Magnesium systems. Magnesium - description, beneficial properties, methods of use, daily intake of magnesium. Release form and composition

Magnesium B6: instructions for use and reviews

Magnesium B6 is a biologically active food supplement (BAA), an additional source of magnesium and vitamin B6.

Release form and composition

Magnesium B6 is available in the form of tablets: round, white; with a mass of 200 mg - small in size, almost tasteless, easy to swallow or with a mass of 600 mg (200 mg tablets - 25 pieces in blisters, 2 blisters in a cardboard pack; 600 mg tablets - 15 pieces in a blister, in a cardboard box 4 blisters).

1 tablet weighing 600 mg contains:

  • active ingredients: magnesium citrate – 50 mg; pyridoxine hydrochloride (vitamin B 6) – 5 mg;
  • auxiliary components: maltodextrin, microcrystalline cellulose (E460i), amorphous silicon dioxide (E551), hydroxypropyl methylcellulose (E464), stearic acid (E570), croscarmellose sodium (E468), dye titanium dioxide (E171), propylene glycol (E1520), talc ( E553).

1 tablet weighing 200 mg contains:

  • active ingredients: magnesium lactate (citrate) 2-water – 9 mg; pyridoxine (vitamin B 6) – 0.3 mg;
  • auxiliary components: sorbitol (E420), magnesium stearate (E470).

Pharmacological properties

Magnesium B6 is a vitamin and mineral complex, including pyridoxine (vitamin B 6) and magnesium, its effect is due to the following properties of the active components:

  • Magnesium is a vital macroelement that ensures carbohydrate-phosphorus and energy processes in the body, transmission of nerve impulses from the brain to peripheral nerve endings and muscles. It is necessary for protein synthesis and cell division, and is involved in the transmission genetic information, regulation of metabolism and enzymatic reactions. Supports cellular immunity, regulates the balance and proper distribution of calcium and sodium in the body. Improves blood circulation, normalizes heart function. A lack of magnesium in the body affects the functioning of the nervous, musculoskeletal, digestive, and cardiovascular systems;
  • pyridoxine – promotes the fixation of magnesium in the cell, improves its absorption and metabolism at the cellular level. In addition, it is necessary for the synthesis of hemoglobin and brain mediators, the normal functioning of a number of enzymatic systems, ensures the functioning of the nervous system, participates in the metabolism of fats and proteins, and regulates the use of glycogen.

For an adult physiological need in magnesium is 400 mg per day. Magnesium deficiency in the body can occur due to a violation of the diet or food intake, stress, physical activity, mental activity, or during pregnancy. In addition, the absorption of magnesium is impaired due to a lack of vitamin B 6 or diseases of the thyroid gland.

The body compensates for magnesium deficiency by reducing the supply of magnesium to vital organs, which leads to a deterioration in overall well-being. Taking Magnesium B6 has a beneficial effect on general health, eliminates headache, reduces the risk of developing cardiovascular diseases, increases the body's resistance to stress, normalizes blood pressure, and prevents the appearance of spasms.

Indications for use

According to the instructions, Magnesium B6 is indicated as an additional source of magnesium and pyridoxine to improve the body’s condition in the following cases:

  • muscle pain;
  • sleep disorders;
  • dysfunction of the nervous system;
  • hair loss;
  • spasms;
  • other conditions caused by magnesium and vitamin B6 deficiency.

Contraindications

Tablets are contraindicated for patients with individual intolerance to the components.

200 mg tablets should not be taken during pregnancy and breastfeeding.

Do not use Magnesium B6 for children.

Instructions for use of Magnesium B6: method and dosage

The drug is taken orally with meals.

  • tablets weighing 200 mg: 2 pcs. 3 times a day. The duration of the course is 21–28 days;
  • tablets weighing 600 mg: 1 pc. per day for 30 days.

Side effects

200 mg tablets contain sorbitol, so taking them in large doses can have a laxative effect.

Overdose

Overdose symptoms have not been established.

special instructions

Magnesium B6 is not a drug.

Use during pregnancy and lactation

The use of 200 mg tablets is contraindicated during pregnancy and breastfeeding.

Use in childhood

Magnesium B6 is not indicated for children.

Drug interactions

No data.

