he had found a way to make this metal cheaply and in large quantities. ” Thus Hall became the founder of the American aluminum industry and the Anglo-Saxon national hero, as a man who made a great business out of science.

2) 2Al 2 O 3 + 3 C = 4 Al + 3 CO 2

IT IS INTERESTING:

Metallic aluminum was first isolated in 1825 by the Danish physicist Hans Christian Oersted. By passing gaseous chlorine through a layer of incandescent aluminum oxide mixed with coal, Oersted isolated aluminum chloride without the slightest trace of moisture. To restore metallic aluminum, Oersted needed to treat aluminum chloride with potassium amalgam. After 2 years, the German chemist Friedrich Wöller. He improved the method by replacing the potassium amalgam with pure potassium.
In the 18th and 19th centuries, aluminum was the main jewelry metal. In 1889, D.I. Mendeleev in London for his services in the development of chemistry was awarded a valuable gift - a balance made of gold and aluminum.
By 1855, the French scientist Saint-Clair Deville had developed a method for producing metallic aluminum on a technical scale. But the method was very expensive. Deville enjoyed the special patronage of Napoleon III, Emperor of France. As a sign of his devotion and gratitude, Deville made for Napoleon's son, the newborn prince, an exquisitely engraved rattle - the first "consumer goods" made of aluminum. Napoleon even intended to equip his guardsmen with aluminum cuirass, but the price turned out to be prohibitively high. At that time, 1 kg of aluminum cost 1000 marks, i.e. 5 times more expensive than silver. Only after the invention of the electrolytic process did aluminum become equal in cost to conventional metals.
Did you know that aluminum, entering the human body, causes a disorder of the nervous system. With its excess, metabolism is disturbed. And the protective agents are vitamin C, calcium compounds, zinc.
When aluminum burns in oxygen and fluorine, a lot of heat is generated. Therefore, it is used as an additive to rocket fuel. The Saturn rocket burns 36 tons of aluminum powder during the flight. The idea of using metals as a component of rocket fuel was first expressed by F. A. Tsander.

3. Consolidation of the studied material

# 1. For the production of aluminum from aluminum chloride, metallic calcium can be used as a reducing agent. Make an equation for a given chemical reaction, characterize this process using electronic balance.
Think! Why can't this reaction be carried out in aqueous solution?

# 2. Complete the chemical reaction equations:
Al + H 2 SO 4 (solution) ->
Al + CuCl 2 ->
Al + HNO 3 (conc) - t ->
Al + NaOH + H 2 O ->

No. 3. Solve the problem:
The aluminum-copper alloy was exposed to an excess of concentrated sodium hydroxide solution when heated. Emitted 2.24 liters of gas (n.o.). Calculate the percentage of the alloy if its total weight was 10 g?

4. Homework Slide 2

AL Element III (A) of the table group D.I. Mendeleev Element with ordinal number 13, its Element of the 3rd period The third most common in the earth's crust name is derived from lat. "Aluminis" - alum

Danish physicist Hans Oersted (1777-1851) For the first time, he obtained aluminum in 1825 by the action of potassium amalgam on aluminum chloride, followed by distillation of mercury.

Modern aluminum production Modern method receipt was developed independently by the American Charles Hall and the Frenchman Paul Héroux in 1886. It consists in dissolving aluminum oxide in a cryolite melt, followed by electrolysis using consumable coke or graphite electrodes.

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

Paul Héroux (1863-1914) - French chemical engineer. In 1889 he opened an aluminum plant in Frona (France), becoming its director, he designed an electric arc furnace for smelting steel, named after him; he also developed an electrolytic method for producing aluminum alloys

8 Aluminum 1. From the history of discovery Home Next In the period of discovery of aluminum - metal was more expensive than gold. The British wanted to honor the great Russian chemist D.I. Mendeleev with a rich gift, presented him with a chemical balance, 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. Further

9 Aluminum 7. Content in the earth's crust home Next

Finding in nature The most important aluminum mineral today is bauxite. The main chemical component of bauxite is alumina (Al 2 O 3) (28 - 80%).

