Zn is what metal?

Is zinc a metal or non-metal?

 Zinc is a brittle, bluish-white transition metal (tarnishes in air, becoming coated with a thin layer of zinc oxide).
  Essential (irreplaceable) microelement of human tissues. In terms of quantitative ratio in the body, it ranks second, after iron, in place. It plays a key role in the regeneration of damaged tissues, since without zinc the synthesis of nucleic acids and proteins is disrupted.

STRUCTURE

Zinc crystals have a hexagonal packing of atoms. But unlike the dense hexagonal packing of spherical atoms, zinc lattices are elongated in one direction. Each atom is surrounded by six other atoms lying in the same plane or layer. The distance between the centers of neighboring atoms in this flat layer is equal to 0.26649 nm. The external electronic configuration of the atom is 3d104s2. Not polymorphic.

PROPERTIES

At room temperature it is fragile; when the plate is bent, a cracking sound is heard from the friction of the crystallites (usually stronger than the “cry of tin”). Has a low melting point. The volume of metal during melting increases in accordance with the decrease in density.

With increasing temperature, the kinetic viscosity and electrical conductivity of zinc decrease and its electrical resistivity increases. At 100-150 °C zinc is plastic. Impurities, even minor ones, dramatically increase the fragility of zinc.

Is diamagnetic.

Reserves and production

The average zinc content in the earth's crust is 8.3·10-3%; in basic igneous rocks it is slightly higher (1.3·10-2%) than in acidic rocks (6·10-3%). Zinc is an energetic aquatic migrant; its migration in thermal waters along with lead is especially characteristic.

Zinc sulfides, which are of industrial importance, precipitate from these waters. Zinc also migrates vigorously in surface and underground waters; the main precipitant for it is hydrogen sulfide; sorption by clays and other processes play a lesser role.

Zinc deposits are known in Iran, Australia, Bolivia, and Kazakhstan. In Russia, the largest producer of lead-zinc concentrates is JSC MMC Dalpolimetal

Zinc is extracted from polymetallic ores containing 1-4% Zn in the form of sulfide, as well as Cu, Pb, Ag, Au, Cd, Bi. Ores are enriched by selective flotation, obtaining zinc concentrates (50-60% Zn) and at the same time lead, copper, and sometimes also pyrite concentrates.

The main method of obtaining zinc is electrolytic (hydrometallurgical). Calcined concentrates are treated with sulfuric acid; the resulting sulfate solution is cleaned of impurities (by precipitating them with zinc dust) and subjected to electrolysis in baths tightly lined inside with lead or vinyl plastic.

Zinc is deposited on aluminum cathodes, from which it is removed (stripped off) daily and melted in induction furnaces.

ORIGIN

Zinc does not occur in nature as a native metal. There are 66 known zinc minerals, in particular zincite, sphalerite, willemite, calamine, smithsonite, and franklinite. The most common mineral is sphalerite, or zinc blende. The main component of the mineral is zinc sulfide ZnS, and various impurities give this substance all kinds of colors.

Due to the difficulty of identifying this mineral, it is called blende (ancient Greek σφαλερός - deceptive). Zinc blende is considered the primary mineral from which other minerals of element No. 30 were formed: smithsonite ZnCO3, zincite ZnO, calamine 2ZnO · SiO2 · H2O. In Altai you can often find striped “chipmunk” ore - a mixture of zinc blende and brown spar.

From a distance, a piece of such ore really looks like a hidden striped animal.

APPLICATION

Pure zinc metal is used to recover precious metals mined by underground leaching (gold, silver). In addition, zinc is used to extract silver, gold (and other metals) from crude lead in the form of zinc-silver-gold intermetallic compounds (so-called “silver foam”), which are then processed by conventional refining methods.

It is used to protect steel from corrosion (galvanization of surfaces not subject to mechanical stress, or metallization - for bridges, tanks, metal structures).

Zinc is used as a material for the negative electrode in chemical power sources, that is, in batteries and accumulators.

Zinc plates are widely used in printing, in particular, for printing illustrations in large-circulation publications. For this purpose, zincography has been used since the 19th century - making cliches on a zinc plate by etching the design in it with acid. Impurities, with the exception of a small amount of lead, impair the etching process. Before etching, the zinc plate is annealed and rolled in a heated state.

Zinc is added to many hard solders to reduce their melting point.

Zinc oxide is widely used in medicine as an antiseptic and anti-inflammatory agent. Zinc oxide is also used to produce paint - zinc white.

Zinc is an important component of brass. Zinc alloys with aluminum and magnesium (ZAM, ZAMAK), due to their relatively high mechanical and very high casting qualities, are very widely used in mechanical engineering for precision casting.

In particular, in the arms industry, pistol bolts are sometimes cast from the ZAMAK (-3, −5) alloy, especially those designed for the use of weak or traumatic cartridges.

Also, all kinds of technical accessories are cast from zinc alloys, such as car handles, carburetor bodies, scale models and all kinds of miniatures, as well as any other products that require precise casting with acceptable strength.

Zinc chloride is an important flux for metal soldering and a component in fiber production.

