Magnesium metal. Structure of the magnesium atom

The predominant industrial method for producing magnesium is electrolysis of a melt mixture of MgCl 2

MgCl 2 Mg 2+ 2Cl -

Mg 2+ +2e Mg 0 2Cl - -2e Cl 2 0

2MgCl 2 2Mg+ 2Cl 2

melt

in anhydrous MgCl 2, KCl, NaCl. To obtain the melt, dehydrated carnallite or bimophyte is used, as well as MgCl 2 obtained by chlorination of MgO or as a waste from the production of Ti.

Electrolysis temperature 700-720 o C, graphite anodes, steel cathodes. The MgCl 2 content in the melt is 5-8%; when the concentration decreases to 4%, the current output of magnesium decreases; when the MgCl 2 concentration increases above 8%, the power consumption increases. To ensure optimal MgCl 2 content, a portion of the spent electrolyte is periodically removed and fresh carnallite or MgCl 2 is added. Liquid magnesium floats to the surface of the electrolyte, from where it is removed with a vacuum ladle. The extracted raw magnesium contains 0.1% impurities. To remove non-metallic impurities, magnesium is melted with fluxes - chlorides or fluorides K, Ba, Na, Mg. Deep purification is carried out by vacuum distillation, zone melting, and electrolytic refining. The result is magnesium with a purity of 99.999%.

In addition to magnesium, electrolysis also produces Cl 2 . In thermal methods for producing magnesium, the raw material is magnesite or dolomite, from which MgO is obtained by calcination. 2Mg+O 2 =2MgO. In retort or rotary furnaces with graphite or coal heaters, the oxide is reduced to metal with silicon (siliconothermic method) or CaC 2 (carbidothermic method) at 1280-1300 o C, or carbon (carbothermic method) at temperatures above 2100 o C. In the carbothermic method ( MgO+C Mg+CO) the resulting mixture of CO and magnesium vapor is quickly cooled when leaving the furnace with an inert gas to prevent a reverse reaction with magnesium.

Properties of magnesium.

Physical properties of magnesium.

Magnesium is a silvery-white shiny metal, relatively soft and ductile, a good conductor of heat and electricity. Almost 5 times lighter than copper, 4.5 times lighter than iron; even aluminum is 1.5 times heavier than magnesium. Magnesium melts at a temperature of 651 o C, but under normal conditions it is quite difficult to melt it: when heated in air to 550 o C, it flares up and instantly burns with a dazzlingly bright flame. A strip of magnesium foil can be easily set on fire with an ordinary match, and in an atmosphere of chlorine, magnesium spontaneously ignites even at room temperature. When magnesium burns, it releases a large amount of ultraviolet rays and heat - to heat a glass of ice water to a boil, you only need to burn 4 g of magnesium.

Magnesium is located in the main subgroup of the second group of the periodic table of elements D.I. Mendeleev. Its serial number is 12, atomic weight is 24.312. The electronic configuration of the magnesium atom in the unexcited state is 1S 2 2S 2 P 6 3S 2; The electrons in the outer layer are valence; therefore, magnesium exhibits valency II. Closely related to the structure of the electronic shells of the magnesium atom is its reactivity. Due to the presence of only two electrons in the outer shell, the magnesium atom tends to easily give them up to obtain a stable eight-electron configuration; Therefore, magnesium is chemically very active.

Magnesium oxidizes in air, but the resulting oxide film protects the metal from further oxidation. The normal electronic potential of magnesium in an acidic environment is -2.37V, in an alkaline environment - 2.69V. Magnesium dissolves in dilute acids in the cold. It is insoluble in hydrofluoric acid due to the formation of a film from MgF 2 fluoride, which is sparingly soluble in water; almost insoluble in concentrated sulfuric acid. Magnesium dissolves easily when exposed to solutions of ammonium salts. Alkaline solutions have no effect on it. Magnesium is supplied to laboratories in the form of powder or strips. If you set fire to magnesium tape, it quickly burns with a blinding flash, developing a high temperature. Magnesium flashes are used in photography and in the manufacture of lighting flares. The boiling point of magnesium is 1107 o C, density = 1.74 g/cm 3, atomic radius 1.60 NM.

Chemical properties of magnesium.

The chemical properties of magnesium are quite peculiar. It easily removes oxygen and chlorine from most elements, and is not afraid of caustic alkalis, soda, kerosene, gasoline and mineral oils. Magnesium almost does not interact with cold water, but when heated, it decomposes with the release of hydrogen. In this respect, it occupies an intermediate position between beryllium, which does not react with water at all, and calcium, which easily interacts with it. The reaction is especially intense with water vapor heated above 380 o C:

Mg 0 (solid) + H 2 + O (gas) Mg + 2 O (solid) + H 2 0 (gas).

Since the product of this reaction is hydrogen, it is clear that extinguishing burning magnesium with water is unacceptable: the formation of an explosive mixture of hydrogen and oxygen and an explosion may occur. You cannot extinguish a burning magnesium with carbon dioxide: magnesium reduces it to free carbon

2Mg 0 +C +4 O 2 2Mg +2 O+C 0 ,

You can stop the access of oxygen to burning magnesium by covering it with sand, although magnesium interacts with silicon (IV) oxide, but with significantly less heat release:

2Mg 0 + Si +4 O 2 =2Mg +2 O+Si 0

This determines the possibility of using sand to extinguish silicon. The danger of magnesium catching fire during intense heating is one of the reasons why its use as a technical material is limited.

In the electrochemical voltage series, magnesium is significantly to the left of hydrogen and actively reacts with dilute acids to form salts. Magnesium has peculiarities in these reactions. It does not dissolve in hydrofluoric acid, concentrated sulfuric acid, and in a mixture of sulfuric and nitric acids, which dissolves other metals almost as effectively as aqua regia (a mixture of HCl and HNO 3). The resistance of magnesium to dissolution in hydrofluoric acid is explained simply: the surface of magnesium is covered with a film of magnesium fluoride MgF 2, insoluble in hydrofluoric acid. The resistance of magnesium to sufficiently concentrated sulfuric acid and its mixture with nitric acid is more difficult to explain, although in this case the reason lies in the passivation of the magnesium surface. Magnesium practically does not interact with solutions of alkalis and ammonium hydroxide. But with solutions of ammonium salts, the reaction, although slowly, occurs:

2NH + 4 +Mg=Mg 2+ + 2NH 3 + H 2

There is no surprise in this reaction. This reaction is essentially the same as the reaction of metals displacing hydrogen from acids. In one definition, an acid is a substance that dissociates to form hydrogen ions. This is exactly how the NH4 ion can dissociate:

NH 4 + NH 3 +H +

Mg 0 + 2HCl=Mg +2 Cl 2 +H 0 2

2H + +Mg Mg 2+ + H 0 2

When magnesium is heated in a halogen atmosphere, ignition occurs and halogen salts form.