Analogs

Analogs of Magnesium B6 are: Magnesium B6 Vitamir, Magnesium plus B6, Magnesium B6 – forte, Magnesium plus Vitamin B6 with lemon flavor, Magne B6, etc.

Terms and conditions of storage

Keep away from children.

Store at temperatures up to 25 °C, protected from moisture and direct sunlight.

Shelf life: 600 mg tablets – 3 years; tablets 200 mg – 2 years.

DEFINITION

Magnesium- the twelfth element of the Periodic Table. Designation - Mg from the Latin "magnesium". Located in the third period, group IIA. Refers to metals. The nuclear charge is 12.

Magnesium is very common in nature. It occurs in large quantities as magnesium carbonate, forming the minerals magnesite MgCO 3 and dolomite MgCO 3 ×CaCO 3 . Magnesium sulfate and chloride are part of the minerals kainite KCl × MgSO 4 × 3H 2 O and carnallite KCl × MgCl 2 × 6H 2 O. The Mg 2+ ion is contained in sea ​​water, giving it a bitter taste. Total magnesium in the earth's crust is about 2% (mass.).

In its simple form, magnesium is a silvery-white (Fig. 1), very light metal. In air it changes little, since it is quickly covered with a thin layer of oxide, protecting it from further oxidation.

Rice. 1. Magnesium. Appearance.

Atomic and molecular mass of magnesium

The relative molecular mass of a substance (M r) is a number showing how many times the mass of a given molecule is greater than 1/12 the mass of a carbon atom, and the relative atomic mass element (A r) - how many times the average mass of atoms of a chemical element is greater than 1/12 of the mass of a carbon atom.

Since in the free state magnesium exists in the form of monoatomic Mg molecules, the values ​​of its atomic and molecular weight match up. They are equal to 24.304.

Isotopes of magnesium

It is known that in nature magnesium can be found in the form of three stable isotopes 24 Mg (23.99%), 25 Mg (24.99%) and 26 Mg (25.98%). Their mass numbers are 24, 25 and 26, respectively. The nucleus of an atom of the magnesium isotope 24 Mg contains twelve protons and twelve neutrons, and the isotopes 25 Mg and 26 Mg contain the same number of protons, thirteen and fourteen neutrons, respectively.

There are artificial isotopes of magnesium with mass numbers from 5 to 23 and from 27 to 40.

Magnesium ions

At the outer energy level of the magnesium atom there are two electrons, which are valence:

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

As a result of chemical interaction, manium gives up its valence electrons, i.e. is their donor, and turns into a positively charged ion:

Mg 0 -2e → Mg 2+ .

Magnesium molecule and atom

In the free state, magnesium exists in the form of monoatomic Mg molecules. Here are some properties characterizing the magnesium atom and molecule:

Magnesium alloys

The main area of ​​application of metallic magnesium is the production of various light alloys based on it. The addition of small amounts of other metals to magnesium dramatically changes its mechanical properties, giving the alloy significant hardness, strength and corrosion resistance.

Especially valuable properties possess alloys called electrons. They belong to three systems: Mg-Al-Zn, Mg-Mn and Mg-Zn-Zr. The most widely used are alloys of the Mg-Al-Zn system, containing from 3 to 10% aluminum and from 0.2 to 3% zinc. The advantage of magnesium alloys is their low density (about 1.8 g/cm3).

Examples of problem solving

EXAMPLE 1

A normal concentration of magnesium in the body does not in itself guarantee wellness, 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 into duodenum and partly 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:

  • rises immune activity cells, which is why the chemical element must be present in the diet of young 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. He controls the activities respiratory system, musculoskeletal system, condition skin, the functioning of the heart and sensory organs. That's why when 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 acute form allergies, 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- a result of magnesium deficiency). Thanks to the exchange, calcium is not deposited in the kidneys, gallbladder, ureters and bones.

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

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


Nuts, cereals, green vegetables and dried fruits are the main sources of magnesium (photo: men's magazine MEN's LIFE)
Vegetable oil Cedar, sesame, mustard, almond, olive, peanut, pumpkin, flax, soy
Animal oils Lamb, beef, pork fats, lard, margarine, butter.

