What is manganese: we study a chemical element. Manganese (chemical element): properties, application, designation, oxidation state, interesting facts

Olympiad tasks in chemistry

(1 school stage)

1. Test

1.Manganese has the highest oxidation state in the compound

2. The neutralization reaction corresponds to the abbreviated ionic equation

1) H + + OH - = H 2 O

2) 2H + + CO 3 2- = H 2 O + CO 2

3) CaO + 2H + = Ca 2+ + H 2 O

4) Zn + 2H + = Zn 2+ + H 2

3. Interact with each other

2) MnO and Na 2 O

3) P 2 O 5 and SO 3

4. The equation of the redox reaction is

1) KOH + HNO 3 = KNO 3 + H 2 O

2) N 2 O 5 + H 2 O = 2 HNO 3

3) 2N 2 O = 2N 2 + O 2

4) BaCO 3 = BaO + CO 2

5. The exchange reaction is interaction

1) calcium oxide with nitric acid

2) carbon monoxide with oxygen

3) ethylene with oxygen

4) hydrochloric acid with magnesium

6. Acid rain caused by the presence in the atmosphere

1) nitrogen and sulfur oxides

4) natural gas

7. Methane, along with gasoline and diesel fuel, is used as fuel in internal combustion engines (motor vehicles). The thermochemical equation of combustion of gaseous methane has the form:

CH 4 + 2O 2 = CO 2 + 2H 2 O + 880 kJ

What amount of kJ of heat will be released during the combustion of CH 4 with a volume of 112 liters (at standard level)?

Choose the correct answer:

2. Tasks

1. In the equation of the redox reaction, place the coefficients in any way you know.

SnSO 4 + KMnO 4 + H 2 SO 4 = Sn (SO 4) 2 + MnSO 4 + K 2 SO 4 + H 2 O

Indicate the names of the oxidizing agent and reducing agent and the oxidation state of the elements. (4 points)

2. Write down the reaction equations allowing to carry out the following transformations:

(2) (3) (4) (5)

CO 2 → Ca (HCO 3) 2 → CaCO 3 → CaO → CaCl 2 → CaCO 3

(5 points)

3. Determine the alkadiene formula if its relative density by air is 1.862 (3 points)

4. In 1928, the American chemist of the corporation General Motors (General Motors Research) Thomas Midgley Jr. succeeded in synthesizing and isolating in his laboratory a chemical compound consisting of 23.53% carbon, 1.96% hydrogen and 74.51 % fluorine. The resulting gas was 3.52 times heavier than air and did not burn. Derive the formula of the compound, write down the structural formulas of organic substances corresponding to the obtained molecular formula, give them names. (6 points).

5. Mixed 140 g of 0.5% hydrochloric acid solution with 200 g of 3% hydrochloric acid solution. What is the percentage of hydrochloric acid in the newly obtained solution? (3 points)

3. Crossword

Unravel the words encrypted in the crossword puzzle

Legend: 1 → - horizontally

1 ↓ - vertical

↓ Corrosion product of iron.

→ Formed by the interaction of (6) with the basic oxide.

→ Unit of the amount of heat.

→ Positively charged ion.

→ An Italian scientist, after whom one of the most important constants is named.

→ The number of electrons per external level element number 14.

→ …… gas - carbon monoxide (IV).

→ The great Russian scientist is famous, including as the creator of mosaic paintings, the author of the epigraph.

→ Type of reaction between sodium hydroxide and sulfuric acid solutions.

Give an example of a reaction equation for (1 →).

Indicate the constant mentioned in (4).

Write down the reaction equation (8).

Write electronic structure atom element, which is mentioned in (5). (13 points)

Chemistry of metals

Lecture 2. The main issues discussed in the lecture

Metals of VIIB-subgroup

General characteristics of metals of the VIIB-subgroup.

Manganese chemistry

Natural compounds Mn

Physical and Chemical properties metal.

Mn compounds. Redox properties of compounds

Brief characteristics of Tc and Re.

Metals of VIIB-subgroup

general characteristics

appear in natural compounds. The most common

strange Mn minerals: pyrolusite MnO2 and rhodochrosite MnCO3.

Mn (+7) and (+6) compounds are strong oxidizing agents.