The cause of ignition is a very large heat release, as in the case of the reaction of magnesium with oxygen. Thus, when 1 mole of magnesium chloride is formed from magnesium and chlorine, 642 kJ is released. When heated, magnesium combines with sulfur (MgS) and nitrogen (Mg 3 N 2). When pressurized and heated with hydrogen, magnesium forms magnesium hydride

Mg 0 + H 2 0 Mg +2 H 2 - .

The high affinity of magnesium for chlorine made it possible to create a new metallurgical production - “magnesium” - the production of metals as a result of a reaction

MeCln+0.5nMg=Me+0.5nMgCl 2

This method produces metals that play a very important role in modern technology - zirconium, chromium, thorium, beryllium. A lightweight and durable “space age metal”, almost all titanium is obtained this way.

The essence of production boils down to the following: when producing magnesium metal by electrolysis of a melt of magnesium chloride, chlorine is formed as a by-product. This chlorine is used to produce titanium (IV) chloride TiCl 4, which is reduced by magnesium to titanium metal

Ti +4 Cl 4 + 2Mg 0 Ti 0 +2Mg +2 Cl 2

The resulting magnesium chloride is again used to produce magnesium, etc. Titanium-magnesium plants operate on the basis of these reactions. Along with titanium and magnesium, other products are also obtained, such as bertholite salt KClO 3, chlorine, bromine and products - fiberboard and xylitol boards, which will be discussed below. In such complex production, the degree of use of raw materials, the profitability of production is high, and the mass of waste is not large, which is especially important for protecting the environment from pollution.

The science that studies these elements is chemistry. The periodic table, based on which we can study this science, shows us that there are twelve protons and neutrons contained in a magnesium atom. This can be determined by the atomic number (it is equal to the number of protons, and there will be the same number of electrons if it is a neutral atom and not an ion).

The chemical properties of magnesium are also studied by chemistry. The periodic table is also necessary for their consideration, since it shows us the valency of the element (in this case it is equal to two). It depends on the group to which the atom belongs. In addition, with its help you can find out that the molar mass of magnesium is twenty-four. That is, one mole of this metal weighs twenty-four grams. The formula of magnesium is very simple - it does not consist of molecules, but of atoms united by a crystal lattice.

Characteristics of magnesium from the point of view of physics

Like all metals, except mercury, this compound has a solid state of aggregation under normal conditions. It has a light gray color with a peculiar shine. This metal has quite high strength. The physical characteristics of magnesium do not end there.

Consider the melting and boiling points. The first is equal to six hundred and fifty degrees Celsius, the second is one thousand ninety degrees Celsius. We can conclude that this is a fairly fusible metal. In addition, it is very light: its density is 1.7 g/cm3.

Magnesium. Chemistry

Knowing the physical characteristics of this substance, you can move on to the second part of its characteristics. This metal has a medium level of activity. This can be seen from the electrochemical series of metals - the more passive it is, the more to the right it is. Magnesium is one of the first on the left. Let us consider in order what substances it reacts with and how this happens.

With simple

These include those whose molecules consist of only one chemical element. This includes oxygen, phosphorus, sulfur, and many others. First, let's look at the interaction with oxygen. It's called combustion. In this case, an oxide of this metal is formed. If we burn two moles of magnesium, while spending one mole of oxygen, we get two moles of oxide. The equation for this reaction is written as follows: 2Mg + O 2 = 2MgO. In addition, when magnesium burns in open air, its nitride is also formed, since this metal simultaneously reacts with nitrogen contained in the atmosphere.

When three moles of magnesium are burned, one mole of nitrogen is consumed, and the result is one mole of nitride of the metal in question. The equation for this kind of chemical interaction can be written as follows: 3Mg + N 2 = Mg 3 N 2.

In addition, magnesium can react with other simple substances such as halogens. Interaction with them occurs only if the components are heated to very high temperatures. In this case, an addition reaction occurs. The halogens include the following simple substances: chlorine, iodine, bromine, fluorine. And the reactions are named accordingly: chlorination, iodination, bromination, fluorination. As you might have guessed, as a result of such interactions one can obtain magnesium chloride, iodide, bromide, and fluoride. For example, if we take one mole of magnesium and the same amount of iodine, we get one mole of iodide of this metal. This chemical reaction can be expressed using the following equation: Mg + I 2 = MgI 2. Chlorination is carried out according to the same principle. Here is the reaction equation: Mg + Cl 2 = MgCl 2.

In addition, metals, including magnesium, react with phosphorus and sulfur. In the first case, you can get phosphide, in the second - sulfide (not to be confused with phosphates and sulfates!). If you take three moles of magnesium, add two moles of phosphorus to it and heat it to the desired temperature, one mole of phosphide of the metal in question is formed. The equation for this chemical reaction is as follows: 3Mg + 2P = Mg 3 P 2. In the same way, if you mix magnesium and sulfur in equal molar proportions and create the necessary conditions in the form of high temperature, we obtain the sulfide of this metal. The equation for such a chemical interaction can be written as follows: Mg + S = MgS. So we looked at the reactions of this metal with other simple substances. But the chemical characteristics of magnesium do not end there.

Reactions with complex compounds

These substances include water, salts, and acids. Metals react differently with different groups. Let's look at everything in order.

Magnesium and water

When this metal interacts with the most common chemical compound on Earth, oxide and hydrogen are formed in the form of a gas with a strong, unpleasant odor. To carry out this type of reaction, the components also need to be heated. If you mix one mole of magnesium and water, you get the same amount of oxide and hydrogen. The reaction equation is written as follows: Mg + H 2 O = MgO + H 2.

Interaction with acids

Like other reactive metals, magnesium is capable of displacing hydrogen atoms from their compounds. This kind of process is called In such cases, metal atoms replace hydrogen atoms and a salt is formed, consisting of magnesium (or another element) and an acid precipitate. For example, if you take one mole of magnesium and add it to two moles, one mole of the chloride of the metal in question and the same amount of hydrogen are formed. The reaction equation will look like this: Mg + 2HCl = MgCl 2 + H 2.

Interaction with salts

We have already described how salts are formed from acids, but the characterization of magnesium from a chemical point of view also implies consideration of its reactions with salts. In this case, interaction can only occur if the metal contained in the salt is less active than magnesium. For example, if we take one mole of magnesium and copper sulfate, we get the sulfate of the metal in question and pure copper in an equal molar ratio. The equation for this type of reaction can be written as follows: Mg + CuSO 4 = MgSO 4 + Cu. This is where the restorative properties of magnesium come into play.

Application of this metal

Due to the fact that it is superior to aluminum in many respects - it is approximately three times lighter, but at the same time twice as strong, it is widely used in various industries. First of all, this is the aircraft industry. Here, magnesium-based alloys occupy first place in popularity among all materials used. In addition, it is used in the chemical industry as a reducing agent to extract certain metals from their compounds. Due to the fact that when burned, magnesium produces a very powerful flash, it is used in the military industry for the manufacture of signal flares, flash-noise ammunition, etc.