11 Aluminum 4. Physical properties Color - silvery-white t pl. = 660 ° C. t bales ≈ 2450 ° C. Electrically conductive, thermally conductive Light, density ρ = 2.6989 g / cm 3 Soft, plastic. home Next

12 Aluminum 7. Finding in nature Bauxite - Al 2 O 3 Alumina - Al 2 O 3 home Next

13 Aluminum main Insert the missing words Aluminum is an element of the III group, the main subgroup. The charge of the nucleus of an aluminum atom is +13. There are 13 protons in the nucleus of an aluminum atom. There are 14 neutrons in the nucleus of an aluminum atom. An aluminum atom has 13 electrons. The aluminum atom has 3 energy levels. The electron shell has a structure of 2 e, 8e, 3e. At the outer level, there are 3 electrons in an atom. The oxidation state of an atom in compounds is +3. The simple substance aluminum is a metal. Aluminum oxide and hydroxide are amphoteric in nature. Further

14 Aluminum 3. The structure of a simple substance Metal Bond - metallic Crystal cell- metallic, cubic face-centered main More

15 Aluminum 2. Electronic structure 27 А l +13 0 2e 8e 3e P + = 13 n 0 = 14 e - = 13 1 s 2 2 s 2 2p 6 3s 2 3p 1 Short electronic record 1 s 2 2 s 2 2p 6 3s 2 3p 1 Order of filling home Next

16 Aluminum 6. Chemical properties 4А l + 3O 2 = 2Al 2 O 3 t 2Al + 3S = Al 2 S 3 C nonmetallam and (with oxygen, with sulfur) 2 А l + 3Cl 2 = 2AlCl 3 4Al + 3C = Al 4 C 3 C with non-metals (with halogens, with carbon) (Remove oxide film) 2 Al + 6 H 2 O = 2Al (OH) 2 + H 2 C water 2 Al + 6 HCl = 2AlCl 3 + H 2 2Al + 3H 2 SO 4 = Al 2 (SO 4) 3 + H 2 C to and with a lot and 2 Al + 6NaOH + 6H 2 O = 2Na 3 [Al (OH ) 6] + 3H 2 2Al + 2NaOH + 2H 2 O = 2NaAlO 2 + 3H 2 C about alka and 8Al + 3Fe 3 O 4 = 4Al 2 O 3 + 9Fe 2Al + WO 3 = Al 2 O 3 + WC o c i d a m i m et al lo v home Next

17 Aluminum 8. Obtaining 1825 H. Oersted: AlCl 3 + 3K = 3KCl + Al: Electrolysis (t pl. = 2050 ° C): 2Al 2 O 3 = 4 Al + 3O 2 Electrolysis (in the melt cryolite Na 3 AlF 6, t pl. ≈ 1000 ° С): 2Al 2 O 3 = 4 Al + 3O 2 main Further

Video tutorial 1: Inorganic chemistry. Metals: alkali, alkaline earth, aluminum

Video tutorial 2: Transition metals

Lecture: Typical chemical properties and production of simple substances - metals: alkali, alkaline earth, aluminum; transition elements (copper, zinc, chromium, iron)

Chemical properties of metals

All metals in chemical reactions manifest themselves as restorers. They easily part with valence electrons, oxidizing in the process. Let us recall that the more to the left the metal is located in the electrochemical series of tension, the more powerful a reducing agent it is. Therefore, the strongest is lithium, the weakest is gold and vice versa, gold is the strongest oxidizing agent, and lithium is the weakest.

Li → Rb → K → Ba → Sr → Ca → Na → Mg → Al → Mn → Cr → Zn → Fe → Cd → Co → Ni → Sn → Pb → H → Sb → Bi → Cu → Hg → Ag → Pd → Pt → Au

All metals displace other metals from the salt solution, i.e. restore them. Everything except alkaline and alkaline earth, as they interact with water. Metals located before H displace it from solutions of dilute acids, and they themselves dissolve in them.

Let's take a look at some of the general chemical properties of metals:

The interaction of metals with oxygen forms basic (CaO, Na 2 O, 2Li 2 O, etc.) or amphoteric (ZnO, Cr 2 O 3, Fe 2 O 3, etc.) oxides.
The interaction of metals with halogens (the main subgroup of group VII) forms hydrohalic acids (HF - hydrogen fluoride, HCl - hydrogen chloride, etc.).
The interaction of metals with non-metals forms salts (chlorides, sulfides, nitrides, etc.).
The interaction of metals with metals forms intermetallic compounds (MgB 2, NaSn, Fe 3 Ni, etc.).
The interaction of active metals with hydrogen forms hydrides (NaH, CaH 2, KH, etc.).
The interaction of alkali and alkaline earth metals with water forms alkalis (NaOH, Ca (OH) 2, Cu (OH) 2, etc.).
The interaction of metals (only those standing in the electrochemical series up to H) with acids forms salts (sulfates, nitrites, phosphates, etc.). It should be borne in mind that metals react with acids rather reluctantly, while they almost always interact with bases and salts. In order for the reaction of a metal with an acid to take place, it is necessary for the metal to be active and the acid to be strong.

