Calcium is an important metal for production and essential for human life.

Calcium is a vital macronutrient, in the presence of which more than 300 biochemical reactions occur in the human body.

The mineral plays a primary role in the construction and strengthening of bone tissue, participates in the processes of blood clotting, normalizing the contractility of the myocardium and skeletal muscles, restoring the balance between reactions of excitation and inhibition in the brain, and regulating the activity of certain enzymes.

The compound received its name from the word “Calx”, which translated from Latin means “Lime”.

Biological role

The total concentration of calcium in the human body is 2% of body weight (1000 - 1500 grams), with the main amount (99%) contained in bone tissue, nails, enamel and dentin of teeth.

Content:

• Biological role
• Deficiency and overdose
• Daily norm
• Natural springs
• What affects calcium absorption
• Conclusion

The importance of the macroelement: regulates the pressure of blood, tissue and intercellular fluids (together with sodium, magnesium and potassium); participates in the formation of bone tissue, including teeth and cartilage; supports normal blood clotting by potentiating the transition of prothrombin to thrombin; increases the permeability of membranes for the penetration of hormones and nutrients; potentiates the production of cellular and humoral immunity, as a result of which the body’s resistance to infections improves; maintains skeletal muscle tone; neutralizes the negative effects of lactic and uric acid that accumulate in muscles due to the breakdown of fats and proteins (during physical activity); participates in the mechanisms of transmission of nerve impulses to the brain; normalizes the synthesis of proteins and nucleic acids in smooth muscles; compacts the walls of blood vessels, which leads to a decrease in the release of histamine compounds; stabilizes the acid-base balance in the body; activates the action of enzymes involved in the formation of neurotransmitters.

The normal concentration of calcium in the blood is 2.2 millimoles per liter. Deviations from this indicator indicate a deficiency or excess of the compound in the body. Consider the symptoms indicating the development of hypo or hypercalcemia.

Decrease values:

• DiGeorge syndrome, or a genetic disorder in which the parathyroid and thymus glands are underdeveloped or absent;
• dysfunction of the parathyroid glands due to its autoimmune lesion or surgical intervention;
• decreased magnesium levels;
• decreased vitamin D levels;
• liver and kidney damage, which reduces albumin levels;
• damage to pancreatic tissue or pancreatic necrosis;
• long-term use of certain medications;
• massive blood transfusion.

Deficiency and overdose

Calcium is stored in the porous structure of long bones. In case of insufficient intake of the mineral from food, the body “goes” to mobilize the compound from bone tissue, as a result of which demineralization of the pelvic bones, spine and lower extremities occurs. Signs of calcium deficiency:

• pain in joints, bones, teeth;
• muscle weakness;
• brittle nails;
• increased calcium levels in the blood;
• skin rashes;
• rapid pulse;
• muscle spasms;
• convulsions;
• numbness of the limbs;
• the appearance of microcracks in tooth enamel;
• nervousness;
• fatigue;
• hypertension;
• pale face;
• insomnia;
• decreased mental abilities;
• lack of coordination;
• growth retardation, rickets (in children);
• spinal deformity, frequent bone fractures;
• tooth decay;
• allergic reactions;
• decreased blood clotting;
• heavy menstrual flow.

In 80% of cases, hypocalcemia is asymptomatic, which leads to the development of serious pathologies: osteoporosis, kidney stone formation, hypertension, osteochondrosis. To prevent these problems, it is important to identify and eliminate in advance the factors that provoke macronutrient deficiency in the body.

