Chemical properties of zinc and its compounds

Zinc is a typical representative of the group of metallic elements and has the full range of their characteristics: metallic luster, ductility, electrical and thermal conductivity. However, the chemical properties of zinc differ somewhat from the basic reactions inherent in most metals. An element can behave like a nonmetal under certain conditions, for example, react with alkalis. This phenomenon is called amphotericity. In our article we will study the physical properties of zinc, and also consider typical reactions characteristic of the metal and its compounds.

Position of the element in the periodic table and distribution in nature

The metal is located in a secondary subgroup of the second group of the periodic table. In addition to zinc, it contains cadmium and mercury. Zinc belongs to the d-elements and is in the fourth period. In chemical reactions, its atoms always give up electrons of the last energy level, therefore, in such compounds of the element as oxide, intermediate salts and hydroxide, the metal exhibits an oxidation state of +2. The structure of the atom explains all the physical and chemical properties of zinc and its compounds. The total metal content in the soil is approximately 0.01 wt. %. It is found in minerals such as galmea and zinc blende. Since the zinc content in them is low, the rocks are first subjected to enrichment, which is carried out in shaft furnaces. Most zinc-containing minerals are sulfides, carbonates and sulfates. These are zinc salts, the chemical properties of which underlie their processing processes, such as roasting.

What is zinc

Concept and features

To begin with, we bring to your attention the general characteristics of zinc. This product is not only a necessary production metal, but also an important biological element. In any living organism it is present in up to 4% of all elements. The richest deposits of zinc are Bolivia, Iran, Kazakhstan and Australia. In our country, OJSC MMC Dalpolimetal is considered one of the largest manufacturers.

If we consider zinc from the periodic table of Mendeleev, then it belongs to the transition metals and has the following characteristics:

Sequential number: 30
Weight: 65.37.
Oxidation state - +2.
Colour: bluish white.

If we consider zinc from the side of a simple substance, then this material has the following characteristics:

Type of material – metal.
Color – silver-blue.
The coating is protected by an oxide film, under which the shine and shine are hidden.

Zinc is found in the earth's crust. The share of metal in it is not very large: only 0.0076%.

Zinc does not exist as a single material. It is part of many ores and minerals.

The most common are: zinc blende, cleiophane, marmatite. In addition, zinc can be found in the following natural materials: wurtzite, franklenite, zincite, smithsonite, calamine, willemite.
The satellites of zinc are usually: germanium, cadmium, thallium, gallium, indium, cadmium.
The most popular are alloys of zinc and aluminum, copper, tin, and nickel.

A specialist will talk about the role of zinc in our lives in this video:

Competing metals

Only 4 metals can compete with zinc: titanium, aluminum, chromium and copper. The described materials have the following characteristics:

Aluminum : Silver-white in color, conducts electricity and heat well, can be worked by pressure, is resistant to corrosion, has low density, and is used in the steel production process (to improve heat resistance).
Titanium : silver-white color, high melting point, oxidizes when in contact with air, low thermal conductivity, easy to forge and stamp, at high temperatures a durable protective film is formed on the surface.
Chrome : bluish-shiny color, high hardness, brittleness, oxidation resistance under atmospheric and water conditions, used for decorative coating.
Copper : red metal, has high ductility, good electrical conductivity, high thermal conductivity, resistance to corrosion processes, used in roofing materials.

For construction purposes, other non-ferrous metals (in addition to zinc) are most often used. These include: bronze, brass, silumin, babbitt, duralumin and several others.

Advantages and disadvantages

Pros:

Good fluidity, making molds easy to fill.
High ductility during rolling.
Pure zinc is easily forged.
Due to its properties and the effects of temperature, it can take on different states.
It perfectly protects the product from corrosion, making it popular in construction and mechanical engineering.

May explode if heated together with phosphorus or sulfur.
Loses shine when exposed to air.
At room temperature it has little plasticity.
It is not found in nature in its pure form.

The mass, mechanical, chemical and physical properties of zinc, its main characteristics will be discussed below.

Metal production

The severe oxidation reaction of zinc carbonate or sulfide produces its oxide. The process takes place in a fluidized bed. This is a special method based on close contact of finely ground mineral and a stream of hot air moving at high speed. Next, zinc oxide ZnO is reduced with coke and the resulting metal vapors are removed from the reaction sphere. Another method of producing metal, based on the chemical properties of zinc and its compounds, is electrolysis of a solution of zinc sulfate. It is a redox reaction that occurs under the influence of electric current. High purity metal is deposited on the electrode.