Getting magnesium

The main raw material for this is the chloride of the metal in question. This is done by electrolysis.

Qualitative reaction to cations of a given metal

This is a special procedure designed to determine the presence of ions of a substance. To test the solution for the presence of magnesium compounds, you can add potassium or sodium carbonate to it. As a result, a white precipitate is formed, which easily dissolves in acids.

Where can this metal be found in nature?

This chemical element is quite common in nature. Almost two percent of the earth's crust consists of this metal. It is found in many minerals, such as carnallite, magnesite, dolomite, talc, and asbestos. The formula of the first mineral looks like this: KCl.MgCl 2 .6H 2 O. It looks like crystals of bluish, pale pink, faded red, light yellow or transparent.

Magnesite is its chemical formula - MgCO 3. It is white in color, but depending on impurities, it can have a gray, brown or yellow tint. Dolomite has the following chemical formula: MgCO 3 .CaCO 3 . It is a yellowish-gray or mineral with a glassy luster.

Talc and asbestos have more complex formulas: 3MgO.4SiO 2 .H 2 O and 3MgO.2SiO 2 .2H 2 O, respectively. Due to their high heat resistance, they are widely used in industry. In addition, magnesium is part of the chemical composition of the cell and the structure of many organic substances. We will look at this in more detail.

The role of magnesium for the body

This chemical element is important for both plant and animal creatures. Magnesium is simply vital for the plant body. Just as iron is the basis of hemoglobin, necessary for animal life, so magnesium is the main component of chlorophyll, without which a plant cannot exist. This pigment is involved in the process of photosynthesis, during which nutrients are synthesized from inorganic compounds in the leaves.

Magnesium is also very necessary for the animal body. The mass fraction of this microelement in the cell is 0.02-0.03%. Despite the fact that there is so little of it, it performs very important functions. Thanks to it, the structure of such organelles as mitochondria, which are responsible for cellular respiration and energy synthesis, is maintained, as well as ribosomes, in which proteins necessary for life are formed. In addition, it is part of the chemical composition of many enzymes that are needed for intracellular metabolism and DNA synthesis.

For the body as a whole, magnesium is necessary to take part in the metabolism of glucose, fats and some amino acids. Also, with the help of this trace element a nerve signal can be transmitted. In addition to all of the above, sufficient magnesium in the body reduces the risk of heart attacks, heart attacks and strokes.

Symptoms of increased and decreased content in the human body

A lack of magnesium in the body is manifested by such main symptoms as high blood pressure, fatigue and low performance, irritability and poor sleep, memory impairment, and frequent dizziness. You may also experience nausea, convulsions, trembling fingers, confusion - these are signs of a very low level of intake of this microelement from food.

A lack of magnesium in the body leads to frequent respiratory diseases, disorders of the cardiovascular system, and type 2 diabetes. Next, let's look at the magnesium content in products. To avoid its deficiency, you need to know which foods are rich in this chemical element. It is also necessary to take into account that many of these symptoms can also manifest themselves in the opposite case - an excess of magnesium in the body, as well as a lack of microelements such as potassium and sodium. Therefore, it is important to carefully review your diet and understand the essence of the problem; this is best done with the help of a nutritionist.

As mentioned above, this element is the main component of chlorophyll. Therefore, you can guess that a large amount of it is contained in greens: celery, dill, parsley, cauliflower and white cabbage, lettuce, etc. Also, many cereals, especially buckwheat and millet, as well as oatmeal and barley. In addition, nuts are rich in this microelement: cashews, walnuts, peanuts, hazelnuts, and almonds. Legumes such as beans and peas also contain large amounts of the metal in question.

A lot of it is also found in algae, for example in seaweed. If these products are consumed in normal quantities, then your body will not lack the metal discussed in this article. If you do not have the opportunity to regularly eat the foods listed above, then it is best to purchase nutritional supplements that contain this microelement. However, before doing this, you should definitely consult your doctor.

Conclusion

Magnesium is one of the most important metals in the world. It has found wide application in numerous industries - from chemical to aviation and military. Moreover, it is very important from a biological point of view. Without it, the existence of neither plant nor animal organisms is impossible. Thanks to this chemical element, the process that gives life to the entire planet is carried out - photosynthesis.

Group IIA contains only metals – Be (beryllium), Mg (magnesium), Ca (calcium), Sr (strontium), Ba (barium) and Ra (radium). The chemical properties of the first representative of this group, beryllium, differ most strongly from the chemical properties of the other elements of this group. Its chemical properties are in many ways even more similar to aluminum than to other Group IIA metals (so-called “diagonal similarity”). Magnesium, in its chemical properties, also differs markedly from Ca, Sr, Ba and Ra, but still has much more similar chemical properties with them than with beryllium. Due to the significant similarity in the chemical properties of calcium, strontium, barium and radium, they are combined into one family called alkaline earth metals.

All elements of group IIA belong to s-elements, i.e. contain all their valence electrons on s-sublevel Thus, the electronic configuration of the outer electronic layer of all chemical elements of this group has the form ns 2 , Where n– number of the period in which the element is located.

Due to the peculiarities of the electronic structure of group IIA metals, these elements, in addition to zero, can have only one single oxidation state equal to +2. Simple substances formed by elements of group IIA, when participating in any chemical reactions, are only capable of oxidation, i.e. donate electrons:

Me 0 – 2e — → Me +2

Calcium, strontium, barium and radium have extremely high chemical reactivity. The simple substances formed by them are very strong reducing agents. Magnesium is also a strong reducing agent. The reduction activity of metals obeys the general laws of the periodic law of D.I. Mendeleev and increases down the subgroup.

Interaction with simple substances

with oxygen

Without heating, beryllium and magnesium do not react with either atmospheric oxygen or pure oxygen due to the fact that they are covered with thin protective films consisting of BeO and MgO oxides, respectively. Their storage does not require any special methods of protection from air and moisture, unlike alkaline earth metals, which are stored under a layer of liquid inert to them, most often kerosene.

Be, Mg, Ca, Sr, when burned in oxygen, form oxides of the composition MeO, and Ba - a mixture of barium oxide (BaO) and barium peroxide (BaO 2):

2Mg + O2 = 2MgO

2Ca + O2 = 2CaO

2Ba + O 2 = 2BaO

Ba + O 2 = BaO 2

It should be noted that when alkaline earth metals and magnesium burn in air, a side reaction of these metals with air nitrogen also occurs, as a result of which, in addition to compounds of metals with oxygen, nitrides with the general formula Me 3 N 2 are also formed.

with halogens

Beryllium reacts with halogens only at high temperatures, and the rest of the Group IIA metals - already at room temperature:

Mg + I 2 = MgI 2 – Magnesium iodide

Ca + Br 2 = CaBr 2 – calcium bromide

Ba + Cl 2 = BaCl 2 – barium chloride

with non-metals of groups IV–VI

All metals of group IIA react when heated with all nonmetals of groups IV–VI, but depending on the position of the metal in the group, as well as the activity of the nonmetals, varying degrees of heating are required. Since beryllium is the most chemically inert among all group IIA metals, when carrying out its reactions with non-metals, significant use is required. O higher temperature.