Causes of calcium deficiency:

• lack of foods containing a beneficial compound in the diet;
• impaired absorption of the element in the intestine due to dysbiosis or the absence of the lactase enzyme, which breaks down milk protein;
• excess lead, zinc, magnesium, iron, potassium, phosphorus, sodium in the body;
• chronic diseases of the digestive tract (pancreatitis, diabetes mellitus, renal failure, gastric or duodenal ulcers);
• diseases of the thyroid gland, in which the synthesis of the hormone calcitonin, which controls calcium metabolism, is impaired;
• increased consumption of “bone-forming” nutrients due to stressful situations, smoking, physical activity, pregnancy, breastfeeding;
• excessive consumption of drinks that inhibit the absorption of minerals in the intestines (coffee, alcohol, carbonated water, energy tonics);
• deficiency of vitamin D in the diet, especially when following vegetarianism or a raw food diet;
• long-term use of laxatives and diuretics, which “wash out” the building mineral from the body.

In addition, calcium metabolism is disrupted due to excessive excretion of the compound in the urine (idiopathic hypercalciuria), low absorption of the substance in the intestine (intestinal malabsorption), the formation of kidney stones (calcium nephrolithiasis), hyperfunction of the parathyroid glands, and hypertension.

To eliminate the symptoms of hypocalcemia, you need to enrich your daily diet with calcium-containing products or complex dietary supplements, the main active component of which is the missing macronutrient. When using medications, consult your doctor first.

In the process of drawing up a nutritional plan, keep in mind that daily consumption of more than 2500 milligrams of the mineral against the background of calcium metabolism disorders leads to intense calcification of bones, blood vessels and internal organs, as a result of which persistent hypercalcemia develops.

Symptoms of excess compound in the body:

• thirst;
• nausea;
• vomit;
• loss of appetite;
• weakness;
• frequent urination;
• decreased smooth muscle tone;
• arrhythmia;
• discomfort in the epigastric region;
• increased concentration of calcium in urine and blood;
• angina and bradycardia;
• decreased cognitive function;
• formation of stones in the kidneys and bladder;
• gout.

In some cases, hypercalcemia occurs as a result of hereditary pathologies of the thyroid gland, in particular multiple endocrine neoplasia, and sometimes as a result of malignant neoplasms.

Properties

Physical properties

Calcium metal exists in two allotropic modifications. Up to 443 °C, α-Ca with a cubic face-centered lattice (parameter a = 0.558 nm) is stable; β-Ca with a cubic body-centered lattice of the α-Fe type (parameter a = 0.448 nm) is more stable. Standard enthalpy ΔH

0 transition α → β is 0.93 kJ/mol.

Chemical properties

Calcium is a typical alkaline earth metal. The chemical activity of calcium is high, but lower than that of all other alkaline earth metals. It easily reacts with oxygen, carbon dioxide and moisture in the air, which is why the surface of calcium metal is usually dull gray, so in the laboratory calcium is usually stored, like other alkaline earth metals, in a tightly closed jar under a layer of kerosene or liquid paraffin.

In the series of standard potentials, calcium is located to the left of hydrogen. The standard electrode potential of the Ca2+/Ca0 pair is −2.84 V, so calcium reacts actively with water, but without ignition:

Ca + 2H2O = Ca(OH)2 + H2↑ + Q.

Calcium reacts with active non-metals (oxygen, chlorine, bromine) under normal conditions:

2Ca + O2 = 2CaO, Ca + Br2 = CaBr2.

When heated in air or oxygen, calcium ignites. Calcium reacts with less active non-metals (hydrogen, boron, carbon, silicon, nitrogen, phosphorus and others) when heated, for example:

Ca + H2 = CaH2, Ca + 6B = CaB6,

3Ca + N2 = Ca3N2, Ca + 2C = CaC2,

3Ca + 2P = Ca3P2 (calcium phosphide), calcium phosphides of the compositions CaP and CaP5 are also known;

2Ca + Si = Ca2Si (calcium silicide); calcium silicides of the compositions CaSi, Ca3Si4 and CaSi2 are also known.

The occurrence of the above reactions is usually accompanied by the release of a large amount of heat (that is, these reactions are exothermic). In all compounds with non-metals, the oxidation state of calcium is +2. Most of the calcium compounds with non-metals are easily decomposed by water, for example:

CaH2 + 2H2O = Ca(OH)2 + 2H2↑,

Ca3N2 + 3H2O = 3Ca(OH)2 + 2NH3↑.