Zinc telluride, selenide, phosphide, and sulfide are widely used semiconductors. Zinc sulfide is an integral part of many phosphors. Zinc phosphide is used as a rodent poison.

Zinc selenide is used to make optical glasses with very low absorption coefficients in the mid-infrared region, such as in carbon dioxide lasers.

Zinc - Zn

Crystallographic properties

Source: http://ooo-asteko.ru/tsink-eto-metall-ili-nemetall/

Zinc: production and application

Zinc is a metal that is number 30 on the periodic table and has the designation Zn. It melts at a temperature of 419 °C, but if the boiling point is 913 °C, it begins to turn into steam. At normal temperatures, the condition is fragile, but at one hundred degrees it begins to bend.

The color of zinc is blue-white. When exposed to oxygen, oxidation occurs, as well as a coating of carbonate, which protects the metal from further oxidation reactions. The appearance of hydroxide on zinc means that water has no effect on the chemical element.

Zinc is a chemical element that has its own distinctive properties, advantages and disadvantages. It is widely used in human daily life, in pharmaceuticals and metallurgy.

Zinc

Features of zinc

Metal is necessary and widely used in almost all areas of daily human life.

Mining is mainly carried out in Iran, Kazakhstan, Australia, and Bolivia. In Russia, the manufacturer is OJSC GMK Dalpolimetal.

It is a transition metal, has an oxidation state of +2, a radioactive isotope, a half-life of 244 days.

Aqueous cadmium, zinc and copper arsenate

The element is not mined in its pure form. Contained in ores and minerals: cleiophane, marmatite, wurtzite, zincite. It is necessarily present in an alloy with aluminum, copper, tin, and nickel.

Chemical, physical properties and characteristics of zinc

Zinc is a metal that has a number of properties and characteristics that distinguish it from other elements of the periodic table.

The physical properties of zinc include its state. The main factor is temperature.

If at room temperature it is a brittle material, the density of zinc is 7130 kg/m3 (˃ the density of steel), which practically does not bend, then when raised, it easily bends and is rolled into sheets in factories.

If you take a higher temperature regime, the material acquires a liquid state, and if you raise the temperature by 400-450 °C degrees, then it will simply evaporate. This is uniqueness - changing your condition. If exposed to acids and alkalis, it can crumble, explode, or melt.

Liquid zinc

The formula of zinc is Zn – zinc. The atomic mass of zinc is 65.382 amu.

Electronic formula: the nucleus of a metal atom contains 30 protons, 35 neutrons. There are 4 energy levels in an atom - 30 electrons. (Fig. structure of the zinc atom) 1s22s22p63s23p63d104s2.

The crystal lattice of zinc is a hexagonal crystal system with tightly pressed atoms. Lattice data: A=2.66U, C=4.94.

Mined and not processed material has isotopes 64, 66, 67, electrons 2-8-18-2.

In terms of application, among all the elements of the periodic table, the metal ranks 23rd. In nature, the element appears in the form of sulfide with impurities of lead Pb, cadmium Cd, iron Fe, copper Cu, silver Ag.

Zinc sulfide

Depending on the amount of impurities, the metal is marked.

Zinc production

As mentioned above, there is no pure form of this element in nature. It is mined from other rocks, such as ore - cadmium, gallium, minerals - sphalerite.

The metal is obtained at the factory. Each plant has its own distinctive production features, so the equipment for obtaining pure material is different. It could be like this:

• The rotors, located vertically, are electrolytic.
• Special furnaces with a sufficiently high temperature for firing, as well as special electric furnaces.
• Conveyors and baths for electrolysis.

Depending on the metal mining method adopted, the appropriate equipment is used.

Obtaining pure zinc

As mentioned above, there is no pure species in nature. It is mainly extracted from ores in which it comes with various elements.

To obtain pure material, a special flotation process with selectivity is used. After the process, the ore breaks down into elements: zinc, lead, copper and so on.

The pure metal extracted by this method is fired in a special furnace. There, at certain temperatures, the sulfide state of the material turns into oxide. During roasting, gas containing sulfur is released, which is used to produce sulfuric acid.

Pure zinc

There are 2 ways to obtain metal:

1. Pyrometallurgical - the burning process takes place, after which the resulting mass is restored with the help of black coal and coke. The final process is settling.
2. Electrolytic – the extracted mass is treated with sulfuric acid. The resulting solution is subjected to electrolysis, during which the metal settles and is melted in furnaces.

Smelting zinc in a furnace

The melting temperature of zinc in a furnace is 419-480 °C degrees. If the temperature is exceeded, then the material begins to evaporate. At this temperature, an admixture of iron of 0.05% is allowed.

At an iron interest rate of 0.2, the sheet cannot be rolled.

Various methods are used for smelting pure metal, up to the production of zinc vapor, which is sent to special tanks and there the substance falls down.

Application of metal

The properties of zinc allow its use in many areas. As a percentage:

1. Galvanizing – up to 60%.
2. Medicine – 10%.
3. Various alloys containing this metal 10%.
4. Tire production 10%.
5. Paint production – 10%.

Copper-zinc alloy

The use of zinc is also necessary for the restoration of metals such as gold, silver, and platinum.