Fish: flounder, halibut, chinook salmon
Juices Grape, grapefruit, pumpkin, beet, tomato. As well as orange, apple, asparagus and celery juice
Nuts Cashews, peanuts, sweet almonds, hazelnuts, walnuts. As well as cedar, Brazilian, sunflower, pumpkin and sesame seeds
Cereals Oatmeal, buckwheat, brown rice, barley and millet cereals, rice and wheat bran, sprouted wheat grains
Vegetables Carrots, cabbage, beets, spinach, greens, chard, parsnips, artichoke
Fruits Apricots, plums, apples, peaches with peel
Dried fruits Prunes, dates, dried apricots
Dairy Condensed milk or powdered milk, fermented baked milk, kefir
  • 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. In products intended for long-term storage, no 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 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. Recovery period after allergic rhinitis drags on.
  • 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. Lingering 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.
  • Violation heart rate. 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 organs is disrupted gastrointestinal tract(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 groats, sprouted wheat grains, rice and wheat bran). Dark chocolate will help replenish magnesium deficiency, Rye bread, avocado, seaweed, nuts, dried fruits, legumes.

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

Medicinal and table mineral water eliminates magnesium deficiency.

Magnesium, sodium, bicarbonate sulfate

Medical

Hydrocarbonate sodium-magnesium

Medical dining room

Uleymskaya (magnesium)

Chloride-sulfate calcium-sodium (magnesium-calcium-sodium)

Medical dining room

Hydrocarbonate magnesium siliceous

Medical dining room

Dorokhovskaya

Magnesium-calcium sulfate

Medical dining room

Sulfate-hydrocarbonate sodium-magnesium-calcium

Medical dining room

Advice! Magnesium is absorbed only in a combination of B vitamins and calcium. Eat more cottage cheese, milk, bran bread, fish, cereals and eggs. Full sleep, high efficiency, good memory and physical endurance 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 something for lunch every day buckwheat porridge and lettuce with carrots;
  • 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;
  • get carried away natural coffee and green tea or taking 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. At renal failure, increased catabolism (breakdown) of proteins, 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! Maximum daily dose magnesium – 800 mg. Exceeding the dose by 10-50 mg is fraught 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, as 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, strengthened connective tissues, blood pressure is monitored.

Vitamin B6 supports the full growth and development of the fetus, promotes normal development 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 form: solution in ampoules for intravenous or intramuscular injection, 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, cramps of the calf muscles.

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 acid-base balance with 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; intensive physical exercise, period 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.

Magnesium compounds have been known to man for a very long time. Magnesite (in Greek Magnhsia oliqV) was a soft, white, soapy mineral (soapstone, or talc) found in the Magnesia region of Thessaly. When this mineral was calcined, a white powder was obtained, which became known as white magnesia.

In 1695 N.Gro, evaporating mineral water Epsom spring (England), obtained salt that had a bitter taste and laxative effect (MgSO 4 · 7H 2 O). A few years later it turned out that when interacting with soda or potash, this salt forms a white, loose powder, the same as that formed when magnesite is calcined.

In 1808, the English chemist and physicist Humphry Davy, by electrolysis of slightly moistened white magnesia with mercury oxide as a cathode, obtained an amalgam of a new metal capable of forming white magnesia. It was called magnesium. Davy obtained the contaminated metal, and pure magnesium was isolated only in 1829 by the French chemist Antoine Bussy (1794–1882).

Distribution of magnesium in nature and its industrial extraction.

Magnesium is found in crystalline rocks in the form of insoluble carbonates or sulfates, and also (to a lesser extent) accessible form) in the form of silicates. The estimate of its total content depends significantly on the geochemical model used, in particular, on the weight ratios of volcanic and sedimentary rocks. Currently, values ​​from 2 to 13.3% are used. Perhaps the most reasonable value is 2.76%, which ranks magnesium sixth in abundance after calcium (4.66%) and ahead of sodium (2.27%) and potassium (1.84%).

Large land areas such as Dolomites in Italy they consist predominantly of the dolomite mineral MgCa(CO 3) 2. There are also sedimentary minerals magnesite MgCO 3, epsomite MgSO 4 · 7H 2 O, carnallite K 2 MgCl 4 · 6H 2 O, langbeinite K 2 Mg 2 (SO 4) 3.