The Ca2+ ion is colorless. When soluble calcium salts are added to the flame, the flame turns brick-red.

Calcium salts such as CaCl2 chloride, CaBr2 bromide, CaI2 iodide and Ca(NO3)2 nitrate are highly soluble in water. Insoluble in water are fluoride CaF2, carbonate CaCO3, sulfate CaSO4, orthophosphate Ca3(PO4)2, oxalate CaC2O4 and some others.

It is important that, unlike calcium carbonate CaCO3, acidic calcium carbonate (bicarbonate) Ca(HCO3)2 is soluble in water. In nature, this leads to the following processes. When cold rain or river water, saturated with carbon dioxide, penetrates underground and falls on limestone, their dissolution is observed:

CaCO3 + CO2 + H2O = Ca(HCO3)2.

In the same places where water saturated with calcium bicarbonate comes to the surface of the earth and is heated by the sun's rays, a reverse reaction occurs:

Ca(HCO3)2 = CaCO3 + CO2↑ + H2O.

This is how large masses of substances are transferred in nature. As a result, huge gaps can form underground, and beautiful stone “icicles” - stalactites and stalagmites - form in caves.

The presence of dissolved calcium bicarbonate in water largely determines the temporary hardness of water. It is called temporary because when water boils, bicarbonate decomposes and CaCO3 precipitates. This phenomenon leads, for example, to the fact that scale forms in the kettle over time.

Daily norm

The daily need for calcium directly depends on the age and gender of a person. Moreover, the largest amount of macronutrients is required by a growing body, pregnant and lactating women.

The daily value of calcium is:

• for newborns up to 6 months – 400 milligrams;
• for preschool children (1 – 5 years) – 600 milligrams;
• for schoolchildren under 10 years old – 800 milligrams;
• for children from 10 to 13 years old – 1000 milligrams;
• for teenagers and young people under 24 years old – 1300 – 1500 milligrams;
• for women (from 25 to 55 years) and men (from 25 to 65 years) – 1000 milligrams;
• for women during menopause (from 55 to 85 years old) and older men (from 65 to 85 years old) – 1300 – 1500 milligrams;
• for pregnant and lactating women – 1500 – 2000 milligrams.

The need for calcium increases with:

• intense sports activities;
• profuse sweating;
• taking anabolic steroids;
• hormonal therapy.

Remember, it is important to monitor the amount of calcium consumed daily, since a lack of the mineral can lead to osteoporosis of the bones, and an excess can lead to stone formation in the kidneys and bladder.

When and what medications are prescribed to meet calcium needs?

Based on the external signs described above, it cannot be determined that this is a calcium deficiency. You need to see a doctor, he will determine the true cause of the symptoms and determine the indications for taking medications.

In the arsenal of pharmacies there are preparations with calcium in 3 types: pure calcium salts - gluconate, citrate, carbonate, mixtures with vitamin D, food supplements with vitamins and high calcium content.

Today, combination preparations are popular that ensure maximum absorption of the element: Calcium-D3 in the variants Mik, Mik-Forte, Nycomed and Nycomed-Forte. Complex products have also proven themselves well: Kalcemin, Kalcemin-Silver, Kalcemin-Advance, Pharmaton-Kiddy, Osteogenon, Vitrum-Osteomag.

Important: despite the fact that all these calcium preparations can be bought without a prescription, they should not be taken indiscriminately, but only as prescribed by a doctor in a strict dosage. Exceeding it is fraught with the development of complications.

Natural springs

Considering that calcium is involved in the formation of bone, connective and nervous tissues, it is important to ensure a regular supply of the macronutrient with food.
Table No. 1 “Sources of calcium”

Calcium is found in small quantities in cereals, fruits, vegetables, berries, meat and honey. The content of the element in these products varies from 5 to 50 milligrams per 100 grams.

Interpretation of results.