Chemical properties of alkali metals

The following chemical elements belong to the group of alkali metals: lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), francium (Fr). Moving from top to bottom in group I of the Periodic Table, their atomic radii increase, which means that their metallic and reducing properties increase.

Consider the chemical properties of alkali metals:

They have no signs of amphotericity, since they have negative values of electrode potentials.
The strongest reducing agent of all metals.
The compounds exhibit only an oxidation state of +1.
By donating a single valence electron, the atoms of these chemical elements are converted into cations.
Form numerous ionic compounds.
Almost everyone dissolves in water.

Interaction of alkali metals with other elements:

1. With oxygen, forming individual compounds, so the oxide forms only lithium (Li 2 O), sodium forms peroxide (Na 2 O 2), and potassium, rubidium and cesium - superoxides (KO 2, RbO 2, CsO 2).

2. With water, forming alkalis and hydrogen. Remember, these reactions are explosive. Only lithium reacts with water without explosion:

2Li + 2Н 2 О → 2LiO Н + Н 2.

3. With halogens, forming halides (NaCl - sodium chloride, NaBr - sodium bromide, NaI - sodium iodide, etc.).

4. With hydrogen when heated, forming hydrides (LiH, NaH, etc.)

5. With sulfur when heated, forming sulfides (Na 2 S, K 2 S, etc.). They are colorless and readily soluble in water.

6. With phosphorus when heated, forming phosphides (Na 3 P, Li 3 P, etc.), they are very sensitive to moisture and air.

7. With carbon, when heated, carbides form only lithium and sodium (Li 2 CO 3, Na 2 CO 3), while potassium, rubidium and cesium do not form carbides, they form binary compounds with graphite (C 8 Rb, C 8 Cs, etc.) ...

8. Under normal conditions, only lithium reacts with nitrogen, forming nitride Li 3 N, with the rest of the alkali metals, the reaction is possible only when heated.

9. They react with acids explosively, therefore carrying out such reactions is very dangerous. These reactions are ambiguous, because the alkali metal actively reacts with water, forming an alkali, which is then neutralized with an acid. This creates competition between alkali and acid.

10. With ammonia, forming amides - analogs of hydroxides, but stronger bases (NaNH 2 - sodium amide, KNH 2 - potassium amide, etc.).

11. With alcohols, forming alcoholates.

Francium is a radioactive alkali metal, one of the rarest and least stable among all radioactive elements. Its chemical properties are not well understood.

Getting alkali metals:

To obtain alkali metals, electrolysis of melts of their halides is mainly used, most often chlorides, which form natural minerals:

NaCl → 2Na + Cl 2.

There are other ways to get alkali metals:
Sodium can also be obtained by calcining soda and coal in closed crucibles:

Na 2 CO 3 + 2C → 2Na + 3CO.

A known method for producing lithium from its oxide in vacuum at 300 ° C:

2Li 2 O + Si + 2CaO → 4Li + Ca 2 SiO 4.

Potassium is obtained by passing sodium vapors through a potassium chloride melt at 800 ° C, emitting potassium vapors condense:

KCl + Na → K + NaCl.

Chemical properties of alkaline earth metals

Alkaline earth metals include elements of the main subgroup of group II: calcium (Ca), strontium (Sr), barium (Ba), radium (Ra). The chemical activity of these elements increases in the same way as that of alkali metals, i.e. with an increase down the subgroup.

Chemical properties of alkaline earth metals:

The structure of the valence shells of the atoms of these elements is ns 2.

By donating two valence electrons, the atoms of these chemical elements are converted into cations.
The compounds exhibit an oxidation state of +2.
The charges of atomic nuclei are one unit higher than that of alkaline elements of the same periods, which leads to a decrease in the radius of the atoms and an increase in ionization potentials.

