Sodium. Properties of sodium

Na 2 O → NaCl → NaOH → Na.

Na 2 O+ 2HCl → 2NaCl + H 2 O.

To obtain sodium hydroxide from the chloride of the same metal, it is necessary to dissolve it in water, however, it should be remembered that hydrolysis does not occur in this case:

NaCl+ H 2 O → NaOH + HCl.

Obtaining sodium from the corresponding hydroxide is possible if the alkali is subjected to electrolysis:

NaOH ↔ Na + + Cl - ;

K(-): Na + + e → Na 0:

A(+): 4OH — — 4e → 2H 2 O + O 2 .

Is sodium a metal or a non-metal? It is a mistake to believe that the second option. Sodium is soft silver-white metal, which is included in the periodic table under atomic number 11.

Moreover, it (or rather its compounds) has been known since ancient times! Even the Bible mentions sodium as an ingredient in cleaning products. However, this historical reference, albeit interesting. Now it’s worth talking about the features of this element and its other characteristics.

Physical properties

So, the answer to the question “Is sodium a metal or a non-metal?” very clear. Even just looking at this substance, you can understand everything. It is obvious that Which, by the way, although it has a silvery-white color, has a violet tint in thin layers.

This is a very plastic substance. Soft metals are those that can be forged without much effort and are also characterized by ductility and fusibility. But in relation to sodium, this word can be applied in the literal sense. It can be cut with a knife without effort. By the way, a fresh cut shines very brightly. Other properties include:

• Density. At normal conditions- 0.971 g/cm³.
• The melting and boiling points are 97.81 °C and 882.95 °C, respectively.
• Molar heat capacity - 28.23 J/(K.mol).
• The specific heat of fusion and evaporation is 2.64 kJ/mol and 97.9 kJ/mol, respectively.
• Molar volume - 23.7 cm³/mol.

It is worth noting that under pressure, sodium (Na) turns red and transparent. In this state, this metal is very similar to ruby.

If you place it at room temperature, it forms crystals in cubic symmetry. However, by lowering it to −268 °C, you can see how the metal transforms into the hexagonal phase. To understand what we are talking about, just remember graphite. This is a prime example of a hexagonal crystal.

Oxidation and combustion

Now we can move on to the chemical properties of sodium (Na). This alkali metal, when exposed to air, easily oxidizes. As a result, sodium oxide (Na 2 O) is formed. It looks like colorless cubic crystals. This is a salt-forming binary inorganic substance, which is used as a reagent in the synthesis process. It is used to make sodium hydroxide and other compounds.

Therefore, to protect the metal from oxygen exposure, it is stored in kerosene.

But during combustion, sodium peroxide (Na 2 O 2) is formed. They look like white-yellow crystals, which are characterized by vigorous interaction with water, accompanied by the release of heat. Na 2 O 2 is used for bleaching silk, wool, fabrics, straw, viscose and wood pulp.

Reactions with water

The silvery-white soft metal sodium also interacts successfully with H2O. The reaction with water is very violent. A small piece of sodium placed in this liquid floats to the surface and begins to melt due to the heat generated. As a result, it turns into a white ball, which moves quickly along the surface of the water in different directions.

This very spectacular reaction is accompanied by the release of hydrogen. When conducting such an experiment, care must be taken as it may ignite. And everything happens according to the following equation: 2Na + 2H 2 O → 2NaOH + H 2.

Interactions with nonmetals

Sodium is a metal, it can also be called a strong reducing agent, which it is. Like other alkaline substances, however. So it reacts vigorously with many nonmetals other than carbon, iodine, and noble gases, which include radioactive radon, krypton, neon, xenon, argon, and helium. Such reactions look like this: 2Na + Cl 2 → 2NaCl. Or here’s another example: 2Na + H 2 → 250-450 °C 2NaH.

It is worth noting that sodium is more active than lithium. In principle, it can react with nitrogen, but very poorly (in a glow discharge). As a result of this interaction, an unstable substance called sodium nitride is formed. These are dark gray crystals that react with water and decompose when heated. They are formed according to the equation: 6Na + N 2 → 2Na 3 N.

Reactions with acids

They should also be listed, talking about chemical characteristics sodium This substance reacts with dilute acids as ordinary metal. It looks like this: 2Na + 2HCl → 2NaCl + H2.

Sodium interacts differently with concentrated substances that are characterized by oxidative reactions; such reactions are accompanied by the release of reduction products. Here is an example of a formula: 8Na + 10NHO 3 → 8NaNO 3 + 3H 2 O.

It is also worth noting that the alkali metal sodium easily dissolves in liquid ammonia (NH 3), a 10% solution of which is well known to everyone as ammonia. The equation looks like this: Na + 4NH3 → - 40°C Na 4. As a result of this reaction, a blue solution is formed.

The metal also interacts with gaseous ammonia, but when heated. This reaction looks like this: 2Na + 2NH3 → 35 0°C 2NaNH 2 + H 2.

Other connections

When listing the main properties of sodium, it is also worth mentioning that it can interact with mercury, a unique element that under normal conditions is a white-silver heavy liquid, while being a metal.

As a result of this reaction, an alloy is formed. Its exact name is sodium amalgam. This substance is used as a reducing agent, its properties being softer than pure metal. If you heat it with potassium, you get a liquid alloy.

This metal can also dissolve in so-called crown ethers - macroheterocyclic compounds, but only in the presence of organic solvents. As a result of this reaction, an alkalide (a salt, a strong reducing agent) or an electride (a blue solvent) is formed.

It is also impossible not to mention that alkyl halides, which are halogen-carbon substances, with an excess of sodium give organosodium compounds. In air they usually ignite spontaneously. And in water they explode.