The greatest similarity Mn, Tc, Re are shown in the highest oxidation state.

lehenia, it is expressed in the acidic nature of higher oxides and hydroxides.

The higher hydroxides of all elements of the VIIB-subgroup are strong

acids with the general formula NEO4.

In the highest oxidation state, the elements Mn, Tc, Re are similar to the element of the main subgroup chlorine. Acids: HMnO4, HTcO4, HReO4 and

HClO4 are strong. Elements of the VIIB-subgroup are characterized by a noticeable

It is very similar to its neighbors in the row, in particular, Mn is similar to Fe. In nature, Mn compounds always coexist with Fe compounds.

M ar ganets

Typical oxidation states

neutral, slightly alkaline and slightly acidic environment.

Mn (+7) and (+6) compounds exhibit strong oxidizing properties.

The acid-base character of Mn oxides and hydroxides is naturally due to

varies depending on the oxidation state: in the oxidation state +2, the oxide and hydroxide are basic, and in the highest oxidation state they are acidic,

moreover, HMnO4 is a strong acid.

In aqueous solutions, Mn (+2) exists in the form of aquacations

2+, which for simplicity denotes Mn2 +. Manganese in high oxidation states is in solution in the form of tetraoxoanions: MnO4 2– and

MnO4 -.

Natural compounds and metal production

The element Mn is most abundant in the earth's crust among heavy metal

Fishing follows iron, but is noticeably inferior to it - the Fe content is about 5%, and Mn is only about 0.1%. Manganese has more common oxide

ny and carbonate and ores. The most important minerals are: pyrol-

zite MnO2 and rhodochrosite MnCO3.

to obtain Mn

In addition to these minerals, hausmanite Mn3 O4 is used to obtain Mn.

and hydrated psilomelan oxide MnO2. xH2 O. In manganese ores, all

Manganese is mainly used in the production of special steels with high strength and impact resistance. Therefore, os-

a new amount of Mn is obtained not in pure form, but in the form of ferromanganese

tsa - an alloy of manganese and iron, containing from 70 to 88% Mn.

The total volume of the annual world production of manganese, including in the form of ferromanganese, ~ (10 12) million tons / year.

To obtain ferromanganese, manganese oxide ore was reduced

coal.

MnO2 + 2C = Mn + 2CO

Together with the Mn oxides, the Fe oxides contained in the ru-

de. To obtain manganese with a minimum content of Fe and C, compounds

Fe is preliminarily separated and mixed oxide Mn3 O4 is obtained

(MnO. Mn2 O3). It is then reduced with aluminum (pyrolusite reacts with

Al is too violent).

3Mn3 O4 + 8Al = 9Mn + 4Al2 O3

Pure manganese is obtained by hydrometallurgical method. After preliminary preparation of the MnSO4 salt, through a solution of Mn sulfate,

let electricity, manganese is reduced at the cathode:

Mn2 + + 2e– = Mn0.

Simple substance

Manganese is a light gray metal. Density - 7.4 g / cm3. Melting point - 1245 ° C.

Mn2 +. When heated, powdered manganese interacts with water with

release of H2.

Due to oxidation in air, manganese becomes covered with brown spots,

When heated, manganese reacts with halogens and sulfur. Affinity Mn

to sulfur more than iron, therefore, when adding ferromanganese to steel,

the sulfur dissolved in it binds to MnS. MnS sulfide does not dissolve in the metal and goes into the slag. The strength of the steel increases after the removal of the brittle sulfur.

At very high temperatures (> 1200 0 C), manganese, interacting with nitrogen and carbon, forms non-stoichiometric nitrides and carbides.

Manganese compounds

Manganese compounds (+7)

All Mn (+7) compounds exhibit strong oxidizing properties.

Potassium permanganate KMnO 4 - the most common compound

Mn (+7). In its pure form, this crystalline substance is dark

purple. When heating crystalline permanganate, it decomposes

To slow down this reaction, which is accelerated by light, KMnO4 solutions are stored

nat in dark bottles.

When a few drops are added to the permanganate crystals,

Trated sulfuric acid forms manganic anhydride.