It should be noted that the reaction of metals with carbon can form carbides of different natures. There are carbides that belong to methanides and are conventionally considered derivatives of methane, in which all hydrogen atoms are replaced by metal. They, like methane, contain carbon in the -4 oxidation state, and when they are hydrolyzed or interact with non-oxidizing acids, one of the products is methane. There is also another type of carbides - acetylenides, which contain the C 2 2- ion, which is actually a fragment of the acetylene molecule. Carbides such as acetylenides, upon hydrolysis or interaction with non-oxidizing acids, form acetylene as one of the reaction products. The type of carbide - methanide or acetylenide - obtained when a particular metal reacts with carbon depends on the size of the metal cation. Metal ions with a small radius usually form metanides, and larger ions form acetylenides. In the case of metals of the second group, methanide is obtained by the interaction of beryllium with carbon:

The remaining metals of group II A form acetylenides with carbon:

With silicon, group IIA metals form silicides - compounds of the type Me 2 Si, with nitrogen - nitrides (Me 3 N 2), with phosphorus - phosphides (Me 3 P 2):

with hydrogen

All alkaline earth metals react with hydrogen when heated. In order for magnesium to react with hydrogen, heating alone, as in the case of alkaline earth metals, is not enough; in addition to high temperature, increased hydrogen pressure is also required. Beryllium does not react with hydrogen under any conditions.

Interaction with complex substances

with water

All alkaline earth metals react actively with water to form alkalis (soluble metal hydroxides) and hydrogen. Magnesium reacts with water only when boiled due to the fact that when heated, the protective oxide film MgO dissolves in water. In the case of beryllium, the protective oxide film is very resistant: water does not react with it either when boiling or even at red-hot temperatures:

with non-oxidizing acids

All metals of the main subgroup of group II react with non-oxidizing acids, since they are in the activity series to the left of hydrogen. In this case, a salt of the corresponding acid and hydrogen are formed. Examples of reactions:

Be + H 2 SO 4 (diluted) = BeSO 4 + H 2

Mg + 2HBr = MgBr 2 + H 2

Ca + 2CH 3 COOH = (CH 3 COO) 2 Ca + H 2

with oxidizing acids

− diluted nitric acid

All metals of group IIA react with dilute nitric acid. In this case, the reduction products, instead of hydrogen (as in the case of non-oxidizing acids), are nitrogen oxides, mainly nitrogen oxide (I) (N 2 O), and in the case of highly dilute nitric acid, ammonium nitrate (NH 4 NO 3):

4Ca + 10HNO3 ( razb .) = 4Ca(NO 3) 2 + N 2 O + 5H 2 O

4Mg + 10HNO3 (very blurry)= 4Mg(NO 3) 2 + NH 4 NO 3 + 3H 2 O

− concentrated nitric acid

Concentrated nitric acid at ordinary (or low) temperature passivates beryllium, i.e. does not react with it. When boiling, the reaction is possible and proceeds predominantly in accordance with the equation:

Magnesium and alkaline earth metals react with concentrated nitric acid to form a wide range of different nitrogen reduction products.

− concentrated sulfuric acid

Beryllium is passivated with concentrated sulfuric acid, i.e. does not react with it under normal conditions, but the reaction occurs at boiling and leads to the formation of beryllium sulfate, sulfur dioxide and water:

Be + 2H 2 SO 4 → BeSO 4 + SO 2 + 2H 2 O

Barium is also passivated by concentrated sulfuric acid due to the formation of insoluble barium sulfate, but reacts with it when heated; barium sulfate dissolves when heated in concentrated sulfuric acid due to its conversion to barium hydrogen sulfate.

The remaining metals of main group IIA react with concentrated sulfuric acid under any conditions, including in the cold. Reduction of sulfur can occur to SO 2, H 2 S and S depending on the activity of the metal, reaction temperature and acid concentration:

Mg + H2SO4 ( conc. .) = MgSO 4 + SO 2 + H 2 O

3Mg + 4H 2 SO 4 ( conc. .) = 3MgSO 4 + S↓ + 4H 2 O

4Ca + 5H 2 SO 4 ( conc. .) = 4CaSO 4 +H 2 S + 4H 2 O

with alkalis

Magnesium and alkaline earth metals do not interact with alkalis, and beryllium easily reacts both with alkali solutions and with anhydrous alkalis during fusion. Moreover, when a reaction is carried out in an aqueous solution, water also participates in the reaction, and the products are tetrahydroxoberyllates of alkali or alkaline earth metals and hydrogen gas:

Be + 2KOH + 2H 2 O = H 2 + K 2 - potassium tetrahydroxoberyllate

When carrying out a reaction with a solid alkali during fusion, beryllates of alkali or alkaline earth metals and hydrogen are formed

Be + 2KOH = H 2 + K 2 BeO 2 - potassium beryllate

with oxides

Alkaline earth metals, as well as magnesium, can reduce less active metals and some nonmetals from their oxides when heated, for example:

The method of reducing metals from their oxides with magnesium is called magnesium.

In itself, a normal concentration of magnesium in the body does not guarantee good health, high immunity, absence of diseases and good performance. No less important is the interaction of a microelement with other substances, because the functions of some can negatively affect the functions of others.

Avoid combining magnesium with:

• Calcium. It may reduce the absorption of magnesium because both metals are absorbed through the same pathway in the intestine. To prevent this from happening, you need to maintain a 2:1 proportion of calcium and magnesium in the diet.
• Fatty foods. The higher the percentage of fat in a dish, the worse magnesium is absorbed. Interacting with fatty acids, magnesium forms soap-like salts that are not processed by the digestive system, causing constipation or diarrhea.
• Highly fibrous foods, as they block the absorption of magnesium. Fibrous foods are rich in oxalates and phytic acid salts, which are poorly digested in the intestines and interfere with the absorption of other substances.
• Folic acid. It increases the activity of enzymes that require magnesium to function. The microelement costs increase, causing its deficiency.
• Iron. Both metals are not absorbed at the same time.
• Cholecalciferol (vitamin D3). It helps to absorb not only magnesium, but also calcium in the intestines. Microelements do not combine well together - only in a 2:1 ratio (with a predominance of magnesium). Otherwise, a deficiency of the latter develops.

Features of magnesium absorption

Magnesium is absorbed in the duodenum and partially in the large intestine. Organic compounds of the element - complexes with amino acids and organic acids (magnesium lactate and citrate) are absorbed better than inorganic salts (magnesium sulfate).