Calcium levels are assessed over time by a doctor in combination with other laboratory parameters and clinical data. Independent, isolated assessment leads to incorrect conclusions.

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What affects calcium absorption

Calcium is a difficult-to-digest macronutrient, since its absorption requires the presence of the following substances in the body: magnesium, phosphorus, potassium, zinc, manganese, silicon, chromium, vitamins D, etc. Moreover, an excess amount of the first two compounds prevents its full absorption.

The optimal ratio of calcium, magnesium and phosphorus in food or dietary supplements is 2: 1: 1. Considering that the mineral “transforms” into a bioavailable form only under the influence of gastric juice, taking it and alkaline substances that neutralize hydrochloric acid, including carbohydrates, leads to to reduce the absorption of the element in the intestines. At the same time, the combined use of the compound with rhubarb, spinach, parsley, cabbage, sorrel, radish and currants potentiates the formation of oxalate kidney stones.

Remember, calcium is well absorbed from dairy products due to the optimal ratio of nutrients and the presence of lactic acid bacteria in such products. Moreover, to increase the bioavailability of the mineral, it is permissible to use healthy fats. However, it is important to take into account that an excess or lack of lipids in the diet prevents the complete absorption of the “bone” substance, since in the first case there are not enough bile acids to break it down, and in the second - fatty acids.

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The optimal ratio of calcium to fat per serving of food is 1:100.

Application

Applications of calcium metal

The main use of calcium metal is as a reducing agent in the production of metals, especially nickel, copper and stainless steel. Calcium and its hydride are also used to produce difficult-to-reduce metals such as chromium, thorium and uranium. Calcium-lead alloys are used in batteries and bearing alloys. Calcium granules are also used to remove traces of air from vacuum devices.

Metallothermy

Pure metallic calcium is widely used in metallothermy for the production of rare metals.

Alloying of alloys

Pure calcium is used to alloy lead used for the production of battery plates and maintenance-free starter lead-acid batteries with low self-discharge. Also, metallic calcium is used for the production of high-quality calcium babbits BKA.

Nuclear fusion

The 48Ca isotope is the most effective and commonly used material for the production of superheavy elements and the discovery of new elements on the periodic table. For example, in the case of using 48Ca ions to produce superheavy elements in accelerators, the nuclei of these elements are formed hundreds and thousands of times more efficiently than when using other “projectiles” (ions).

Application of calcium compounds

Calcium hydride

By heating calcium in a hydrogen atmosphere, CaH2 (calcium hydride) is obtained, which is used in metallurgy (metallothermy) and in the production of hydrogen in the field.

Optical and laser materials

Calcium fluoride (fluorite) is used in the form of single crystals in optics (astronomical objectives, lenses, prisms) and as a laser material. Calcium tungstate (scheelite) in the form of single crystals is used in laser technology and also as a scintillator.

Calcium carbide

Calcium carbide CaC2 is widely used for the production of acetylene and for the reduction of metals, as well as in the production of calcium cyanamide (by heating calcium carbide in nitrogen at 1200, the reaction is exothermic, carried out in cyanamide furnaces).

Chemical current sources

Calcium, as well as its alloys with aluminum and magnesium, are used in backup thermal electric batteries as an anode (for example, calcium-chromate element). Calcium chromate is used in such batteries as a cathode. The peculiarity of such batteries is an extremely long shelf life (decades) in a suitable condition, the ability to operate in any conditions (space, high pressures), and a high specific energy in terms of weight and volume. Disadvantage: short lifespan. Such batteries are used where it is necessary to create colossal electrical power for a short period of time (ballistic missiles, some spacecraft, etc.).

Fireproof materials

Calcium oxide, both in free form and as part of ceramic mixtures, is used in the production of refractory materials.

Medicines

Calcium compounds are widely used as an antihistamine.

Calcium chloride Calcium gluconate Calcium glycerophosphate

In addition, calcium compounds are included in drugs for the prevention of osteoporosis, in vitamin complexes for pregnant women and the elderly.-