2KMnO4 + H2 SO4 2Mn2 O7 + K2 SO4 + H2 O

Mn 2 O 7 oxide is a dark green heavy oily liquid. This is the only metal oxide that, when normal conditions find

in liquid state(melting point 5.9 0 С). The oxide has a molecular

a curious structure, very unstable, at 55 0 С it decomposes with an explosion. 2Mn2 O7 = 4MnO2 + 3O2

Mn2 O7 oxide is a very strong and energetic oxidizing agent. Many or-

ganic substances are oxidized under its influence to CO2 and H2O. Oxide

Mn2 O7 is sometimes called chemical matches. If a glass rod is moistened with Mn2 O7 and brought to an alcohol lamp, it will light up.

When Mn2 O7 dissolves in water, manganic acid is formed.

Acid HMnO 4 is a strong acid that exists only in water

nominal solution, in a free state it is not isolated. The acid HMnO4 decomposes

with the release of O2 and MnO2.

When solid alkali is added to the KMnO4 solution,

green manganate.

4KMnO4 + 4KOH (c) = 4K2 MnO4 + O2 + 2H2 O.

When heated, KMnO4 with concentrated hydrochloric acid forms

Cl2 gas is supplied.

2KMnO4 (c) + 16HCl (conc.) = 2MnCl2 + 5Cl2 + 8H2 O + 2KCl

In these reactions, the strong oxidizing properties of permanganate are manifested.

The products of the interaction of KMnO4 with reducing agents depend on the acidity of the solution. in which the reaction takes place.

In acidic solutions, a colorless cation Mn2 + is formed.

MnO4 - + 8H + + 5e–  Mn2 + + 4H2 O; (E0 = +1.53 V).

A brown precipitate of MnO2 precipitates from neutral solutions.

MnO4 - + 2H2 O + 3e–  MnO2 + 4OH–.

In alkaline solutions, the green anion MnO4 2– is formed.

Potassium permanganate is industrially obtained either from manganese

(oxidizing it at the anode in an alkaline solution), or from pyrolusite (MnO2 pre-

they are oxidized by variationally to K2 MnO4, which is then oxidized at the anode to KMnO4).

Manganese compounds (+6)

Manganates - salts with the MnO4 2– anion, have a bright green color.

Anion MnO4 2─ is stable only in strongly alkaline environment... Under the action of water and, especially, acid, manganates disproportionate with the formation of compounds

Mn in oxidation states 4 and 7.

3MnO4 2– + 2H2 O = MnO2 + 2MnO4 - + 4OH–

For this reason, the acid H2 MnO4 does not exist.

Manganates can be obtained by fusing MnO2 with alkalis or carbonate-

mi in the presence of an oxidizing agent.

2MnO2 (q) + 4KOH (l) + О2 = 2K2 MnO4 + 2H2 O

Manganates are strong oxidizing agents , but if they are affected

with an even stronger oxidizing agent, then they pass into permanganates.

Disproportionation

Manganese compounds (+4)

- the most stable Mn compound. This oxide occurs naturally (pyrolusite mineral).

MnO2 oxide is a black-brown substance with a very strong crystalline

lattice (the same as that of rutile TiO2). For this reason, despite the fact that MnO 2 is amphoteric, it does not react with alkali solutions and with dilute acids (as well as TiO2). It dissolves in concentrated acids.

MnO2 + 4HCl (conc.) = MnCl2 + Cl2 + 2H2 O

The reaction is used in the laboratory to produce Cl2.

When MnO2 is dissolved in concentrated sulfuric and nitric acid, Mn2 + and O2 are formed.

Thus, in a very acidic environment, MnO2 tends to go into

Mn2 + cation.

MnO2 reacts with alkalis only in melts with the formation of mixed

ny oxides. In the presence of an oxidizing agent, manganates are formed in alkaline melts.

MnO2 oxide is used industrially as a cheap oxidizing agent. In particular, redox interaction

by the formation of oxides Mn2 O3 and Mn3 O4 (MnO. Mn2 O3).

Hydroxide Mn (+4) is not isolated, during the reduction of permanganate and man-

ganata in neutral or slightly alkaline media, as well as during oxidation

Mn (OH) 2 and MnOOH, a dark brown precipitate is precipitated from solutions.

MnO2.