Interaction of alkaline earth metals with other elements:

1. With oxygen, all alkaline earth metals, except barium, form oxides, barium forms peroxide BaO 2. Of these metals, beryllium and magnesium, covered with a thin protective oxide film, interact with oxygen only at very high t. Basic oxides of alkaline earth metals react with water, with the exception of beryllium oxide BeO, which has amphoteric properties. The reaction of calcium oxide and water is called the slaking reaction. If the reagent is CaO, quicklime is formed, if Ca (OH) 2, slaked lime. Also basic oxides react with acidic oxides and acids. For example:

3CaO + P 2 O 5 → Ca 3 (PO 4) 2 .

2. With water, alkaline earth metals and their oxides form hydroxides - white crystalline substances that, in comparison with alkali metal hydroxides, are less soluble in water. Alkaline earth metal hydroxides are alkalis, except for amphoteric Be (OH ) 2 and weak base Mg (OH) 2. Since beryllium does not react with water, Be (OH ) 2 can be obtained by other methods, for example, by hydrolysis of nitride:

Be 3 N 2+ 6H 2 O → 3 Be (OH) 2+ 2N H 3.

3. Under normal conditions, I react with halogens, except for beryllium. The latter reacts only at high t. Halides are formed (MgI 2 - magnesium iodide, CaI 2 - calcium iodide, CaBr 2 - calcium bromide, etc.).

4. All alkaline earth metals, except beryllium, react with hydrogen when heated. Hydrides are formed (BaH 2, CaH 2, etc.). For the reaction of magnesium with hydrogen, in addition to high t, it is also required high blood pressure hydrogen.

5. Form sulfides with sulfur. For example:

Ca + S → СaS.

Sulfides are used to produce sulfuric acid and the corresponding metals.

6. Form nitrides with nitrogen. For example:

3Be + N 2 → Be 3 N 2.

7. With acids, forming salts of the corresponding acid and hydrogen. For example:

Be + H 2 SO 4 (dil.) → BeSO 4 + H 2.

These reactions proceed in the same way as in the case of alkali metals.

Obtaining alkaline earth metals:

Beryllium is obtained by reduction of fluoride:

BeF 2 + Mg –t o → Be + MgF 2

Barium is obtained by oxide reduction:

3BaO + 2Al –t o → 3Ba + Al 2 O 3

The rest of the metals are obtained by electrolysis of chloride melts:

CaCl 2 → Ca + Cl 2

Chemical properties of aluminum

Aluminum is an active, light metal, at number 13 in the table. The most abundant of all metals in nature. And of the chemical elements it takes the third position in terms of distribution. High heat and electrical conductor. Resistant to corrosion, since it is covered with an oxide film. The melting point is 660 0 С.

Consider the chemical properties and interaction of aluminum with other elements:

1. In all compounds, aluminum is in the +3 oxidation state.

2. It exhibits reducing properties in almost all reactions.

3. Amphoteric metal exhibits both acidic and basic properties.

4. Recovers many metals from oxides. This method of obtaining metals is called alumothermy. An example of getting chrome:

2Al + Cr 2 О 3 → Al 2 О 3 + 2Cr.

5. Reacts with all dilute acids to form salts and evolve hydrogen. For example:

2Al + 6HCl → 2AlCl 3 + 3H 2;

2Al + 3H 2 SO 4 → Al 2 (SO 4) 3 + 3H 2.

In concentrated HNO 3 and H 2 SO 4, aluminum is passivated. Thanks to this, it is possible to store and transport these acids in containers made of aluminum.

6. Interacts with alkalis, as they dissolve the oxide film.

7. Interacts with all non-metals except hydrogen. To carry out the reaction with oxygen, finely crushed aluminum is needed. The reaction is possible only at high t:

4Al + 3O 2 → 2Al 2 O 3 .

In terms of its thermal effect, this reaction is exothermic. Interaction with sulfur forms aluminum sulfide Al 2 S 3, with phosphorus phosphide AlP, with nitrogen nitride AlN, with carbon carbide Al 4 C 3.

8. Interacts with other metals to form aluminides (FeAl 3 CuAl 2, CrAl 7, etc.).

Receiving aluminum:

Metallic aluminum is obtained by electrolysis of a solution of alumina Al 2 O 3 in molten cryolite Na 2 AlF 6 at 960–970 ° C.

2Al 2 O 3 → 4Al + 3O 2.

Chemical properties of transition elements

Transitional elements include elements of secondary subgroups of the Periodic Table. Consider the chemical properties of copper, zinc, chromium and iron.