Zinc in metallurgy

The metallurgical industry uses this element of the periodic table as the main one to achieve certain goals. The smelting of cast iron and steel is the main one in the entire metallurgy of the country. But these metals are susceptible to negative environmental influences. Without certain treatment, metals rapidly oxidize, which leads to their deterioration. The best protection is galvanizing.

Applying a protective film to cast iron and steel is the best remedy against corrosion. About 40% of the total production of pure material is spent on galvanizing.

Galvanizing methods

Metallurgical plants are distinguished not only by their equipment, but also by the production methods used. It depends on the pricing policy, and location (natural resources used for the metallurgical industry). There are several galvanizing methods, which are discussed below.

Hot galvanizing method

This method involves dipping a metal part in a liquid solution. It happens like this:

1. The part or product is degreased, cleaned, washed and dried.
2. Next, the zinc is melted to a liquid state at temperatures up to 480 °C.
3. The prepared product is lowered into the liquid solution. At the same time, it is well wetted in the solution and a coating up to 450 microns thick is formed. This is 100% protection against the effects of external factors on the product (moisture, direct sunlight, water with chemical impurities).

Hot galvanizing of metal structures

But this method has a number of disadvantages:

• The zinc film on the product results in an uneven layer.
• This method cannot be used for parts that meet exact standards according to GOST. Where every millimeter is considered a defect.
• After hot-dip galvanizing, not every part will remain strong and wear-resistant, since brittleness appears after passing through high temperatures.

This method is also not suitable for products coated with paints and varnishes.

Cold galvanizing

This method has 2 names: galvanic and electrolytic. The method of coating a product with corrosion protection is as follows:

1. The metal part, the product is prepared (degreased, cleaned).
2. After this, the “staining method” is carried out - a special composition is used, which has the main component - zinc.
3. The part is coated with this composition by spraying.

Cold galvanizing

Thanks to this method, parts with precise tolerances and products coated with paints and varnishes are protected. Increases resistance to external factors leading to corrosion.

Disadvantages of this method: thin protective layer - up to 35 microns. This results in less protection and shorter protection periods.

Thermal diffusion method

This method makes a coating that is an electrode with positive polarity, while the metal of the product (steel) becomes negative polarity. An electrochemical protective layer appears.

The method is applicable only if the parts are made of carbon steel, cast iron, or steel with impurities. Zinc is used in the following ways:

1. At temperatures from 290 °C to 450 °C in a powder medium, the surface of the part is saturated with Zn. Here, the marking of the steel, as well as the type of product, matter - the appropriate temperature is selected.
2. The thickness of the protective layer reaches 110 microns.
3. A product made of steel or cast iron is placed in a closed tank.
4. A special mixture is added there.
5. The last step is special treatment of the product to prevent the appearance of white efflorescence from salt water.

Thermal diffusion galvanizing

This method is mainly used when it is necessary to coat parts that have a complex shape: threads, small strokes. The formation of a uniform protective layer is important, since these parts undergo multiple exposures to external aggressive environments (constant moisture).

This method provides the highest percentage of product protection against corrosion. Galvanized coating is wear-resistant and practically indestructible, which is very important for parts that are rotated and disassembled over time.

Other uses of zinc

In addition to galvanizing, the metal is also used in other industries.

1. Zinc sheets. To produce sheets, rolling is performed, in which ductility is important. It depends on the temperature. A temperature of 25 °C gives plasticity only in one plane, which creates certain properties of the metal. The main thing here is why the sheet is made. The higher the temperature, the thinner the metal becomes. Depending on this, the product is marked Ts1, Ts2, Ts3. After this, various products for cars, profiles for construction and repair, for printing, and so on are created from the sheets.
2. Zinc alloys. For improved properties of metal products, zinc is added. These alloys are created at high temperatures in special furnaces. The most commonly produced alloys are copper and aluminum. These alloys are used for the production of bearings and various bushings, which are applicable in mechanical engineering, shipbuilding and aviation.

In household use, a galvanized bucket, trough, and sheets on the roof are the norm. Zinc is used, not chromium or nickel. And it’s not just that galvanizing is cheaper than coating with other materials. This is the most reliable and long-lasting protective material than chrome or other materials used.

As a result, zinc is the most common metal widely used in metallurgy. In mechanical engineering, construction, medicine, the material is used not only as protection against corrosion, but also to increase strength and long service life. In private houses, galvanized sheets protect the roof from precipitation; in buildings, walls and ceilings are lined with plasterboard sheets based on galvanized profiles.

Almost every housewife has a galvanized bucket or trough in her house, which she uses for a long time.

Source: https://stankiexpert.ru/spravochnik/materialovedenie/proizvodstvo-i-primenenie-cinka.html

Zinc mining, application. Physical and chemical properties of metal

Under standard conditions, zinc is a brittle metal. It has a white-bluish color.

History of metal

For a long time, zinc could not be obtained in its pure form. This was first done in 1738. The author of the discovery was William Champion. At the same time, the metallurgist patented its distillation version.

5 years later, in 1743, the same metallurgist opened the first plant. In 1746, chemist A.S. Marggraf developed a similar option for obtaining pure zinc. In 1805, rolling was patented as a metal processing method in Sheffield, England. It was produced at 1500C.