Mn oxide and hydroxide (+3) are basic in nature. It's solid

brown, water-insoluble and unstable substances.

When interacting with dilute acids, they are disproportionate

they form Mn compounds in oxidation states 4 and 2.2MnOOH + H2 SO4 = MnSO4 + MnO2 + 2H2 O

WITH concentrated acids they interact in the same way as

MnO2, i.e. in an acidic medium they pass into the Mn2 + cation. In an alkaline environment, they are easily oxidized in air to MnO2.

Manganese compounds (+2)

In aqueous solutions, Mn (+2) compounds are stable in an acidic environment.

Oxide and hydroxide Mn (+2) have a basic character, easily dissolve

ripple in acids with the formation of a hydrated Mn2 + cation.

MnO oxide - gray-green refractory crystalline compound

(melting point - 18420 C). It can be obtained by decomposing car-

bonata in the absence of oxygen.

MnCO3 = MnO + CO2.

MnO does not dissolve in water.

The electronic configuration of the unexcited manganese atom is 3d 5 4s 2; the excited state is expressed by the electronic formula 3d 5 4s 1 4p 1.

The oxidation states +2, +4, +6, +7 are most typical for manganese in compounds.

Manganese is a silvery-white, brittle, quite active metal: in the series of voltages, it is located between aluminum and zinc. In air, manganese is covered with an oxide film that protects it from further oxidation. In a finely divided state, manganese is easily oxidized.

Manganese (II) oxide MnO and the corresponding hydroxide Mn (OH) 2 have basic properties - when they interact with acids, divalent manganese salts are formed: Mn (OH) 2 + 2 H + ® Mn 2+ + 2 H 2 O.

Mn 2+ cations are also formed upon dissolution of metallic manganese in acids. Manganese (II) compounds exhibit reducing properties, for example, the white precipitate Mn (OH) 2 darkens rapidly in air, gradually oxidizing to MnO 2: 2 Mn (OH) 2 + O 2 ® 2 MnO 2 + 2 H 2 O.

Manganese (IV) oxide MnO 2 is the most stable manganese compound; it is easily formed both during the oxidation of manganese compounds in a lower oxidation state (+2), and during the reduction of manganese compounds in higher oxidation states (+6, +7):

Mn (OH) 2 + H 2 O 2 ® MnO 2 + 2 H 2 O;

2 KMnO 4 + 3 Na 2 SO 3 + H 2 O ® 2 MnO 2 ¯ + 3 Na 2 SO 4 + 2 KOH.

MnO 2 is an amphoteric oxide, however, it is acidic, and its basic properties are poorly expressed. One of the reasons that MnO 2 does not show clearly pronounced basic properties is its strong oxidative activity in an acidic medium (= +1.23 V): MnO 2 is reduced to Mn 2+ ions, and does not form stable salts of tetravalent manganese. The hydrated form corresponding to manganese (IV) oxide should be considered as hydrated manganese dioxide MnO 2 × xH 2 O. Manganese (IV) oxide as an amphoteric oxide formally corresponds to ortho- and meta-forms of permanganous acid not isolated in the free state: H 4 MnO 4 - ortho-form and H 2 MnO 3 - meta-form. Known manganese oxide Mn 3 O 4, which can be considered as a salt of divalent manganese of the ortho-form of permanganous acid Mn 2 MnO 4 - manganese (II) orthomanganite. There are reports in the literature on the existence of oxide Mn 2 O 3. The existence of this oxide can be explained by considering it as a salt of divalent manganese of the meta-form of permanganate acid: MnMnO 3 - manganese (II) metamanganite.

When manganese dioxide is fused with oxidants such as chlorate or potassium nitrate in an alkaline medium, tetravalent manganese is oxidized to a hexavalent state, and potassium manganate is formed, a salt that is very unstable even in a solution of permanganous acid H 2 MnO 4, the anhydride of which (MnO 3) is unknown:

MnO 2 + KNO 3 + 2 KOH ® K 2 MnO 4 + KNO 2 + H 2 O.