Chemical properties of copper

1. In the electrochemical row, it is located to the right of H, therefore this metal is inactive.

2. Weak reducing agent.

3. In compounds, it exhibits oxidation states +1 and +2.

4. Reacts with oxygen when heated, forming:

copper (I) oxide 2Cu + O 2 → 2CuO(at t 400 0 C)
or copper (II) oxide: 4Cu + O 2 → 2Cu 2 O(at t 200 0 C).

Oxides have basic properties. When heated in an inert atmosphere, Cu 2 O disproportionates: Cu 2 O → CuO + Cu... Copper (II) oxide CuO in reactions with alkalis forms cuprates, for example: CuO + 2NaOH → Na 2 CuO 2 + H 2 O.

5. Copper hydroxide Cu (OH) 2 is amphoteric, the main properties prevail in it. It dissolves easily in acids:

Cu (OH) 2 + 2HNO 3 → Cu (NO 3) 2 + 2H 2 O,

and in concentrated solutions of alkalis with difficulty:

Сu (OH) 2 + 2NaOH → Na 2.

6. The interaction of copper with sulfur under different temperature conditions also forms two sulfides. When heated to 300-400 0 С in vacuum, copper (I) sulfide is formed:

2Cu + S → Cu 2 S.

At room temperature, by dissolving sulfur in hydrogen sulfide, copper (II) sulfide can be obtained:

Cu + S → CuS.

7. Of halogens, it interacts with fluorine, chlorine and bromine, forming halides (CuF 2, CuCl 2, CuBr 2), iodine, forming copper (I) iodide CuI; does not interact with hydrogen, nitrogen, carbon, silicon.

8. It does not react with acids - non-oxidants, because they oxidize only metals located before hydrogen in the electrochemical series. This chemical element reacts with acids - oxidizing agents: dilute and concentrated nitric and concentrated sulfuric:

3Cu + 8HNO 3 (decomp) → 3Cu (NO 3) 2 + 2NO + 4H 2 O;

Cu + 4HNO 3 (conc) → Cu (NO 3) 2 + 2NO 2 + 2H 2 O;

Cu + 2H 2 SO 4 (conc) → CuSO 4 + SO 2 + 2H 2 O.

9. Interacting with salts, copper displaces from their composition the metals located to the right of it in the electrochemical series. For example,

2FeCl 3 + Cu → CuCl 2 + 2FeCl 2 .

Here we see that copper went into solution, and iron (III) was reduced to iron (II). This reaction is important practical significance and is used to remove copper deposited on plastic.

Zinc chemical properties

1. Most active after alkaline earth metals.

2. Possesses pronounced restorative properties and amphoteric properties.

3. In compounds, it exhibits an oxidation state of +2.

4. In air, it is covered with a ZnO oxide film.

5. Interaction with water is possible at a temperature of red heat. As a result, zinc oxide and hydrogen are formed:

Zn + H 2 O → ZnO + H 2.

6. Reacts with halogens, forming halides (ZnF 2 - zinc fluoride, ZnBr 2 - zinc bromide, ZnI 2 - zinc iodide, ZnCl 2 - zinc chloride).

7. With phosphorus forms phosphides Zn 3 P 2 and ZnP 2.

8. With gray ZnS chalcogenide.

9. Does not react directly with hydrogen, nitrogen, carbon, silicon and boron.

10. Reacts with non-oxidizing acids, forming salts and displacing hydrogen. For example:

H 2 SO 4 + Zn → ZnSO 4 + H 2
Zn + 2HCl → ZnCl 2 + H 2.

It also reacts with acids - oxidizing agents: with conc. sulfuric acid forms zinc sulfate and sulfur dioxide:

Zn + 2H 2 SO 4 → ZnSO 4 + SO 2 + 2H 2 O.

11. Reacts actively with alkalis, since zinc is an amphoteric metal. Forms tetrahydroxozincates with alkali solutions and releases hydrogen:

Zn + 2NaOH + 2H 2 O → Na 2 + H 2 .

On granules of zinc, after reaction, gas bubbles appear. With anhydrous alkalis, when fusion, forms zincates and releases hydrogen:

Zn + 2NaOH → Na 2 ZnO 2 + H 2.

Chemical properties of chromium

1. Under normal conditions it is inert, when heated it is active.

3. Forms colored compounds.

4. In compounds, it exhibits oxidation states +2 (basic oxide CrO black), +3 (amphoteric oxide Cr 2 O 3 and hydroxide Cr (OH) 3 green) and +6 (acidic chromium (VI) oxide CrO 3 and acids: chromic H 2 CrO 4 and two-chromic H 2 Cr 2 O 7, etc.).