In Russia, zinc was produced at the Alagir metallurgical plant. The event dates back to the beginning of 1905. The electrolytic method of producing metal began to be used in 1915 at American and Canadian factories.

Where does the name "zinc" come from?

The word “zinc” began to appear in various sources from the first half of the 16th century. The name "zincum" as well as "zinken" is mentioned in the works of the Swiss alchemist Paracelsus. In German, the term "zinke" means "tooth". Metal crystallites resemble needles in appearance.

Zinc in nature

There are about 66 types of zinc. Sphalerite is more common than others. It is also called zinc blende. The metal is mostly present in igneous rocks.

The molar mass of zinc is 65.38 g/mol. Migration of the element is noted in both underground and surface waters. Hydrogen sulfide is a good precipitant for zinc. Metal is an important component of living organisms.

The world's largest zinc deposits

Zinc mining due to extensive deposits of the metal is developed in China, Australia, Peru, and the USA. There are also significant deposits in Kazakhstan. Major players on the zinc exchange are India, Canada, and Mexico.

Specifics of metal production

The hydrometallurgical method serves as the basic option for obtaining metal. First, the concentrates are fired. Subsequently, they are treated with sulfuric acid. The result is a sulfate solution. It is purified from impurities. Then electrolysis is carried out in special lead baths.

As a result of electrolysis, zinc is deposited on aluminum cathodes. Pure metal is removed from them every day, after which it is melted in induction furnaces.

Interesting fact! Zinc is not found in its native form anywhere in nature.

Properties of zinc metal include the following characteristics:

• average ductility;
• white-silver color;
• fragility.

The physical properties of zinc are such that its plasticity at a temperature of 1000C becomes high. The fragility of an element increases with the presence of even small amounts of impurities.

Chemical signatures

The following properties of zinc are noted:

• formation of amphoteric compounds;
• active reaction with acid solutions and alkaline media;
• lack of direct reaction with hydrogen and carbon;
• formation of aqua complexes by metal ions in aqueous solutions.

The chemical properties of zinc are also characteristic in the form of an electronegativity index of 1.65. The electrode potential of the metal is -0.76 V.

Application

The metal is used as follows:

• to protect steel from the corrosion process;
• as a component of zinc-air batteries;
• in printing;
• as a component of hard solders to reduce their melting point;
• for making paint;
• as an antiseptic and anti-inflammatory agent;
• in the manufacture of brass;
• in the production of phosphors;
• for the production of optical glasses.

World production, reserves and extraction methods

About 10 million tons are produced worldwide. The chemical element zinc is predominantly mined in China. This country accounts for 29% or 3.5 million tons. The top three zinc reserves are Peru and Australia. The top 5 list also includes India and the USA.

In Russia, zinc reserves amount to 190 thousand tons. This is 11th place among all leading countries in zinc production.

Interesting fact! Zinc ranks fourth in terms of use among all known metals. Iron comes in first place, aluminum comes in second, and copper comes in third.

The element is mainly mined by open-pit mining. To do this, a quarry is formed using heavy equipment. Today this is the most affordable option for metal mining. The closed type of mining is used much less frequently. The creation of underground quarries is considered an unprofitable undertaking.

Importance for the body

The element in an amount of 2 g is mainly found in the liver, muscles and pancreas. The presence of zinc in over 400 enzymes is noted.

The element plays the following role:

• participates in the production of sperm and hormones in men;
• takes part in the transformation of vitamin E;
• normalizes prostate function;
• takes part in the synthesis of testosterone and insulin;
• participates in the breakdown of alcohol.

Zinc and its concentration in products

The leading products in terms of the content of this element are oysters, pumpkin and sunflower seeds, sesame seeds, cheese, legumes, meat and chocolate. The presence of metal in mineral water is noted.

Interesting fact! 100 g of oysters can contain up to 40 mg of zinc. This is the richest food product in this microelement. In second place in terms of its content are pumpkin seeds (10 mg).

Taking into account the characteristics of zinc, a deficiency of this element can provoke in a person:

• fatigue;
• memory impairment;
• irritability;
• depression;
• blurred vision;
• weight loss;
• decreased insulin levels;
• allergic reactions;
• anemia.

Metal toxicity

Given the formula of zinc, the element can be toxic to humans. Zinc sulfates are dangerous, causing growth disturbances, anemia and even infertility. Zinc oxide poisoning causes loss of appetite, thirst and a sweet taste in the mouth. Subsequently, the person becomes drowsy and begins to feel chest pain. He develops a dry cough.

Dynamics of zinc prices, forecast for 2018

Since the beginning of the year, there has been a general negative dynamics in zinc prices. If in February 2018, per ton of metal was $3,577.25, then as of May 18, the London Metal Exchange (LME) set the zinc rate at $3,096.50.

Where to invest money in 2018?

In 2016, zinc had the status of the most profitable and suitable metal for investment. In 2017, there was a trend towards a decrease in the investment attractiveness of this element. At the same time, most analysts believe that zinc will remain the leader among non-ferrous metals in 2018.