Basic functions in the body

The main task of magnesium in the body is to accelerate metabolism (metabolism) and the formation of bone tissue. However, the functional potential of the chemical element is not limited to this. Thanks to magnesium:

• the immune activity of cells increases, which is why the chemical element must be present in the diet of small children (otherwise the immune system will fail);
• the stability of genetic information contained in DNA and RNA molecules is maintained. If the absorption of magnesium in the body is impaired or is insufficient, protein structures can mutate;
• histamine synthesis in mast cells slows down. Histamine is a hormone responsible for all metabolic processes in the body. It controls the activity of the respiratory system, musculoskeletal system, the condition of the skin, the functioning of the heart and sensory organs. This is why in allergic reactions, when histamine is released, symptoms such as dry cough, watery eyes, and redness appear. The more histamine, the more severe the symptoms. In the acute form of an allergy, the cough turns into an attack of suffocation or anaphylactic shock. Tearfulness - due to inflammation of the conjunctiva. Inflammation of the skin - dry eczema (cracks and erosions on the skin that itch and bleed). Spasm of smooth muscles (lining the internal organs) provokes suffocation and Quincke's edema;
• heart rate is regulated. The heart is a resilient organ, but it also needs to rest. With the help of magnesium, myocardial contractility decreases, heart rate and high blood pressure decrease;
• bone mineral density increases. In children, cartilaginous tissue predominates, which is gradually covered with minerals and ossifies. The thicker the protective “mineral” layer, the lower the risk of fractures. Calcium and phosphorus help magnesium in this.

Magnesium also stimulates the functioning of enzymes. Peptidase, phosphatase, carboxylase, phosphorylase, cholinesterase, pyruvate kinase, decarboxylase and keto acids are a kind of “wards” of magnesium.

In the presence of magnesium, not only nucleic acids, fats, proteins, B vitamins, and collagen are synthesized. It is responsible for the resynthesis (regeneration) of the ATP molecule. The latter is the main unit of energy. Its reserves in the body are small, therefore, to maintain activity, the ATP molecule must be constantly restored from breakdown products, which is what magnesium helps with.

Thanks to magnesium, the balance of potassium, calcium, and sodium is maintained. Chemical elements are responsible for transmitting impulses from nerve fibers to muscles. If the concentration of one of them increases or decreases, the impulse is not transmitted or is transmitted late. Well-coordinated muscle function is the result of magnesium.

The same thing happens in the brain - magnesium stabilizes the processes of inhibition and excitation.

If there is a lot of cholesterol in the body, it means that the absorption of magnesium is impaired. The chemical element promotes the elimination of toxins and end products of metabolism (metabolism), regulates glucose levels (diabetes mellitus is the result of magnesium deficiency). Thanks to the exchange, calcium is not deposited in the kidneys, gall bladder, ureters and bones.

Magnesium deficiency is fraught with “thickening” of the blood due to the accumulation of platelets; in the daily diet, it improves the “fluidity” of the blood.

Magnesium supports cellular respiration - oxygen molecules are stored in mitochondria (oxygen depots) and released during metabolic processes.

A lack of magnesium is fraught with insomnia, migraines, anxiety, and nervous disorders.

Source of magnesium

• half a cup of almonds – 136;
• raw spinach: 1 cup raw – 30, 1 cup cooked – 1157;
• nuts and seeds of zucchini and pumpkin: half a cup – 325;
• beans and lentils: 1 cup boiled – 148;
• brown rice: 1 cup – 86;
• avocado: 1 pc. – 58;
• natural yogurt: 1 cup – 47;
• bananas: 1 pc. – 32;
• figs: half a cup dried – 51;
• dark chocolate: 100 g bar – 280.

Advice! Adjust your diet depending on the season. In winter, include honey, raisins, dried apricots, prunes, dates, nuts, cocoa and porridge in your menu. In spring, pamper your body with greens: parsley, dill, spinach and green salad

Cherries, black currants and legumes are the best summer delicacies. In the fall, lean on watermelons, carrots and beets.

Remember that when grinding grains and heat processing food, about 80% of magnesium is lost. Products intended for long-term storage do not contain magnesium. Take this into account when planning your diet so that magnesium deficiency does not affect your health and performance.

How to preserve magnesium in food

A minimum of heat treatment is the key to preserving magnesium in food products. Make vegetable and fruit salads, add seeds and nuts to them. Experiment with dressings. For example, mix cedar, sesame, mustard, olive oil with citrus fruits and garlic.

Combination with other substances

With vitamin E deficiency, the level of magnesium in tissues decreases.

With alcohol abuse, smoking, and coffee drinking, magnesium is intensively excreted through the kidneys.

People with a sweet tooth are also at risk. The more glucose you consume, the more magnesium is forced to work (stimulates the release of insulin).

Don't get carried away with protein diets. Magnesium is needed to break down proteins, so the load on it increases. The more protein in the diet, the more magnesium you should have.

Take B vitamins along with magnesium, which is involved in the formation of thiamine pyrophosphate. Without it, other B vitamins are not absorbed.

Daily norm

• up to 6 months – 30;

• from 6 to 12 months – 75;
• from 1 to 3 years – 80;
• from 4 to 8 years – 130;
• from 9 to 13 years – 240.

Adolescents (14-18 years), mg:

• boys – 410;
• girls - 360.

Adults, mg:

• men: 19-30 years old – 400; 31 and older – 420;
• women: 19-30 years old – 310; 31 and older – 320;
• pregnant women: up to 18 years – 400; 19-30 years old – 350; 31 and older – 360;
• breastfeeding: up to 18 years – 360; 19-30 years old – 310; 31 and older – 320.

Why is a lack of magnesium in the body dangerous?

A lack of magnesium in the body is dangerous due to the following conditions:

• Weakened immunity. The immune system synthesizes specific cells that identify and neutralize foreign protein structures. If these cells are not enough or their functions are impaired, a person often gets sick, and a common runny nose quickly turns into an infectious disease. To overcome the infection, the body uses additional reserves. The recovery period after allergic rhinitis is delayed.
• Constant fatigue. Magnesium controls not only the transmission of nerve impulses to the muscles, but also the processes of excitation and inhibition in the brain. A deficiency of the chemical element is fraught with insomnia, due to which the body does not have time to replenish energy resources. Prolonged seasonal depression, decreased performance, anxiety, phobias, worries - links in the same chain.
• Glare before the eyes, dizziness. Due to lack of sleep, vision and concentration are impaired. Lack of proper sleep for more than two days is fraught with hallucinations.
• Muscle spasms, cramps. Magnesium deficiency can impair the functioning of the potassium-sodium pump, which regulates the transmission of impulses from nerve endings to muscle fibers. Signs of magnesium deficiency are impaired coordination of movements, loss of endurance, inhibited reaction.
• Heart rhythm disturbance. The heart is made up of muscle tissue. If the balance of potassium and sodium is disturbed, muscle fibers contract voluntarily, tachycardia (rapid heartbeat) and heart murmurs begin.