There are dolomite deposits in many other areas, including Moscow and Leningrad regions. Rich deposits of magnesite were found in the Middle Urals and in the Orenburg region. The largest carnallite deposit is being developed in the Solikamsk region. Magnesium silicates are represented by the basalt mineral olivine (Mg,Fe) 2 (SiO 4), soapstone (talc) Mg 3 Si 4 O 10 (OH) 2, asbestos (chrysotile) Mg 3 Si 2 O 5 (OH) 4 and mica. Spinel MgAl 2 O 4 belongs to precious stones.

A large amount of magnesium is found in the waters of the seas and oceans and in natural brines ( cm. CHEMISTRY OF HYDROSPHERE). In some countries, they are the raw materials for the production of magnesium. In terms of metallic element content in seawater, it is second only to sodium. Each cubic meter of sea water contains about 4 kg of magnesium. Magnesium is also found in fresh water, determining, along with calcium, its rigidity.

Magnesium is always found in plants, as it is part of chlorophylls.

Characteristics of simple substances and industrial production of metallic magnesium.

Magnesium is a silvery-white shiny metal, relatively soft, ductile and malleable. Its strength and hardness are minimal in prevalence for cast samples, higher for pressed ones.

Under normal conditions, magnesium is resistant to oxidation due to the formation of a strong oxide film. However, it reacts actively with most non-metals, especially when heated. Magnesium ignites in the presence of halogens (in the presence of moisture), forming the corresponding halides, and burns with a blindingly bright flame in air, turning into MgO oxide and Mg 3 N 2 nitride:

2Mg (k) + O 2 (g) = 2MgO (k) ; DG° = –1128 kJ/mol

3Mg (k) + N 2 (t) = Mg 3 N 2 (k); DG° = –401 kJ/mol

Despite the low melting point (650° C), it is impossible to melt magnesium in air.

When exposed to hydrogen under a pressure of 200 atm at 150°C, magnesium forms the hydride MgH 2 . WITH cold water magnesium does not react, but displaces hydrogen from boiling water and forms hydroxide Mg(OH) 2:

Mg + 2H 2 O = Mg(OH) 2 + H 2

At the end of the reaction, the pH value (10.3) of the resulting saturated solution of magnesium hydroxide corresponds to equilibrium:

In the latter case, the resulting mixture of carbon monoxide and magnesium vapor must be quickly cooled with an inert gas to prevent a reverse reaction.

World magnesium production is approaching 400 thousand tons per year. The main producers are the USA (43%), CIS countries (26%) and Norway (17%). In recent years, China has been sharply increasing its magnesium exports. In Russia, one of the largest producers of magnesium is the titanium-magnesium plant in Berezniki (Perm region) and the Solikamsk magnesium plant. Magnesium production is also taking place in the city of Asbest.

Magnesium is the lightest structural material used on an industrial scale. Its density (1.7 g cm–3) is less than two-thirds that of aluminum. Magnesium alloys weigh four times less than steel. In addition, magnesium is perfectly processed and can be cast and remade by any standard methods metalworking (rolling, stamping, drawing, forging, welding, soldering, riveting). Therefore, its main application is as a lightweight structural metal.

Magnesium alloys typically contain more than 90% magnesium, as well as 2–9% aluminum, 1–3% zinc, and 0.2–1% manganese. Maintaining strength at high temperature(up to 450 ° C) is noticeably improved when alloyed with rare earth metals (for example, praseodymium and neodymium) or thorium. These alloys can be used for automobile engine housings, as well as aircraft fuselages and landing gear. Magnesium is used not only in aviation, but also in the manufacture of stairs, dock walkways, cargo platforms, conveyors and lifts, as well as in the production of photographic and optical equipment.

Up to 5% magnesium is added to industrial aluminum to improve mechanical properties, weldability and corrosion resistance. Magnesium is also used for cathodic protection other metals against corrosion, as an oxygen scavenger and reducing agent in the production of beryllium, titanium, zirconium, hafnium and uranium. Mixtures of magnesium powder with oxidizing agents are used in pyrotechnics for the preparation of lighting and incendiary compositions.

Magnesium compounds.