Manganates are unstable and prone to disproportionate reversible reaction: 3 K 2 MnO 4 + 2 H 2 O ⇆ 2 KMnO 4 + MnO 2 ¯ + 4 KOH,

as a result, the green color of the solution, caused by the manganate ions MnO 4 2–, changes to a violet color, which is characteristic of the permanganate ions MnO 4 -.

The most widely used compound of heptavalent manganese is potassium permanganate KMnO 4 - a salt known only in a solution of manganic acid HMnO 4. Potassium permanganate can be obtained by oxidizing manganates with strong oxidants, for example, chlorine:

2 K 2 MnO 4 + Cl 2 ® 2 KMnO 4 + 2 KCl.

Manganese oxide (VII), or manganese anhydride, Mn 2 O 7 is an explosive green-brown liquid. Mn 2 O 7 can be obtained by the reaction:

2 KMnO 4 + 2 H 2 SO 4 (conc.) ® Mn 2 O 7 + 2 KHSO 4 + H 2 O.

Manganese compounds in the highest oxidation state +7, in particular permanganates, are strong oxidizing agents. The depth of reduction of permanganate ions and their oxidative activity depends on the pH of the medium.

In a strongly acidic environment, the product of the reduction of permanganates is the Mn 2+ ion, and bivalent manganese salts are obtained:

MnO 4 - + 8 H + + 5 e - ® Mn 2+ + 4 H 2 O (= +1.51 V).

In a neutral, slightly alkaline or slightly acidic medium, as a result of the reduction of permanganate ions, MnO 2 is formed:

MnO 4 - + 2 H 2 O + 3 e - ® MnO 2 ¯ + 4 OH - (= +0.60 V).

MnO 4 - + 4 H + + 3 e - ® MnO 2 ¯ + 2 H 2 O (= +1.69 V).

In a strongly alkaline medium, permanganate ions are reduced to manganate ions MnO 4 2–, and salts of the type K 2 MnO 4, Na 2 MnO 4 are formed:

MnO 4 - + e - ® MnO 4 2– (= +0.56 V).

Manganese is one of the most important metals for metallurgy. In addition, he is generally quite an unusual element, with which they are associated Interesting Facts... Important for living organisms, required in the production of many alloys, chemical substances... Manganese - a photo of which can be seen below. It is its properties and characteristics that we will consider in this article.

Characteristics of a chemical element

If we talk about manganese as an element, then first of all it is necessary to characterize its position in it.

1. It is located in the fourth large period, seventh group, side subgroup.
2. The serial number is 25. Manganese is a chemical element, the atoms of which are +25. The number of electrons is the same, neutrons - 30.
3. Meaning atomic mass - 54,938.
4. The designation of the chemical element manganese is Mn.
5. The Latin name is manganese.

It is located between chromium and iron, which explains its similarity with them in physical and chemical characteristics.

Manganese - chemical element: transition metal

If we consider the electronic configuration of the reduced atom, then its formula will have the form: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5. It becomes obvious that the element we are considering is a transition metal from the d-family. Five electrons on the 3d sublevel indicate the stability of the atom, which is manifested in its chemical properties.

As a metal, manganese is a reducing agent, however, most of its compounds are capable of exhibiting rather strong oxidizing abilities. It's connected with varying degrees oxidation and valencies possessed by this element. This is the peculiarity of all metals in this family.

Thus, manganese is a chemical element located among other atoms and having its own special characteristics. Let's consider what these properties are in more detail.

Manganese is a chemical element. Oxidation state

We have already given the electronic formula of the atom. According to her, this element is capable of showing several positive degrees oxidation. It:

The valency of the atom is IV. The most stable are those compounds in which the values ​​of +2, +4, +6 appear in manganese. The highest degree oxidation allows compounds to act as the strongest oxidizing agents. For example: KMnO 4, Mn 2 O 7.

Compounds with +2 are reducing agents, manganese (II) hydroxide has amphoteric properties, with a predominance of basic ones. Intermediate oxidation states form amphoteric compounds.

Discovery history

Manganese is a chemical element that was not discovered immediately, but gradually and by different scientists. However, people have used its compounds since ancient times. Manganese (IV) oxide was used to melt glass. One Italian stated that the addition of this compound in the chemical production of glasses dyes their color purple. Along with this, the same substance helps to eliminate turbidity in colored glasses.