Deutsche Bank gives a forecast for zinc, which assumes an increase in the price of the metal by 8%. In the coming months, the cost of a ton of metal is predicted to be between $3,120-3,160.

Source: https://promdevelop.ru/tsink-metall-s-shirokim-primeneniem-i-vazhnym-biologicheskim-znacheniem/

Zinc: characteristics, properties, features of the metal

Stainless steel roofing, a very effective fight against colds, technology for storing electricity inside a battery, and a number of other applications.

All this is zinc - a chemical element, of course, far from the values ​​of platinum or gold, not as spectacular as silver or copper, nevertheless, quite attractive and popular. The bluish-white metal ranks 24th in abundance among the 92 elements of the earth's crust.

However, to extract 65 grams of metal, it will be necessary to process at least one ton of rock in the zone of deposits of this chemical element.

Natural formation and final formation

Like many other metals, zinc does not occur in nature in its pure form. Typically, this chemical element is present in minerals, combined with other elements, and is present as:

• oxide,
• silicate,
• carbonate.

We can say this is a traditional zinc component. Therefore, in order to reproduce pure metal, you will have to resort to processing the raw material of the zinc-containing mineral, a procedure that involves a multi-stage purification process (including several separate physical and chemical steps).

A naturally occurring mineral containing a high percentage of a chemical, widely used for a variety of purposes.

The structure of the mineral resembles quartz formations with characteristic sparkle inclusions

For example, to process zinc sulfide, it is necessary to grind the raw material into powder and wash it thoroughly to get rid of other metal sulfides present as impurities. The end result is zinc oxide (ZnO). Leaching (reaction with sulfuric acid) produces a sulfate solution.

Electrolysis (an electrochemical process) is then used to separate the pure chemical element. It is also permissible to reproduce metal from mineral raw materials by smelting (heating with carbon), which is traditionally used in the industrial sector.

Properties, features, characteristics of zinc

If you visually examine a piece of zinc, the external appearance of the metal will most likely appear grayish-white in color. However, this is exactly what the oxide looks like, which is formed as a result of the reaction of pure metal with oxygen and carbon dioxide in a humid environment. The appearance of pure zinc is slightly different:

• brilliant,
• bluish,
• whitish,
• silver.

This metal is not like iron, primarily due to its pronounced fragility. However, you just need to heat the metal to a temperature of 100–150°C, after which the structure acquires flexible properties and is easy to process.

Thanks to heating, the material can be converted into various shapes and even rolled into thin sheets. Like other metals, zinc is a crystalline solid. Zinc atoms combine into hexagonal, densely packed crystals.

The galvanization process is used quite widely in the national economy for processing a wide variety of metal structures in order to protect them from the negative influence of the environment.

Most of the extracted chemical element is used for galvanization. The galvanization process is based on electrolysis, which involves coating iron (steel) with a thin protective layer of zinc.

Under the influence of ambient air (oxygen and carbon dioxide), the clean coating oxidizes with the subsequent formation of zinc carbonate. In this way, the factor of rusting (corrosion) of metals in a humid environment is prevented.

Production and use of pure metal

Many types of everyday household items are galvanized. For example:

• metal roofs of buildings,
• building gutters,
• water tanks, etc.

A fairly large proportion of zinc is used in the designs of disposable zinc-carbon non-rechargeable batteries. The brass manufacturing process also requires significant amounts of this substance.

A characteristic feature of zinc is the formation of a number of useful compounds:

1. Sulfide (phosphor of old TV screens, oscilloscopes, fluorescent lamps and luminous paints);
2. Sulfate (weed protectants, use in textile production);
3. Oxide (used to make rubber, helps improve the properties of plastics, paints, inks, concrete, cosmetics).

Many well-known alloys are formed on the zinc component. For example, brass, dental amalgam, bronze and some types of solders. Galvanizing not only prevents water tanks from rusting. Almost all types of cough and cold medicines, vitamin tablets and supplements cannot do without this substance.

Common dietary supplement tablets (capsules) include calcium supplements for strong teeth and bones, vitamin C, omega-3 for the eyes, and zinc for a stronger immune system.

Zinc deficiency in the body is accompanied by various problems in relation to the health of the body and leads to the development of diseases. True, this problem is mainly typical for developing countries, where there are factors of malnutrition in the population and a lack of balanced healthy nutrition.

History of the appearance and approval of a chemical element

It is not known exactly who, where and when zinc was first discovered. However, archaeologists have discovered zinc alloys in places dating back to prehistoric times. It is reliably known that the ancient Romans produced copper coins, the composition of which included this substance, although with impurities.

Almost a thousand years passed before people began to use zinc as a metal itself. Historians suggest that metal production was first noted in India in the 13th century. Another 300 years later, zinc production began on a large scale in China.

The modern history of the beginning of zinc production dates back to the middle of the 18th century. The first to develop and patent a process for the production of pure zinc was the English metallurgist William Champion in 1737. Production on a huge industrial scale was carried out by smelting calamine with charcoal.

Meanwhile, the substance was finally recognized as a chemical element in 1746, thanks to the efforts of a German chemist named Andreas Sigismund Marggraff. The German scientist used methods similar to those used by Champion to study the zinc in detail within the walls of the laboratory.