Calcium absorption depends on the amount of magnesium. If the latter is not enough, the functioning of the gastrointestinal tract organs is disrupted (constipation, diarrhea, nausea, flatulence, vomiting, cramping abdominal pain). The condition of the skin and hair worsens, the nail plates peel and break.

Magnesium deficiency can be caused by the factors described below.

• compliance with mono-diet, fasting;
• insufficient magnesium content in the daily diet;
• excessive consumption of calcium, protein and lipid (fatty foods);
• chronic alcoholism, smoking;
• hormonal contraception;
• lack of vitamins B1, B2, B6 in the daily diet.

Hypomagnesemia almost always occurs against the background of pathologies of internal organs.

Internal factors:

• impaired absorption of a chemical element due to diarrhea or small intestinal fistulas;
• kidney diseases;
• diabetes mellitus with persistently high blood sugar levels;
• myocardial infarction;
• hyperfunction of the thyroid and parathyroid glands:
• circulatory failure (blood stagnation, increased “viscosity”;
• cirrhosis of the liver;
• increased synthesis of aldosterone (adrenal hormone).

Not all medications are combined with magnesium. Diuretics (diuretics), glucocorticosteroids, cytotoxic drugs and estrogens remove magnesium from the body.

How to replenish magnesium deficiency in the body

The main sources of magnesium are salt, food and hard drinking water. If you are deficient in an element, lean on cereals (oatmeal, buckwheat, brown rice, barley and millet cereals, sprouted wheat grains, rice and wheat bran). Dark chocolate, rye bread, avocado, seaweed, nuts, dried fruits, and legumes will help replenish magnesium deficiency.

Medicinal plants are an additional source of magnesium. There is no less of it in nettle, tinctures and aloe vera syrup, rose hips and chokeberry than in cereals.

Medicinal and table mineral water eliminates magnesium deficiency.

Advice! Magnesium is absorbed only in a combination of B vitamins and calcium. Eat more cottage cheese, milk, bran bread, fish, cereals and eggs. Adequate sleep, high performance, good memory and physical endurance are guaranteed

Increase the amount of magnesium-containing foods in your diet if:

• you are physically and emotionally tired. Emergency situations at work are not scary if you eat buckwheat porridge and lettuce with carrots for lunch every day;
• are expecting a baby or breastfeeding. The immunity of the baby and mother depends on proper diet, and 81.2% of pregnant women are diagnosed with magnesium deficiency;
• get ready for the competition. Professional athletes use magnesium-containing preparations, but also do not forget about dried fruits and cereals;
• are fond of natural coffee and green tea or take diuretics (diuretics). All of them not only remove excess fluid from the body, but also flush out nutrients. Magnesium is no exception;
• raising hyperactive children. A growing body needs magnesium for the formation of all functional systems;
• fight dry and flaky skin. Magnesium is involved in the synthesis of collagen, which is responsible for the density and strength of connective tissue and skin elasticity.

Is excess magnesium dangerous?

Despite the wide functional potential of the chemical element, its excess is fraught with pathological conditions.

Excess magnesium is diagnosed:

• for speech impairment, lethargy and loss of coordination;
• drowsiness and slow heart rate;
• dry mucous membranes;
• abdominal pain;
• low blood pressure;
• disruption of the gastrointestinal tract (nausea, vomiting, diarrhea).

In severe cases, hypermagnesemia (excess magnesium) leads to respiratory paralysis and cardiac arrest.

The causes of excess magnesium are associated with pathology of internal organs. In case of renal failure, increased catabolism (breakdown) of proteins, or non-therapeutic diabetic acidosis, the amount of magnesium in the diet is reduced.

An excess of magnesium is diagnosed with uncontrolled use of drugs - most often with an independent increase in the dose of the drug when skipping the next dose.

The least common causes of an overabundance of the element are type 2 diabetes mellitus, extensive trauma with tissue crushing, pathologies provoked by radiation or taking cytostatics.

Remember! The maximum daily dose of magnesium is 800 mg. Exceeding the dose by 10-50 mg is fraught with chronic fatigue, kidney stones, hyperthyroidism, psoriasis

Preparations containing magnesium

Magnesium and calcium are the main participants in muscle contraction. In their presence, impulses are transmitted from the nerve fiber to the muscle fiber. A decrease in the concentration of one microelement is fraught with impaired coordination of movement, loss of vascular tone and spasms.

Magnesium is rarely prescribed on its own, often together with calcium (2:1 ratio). It is contraindicated to take it if:

• hypersensitivity to the components of the drug;
• severe renal or adrenal insufficiency (creatinine clearance less than 30 ml/min.).
• phenylketonuria;
• hereditary galactosemia, glucose and galactose malabsorption syndrome or lactase deficiency (due to the presence of lactose in the drug);
• concomitant use with Levodopa.

Magnesium preparations are not prescribed to children under 6 years of age, since their effectiveness and safety have not been confirmed.

Features of taking medications are described below.

• taken with vitamin B6, as they enhance each other’s effects. The latter helps magnesium penetrate cells, be stored inside and enhances its functions;
• not compatible with iron. Ferrum impairs the absorption of magnesium. To avoid interfering with the absorption of microelements, take iron and magnesium at intervals of 2-3 hours. The situation is similar with the drugs Sodium fluoride and Tetracycline;
• taken during or after meals. Taking magnesium between meals will cause diarrhea and bloating.

Features of use during pregnancy are described below.

During pregnancy, a combination of magnesium + vitamin B6 is prescribed. The drugs relax the muscles of the uterus and reduce its tone, preventing miscarriage.

Thanks to magnesium, the functions of the placenta and balance in the blood coagulation system are maintained, connective tissues are strengthened, and blood pressure is controlled.

Vitamin B6 supports the full growth and development of the fetus and promotes the normal development of the nervous system.

When choosing magnesium preparations, the form of release, the amount of “elemental” magnesium (in its pure form), bioavailability and combination with other elements are taken into account.

The amount of “elemental” magnesium depends on the chemical compound used by the manufacturer as a source of magnesium,%:

• Magnesium gluconate – 5.8 (100 mg of the drug is taken as 100%);
• Magnesium chloride – 12;
• Magnesium citrate – 16.2;
• Magnesium glycinate – 50;
• Magnesium oxide – 60.3.

Advice! When choosing a drug, pay attention first to the combination of substances, then to the amount of “elemental” magnesium. The higher the percentage of the latter, the more effective the drug

A review of the drugs is given below.

Magnesium sulfate. Release forms: solution in ampoules for intravenous or intramuscular administration, powder.

Solution in ampoules. Indications: hypertensive crisis, late toxicosis in pregnant women, convulsive syndrome, relief of status epilepticus.

Contraindications: sensitivity to magnesium, arterial hypotension, AV block and calcium deficiency.

Dosage:

• for hypertensive or convulsive conditions - 5-20 ml of a 25% solution intramuscularly or intravenously;
• for poisoning with mercury or arsenic - 5-10% solution intravenously, 5-10 ml.