Later in Austria, the scientist Keim managed to obtain a piece of metallic manganese by acting high temperature for purolysite (manganese (IV) oxide), potash and coal. However, this sample had many impurities, which he could not eliminate, so the discovery did not take place.

Still later, another scientist also synthesized a mixture, in which a significant proportion was pure metal. It was Bergman, who had previously discovered the element nickel. However, he was not destined to complete the matter.

Manganese is a chemical element, which can be obtained and isolated in the form simple substance Karl Scheele first succeeded in 1774. However, he did it together with I. Gan, who completed the process of smelting a piece of metal. But even they failed to completely rid it of impurities and get 100% product yield.

Nevertheless, it was this time that became the discovery of this atom. The same scientists attempted to give the name, as the discoverers. They chose the term manganesium. However, after the discovery of magnesium, confusion began, and the name of manganese was changed to the modern one (H. David, 1908).

Since manganese is a chemical element, the properties of which are very valuable for many metallurgical processes, over time, it became necessary to find a way to obtain it in the purest possible form. This problem was solved by scientists from all over the world, but managed to be resolved only in 1919 thanks to the works of R. Agladze, a Soviet chemist. It was he who found a way to obtain pure metal with a substance content of 99.98% from manganese sulfates and chlorides by electrolysis. Now this method is used all over the world.

Being in nature

Manganese is a chemical element, a photo of a simple substance of which can be seen below. In nature, there are a lot of isotopes of this atom, the number of neutrons in which fluctuates strongly. Thus, the mass numbers vary from 44 to 69. However, the only stable isotope is an element with a value of 55 Mn, all the rest have either an negligibly short half-life, or exist in too small quantities.

Since manganese is a chemical element, the oxidation state of which is very different, it also forms many compounds in nature. In its pure form, this element does not occur at all. In minerals and ores, its constant neighbor is iron. In total, several of the most important rocks can be identified, which include manganese.

1. Pyrolusite. Compound formula: MnO 2 * nH 2 O.
2. Psilomelan, MnO2 * mMnO * nH2O molecule.
3. Manganite, formula MnO * OH.
4. Brownite is less common than the rest. Formula Mn 2 O 3.
5. Gausmanite, formula Mn * Mn 2 O 4.
6. Rhodonite Mn 2 (SiO 3) 2.
7. Manganese carbonate ores.
8. Raspberry spar or rhodochrosite - MnCO 3.
9. Purpurite - Mn 3 PO 4.

In addition, several more minerals can be designated, which also include the element in question. It:

• calcite;
• siderite;
• clay minerals;
• chalcedony;
• opal;
• sandy-silty compounds.

In addition to rocks and sedimentary rocks, minerals, manganese is a chemical element that is part of the following objects:

1. Plant organisms. The largest accumulators of this element are: water nut, duckweed, diatoms.
2. Rusty mushrooms.
3. Some types of bacteria.
4. The following animals: red ants, crustaceans, molluscs.
5. Humans - The daily requirement is approximately 3-5 mg.
6. The waters of the World Ocean contain 0.3% of this element.
7. The total content in the earth's crust is 0.1% by weight.

In general, it is the 14th most common element of all on our planet. Among heavy metals, it is the second after iron.

Physical properties

From the point of view of the properties of manganese as a simple substance, several main physical characteristics for him.

1. In the form of a simple substance, it is a fairly hard metal (on the Mohs scale, the indicator is 4). Color - silvery-white, in the air it is covered with a protective oxide film, glitters on the cut.
2. The melting point is 1246 0 С.
3. Boiling - 2061 0 C.
4. It has good conductive properties and is paramagnetic.
5. The density of the metal is 7.44 g / cm 3.
6. It exists in the form of four polymorphic modifications (α, β, γ, σ), differing in structure and shape crystal lattice and the packing density of atoms. Their melting point also differs.

In metallurgy, three main forms of manganese are used: β, γ, σ. Alpha is less common, as it is too fragile in its properties.

Chemical properties

From the point of view of chemistry, manganese is a chemical element, the ionic charge of which varies greatly from +2 to +7. This leaves its mark on his activity. In free form in air, manganese reacts very weakly with water and dissolves in dilute acids. However, as soon as the temperature is increased, the activity of the metal rises sharply.