Source: https://zetsila.ru/%D1%86%D0%B8%D0%BD%D0%BA-%D1%85%D0%B0%D1%80%D0%B0%D0%BA%D1% 82%D0%B5%D1%80%D0%B8%D1%81%D1%82%D0%B8%D0%BA%D0%B0-%D1%8D%D0%BB%D0%B5%D0%BC %D0%B5%D0%BD%D1%82%D0%B0/

Properties, history and alloys of zinc 2020

Zinc (Zn) is an abundant metal found in the earth's crust with many industrial and biological uses.

At room temperature, zinc is brittle and blue-white in color, but can be polished to a bright finish.

A base metal, zinc is primarily used to galvanize steel, to protect the metal from unwanted corrosion. But zinc alloys, including brass, are vital for a wide range of applications, from corrosion-resistant marine components to musical instruments.

Physical properties

• Strength: Zinc is a weak metal with less than half the tensile strength of mild carbon steel. It is generally not used in load-bearing applications, although inexpensive mechanical parts can be cast from zinc.
• Hardness: Pure zinc has low toughness and is usually brittle, but zinc alloys generally have high toughness compared to other cast alloys.
• Ductility: Between 212-302 o F, zinc becomes ductile and malleable, but returns to a brittle state at elevated temperatures. Again, zinc alloys greatly improve this property over pure metal, allowing for more sophisticated fabrication methods.
• Electrical Conductivity: Zinc's conductivity is moderate for a metal. However, its strong electrochemical properties work well in the galvanization process and alkaline batteries

Story

Man-made zinc alloy products have been reliably dated as early as 500 BC, and zinc was first deliberately added to copper to form brass around 200-300 BC.

Brass complemented bronze during the Roman Empire in the making of coins, weapons and art, and remained the main use of zinc until 1746, when Andreas Sigismund Marggraf deliberately isolated the pure element. Because he carefully described his process and how it worked, zinc was soon commercially available.

Alessandro Volta created the first battery in 1800 using copper and zinc plates, ushering in a new era of electrical knowledge. By 1837, Stanislav Sorel named his new galvanizing process, galvanization, after Luigi Galvani, who discovered the animating effect of electricity in autopsies of frogs. Galvanization, a form of cathodic protection, can protect a large number of metals and is currently the main industrial use of pure zinc.

Zinc in the shopping area

Zinc is primarily extracted from ores containing zinc sulfide, zincblende, or sphalerite.

The countries that mine and produce the most refined zinc, in descending order, are China, Peru, Australia, the United States and Canada. According to the US Geological Survey, about 13.4 million tons of zinc in concentrate were mined in 2014, with China accounting for about 36 percent of the total.

According to the International Lead and Zinc Research Group, approximately 13 million metric tons of zinc were consumed in 2013 in electroplating, brass and bronze alloys, zinc alloys, chemical manufacturing and die casting.

Zinc is traded on the LME as "Special High Grade" contracts at 99.995% minimum purity in 25 tonne bars.

Common alloys

• Brass: 3-45% Zn by weight. Used in musical instruments, valves and equipment.
• Nickel Silver: 20% Zn by weight. Used for its shiny silver appearance in jewelry, silverware, railroad tracks, and musical instruments.
• Zinc cast alloys: >> 78% by weight. Typically contain small amounts (less than a few percent) of Pb, Sn, Cu, Al and Mg to improve casting performance and mechanical properties. Used for making small complex shapes and suitable for moving parts in machines. The cheapest of these alloys is called pot metal and serves as an inexpensive replacement for steel. Interesting Facts

Zinc is critical to all life on Earth and is used in more than 300 enzymes; Zinc deficiency was recognized as a clinical health problem in 1961. The International Zinc Association explains that zinc is critical for proper cell growth and mitosis, fertility, immune system function, taste and smell, healthy skin and vision.

• United States pennies are constructed with a zinc core containing 98% of their weight. The remaining 2% is electroplated copper. The amount of copper used in pennies can be changed if the U.S. Treasury deems them too expensive to produce. There are as many as two billion zinc-core coins circulating in the United States!

Source: https://ru.routestofinance.com/what-is-zinc-metal

Zinc in construction: features of the metal, its pros and cons

Zinc has long established itself as an important chemical element. Even before our era, people knew a lot about it and widely used it in various fields. The properties of this material make it possible to use zinc in many industries and in everyday life.

The material is successfully used in the chemical industry, mechanical engineering and construction.

Therefore, today we will look at the useful properties and characteristics of zinc metal and alloys based on it, the price per kg, features of use, as well as the manufacture of the material.

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.

Zinc is a radioactive isotope with a half-life of 244 days.

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:

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

1. 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).
2. 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.
3. Chrome : bluish-shiny color, high hardness, brittleness, oxidation resistance under atmospheric and water conditions, used for decorative coating.
4. 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.

Zinc differs from other metals in that it is easily deformed at temperatures from 100 ºС to 150 ºС. In this temperature range, zinc can also be forged and rolled into thin sheets.

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.

Minuses:

• 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.