Production

As stated, zinc is not found in nature in its pure form. It is mainly obtained from polymer ores. In these ores, zinc is present in the form of sulfide. It always comes with the accompanying metals listed above.

The selective flotation beneficiation process produces zinc concentrate. In parallel with this process, other substance concentrates are released from polymetallic ores. For example, lead and copper.

The resulting zinc concentrates are fired in a furnace. As a result of high temperatures, zinc changes from the sulfide state to the oxide state. During the production process, sulfur dioxide is released, which is used to produce sulfuric acid. Pure zinc is obtained from zinc oxide by two methods: pyrometallurgical and electrolytic.

The pyrometallurgical method has a very long history. The concentrate is fired and subjected to a sintering process. The zinc is then reduced using coal or coke. The zinc obtained by this method is brought to a pure state by settling.
In the electrolytic method, zinc concentrate is treated with sulfuric acid. The result is a solution that is subjected to the process of electrolysis. Here the zinc is deposited and melted in special furnaces.

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Physical characteristics

A bluish-silver, brittle metal under normal conditions. In the temperature range from 100° to 150°, zinc becomes flexible and can be rolled into sheets. When heated above 200°, the metal becomes unusually brittle. Under the influence of atmospheric oxygen, pieces of zinc are covered with a thin layer of oxide, and upon further oxidation it turns into hydroxycarbonate, which plays the role of a protector and prevents further interaction of the metal with atmospheric oxygen. The physical and chemical properties of zinc are interrelated. Let's consider this using the example of the interaction of a metal with water and oxygen.

In food

The element is found in meat, cheese, sesame seeds, oysters, chocolate, legumes, oatmeal, sunflower and pumpkin seeds, and is often present in mineral water. The highest percentage of zinc is found in the following products (per 100 grams):

Oysters (up to 40 mg), anchovies (1.72 mg), octopus (1.68 mg), carp (1.48 mg), caviar (up to 1 mg), herring (about 1 mg).
Pumpkin seeds (10 mg), sesame seeds (7 mg), sunflower seeds (5.3 mg), peanuts (4 mg), walnuts (3 mg), almonds (3 mg).
Beef (up to 8.4 mg), lamb (up to 6 mg), beef liver (4 mg), pork (up to 3.5 mg), chicken (up to 3.5 mg).
Cocoa powder without sugar and sweeteners (6.81 mg), pure dark chocolate (2.3 mg), chocolate candies (up to 2 mg depending on the amount and type of chocolate).
Lentils (4.78 mg), oats (3.97 mg), wheat (3.46 mg), soybeans (3 mg), rye (2.65 mg), bread (up to 1.5 mg), green peas (1.24 mg), peas (1.2 mg), bamboo shoots (1.1 mg), rice (1 mg), cereal cookies (up to 1 mg).
Hard cheese (up to 4 mg).

Redox reactions involving zinc

Since the element comes before hydrogen in the activity series of metals, it is able to displace it from acid molecules.

The reaction products between zinc and acids will depend on two factors:

type of acid
its concentration

Dilute sulfuric acid, which does not exhibit pronounced oxidizing properties, reacts with the metal according to the following scheme:

H₂SO₄ + Zn = ZnSO₄ + H₂↑

Reactions of the element with phosphoric and dilute sulfuric acids proceed in the same way. The chemical properties and reactions of zinc with nitrate acid have their own characteristics. A dilute solution of nitric acid of average concentration and zinc interact with each other to form nitrogen oxide (II), water and an average salt - zinc nitrate. Concentrated nitrate acid reacts with the metal in such a way that nitric oxide (IV), average salt and water can be detected in the products.

A very dilute solution of nitric acid and zinc as a reducing agent react to form zinc nitrate, water, and several possible products: ammonia, free nitrogen, or nitric oxide.

Features of smelting

The temperature required to melt zinc should be less than 419 C o, but not more than 480 C o. Otherwise, metal waste will increase and wear on the walls of the bath, which is usually made from iron, will increase. In the molten state, no more than 0.05% iron admixture is allowed, otherwise the temperature required for melting will begin to rise. If the percentage of iron content exceeds 0.2%, zinc cannot be rolled.