So, he is able to interact with:

• nitrogen;
• carbon;
• halogens;
• silicon;
• phosphorus;
• gray and other non-metals.

When heated without air access, the metal easily turns into a vaporous state. Depending on the oxidation state that manganese exhibits, its compounds can be both reducing and oxidizing agents. Some exhibit amphoteric properties. So, the main ones are typical for compounds in which it is +2. Amphoteric - +4, and acidic and strong oxidative in the highest value +7.

Despite the fact that manganese is a complex compound, there are few for it. This is due to sustainable electronic configuration atom, because its 3d-sublevel contains 5 electrons.

Methods of obtaining

There are three main ways in which manganese (chemical element) is obtained in industry. As the name reads in Latin, we have already designated - manganum. If you translate it into Russian, it will be "yes, I really do clarify, discolor." Manganese owes this name to the manifested properties known since antiquity.

However, despite the fame, they managed to get it in its pure form for use only in 1919. This is done by the following methods.

1. Electrolysis, the product yield is 99.98%. In this way, manganese is obtained in the chemical industry.
2. Silicothermic, or reduction with silicon. At this method fusion of silicon and manganese (IV) oxide occurs, as a result of which a pure metal is formed. The yield is about 68%, since the compound of manganese with silicon to form silicide is a side process. This method used in the metallurgical industry.
3. Aluminothermic method - recovery with aluminum. Also does not give too high a product yield, manganese is formed contaminated with impurities.

The production of this metal is essential for many processes in metallurgy. Even a small addition of manganese can greatly affect the properties of alloys. It has been proven that many metals dissolve in it, filling its crystal lattice.

For the extraction and production of this element, Russia ranks first in the world. Also, this process is carried out in countries such as:

• China.
• Kazakhstan.
• Georgia.
• Ukraine.

Industrial use

Manganese is a chemical element, the use of which is important not only in metallurgy. but also in other areas. In addition to pure metal, various compounds of a given atom are also of great importance. Let's designate the main ones.

1. There are several types of alloys that, thanks to manganese, have unique properties... So, for example, it is so strong and wear-resistant that it is used for smelting parts of excavators, stone processing machines, crushers, ball mills, and armor parts.
2. Manganese dioxide is an indispensable oxidizing element of electroplating; it is used to create depolarizers.
3. Many manganese compounds are needed for the organic synthesis of various substances.
4. Potassium permanganate (or potassium permanganate) is used in medicine as a strong disinfectant.
5. This element is part of bronze, brass, forms its own alloy with copper, which is used for the manufacture of aircraft turbines, blades and other parts.

Biological role

The daily requirement for manganese for humans is 3-5 mg. Deficiency of this element leads to oppression nervous system, sleep disturbance and anxiety, dizziness. Its role has not yet been fully studied, but it is clear that, first of all, it influences:

• height;
• activity of the sex glands;
• the work of hormones;
• blood formation.

This element is present in all plants, animals, humans, which proves its important biological role.

Manganese is a chemical element, interesting facts about which can impress any person, and also make them understand how important it is. Here are the most basic ones that have found their imprint in the history of this metal.

1. In hard times civil war in the USSR, one of the first export products was ore containing large amounts of manganese.
2. If manganese dioxide is fused with nitrate and then the product is dissolved in water, then amazing transformations will begin. First, the solution will turn green, then the color will change to blue, then purple. Finally, it will turn crimson and gradually brown precipitate will fall out. If the mixture is shaken, then the green color will be restored again and everything will happen again. It is for this that potassium permanganate got its name, which translates as "mineral chameleon".
3. If fertilizers containing manganese are applied to the soil, then the productivity of plants will increase and the rate of photosynthesis will increase. Winter wheat will form better grains.
4. The largest block of manganese mineral rhodonite weighed 47 tons and was found in the Urals.
5. There is a ternary alloy called manganin. It is composed of elements such as copper, manganese and nickel. Its uniqueness is that it has great electrical resistance, which does not depend on temperature, but is influenced by pressure.

Of course, this is not all that can be said about this metal. Manganese is a chemical element, interesting facts about which are quite diverse. Especially if we talk about the properties that it gives to various alloys.