The predominant oxidation state (+2) for magnesium is determined by its electronic configuration, ionization energies and atomic sizes. The oxidation state (+3) is impossible, since the third ionization energy for magnesium is 7733 kJ mol –1. This energy is much higher than can be compensated for by the formation of additional bonds, even if they are predominantly covalent. The reasons for the instability of magnesium compounds in the oxidation state (+1) are less obvious. An assessment of the enthalpy of formation of such compounds shows that they must be stable with respect to their constituent elements. The reason that magnesium(I) compounds are not stable is the much higher enthalpy of formation of magnesium(II) compounds, which should lead to rapid and complete disproportionation:

Mg(k) + Cl 2 (g) = MgCl 2 (k);

D N° arr = –642 kJ/(mol MgCl 2)

2Mg(k) + Cl 2 (g) = 2MgCl(k);

D N° arr = –250 kJ/(2 mol MgCl)

2MgCl(k) = Mg(k) + MgCl 2 (k);

D N° disprop = –392 kJ/(2 mol MgCl)

If a synthetic route can be found that makes disproportionation difficult, such compounds may be obtained. There is some evidence for the formation of magnesium(I) particles during electrolysis on magnesium electrodes. Thus, during the electrolysis of NaCl on a magnesium anode, hydrogen is released, and the amount of magnesium lost by the anode corresponds to a charge of +1.3. Similarly, during the electrolysis of an aqueous solution of Na 2 SO 4, the amount of hydrogen released corresponds to the oxidation of water by magnesium ions, the charge of which corresponds to +1.4.

Most magnesium salts are highly soluble in water. The dissolution process is accompanied by slight hydrolysis. The resulting solutions have a weakly acidic environment:

2+ + H 2 O + + H 3 O +

Compounds of magnesium with many non-metals, including carbon, nitrogen, phosphorus, and sulfur are irreversibly hydrolyzed by water.

Magnesium hydride composition MgH 2 is a polymer with bridging hydrogen atoms. The coordination number of magnesium in it is 4. This structure leads to sharp decline thermal stability of the connection. Magnesium hydride is easily oxidized by atmospheric oxygen and water. These reactions are accompanied by a large release of energy.

Magnesium nitride Mg 3 N 2. Forms yellowish crystals. The hydrolysis of magnesium nitride produces ammonia hydrate:

Mg 3 N 2 + 8H 2 O = 3Mg(OH) 2 + 2NH 3 H 2 O

If the hydrolysis of magnesium nitride is carried out in an alkaline medium, ammonia hydrate is not formed, but ammonia gas is released. Hydrolysis in an acidic environment leads to the formation of magnesium and ammonium cations:

Mg 3 N 2 + 8H 3 O + = 3Mg 2+ + 2NH 4 + + 8H 2 O

Magnesium oxide MgO is called burnt magnesia. It is obtained by firing magnesite, dolomite, basic magnesium carbonate, magnesium hydroxide, as well as calcining bischofite MgCl 2 ·6H 2 O in an atmosphere of water vapor.

The reactivity of magnesium oxide depends on the temperature at which it is produced. Magnesium oxide prepared at 500–700°C is called light magnesia. It reacts easily with dilute acids and water to form the corresponding salts or magnesium hydroxide, and absorbs carbon dioxide and moisture from the air. Magnesium oxide obtained at 1200–1600° C is called heavy magnesia. It is characterized by acid resistance and water resistance.

Magnesium oxide is widely used as a heat-resistant material. It is characterized by both high thermal conductivity and good electrical insulating properties. Therefore, this compound is used in insulating radiators for local heating.

Lighter grades of magnesia are used to prepare magnesia cement and building materials based on it, and also as a vulcanizing agent in the rubber industry.

Magnesium hydroxide Mg(OH) 2 forms colorless crystals. The solubility of this compound is low (2·10 –4 mol/l at 20°C). It can be converted into solution by the action of ammonium salts:

Mg(OH) 2 + 2NH 4 Cl = MgCl 2 + 2NH 3 H 2 O

Magnesium hydroxide is thermally unstable and decomposes when heated:

Mg(OH) 2 = MgO + H 2 O

On an industrial scale, magnesium hydroxide is produced by precipitation with lime from sea water and natural brines.

Magnesium hydroxide is a mild base that, in the form of an aqueous solution (milk of magnesia), is widely used to reduce acidity gastric juice. Moreover, despite its softness, Mg(OH) 2 neutralizes acids 1.37 times more than sodium hydroxide NaOH and 2.85 times more than sodium bicarbonate NaHCO 3.

It is also used to produce magnesium oxide, sugar refining, water purification in boiler plants, and as a component of toothpastes.