Zinc is obtained from polymetallic ores, which can contain up to 4% of the element . If the ores have been enriched by selective flotation, up to 60% of zinc concentrates can be obtained from them, the rest will be occupied by concentrates of other metals. Zinc concentrates are fired in furnaces in a fluidized bed, after which zinc sulfide turns into oxide and sulfur dioxide is released. The latter is consumed: sulfuric acid is obtained from it.

To convert zinc oxide into the metal itself, two methods are used.

Distillation or pyrometallurgical. The concentrate is fired, then sintered to impart gas permeability and granularity and reduced with coke or coal at temperatures of 1200-1300 C o. During the reaction, metal vapors are formed, which are condensed and poured into molds. The purity of zinc reaches 98.7%, after which it can be increased to 99.995% using rectification, but the latter method is quite expensive and complex.
Electrolytic or hydrometallurgical. The fired concentrates are treated with sulfuric acid, the solution is cleaned of impurities using zinc dust and subjected to electrolysis in bathtubs lined with lead or vinyl plastic. Zinc is deposited on aluminum cathodes, from where it is collected and melted in induction furnaces. The purity of the metal obtained by this method reaches 99.95%.

Chemical properties of zinc

The reaction equations for the interaction of a metal with alkali solutions confirm its amphoteric properties. Complex salts - tetrahydroxycinates and hydrogen - are found in the products.

Zn + 2NaOH + 2H2O = Na2 [Zn(OH)4] + H2

By fusing solid alkali and metal, they obtain salts of another type - zincates. A by-product of such a process will also be hydrogen gas.

Zn + 2KOH = K2ZnO2 + H2

The metal actively interacts with halogens, for example, chlorine, bromine or iodine, as well as with nitrogen, sulfur and carbon. As a result, intermediate salts are formed - nitrides, sulfides or carbides.

In the activity series of metals, zinc is placed before hydrogen and is therefore an active metal. However, it is inferior in its properties to alkali and alkaline earth metals.

Areas of use

Zinc, as an element, is found in sufficient quantities in the earth's crust and in water resources.

In the production of oil paints.
In the manufacture of rubber tires.
In medicine.
Capable of reducing noble metals.
Used as a protective agent against corrosion.
Used in the printing industry.
Used in the manufacture of batteries.

Half of all zinc production is used to perform the “corrosion protection” function. Thanks to its properties, critical parts (for example, for aircraft) are successfully cast from zinc. Zinc is widely used in conjunction with copper and lead.

Zinc is also used in powder form for a number of chemical and technological processes.

This video will tell you how to remove zinc:

Zinc is an element of the secondary subgroup of the second group, the fourth period of the periodic table of chemical elements of D.I. Mendeleev, with atomic number 30. It is designated by the symbol Zn (lat. Zincum). The simple substance zinc under normal conditions is a brittle transition metal of a bluish-white color (it becomes dull in air, becoming covered with a thin layer of zinc oxide).

In the fourth period, zinc is the last d-element, its valence electrons are 3d 10 4s 2.

Only electrons from the outer energy level participate in the formation of chemical bonds, since the d 10 configuration is very stable. In compounds, zinc has an oxidation state of +2.

Zinc is a chemically active metal, has pronounced reducing properties, and is inferior in activity to alkaline earth metals. Exhibits amphoteric properties.

Interaction of zinc with nonmetals

When strongly heated in air, it burns with a bright bluish flame to form zinc oxide: 2Zn + O2 → 2ZnO.

When ignited, it reacts vigorously with sulfur: Zn + S → ZnS.

It reacts with halogens under normal conditions in the presence of water vapor as a catalyst: Zn + Cl2 → ZnCl2.

When phosphorus vapor acts on zinc, phosphides are formed: Zn + 2P → ZnP2 or 3Zn + 2P → Zn3P2.

Zinc does not interact with hydrogen, nitrogen, boron, silicon, or carbon.

Interaction of zinc with water

Reacts with water vapor at red heat to form zinc oxide and hydrogen: Zn + H2O → ZnO + H2.

Interaction of zinc with acids

In the electrochemical voltage series of metals, zinc is located before hydrogen and displaces it from non-oxidizing acids: Zn + 2HCl → ZnCl2 + H2; Zn + H2SO4 → ZnSO4 + H2.

Reacts with dilute nitric acid, forming zinc nitrate and ammonium nitrate: 4Zn + 10HNO3 → 4Zn(NO3)2 + NH4NO3 + 3H2O.