5. It interacts with fluorine at t 350-400 0 C, forming chromium (IV) fluoride:

Cr + 2F 2 → CrF 4.

6. With oxygen, nitrogen, boron, silicon, sulfur, phosphorus and halogens at t 600 0 C:

compound with oxygen forms chromium (VI) oxide CrO 3 (dark red crystals),
connection with nitrogen - chromium nitride CrN (black crystals),
compound with boron - chromium boride CrB (yellow crystals),
compound with silicon - chromium silicide CrSi,
compound with carbon - chromium carbide Cr 3 C 2.

7. It reacts with water vapor, being in an incandescent state, forming chromium (III) oxide and hydrogen:

2Cr + 3H 2 O → Cr 2 O 3 + 3H 2 .

8. It does not react with alkali solutions, however, it slowly reacts with their melts, forming chromates:

2Cr + 6KOH → 2KCrO 2 + 2K 2 O + 3H 2.

9. It dissolves in dilute strong acids, forming salts. If the reaction takes place in air, Cr 3+ salts are formed, for example:

2Cr + 6HCl + O 2 → 2CrCl 3 + 2H 2 O + H 2 .

Cr + 2HCl → CrCl 2 + H 2.

10. With concentrated sulfuric and nitric acids, as well as with aqua regia, it reacts only when heated, because at low t these acids passivate chromium. Reactions with acids when heated look like this:

2Сr + 6Н 2 SO 4 (conc) → Сr 2 (SO 4) 3 + 3SO 2 + 6Н 2 О

Cr + 6НNО 3 (conc) → Сr (NO 3) 3 + 3NO 2 + 3Н 2 О

Chromium (II) oxide CrO - solid black or red, insoluble in water.

Chemical properties:

Possesses basic and regenerating properties.
When heated to 100 0 C in air, it is oxidized to Cr 2 O 3 - chromium (III) oxide.
It is possible to reduce chromium with hydrogen from this oxide: CrO + H 2 → Cr + H 2 O or coke: CrO + C → Cr + CO.
Reacts with hydrochloric acid while releasing hydrogen: 2CrO + 6HCl → 2CrCl 3 + H 2 + 2H 2 O.
Does not react with alkalis, diluted sulfuric and nitric acids.

Chromium (III) oxide Cr 2 O 3- a refractory substance, dark green in color, insoluble in water.

Chemical properties:

Possesses amphoteric properties.
How does the basic oxide react with acids: Cr 2 O 3 + 6HCl → CrCl 3 + 3H 2 O.
How acidic oxide interacts with alkalis: Cr 2 O 3 + 2KON → 2KCrO 3 + H 2 O.
Strong oxidants oxidize Cr 2 O 3 to chromate H 2 CrO 4.
Strong reducing agents restoreCr out Cr 2 O 3.

Chromium (II) hydroxide Cr (OH) 2 - a yellow or brown solid, poorly soluble in water.

Chemical properties:

Weak base, showing basic properties.
In the presence of moisture in the air, it is oxidized to Cr (OH) 3 - chromium (III) hydroxide.
Reacts with concentrated acids forming chromium (II) salts of blue color: Cr (OH) 2 + H 2 SO 4 → CrSO 4 + 2H 2 O.
Does not react with alkalis and dilute acids.

Chromium (III) hydroxide Cr (OH) 3 - a gray-green substance that does not dissolve in water.

Chemical properties:

Possesses amphoteric properties.
How does the basic hydroxide react with acids: Cr (OH) 3 + 3HCl → CrCl 3 + 3H 2 O.
How acid hydroxide interacts with alkalis: Cr (OH) 3 + 3NaОН → Na 3 [Cr (OH) 6].

Iron chemical properties

1. A highly reactive active metal.

2. Possesses reducing properties, as well as pronounced magnetic properties.

3. In compounds, it exhibits basic oxidation states +2 (with weak oxidants: S, I, HCl, salt solutions), +3 (with strong oxidants: Br and Cl) and less characteristic +6 (with O and H 2 O). In weak oxidants, iron takes on an oxidation state of +2, in stronger ones, +3. The oxidation state +2 corresponds to black oxide FeO and green hydroxide Fe (OH) 2, which have basic properties. The oxidation state +3 corresponds to the red-brown oxide Fe 2 O 3 and brown hydroxide Fe (OH) 3, which have weakly expressed amphoteric properties. Fe (+2) is a weak reducing agent, and Fe (+3) is more often a weak oxidizing agent. When the redox conditions change, the oxidation states of iron can change with each other.