Important! The drug is taken as prescribed and under the supervision of a doctor

Powder. Indications: arrhythmia, neurological disorders, gestosis in pregnant women, heavy metal poisoning, constipation, accumulation and stagnation of bile.

For constipation, take 10-30 g orally in half a glass of water. For children, the dose is calculated as one gram for each year of life.

For bile stagnation, take a 25% solution, 1 tablespoon three times a day.

Magne-B6. Release form: tablets, oral solution.

Indications: magnesium deficiency.

Dosage: for adults – 6-8 tablets per day or 3-4 ampoules of solution;

for children – 4-6 tablets per day or from one to 4 ampoules of solution.

Important! The drug is taken under medical supervision during pregnancy and insufficient kidney function.

Magnesium B6 analogues are any combination of a macroelement with vitamin B6.

The most popular drugs: Doppelhertz tablets with B vitamins, Magnelis B6, Magvit, Magnesium plus B6, etc.

Magnerot. The basis of the drug is a complex of magnesium and Orotic acid, which activates metabolism and stimulates cell growth, retains magnesium in the cell and enhances its effect.

Release form: 500 mg tablets.

Indications: risk of heart attack, heart failure, atherosclerosis and spastic conditions, calf muscle cramps.

The tablets are taken for 4-6 weeks.

Dosage:

• the first 7 days – 2 tablets three times a day;
• the following weeks – 1 tablet 2-3 times a day;
• for night cramps - 2-3 tablets once in the evening.

Magnesium citrate (natural calm). Release form: an aqueous solution of magnesium carbonate and citric acid.

Action: normalizes the acid-base balance during acidosis and hypoxia.

One teaspoon of the drug contains 205 mg of “elemental” (pure) magnesium.

Dosage:

• children under 10 years old – 1/4 teaspoon 1–2 times a day;
• for children over 10 years old, up to 1/2–1 teaspoon (if there is no diarrhea).

Additive Magnesium. Action: normalizes and activates metabolic processes.

Indications: fatigue, sleep disorders, pain and muscle spasms; intense physical activity, a period of rapid growth in children; prevention of atherosclerosis, myocardial infarction, oxalate urolithiasis.

Available in tablets for preparing an effervescent drink (tubes of 10 and 20 pcs.).

Contraindications: hypersensitivity, phenylketonuria.

Dosage: per day – 1 tablet dissolved in a glass of water.

Magnesium and potassium supplements are described below.

Panangin. Available in tablets. Prescribed for heart problems (arrhythmia, angina), hypertension and chronic heart failure.

The drug compensates for potassium losses when taking diuretics (Furosemide, Torasemide, Ethacrynic acid, Diacarb).

For atrial rhythm disturbances (extrasystole), Panangin is combined with antiarrhythmic drugs.

Contraindications: acidosis, myasthenia gravis, atrioventricular block, cardiogenic shock with low blood pressure, hemolysis, dehydration, disorders of potassium and magnesium metabolism.

Prescribe with caution during pregnancy and breastfeeding.

Analogs of Panangin: Asparkam, Asparkad, Pamaton, Potassium-magnesium asparginate, Orocamag.

In our country, rich magnesite deposits are located in the Middle Urals (Satkinskoye) and in the Orenburg region (Khalilovskoye). And in the area of ​​the city of Solikamsk, the world's largest deposit of carnallite is being developed. Dolomite, the most common of magnesium-containing minerals, is found in the Donbass, Moscow and Leningrad regions and many other places.

Magnesium metal is produced in two ways - electrothermal (or metallothermic) and electrolytic. As the names suggest, both processes involve electricity. But in the first case, its role is reduced to heating the reaction apparatus, and magnesium oxide obtained from minerals is reduced with some reducing agent, for example, coal, silicon, aluminum. This method is quite promising, and recently it has been increasingly used. However, the main industrial method for producing Mg is the second, electrolytic.

The electrolyte is a melt of anhydrous chlorides of magnesium, potassium and sodium; metallic magnesium is released at the iron cathode, and chlorine ions are discharged at the graphite anode. The process takes place in special electrolyzer baths. Molten magnesium floats to the surface of the bath, from where it is removed from time to time with a vacuum ladle and then poured into molds. But the process does not end there: there are still too many impurities in such magnesium. Therefore, the second stage is inevitable - purification of Mg. Magnesium can be refined in two ways - by remelting and fluxes or by sublimation in a vacuum. The meaning of the first method is well known: special additives - fluxes - interact with impurities and transform them into compounds that can be easily separated from the metal mechanically. The second method - vacuum sublimation - requires more complex equipment, but with its help, purer magnesium is obtained. Sublimation is carried out in special vacuum devices - steel cylindrical retorts. The “rough” metal is placed at the bottom of the retort, closed and the air is pumped out. Then the lower part of the retort is heated, and the upper part is constantly cooled by outside air. Under the influence of high temperature, magnesium sublimes - it goes into a gaseous state, bypassing the liquid state. Its vapor rises and condenses on the cold walls of the upper part of the retort. In this way it is possible to obtain a very pure metal containing over 99.99% magnesium.

From the kingdom of Neptune

But not only the earth’s crust is rich in magnesium - practically inexhaustible and constantly replenished reserves are stored in the blue pantries of the oceans and seas. Each cubic meter of sea water contains about 4 kg of magnesium. In total, more than 64,016 tons of this element are dissolved in the waters of the world's oceans.

Magnesium mining

How is magnesium obtained from the sea? Sea water is mixed in huge tanks with lime milk made from ground sea shells. This produces so-called milk of magnesia, which is dried and converted into magnesium chloride. Well, then electrolytic processes come into play.

The source of magnesium can be not only sea water, but also water from salt lakes containing magnesium chloride. We have such lakes in our country: in Crimea - Saki and Sasyk-Sivash, in the Volga region - Lake Elton and many others.

For what purposes are element No. 12 and its connections used?

Magnesium is extremely light, and this property could make it an excellent construction material, but, alas, pure magnesium is soft and fragile. Therefore, designers use magnesium in the form of alloys with other metals. Alloys of magnesium with aluminum, zinc and manganese are especially widely used. Each of the components contributes its own contribution to the overall properties: aluminum and zinc increase the strength of the alloy, manganese increases its anti-corrosion resistance. Well, what about magnesium? Magnesium makes the alloy light - parts made of magnesium alloy are 20-30% lighter than aluminum and 50-75% lighter than cast iron and steel... There are many elements that improve magnesium alloys, increase their heat resistance and ductility, and make them more resistant to oxidation. These are lithium, beryllium, calcium, cerium, cadmium, titanium and others.

The magnesium rocket won't take off, but...

But, unfortunately, there are also “enemies” - iron, silicon, nickel; they worsen the mechanical properties of alloys and reduce their corrosion resistance.