Reacts with concentrated sulfuric and nitric acids to form zinc salt and acid reduction products: Zn + 2H2SO4 → ZnSO4 + SO2 + 2H2O; Zn + 4HNO3 → Zn(NO3)2 + 2NO2 + 2H2O

Interaction of zinc with alkalis

Reacts with alkali solutions to form hydroxo complexes: Zn + 2NaOH + 2H2O → Na2[Zn(OH)4] + H2

when fused, it forms zincates: Zn + 2KOH → K2ZnO2 + H2.

Interaction with ammonia

With gaseous ammonia at 550–600°C it forms zinc nitride: 3Zn + 2NH3 → Zn3N2 + 3H2; dissolves in an aqueous solution of ammonia, forming tetraammine zinc hydroxide: Zn + 4NH3 + 2H2O → [Zn(NH3)4](OH)2 + H2.

Interaction of zinc with oxides and salts

Zinc displaces metals located in the voltage series to the right of it from solutions of salts and oxides: Zn + CuSO4 → Cu + ZnSO4; Zn + CuO → Cu + ZnO.

Zinc(II) oxide ZnO

– white crystals, when heated they acquire a yellow color. Density 5.7 g/cm 3, sublimation temperature 1800°C. At temperatures above 1000°C, it is reduced to metallic zinc by carbon, carbon monoxide and hydrogen: ZnO + C → Zn + CO; ZnO + CO → Zn + CO2; ZnO + H2 → Zn + H2O.

Does not interact with water. Exhibits amphoteric properties, reacts with solutions of acids and alkalis: ZnO + 2HCl → ZnCl2 + H2O; ZnO + 2NaOH + H2O → Na2[Zn(OH)4].

When alloyed with metal oxides, it forms zincates: ZnO + CoO → CoZnO2.

When interacting with non-metal oxides, it forms salts, where it is a cation: 2ZnO + SiO2 → Zn2SiO4, ZnO + B2O3 → Zn(BO2)2.

Zinc(II) hydroxide Zn(OH)2

– a colorless crystalline or amorphous substance. Density 3.05 g/cm 3, at temperatures above 125°C it decomposes: Zn(OH)2 → ZnO + H2O.

Zinc hydroxide exhibits amphoteric properties, easily dissolves in acids and alkalis: Zn(OH)2 + H2SO4 → ZnSO4 + 2H2O; Zn(OH)2 + 2NaOH → Na2[Zn(OH)4];

also easily dissolves in an aqueous solution of ammonia to form tetraamminium zinc hydroxide: Zn(OH)2 + 4NH3 → [Zn(NH3)4](OH)2.

It is obtained in the form of a white precipitate when zinc salts react with alkalis: ZnCl2 + 2NaOH → Zn(OH)2 + 2NaCl.

Zinc or Zincum is element 30 of Mendeleev's periodic table of chemical elements and is designated by the symbol Zn. It is mainly used in the creation of deformed semi-finished products and as part of various types of mixtures. In its pure form, it looks like a brittle metal of a bluish-silver color; it quickly oxidizes and becomes covered with a protective film (oxide), due to which it noticeably tarnishes.

It is mined in Kazakhstan, Australia, Iran and Bolivia. Due to the difficulties in identifying the metal, it is often called "blende" .

Use of zinc in galvanic cells

The chemical properties of zinc underlie the operating principle of various types of galvanic devices. The manganese-zinc element is the most common in technology. It works by undergoing a redox reaction between the metal and manganese dioxide. Both electrodes are made from them and placed inside the device. The active substance - ammonium chloride - has the form of a paste, or porous plates inserted between the cathode and anode are impregnated with it. The zinc air element is represented by a negative zinc electrode - cathode. The anode is a carbon-graphite rod filled with air. Solutions of ammonium chloride or sodium hydroxide are used as an electrolyte.

Zinc oxide

A white porous powder that turns yellow when heated and returns to its original color when cooled is a metal oxide. The chemical properties of zinc oxide and the reaction equations for its interaction with acids and alkalis confirm the amphoteric nature of the compound. Thus, the substance cannot react with water, but interacts with both acids and alkalis. The reaction products will be medium salts (in case of interaction with acids) or complex compounds - tetrahydroxocinates.

Zinc oxide is used in the production of white paint, which is called zinc white. In dermatology, the substance is included in ointments, powders and pastes that have an anti-inflammatory and drying effect on the skin. Most of the zinc oxide produced is used as a filler for rubber. Continuing to study the chemical properties of zinc and its compounds, let's consider Zn(OH)2 hydroxide.