4. In air at t 200 0 C it is covered with an oxide film. It corrodes easily under normal atmospheric conditions. NS When oxygen is passed through the iron melt, FeO oxide is formed. When iron burns in air, oxide Fe 2 O 3 is formed. When burned in pure oxygen, an oxide is formed - iron scale:

3Fe + 2O 2 → Fe 3 O 4.

5. Reacts with halogens when heated:

compound with chlorine forms iron (III) chloride FeCl 3,
compound with bromine - iron (III) bromide FeBr 3,
compound with iodine - iron (II, III) iodide Fe 3 I 8,
compound with fluorine - iron (II) fluoride FeF 2, iron (III) fluoride FeF 3.

6. It also reacts with sulfur, nitrogen, phosphorus, silicon and carbon when heated:

compound with sulfur forms iron (II) sulfide FeS,
connection with nitrogen - iron nitride Fe 3 N,
compound with phosphorus - phosphides FeP, Fe 2 P and Fe 3 P,
compound with silicon - iron silicide FeSi,
compound with carbon - iron carbide Fe 3 C.

2Fe + 4H 2 SO 4 → Fe 2 (SO 4) 3 + SO 2 + 4H 2 O

9. It does not react with alkali solutions, but reacts slowly with alkali melts, which are strong oxidizing agents:

Fe + KClO 3 + 2KOH → K 2 FeO 4 + KCl + H 2 O.

10. Restores metals located in the electrochemical row to the right:

Fe + SnCl 2 → FeCl 2 + Sn.

Getting iron: In industry, iron is obtained from iron ore, mainly from hematite (Fe 2 O 3) and magnetite (FeO · Fe 2 O 3).

3Fe 2 O 3 + CO → CO 2 + 2Fe 3 O 4,
Fe 3 O 4 + CO → CO 2 + 3FeO,
FeO + CO → CO 2 + Fe.

Iron (II) oxide FeO - a black crystalline substance (wustite), which does not dissolve in water.

Chemical properties:

Possesses basic properties.
Reacts with dilute hydrochloric acid: FeO + 2HCl → FeCl 2 + H 2 O.
Reacts with concentrated nitric acid:FeO + 4HNO 3 → Fe (NO 3) 3 + NO 2 + 2H 2 O.
Does not react with water and salts.
With hydrogen at t 350 0 C it is reduced to pure metal: FeO + H 2 → Fe + H 2 O.
It is also reduced to pure metal when combined with coke: FeO + C → Fe + CO.
This oxide can be obtained in various ways, one of them is heating Fe at low pressure O: 2Fe + O 2 → 2FeO.

Iron (III) oxideFe 2 O 3- powder of a brown color (hematite), a substance insoluble in water. Other names: iron oxide, red lead, food coloring E172, etc.

Chemical properties:

Fe 2 O 3 + 6HCl → 2 FeCl 3 + 3H 2 O.
Does not react with alkali solutions, reacts with their melts, forming ferrites: Fe 2 O 3 + 2NaOH → 2NaFeO 2 + H 2 O.
When heated with hydrogen, it exhibits oxidizing properties:Fe 2 O 3 + H 2 → 2FeO + H 2 O.
Fe 2 O 3 + 3KNO 3 + 4KOH → 2K 2 FeO 4 + 3KNO 2 + 2H 2 O.

Iron oxide (II, III) Fe 3 O 4 or FeO Fe 2 O 3 - a grayish-black solid (magnetite, magnetic iron ore), a substance that does not dissolve in water.

Chemical properties:

Decomposes on heating more than 1500 0 С: 2Fe 3 O 4 → 6FeO + O 2.
Reacts with dilute acids: Fe 3 O 4 + 8HCl → FeCl 2 + 2FeCl 3 + 4H 2 O.
Does not react with alkali solutions, reacts with their melts: Fe 3 O 4 + 14NaOH → Na 3 FeO 3 + 2Na 5 FeO 4 + 7H 2 O.
Upon reaction with oxygen, it is oxidized: 4Fe 3 O 4 + O 2 → 6Fe 2 O 3.
With hydrogen, when heated, it is reduced:Fe 3 O 4 + 4H 2 → 3Fe + 4H 2 O.
It is also reduced when combined with carbon monoxide: Fe 3 O 4 + 4CO → 3Fe + 4CO 2.