Magnesium alloys are widely used. Aviation and jet technology, nuclear reactors, engine parts, gasoline and oil tanks, instruments, car bodies, buses, cars, wheels, oil pumps, jackhammers, pneumatic drills, photo and movie cameras, binoculars - this is not a complete list of applications magnesium alloys.

Magnesium plays a significant role in metallurgy. It is used as a reducing agent in the production of some valuable metals - vanadium, chromium, titanium, zirconium. Magnesium introduced into molten cast iron modifies it, that is, improves its structure and increases its mechanical properties. Modified iron castings successfully replace steel forgings. In addition, metallurgists use magnesium to deoxidize steel and alloys.

The property of magnesium (in the form of powder, wire or tape) - to burn with a white, dazzling flame - is widely used in military equipment for the manufacture of lighting and signal flares, tracer bullets and shells, and incendiary bombs. Photographers are familiar with magnesium: “Calm down! I’m filming!” - and a bright flash of magnesium blinds you for a moment. However, magnesium plays this role less and less often - the electric lamp “blitz” has replaced it almost everywhere.

Applications of magnesium

And magnesium is involved in another grandiose work - the accumulation of solar energy. It is part of chlorophyll, which absorbs solar energy and, with its help, converts carbon dioxide and water into complex organic substances (sugar, starch, etc.) necessary for the nutrition of humans and animals. Without chlorophyll there would be no life, and without magnesium there would be no chlorophyll - it contains 2% of this element. Is this too much? Judge for yourself: the total amount of magnesium in the chlorophyll of all plants on Earth is about 100 billion tons! Element No. 12 is also found in almost all living organisms.

If you weigh 60kg, approximately 25g of this is magnesium. The services of magnesium are widely used in medicine: everyone is familiar with the “Epsom salt” MgSO 4 -7H 2 O. When taken orally, it serves as a reliable and fast-acting laxative, and when administered intramuscularly or intravenously, it relieves convulsive conditions and reduces vascular spasms. Pure magnesium oxide (burnt magnesia) is used for increased acidity of gastric juice, heartburn, and acid poisoning. Magnesium peroxide serves as a disinfectant for stomach disorders.

But medicine is not limited to the areas of application of magnesium compounds. Thus, magnesium oxide is used in the production of cements, refractory bricks, and in the rubber industry. Magnesium peroxide (“Novozon”) is used to bleach fabrics. Magnesium sulfate is used in the textile and paper industries as a mordant for dyeing, and an aqueous solution of magnesium chloride is used for the preparation of magnesium cement, xylolite and other synthetic materials. Magnesium carbonate MgCO 3 is used in the production of thermal insulation materials.

And finally, another broad field of activity for magnesium is organic chemistry. Magnesium powder is used to dehydrate important organic substances such as alcohol and aniline. Organomagnesium compounds are widely used in the synthesis of many organic substances.

So, the activity of magnesium in nature and the national economy is very multifaceted. But those who think: “he has already done everything he could” are hardly right. There is every reason to believe that magnesium's best role is yet to come.

• RAW MATERIALS ON THE PAVEMENT. If desired, magnesium can be extracted even from... simple cobblestones: after all, every kilogram of stone used for paving roads contains approximately 20 g of magnesium. There is, however, no need for such a process yet - magnesium from road stone would be too expensive.
• MAGNESIUM, SECOND AND ERA. How much magnesium is in the ocean? Let's imagine that from the first days of our era, people began to uniformly and intensively extract magnesium from sea water and by today have exhausted all the water reserves of this element. What do you think the “intensity” of mining should be? It turns out that every second for almost 2000 years it would be necessary to mine. million tons! But even during the Second World War, when the production of this metal was at its maximum, only 80 thousand tons of magnesium were obtained from sea water annually (!).

• TASTY MEDICINES. Statistics show that residents of areas with warmer climates experience spasms of blood vessels less frequently than northerners. Medicine explains this by the nutritional characteristics of both. After all, it is known that intravenous and intramuscular infusions of solutions of certain magnesium salts relieve spasms and cramps. Fruits and vegetables help accumulate the necessary supply of these salts in the body. Apricots, peaches and cauliflower are especially rich in magnesium. It is also found in regular cabbage, potatoes, and tomatoes.
• CAUTION DO NOT DAMAGE. Working with magnesium alloys sometimes causes a lot of trouble - magnesium oxidizes easily. Melting and casting of these alloys must be carried out under a layer of slag - otherwise the molten metal may catch fire from contact with air.

When grinding or polishing magnesium products, a dust suction device must be installed above the machine, because tiny particles of magnesium dispersed in the air create an explosive mixture.

However, this does not mean that any work with magnesium is fraught with the danger of fire or explosion. You can set fire to magnesium only by melting it, and this is not so easy to do under normal conditions - the high thermal conductivity of the alloy will not allow a match or even a torch to turn cast products into white oxide powder. But shavings or magnesium heating tape really need to be handled very carefully.

• YOU WILL NOT HAVE TO WAIT. Conventional radio tubes begin to work normally only after their grids are heated to 800°C. Every time you turn on the radio or TV, you have to wait a while before the music starts flowing or the blue screen flickers. To eliminate this drawback of radio tubes, Polish scientists from the Department of Electrical Engineering of the Wroclaw University of Technology proposed coating the cathodes of lamps with MgO: such lamps begin to work immediately after switching on.
• EGGSHELL PROBLEM. Several years ago, scientists at the University of Minnesota in the USA chose eggshells as an object of scientific research. They were able to establish that the more magnesium it contains, the stronger the shell. This means that by changing the composition of feed for laying hens, the strength of the shell can be increased. The importance of this conclusion for agriculture can be judged by the following figures: in Minnesota alone, annual losses due to egg fighting exceed a million dollars. No one here will say that this work of scientists is “not worth a damn.”
• MAGNESIUM AND... HEART ATTACK. Experiments conducted by Hungarian scientists on animals showed that a lack of Mg in the body increases susceptibility to heart attacks. Some dogs were given food rich in salts of this element, others - poor. By the end of the experiment, those dogs whose diet was low in magnesium suffered myocardial infarction.

• TAKE CARE OF MAGNESIUM! French biologists believe that magnesium will help doctors in the fight against such a serious illness of the 20th century as overwork. Studies show that the blood of tired people contains less magnesium than that of healthy people, and even the most insignificant deviations of “magnesium blood” from the norm do not pass without a trace.

It is important to remember that in cases where a person is often irritated for any reason, the magnesium contained in the body “burns out.” That is why in nervous, easily excitable people, disturbances in the functioning of the heart muscles are observed much more often.

• MAGNESIUM CARBONIC AND LIQUID OXYGEN. Large containers for storing liquid oxygen are usually made in the shape of a cylinder or ball to reduce heat loss. But a well-chosen form of storage is not everything. Reliable thermal insulation is needed. For these purposes, you can use a deep vacuum (as in a Dewar flask), you can use mineral wool, but often loose magnesium carbonate powder is poured between the inner and outer walls of the storage facility. This thermal insulation is both cheap and reliable.