Application

Zinc is one of the most popular metals in the world: it is in third place in terms of production among non-ferrous metals, second only to copper and aluminum. This is also facilitated by its low price. It is most often used for corrosion protection and as part of an alloy such as brass.

In metallurgy, zinc is especially valuable. It is applied in a thin layer to the steel surface of many metal structures to completely protect them from rust on a mechanical and chemical level. Up to 40% of all production is spent on this. Since zinc, unlike nickel, cobalt, tin and cadmium, is more active than iron, it is the first to come into contact with an unfriendly external environment, completely protecting the base.
Pure metal is used to recover precious metals after mining by leaching. It is also used to extract gold and silver from rough lead.
Zinc is the most electropositive metal and practically does not react to water. This made it possible to create a large number of different chemical current sources: zinc-air, silver-zinc, mercury-zinc, “dry” Leclanchet elements.
Zinc dust is used in fireworks and pyrotechnics to create blue fire, and in paint, especially zinc white, for anti-corrosion protection and better adhesion to the substrate. It is also used to displace precious metals from cyanide solutions and to purify zinc sulfate solutions from cadmium and copper.
In printing, zinc is used for casting fonts and printing illustrations: zincography has been used since the 19th century. In this case, the printing plate is prepared on a zinc base with a small - no more than 5% - addition of other metals. Before each etching, the plate is annealed and rolled in a heated state.
In medicine, zinc oxide is used as an antiseptic in the ointments “Lassara Paste”, “Sudocrem”, “Zinc Ointment”, as well as as a powder, toothpastes and material for cementing teeth. Metal is used to create bactericidal ceilings and self-cleaning surfaces. Previously, zinc was used for photocatalytic water purification on an industrial scale.

Amphoteric nature of zinc hydroxide

The white precipitate that precipitates under the action of alkali on solutions of metal salts is the base of zinc. The compound dissolves quickly when exposed to acids or alkalis. The first type of reaction ends with the formation of medium salts, the second - zincates. Complex salts—hydroxycinates—are isolated in solid form. A special feature of zinc hydroxide is its ability to dissolve in an aqueous solution of ammonia to form tetraamminium zinc hydroxide and water. Zinc base is a weak electrolyte, therefore both its average salts and zincates in aqueous solutions are hydrolyzable, that is, their ions react with water and form zinc hydroxide molecules. Solutions of metal salts such as chloride or nitrate will be acidic due to the accumulation of excess hydrogen ions.

Characteristics of zinc sulfate

The chemical properties of zinc that we examined earlier, in particular, its reactions with dilute sulfate acid, confirm the formation of an average salt - zinc sulfate. These are colorless crystals, which, when heated to 600° and above, can produce oxosulfates and sulfur trioxide. With further heating, zinc sulfate is converted to zinc oxide. The salt is soluble in water and glycerin. The substance is isolated from solution at temperatures up to 39°C in the form of crystalline hydrate, the formula of which is ZnSO4 × 7H2O. In this form it is called zinc sulfate.

In the temperature range 39°-70°, a hexahydrate salt is obtained, and above 70° only one molecule of water remains in the crystalline hydrate. The physicochemical properties of zinc sulfate make it possible to use it as a bleach in paper production, as a mineral fertilizer in crop production, and as a fertilizer in the diet of domestic animals and poultry. In the textile industry, the compound is used in the production of viscose fabric and in the dyeing of chintz.

Zinc sulfate is also included in the electrolyte solution used in the process of galvanic coating of iron or steel products with a layer of zinc using the diffuse method or hot-dip galvanizing method. A layer of zinc protects such structures from corrosion for a long time. Considering the chemical properties of zinc, it should be noted that in conditions of high salinity of water, significant fluctuations in temperature and air humidity, galvanizing does not give the desired effect. Therefore, metal alloys with copper, magnesium and aluminum are widely used in industry.

Historical reference

The name “zinc” itself was first mentioned in the book “Liber Mineralium” by Paracelsus. According to some sources, it meant “prong.” The alloy of zinc with copper or brass has been known for a long time. It was used in Ancient Greece, India and Ancient Egypt, and later the material became known in China.

The metal was obtained in its pure form only in the first half of the 18th century in 1738 in Great Britain using the distillation method. Its discoverer was William Champion. Industrial production began 5 years later, and in 1746 in Germany, the chemist Andreas Sigismund Marggraff developed and described in detail his own method for producing zinc . He proposed using the method of calcining a mixture of metal oxide and coal in fireproof clay retorts without air access. Subsequent condensation of the vapors had to take place in the refrigerator. Due to his detailed description and painstaking development, Marggraf is often called the discoverer of the substance.