Iron (II) hydroxide Fe (OH) 2 - white, rarely greenish crystalline substance, insoluble in water.

Chemical properties:

It has amphoteric properties with a predominance of basic ones.
It enters into the reaction of neutralization of the non-oxidizing acid, showing the main properties: Fe (OH) 2 + 2HCl → FeCl 2 + 2H 2 O.
When interacting with nitric or concentrated sulfuric acids, it exhibits reducing properties, forming iron (III) salts: 2Fe (OH) 2 + 4H 2 SO 4 → Fe 2 (SO 4) 3 + SO 2 + 6H 2 O.
When heated, it reacts with concentrated alkali solutions: Fe (OH) 2 + 2NaOH → Na 2.

Iron hydroxide (I I I) Fe (OH) 3- brown crystalline or amorphous substance, insoluble in water.

Chemical properties:

It has mild amphoteric properties with a predominance of the main ones.
Reacts easily with acids: Fe (OH) 3 + 3HCl → FeCl 3 + 3H 2 O.
Forms hexahydroxoferrates (III) with concentrated alkali solutions: Fe (OH) 3 + 3NaOH → Na 3.
Forms ferrates with alkali melts:2Fe (OH) 3 + Na 2 CO 3 → 2NaFeO 2 + CO 2 + 3H 2 O.
In an alkaline medium with strong oxidizing agents, it exhibits reducing properties: 2Fe (OH) 3 + 3Br 2 + 10KOH → 2K 2 FeO 4 + 6NaBr + 8H 2 O.

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At the end of the 90s, the Rules for Electrical Installations (PUE) of the 7th edition were put into effect in Russia, according to which it is prohibited to wiring internal networks of buildings from aluminum cables and wires with a cross section of less than 16 mm2, and it is prescribed to carry them out of copper wire. Certain properties of aluminum are responsible for the regulatory change.

Aluminum as an electrical conductor

Aluminum cables and wires have long been massively used both for wiring internal power networks in buildings for various purposes, and for laying external power lines. This is due to the following properties of aluminum:

low specific gravity, which is three times lighter than that of copper;
ease of processing;
low material cost;
good electrical conductivity, per unit weight;
high corrosion resistance.

However, other features of aluminum: high fluidity, which does not provide sufficient quality of contacts for a long time; low strength at mechanical stress for a break; low temperature resistance, leading to increased fragility during overheating - served as the introduction of a ban on the wiring of aluminum wires of small cross-section for internal power supply networks.

One of the main reasons that influenced the change in the PUE requirements is that during operation a thin oxide film is formed on the surface of aluminum wires, which has a much worse electrical conductivity than the base metal. As a result, a higher transition resistance is formed at the junction of the wires, which significantly increases the possibility of heating the contacts, the risk of their destruction and fire.

Copper used as a material for electrical cables and wires, despite the higher cost, is devoid of the listed disadvantages of aluminum and has a number of advantages: higher conductivity; does not form an oxide film on the surface; higher flexibility, this allows the manufacture of wires with a very small cross-section of up to 0.3 mm2, which is impossible to make from aluminum.

Connecting aluminum and copper wires

Since many old buildings retain electrical networks made of aluminum wires, during repairs it is often necessary to connect wires made of different materials - copper and aluminum. According to the same Electrical Installation Rules, the connection of aluminum and copper wires can be done in several ways:

with the help of connections of the "nutty" type, consisting of three plates, between which the wires are clamped with the help of bolts;
by means of clamps of the WAGO type. The ends of the wires to be connected are stripped by 10-15 mm, inserted into different holes of the terminal block, and then clamped with falling blocks;
using terminal blocks, which are a strip with two holes. The ends of the wires to be connected are inserted into the holes from different ends and clamped with a screw
using a simple bolt connection, when the wires are clamped with a nut with a metal washer between them. This method is considered temporary, since it is not suitable for rooms with high humidity and is not used for external connections.

The article was prepared based on materials from the site http://energy-systems.ru/

Aluminum - general characteristics of the element, chemical properties. Adapter plates MA and AP for connecting aluminum buses to copper leads of electrical devices

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Aluminum as an electrical conductor

Connecting aluminum and copper wires