Properties and characteristics

So, what properties does zinc have?

Physical

Physical properties:

• It is a medium hard metal.
• Zinc has no polymorphic modifications.
• Cold zinc becomes a brittle metal.
• It acquires plasticity at a temperature of 100-100 ºС.
• At a higher temperature of 250 ºС it again turns into a brittle metal.
• The melting point of solid zinc is 419.5 ºС.
• The temperature of transition to steam is 913ºС.
• The boiling point is 906 ºС.
• The density of zinc in the solid state is 7.133 g/cm3, in the liquid state - 6.66 g/cm3.
• Relative elongation 40-50%.
• Easily soluble in acids.
• Easily soluble in alkalis.

To learn how to properly melt zinc, watch the video:

Chemical properties of zinc:

• 3d104s2 - atomic configuration.
• Zinc is considered an active metal.
• It is an energy restorer.
• Electrode potential: -0.76 V.
• At temperatures below 100 ºС it loses its shine and becomes coated with a film.
• In humid air (especially if it contains carbon dioxide), the metal is destroyed.
• During intense heating, zinc burns violently, producing a bluish flame.
• Oxidation state: .
• Acids and alkalis act differently on zinc depending on the presence of various impurities in the metal.
• When zinc is heated in water, a process of hydrolysis occurs with the formation of a white precipitate.
• High-strength mineral acids can easily dissolve zinc.

Structure and composition

The formula of zinc is as follows: Zn. The configuration of the outer layer of the atom is 4s2. Zinc has a metallic chemical bond and a hexagonal, dense crystal lattice.

Zinc in nature consists of three stable isotopes (we list them: 64Zn (48.6%), 66Zn (26.9%) and 67Zn (4.1%)) and several radioactive ones. The most important of the radioactive ones has a half-life of 244 days.

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.

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

Zinc is used in the following industries:

• 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:

Source: http://stroyres.net/metallicheskie/vidyi/tsvetnyie/tsink/osobennosti-ego-plyusyi-i-minusyi.html

Zinc and its alloys - production, properties, types and applications

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Zinc is a brittle bluish-white metal. It is not found in nature without impurities. In 1738, William Champion obtained pure zinc vapor by condensation. In the periodic table of Mendeleev it is number 30 and is designated by the symbol Zn.

Chemical properties of zinc

Zinc is an active metal. At room temperature it fades and becomes coated with a layer of zinc oxide.

• Reacts with many non-metals: phosphorus, sulfur, oxygen.
• When the temperature rises, it reacts with water and hydrogen sulfide, releasing hydrogen.
• When fused with alkalis, it forms zincates - salts of zinc acid.
• Reacts with sulfuric acid, forming various substances depending on the concentration of the acid.
• When heated strongly, it reacts with many gases: chlorine gas, fluorine, iodine.
• Does not react with nitrogen, carbon and hydrogen.

Physical properties of zinc

Zinc is a hard metal, but becomes ductile at 100–150 °C. At temperatures above 210 °C it may become deformed. The melting point is very low for metals. Despite this, zinc has good electrical conductivity.

• Density - 7.133 g/cm³.
• Thermal conductivity - 116 W/(m K).
• The melting point of zinc is 419.6 °C.
• Boiling point - 906.2 °C.
• The specific heat of evaporation is 114.8 kJ/mol.
• The specific heat of fusion is 7.28 kJ/mol.
• Specific magnetic susceptibility - 0.175·10-6.
• Tensile strength - 200–250 MN/m2.

The detailed chemical composition of various grades of zinc is shown in the table below.

Brand designation	Zinc, no less	Impurity, no more
lead	cadmium	iron	copper	tin	arsenic	aluminum	Total
TsV00	99,997	0,00001	0,002	0,00001	0,00001	0,00001	0,0005	0,00001	0,003
CV0	99,995	0,003	0,002	0,002	0,001	0,001	0,0005	0,005	0,005
CV	99,99	0,005*	0,002	0,003	0,001	0,001	0,0005	0,005	0,01
Ts0A	99,98	0,01	0,003	0,003	0,001	0,001	0,0005	0,005	0,02
Ts0	99,975	0,013	0,004	0,005	0,001	0,001	0,0005	0,005	0,025
C 1	99,95	0,02	0,01	0,01	0,002	0,001	0,0005	0,005	0,05
Ts2	98,7	1,0	0,2	0,05	0,005	0,002	0,01	0,010**	1,3
Ts3	97,5	2,0	0,2	0,1	0,05	0,005	0,01	—	2,5
* In zinc used for the production of TsAM4-1o alloy, the mass fraction of lead should be no more than 0.004%. ** In zinc used for rolling, the mass fraction of aluminum should be no more than 0.005%.

impurities in zinc depend on the production method and the quality of the raw materials.

In Russia, the main percentage of zinc is obtained by the hydrometallurgical method - the metal is reduced from salts in solutions. This method allows you to obtain the purest metal. But some zinc is processed at high temperatures. This method is called pyrometallurgical.

Lead is a special impurity in zinc, since most of it is deposited due to insoluble anodes contained in the metal. Cathode zinc, in addition to all these impurities, consists of chlorine and fluorine.