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At the beginning of the 19th century, a method was found for isolating metal by rolling at 100 C o -150 C o . At the beginning of the next century, they learned to extract zinc using the electrolytic method. In Russia, the first metal was produced only in 1905.

Application of alloys containing zinc

Transporting many chemicals, such as ammonia, through pipelines requires special requirements for the composition of the metal from which the pipes are made. They are made on the basis of alloys of iron with magnesium, aluminum and zinc and have high anti-corrosion resistance to aggressive chemical environments. In addition, zinc improves the mechanical properties of alloys and neutralizes the harmful effects of impurities such as nickel and copper. Copper and zinc alloys are widely used in industrial electrolysis processes. Tankers are used to transport petroleum products. They are built from aluminum alloys containing, in addition to magnesium, chromium and manganese, a large proportion of zinc. Materials of this composition not only have high anti-corrosion properties and increased strength, but also cryogenic resistance.

Mixtures and alloys

To enhance strength and increase the melting point, the metal is mixed with copper, aluminum, tin, magnesium and lead.

The most famous and sought after alloy is brass. This is a mixture of copper with the addition of zinc, sometimes tin, nickel, manganese, iron, and lead are also found. The density of brass reaches 8700 kg/m3 . The temperature required for melting is kept at around 880 C o - 950 C o: the higher the zinc content in it, the lower it is. The alloy perfectly resists unfavorable external environments, although it turns black in air if not varnished, it is perfectly polished and welded by resistance welding.

There are two types of brass:

Alpha brass: more ductile, bends well in any condition, but wears out more.
Alpha+beta brass: deforms only when heated, but is more wear-resistant. Often alloyed with magnesium, aluminum, lead and iron. This increases strength, but reduces ductility.

Zamak or Zamac alloy is composed of zinc, aluminum, copper and magnesium . The name itself is formed from the first letters of the Latin names: Zink - Aluminum - Magnesium - Kupfer / Cuprum (Zinc-Aluminum-Magnesium-Copper). In the USSR, the alloy was known as TsAM: Zinc-Aluminum-Copper. Actively used in injection molding, melting begins at low temperatures (381 C o - 387 C o) and has a low coefficient of friction (0.07). It has increased strength, which makes it possible to produce products of complex shapes that are not afraid of breaking: door handles, golf clubs, firearms, construction fittings, fasteners of various types and fishing tackle.

The role of zinc in the human body

The Zn content in cells is 0.0003%, so it is classified as a microelement. The chemical properties and reactions of zinc and its compounds play an important role in metabolism and maintaining a normal level of homeostasis, both at the level of the cell and the entire organism as a whole. Metal ions are part of important enzymes and other biologically active substances. For example, it is known that zinc has a serious effect on the formation and functions of the male reproductive system. It is part of the coenzyme of the hormone testosterone, which is responsible for the fertility of seminal fluid and the formation of secondary sexual characteristics. The non-protein part of another important hormone, insulin, produced by the beta cells of the islets of Langerhans in the pancreas, also contains a trace element. The immune status of the body is also directly related to the concentration of Zn+2 ions in cells, which are found in the thymus hormone - thymulin and thymopoietin. A high concentration of zinc is recorded in nuclear structures - chromosomes containing deoxyribonucleic acid and participating in the transmission of hereditary information of the cell.

In our article, we studied the chemical functions of zinc and its compounds, and also determined its role in the life of the human body.

In living organisms

The human body contains about 2 grams of zinc , and about 400 enzymes contain it. The latter include enzymes that catalyze the hydrolysis of proteins, esters and leptids, the polymerization of RNA and DNA, and the formation of aldehydes. The pure element is found in muscles, pancreas and liver. Men require 11 mg of zinc per day, women - 8 mg.

In the body, zinc performs the following functions:

Normalizes prostate activity;
Promotes vitamin E metabolism;
Takes part in the synthesis of anabolic hormones: growth hormone, insulin, testosterone and others;
Participates in the production of male hormones and sperm;
Helps break down alcohol in the body.

With a deficiency of the element in the body, rapid fatigue, irritability , memory loss, loss of vision and weight without an objective reason, allergy attacks, and depression are observed. There is a decrease in insulin levels and accumulation of certain elements in the body: iron, lead, copper, cadmium.