Magnesium carbonate MgCO 3 forms colorless crystals. It occurs naturally in anhydrous form (magnesite). In addition, penta-, tri- and monohydrates of magnesium carbonate are known.

The solubility of magnesium carbonate in the absence of carbon dioxide is about 0.5 mg/l. In the presence of excess carbon dioxide and water, magnesium carbonate transforms into soluble bicarbonate, and when boiling, the reverse process occurs. Carbonate and bicarbonate react with acids to release carbon dioxide and form the corresponding salts. When heated, magnesium carbonate, without melting, decomposes:

MgCO 3 = MgO + CO 2

This process is used to produce magnesium oxide. In addition, natural magnesium carbonate is the starting material for the production of metallic magnesium and its compounds. It is also used as fertilizer and to reduce soil acidity.

Loose magnesium carbonate powder is poured between the double walls of liquid oxygen storage tanks. This thermal insulation is cheap and reliable.

Magnesium sulfate MgSO 4 is known in the anhydrous state, as well as in the form of various hydrates. Kieserite MgSO 4 ·H 2 O, epsomite MgSO 4 ·7H 2 O and hexahydrate MgSO 4 ·6H 2 O are found in nature.

In medicine, magnesium sulfate heptahydrate MgSO 4 ·7H 2 O is used, commonly known as Epsom or bitter salt. This compound has a laxative effect. With intramuscular or intravenous infusions Magnesium sulfate relieves convulsions and reduces vascular spasms.

Magnesium sulfate is used in the textile and paper industries as a dyeing mordant, as a weighting agent for cotton and silk, and as a paper filler. It serves as a raw material for the production of magnesium oxide.

Magnesium nitrate Mg(NO 3) 2 are colorless hygroscopic crystals. Solubility in water at 20° C is 73.3 g per 100 g. The hexahydrate crystallizes from aqueous solutions. Above 90°C it dehydrates to monohydrate. Then water is separated with partial hydrolysis and decomposition to magnesium oxide. This process is used in the synthesis of high purity magnesium oxide. From magnesium nitrate, nitrates of other metals are obtained, as well as various magnesium compounds. In addition, magnesium nitrate is part of complex fertilizers and pyrotechnic mixtures.

Magnesium perchlorate Mg(ClO 4) 2 forms very hygroscopic colorless crystals. It is highly soluble in water (99.6 g per 100 g) and organic solvents. The hexahydrate crystallizes from aqueous solutions. Concentrated solutions of magnesium perchlorate in organic solvents and its solvates with reducing agent molecules are explosive.

Partially hydrated magnesium perchlorate containing 2–2.5 molecules of water is released under commercial name"anhydrone". To obtain anhydrous magnesium perchlorate, it is dried in a vacuum at 200–300 ° C. It is used as a gas desiccant. It absorbs not only water vapor, but also ammonia, alcohol vapor, acetone and other polar substances.

Magnesium perchlorate is used as an acylation catalyst in the Friedel–Crafts reaction, and also as an oxidizing agent in microanalysis.

Magnesium fluoride MgF 2 is slightly soluble in water (0.013 g per 100 g at 25 ° C). It occurs naturally as the mineral selaite. Magnesium fluoride is obtained by reacting magnesium sulfate or oxide with hydrofluoric acid or magnesium chloride with potassium or ammonium fluoride.

Magnesium fluoride is part of fluxes, glasses, ceramics, enamels, catalysts, mixtures for producing artificial mica and asbestos. In addition, it is an optical and laser material.

Magnesium chloride MgCl 2 is one of the most industrially important magnesium salts. Its solubility is 54.5 g per 100 g of water at 20 ° C. Concentrated aqueous solutions of magnesium chloride dissolve magnesium oxide. MgCl 2 mMg(OH) 2 nH 2 O crystallizes from the resulting solutions. These compounds are part of magnesia cements.

Magnesium chloride forms crystalline hydrates with 1, 2, 4, 6, 8 and 12 water molecules. As the temperature increases, the number of molecules of water of crystallization decreases.

In nature, magnesium chloride is found in the form of the minerals bischofite MgCl 2 ·6H 2 O, magnesite chloride MgCl 2, and carnallite. It is found in sea water, brine from salt lakes, and some underground brines.