How do impurities change the properties of zinc

Manufacturers limit the content of cadmium, tin and lead in cast zinc alloys to suppress intergranular corrosion.

Tin is a harmful impurity. The metal does not dissolve and is released from the melt - it contributes to the fragility of zinc castings. Cadmium, on the contrary, dissolves in zinc and reduces its ductility when hot. Lead increases the solubility of the metal in an acidic environment.

Iron increases the hardness of zinc, but reduces its strength. At the same time, it complicates the process of filling molds during casting.

Copper increases the hardness of zinc, but reduces its ductility and resistance to corrosion. copper also interferes with the recrystallization of zinc.

The most harmful impurity is arsenic. Even with a small amount of it, the metal becomes brittle and less ductile.

To avoid edge cracking during hot rolling of zinc, the antimony content should not exceed 0.01%. When hot, it increases the hardness of zinc, depriving it of good ductility.

Zinc alloys

Zinc-based alloys with the addition of copper, magnesium and aluminum have a low melting point and have good fluidity. They are easy to process, weld and solder.

Brass

There are two-component and multi-component brasses.

Two-component brass is a zinc alloy with a high copper content. There is yellow brass with copper in the amount of 67%, golden copper or tombac - 75%, and green - 60%. Such alloys can be deformed at temperatures of 300 °C.

Multicomponent brasses, in addition to the 2 main metals, consist of other additives: nickel, iron, lead or manganese. Each of the elements affects the properties of the alloy.

TsAM

TsAM is a family of zinc alloys. They contain magnesium, aluminum and copper. Such zinc alloys are used in foundries. They contain aluminum in the amount of 4%.

The main area of ​​application of TsAM alloys is zinc die casting. Alloys of this family have low melting points and good casting properties. Their high strength allows the production of durable and complex parts.

Virenium

The alloy consists of zinc (24.5%), copper (70%), nickel (5.5%).

Metal mining

Zinc as a native metal does not occur in nature. It is mined from polymetallic ores containing 1–4% metal in the form of sulfide, as well as copper, lead, gold, silver, bismuth and cadmium. The ores are enriched by selective flotation and zinc concentrates (50–60% Zn) are obtained.

Zinc concentrates are fired in furnaces. Zinc sulfide is converted to ZnO oxide. This releases sulfur dioxide SO2, which is used in the production of sulfuric acid.

Metal production

There are two ways to obtain pure zinc from ZnO oxide.

The most ancient method is distillation. The fired concentrated composition is subjected to heat treatment to give it granularity and gas permeability.

The concentrate is then reduced with coke or coal at a temperature of 1200–1300 °C. The process produces metal vapors, which are condensed and poured into molds. The liquid metal is separated from iron and lead at a temperature of 500 °C. This achieves zinc with a purity of 98.7%.

Sometimes complex and expensive processing of zinc by rectification is used - separation of mixtures due to the exchange of heat between steam and liquid. This cleaning allows you to obtain metal with a purity of 99.995% and remove cadmium.

The second method of producing zinc is electrolytic. The calcined concentrate is treated with sulfuric acid. The finished sulfate solution is cleaned of impurities, after which it is subjected to electrolysis in lead baths. Zinc deposits on aluminum cathodes. The resulting metal is removed from the baths and melted in induction furnaces. After this, electrolytic zinc with a purity of 99.95% is obtained.

Metal casting

Hot zinc is a liquid and flowing metal. Thanks to these properties, it is easily filled into molds.

Impurities affect the amount of surface tension of the zinc. The technological properties of the metal can be improved by adding small amounts of lithium, magnesium, tin, calcium, lead or bismuth.

The higher the overheating temperature of zinc, the better it fills molds. When casting metal into cast iron molds, its volume decreases by 1.6%. This makes it difficult to produce large and long zinc castings.

In medicine

Zinc oxide is used in medicine as an antiseptic. The oxide is added to ointments and other wound healing compounds.

Due to its properties, zinc is widely used in various industries. The metal is in demand due to its relatively low price and good physical properties.

Source: https://ferrolabs.ru/blog/tsink-i-ego-splavy/

Zinc

 Zinc is a brittle, bluish-white transition metal (tarnishes in air, becoming coated with a thin layer of zinc oxide).
  Essential (irreplaceable) microelement of human tissues. In terms of quantitative ratio in the body, it ranks second, after iron, in place. It plays a key role in the regeneration of damaged tissues, since without zinc the synthesis of nucleic acids and proteins is disrupted.

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.

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.

Severe oxidation and reaction with water

When heated strongly in air, zinc filings burn with a blue flame, forming zinc oxide.

2Zn + O₂ → 2ZnO

It exhibits amphoteric properties. In water vapor heated to a red-hot temperature, the metal displaces hydrogen from H2O molecules; in addition, zinc oxide is formed. The chemical properties of the substance prove its ability to interact with both acids and alkalis.

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.

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.

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.

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.

The role of zinc in the human body

Zn in cells is 0.0003%, so it is classified as a trace element. 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.

Source: https://www.syl.ru/article/373953/himicheskie-svoystva-tsinka-i-ego-soedineniy