Anhydrous magnesium chloride is used in the production of metallic magnesium and magnesium oxide, and hexahydrate is used to produce magnesium cements. An aqueous solution of magnesium chloride is used as a coolant and antifreeze. It serves as a de-icing agent on airfields, railway tracks and switches, as well as against freezing of coal and ores. The wood is impregnated with a solution of magnesium chloride to make it fire resistant.

Magnesium bromide MgBr 2 is highly soluble in water (101.5 g per 100 g at 20° C). From aqueous solutions it crystallizes from –42.7 to 0.83 ° C in the form of decahydrate, at higher temperatures - in the form of hexahydrate. It forms numerous crystal solvates, such as MgB 2 6ROH (R = Me, Et, Pr), MgBr 2 6Me 2 CO, MgBr 2 3Et 2 O, as well as amines MgBr 2 n NH 3 ( n = 2–6).

Complex magnesium compounds. In aqueous solutions, magnesium ion exists in the form of an aqua complex 2+. In non-aqueous solvents, such as liquid ammonia, the magnesium ion forms complexes with solvent molecules. Solvates of magnesium salts usually crystallize from such solutions. Several halide complexes of the MX 4 2– type are known, where X is the halide anion.

Among complex magnesium compounds, chlorophylls, which are modified porphyrin complexes of magnesium, are of particular importance. They are vital for photosynthesis in green plants.

Organomagnesium compounds. Numerous compounds containing metal–carbon bonds have been obtained for magnesium. Especially a lot of research is devoted to Grignard reagents RMgX (X = Cl, Br, I).

Grignard reagents are the most important organometallic magnesium compounds and probably the most used organometallic reagents. This is due to their ease of production and synthetic versatility. It has been established that in solution these compounds can contain a variety of chemical particles that are in mobile equilibrium.

Grignard reagents are usually prepared by slowly adding an organic halide to a suspension of magnesium turnings in an appropriate solvent under vigorous stirring and in the complete absence of air and moisture. The reaction usually starts slowly. It can be initiated by a small crystal of iodine, which destroys the protective layer on the metal surface.

Grignard reagents are widely used for the synthesis of alcohols, aldehydes, ketones, carboxylic acids, esters and amides and are probably the most important reagents for creating carbon-carbon bonds, as well as bonds between carbon atoms and other elements (nitrogen, oxygen, sulfur, etc.) .d.).

R2Mg compounds usually decompose when heated. In the crystalline state, they have the structure of linear polymers with bridging alkyl groups. The MgMe 2 compound is a non-volatile polymer, stable up to ~250° C, insoluble in hydrocarbons and only slightly soluble in ether. The compound MgEt 2 and higher homologues are very similar to MgMe 2, but they decompose at lower temperatures (175–200 ° C), forming the corresponding alkene and MgH 2 in the opposite reaction to their formation. MgPh 2 is also similar to them; it is insoluble in benzene, dissolves in ether to form the monomeric complex MgPh 2 · 2Et 2 O and decomposes at 280 ° C to form Ph 2 and metallic magnesium.

Biological role of magnesium.

Green plant leaves contain chlorophylls, which are magnesium-containing porphyrin complexes involved in photosynthesis.

Magnesium is also closely involved in biochemical processes in animal bodies. Magnesium ions are necessary for the initiation of enzymes responsible for the conversion of phosphates, for the transfer of nerve impulses and for the metabolism of carbohydrates. They are also involved in muscle contraction, which is initiated by calcium ions.

Several years ago, scientists at the University of Minnesota in the USA found that eggshell the stronger the more magnesium it contains.

The body of an adult weighing 65 kg contains about 20 g of magnesium (mainly in the form of ions). Most of it is concentrated in the bones. Magnesium complexes with ATP and ADP are present in the intracellular fluid.

The daily requirement for this element is 0.35 g. With a monotonous diet, a lack of green vegetables and fruits, as well as with alcoholism, magnesium deficiency often occurs. Apricots, peaches and cauliflower. It is also found in regular cabbage, potatoes, and tomatoes.

Statistics show that residents of areas with warmer climates experience cramps blood vessels happen less often than among northerners. It is believed that the reason for this is the dietary habits in cold regions. They eat less fruits and vegetables, which means they get less magnesium.

Research by French biologists has shown that the blood of tired people contains less magnesium than that of rested people. It is believed that diet rich in magnesium should help doctors in the fight against such a serious illness as overwork.

Elena Savinkina

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