Application

The properties and characteristics of sodium allow it to be widely used in industry, metallurgy and preparative chemistry as a powerful reducing agent. In addition, this substance is involved:

• In the drying of organic solvents.
• In the production of sulfur-sodium batteries.
• In exhaust valves of truck engines. Plays the role of a liquid heat sink.
• During production electrical wires, which are designed for high currents.
• In alloys with cesium, rubidium and potassium. Together with these substances, sodium forms a highly efficient coolant, which, by the way, is used with fast neutrons in nuclear reactors.
• In gas discharge lamps.

And these are just some of the areas of its application. But the most common substance in the world is sodium chloride. It is found in almost every home, because it is table salt.

It is also impossible not to mention that the earth’s crust consists of 2.6% sodium. And in general, it is in 7th place in the ranking of the most common elements in nature and in 5th place in the list of the most common metals. It is impossible to find sodium in nature in its pure form, since it is chemically active, but it is found in huge quantities in the form of sulfate, carbonate, nitrate and chloride.

Biological role

So, all the basics on the topic “Is sodium a metal or a non-metal?” it was said. Finally, a few words about biological role of this substance.

Sodium is an integral part of any living organism. Human is no exception. Here are his roles:

• Maintains osmotic pressure.
• Transports carbon dioxide.
• Normalizes water balance.
• Promotes the transport of glucose, amino acids, anions through cell membranes.
• Its exchange with potassium ions influences the formation of the action potential.
• Positively affects protein metabolism.
• Takes part in the hydration process.

Sodium is included in almost all products. But its main sources are salt and baking soda. Vitamin D improves the absorption of this substance.

Sodium deficiency does not occur, but problems associated with consuming insufficient amounts can occur during fasting. This is fraught with weight loss, vomiting, impaired absorption of monosaccharides, and the formation of gastrointestinal tract gases In particular severe cases Neuralgia and convulsions occur. Therefore, it is better not to subject your body to severe starvation.

Sodium —element main subgroup of the first group, third period periodic table chemical elements of D.I. Mendeleev, with atomic number 11. Denoted by the symbol Na (lat. Natrium). The simple substance sodium (CAS number: 7440-23-5) is a soft alkali metal, silvery white.

In water, sodium behaves almost the same as lithium: the reaction proceeds with the rapid release of hydrogen, and sodium hydroxide is formed in the solution.

History and origin of the name

Sodium (or rather, its compounds) has been used since ancient times. For example, soda (natron), found naturally in the waters of soda lakes in Egypt. The ancient Egyptians used natural soda for embalming, bleaching canvas, cooking food, and making paints and glazes. Pliny the Elder writes that in the Nile Delta soda (it contained a sufficient proportion of impurities) was isolated from river water. It went on sale in the form of large pieces, colored gray or even black due to the admixture of coal.

Sodium was first obtained by the English chemist Humphry Davy in 1807 by electrolysis of solid NaOH.

The name "sodium" comes from the Arabic natrun in Greek - nitron and originally it referred to natural soda. The element itself was previously called Sodium.

Receipt

The first way to produce sodium was the reduction reaction sodium carbonate coal when heating a close mixture of these substances in iron container up to 1000°C:

Na 2 CO 3 +2C=2Na+3CO

Then another method of producing sodium appeared - electrolysis of molten sodium hydroxide or sodium chloride.

Physical properties

Metallic sodium stored in kerosene

Qualitative determination of sodium using a flame - bright yellow color of the emission spectrum of the “sodium D-line”, doublet 588.9950 and 589.5924 nm.

Sodium is a silvery-white metal, in thin layers with purple tint, plastic, even soft (easily cut with a knife), a fresh cut of sodium shines. The electrical and thermal conductivity values ​​of sodium are quite high, the density is 0.96842 g/cm³ (at 19.7° C), the melting point is 97.86° C, and the boiling point is 883.15° C.

Chemical properties

An alkali metal that oxidizes easily in air. To protect against atmospheric oxygen, metallic sodium is stored under a layer kerosene. Sodium is less active than lithium, therefore with nitrogen reacts only when heated:

2Na + 3N 2 = 2NaN 3

When there is a large excess of oxygen, sodium peroxide is formed

2Na + O 2 = Na 2 O 2

Application

Sodium metal is widely used in preparative chemistry and industry as a strong reducing agent, including in metallurgy. Sodium is used in the production of highly energy-intensive sodium-sulfur batteries. It is also used in truck exhaust valves as a heat sink. Occasionally, sodium metal is used as a material for electrical wires intended to carry very high currents.

In an alloy with potassium, as well as with rubidium and cesium used as a highly efficient coolant. In particular, the alloy composition is sodium 12%, potassium 47 %, cesium 41% has a record low melting point of −78 °C and has been proposed as a working fluid for ion rocket engines and a coolant for nuclear power plants.

Sodium is also used in high- and high-gas discharge lamps. low pressure(NLVD and NLND). Lamps NLVD type DNaT (Arc Sodium Tubular) are very widely used in street lighting. They give off a bright yellow light. The service life of HPS lamps is 12-24 thousand hours. Therefore, gas-discharge lamps of the HPS type are indispensable for urban, architectural and industrial lighting. There are also lamps DNaS, DNaMT (Arc Sodium Matte), DNaZ (Arc Sodium Mirror) and DNaTBR (Arc Sodium Tubular Without Mercury).

Sodium metal is used in qualitative analysis organic matter. The alloy of sodium and the test substance is neutralized ethanol, add a few milliliters of distilled water and divide into 3 parts, J. Lassaigne's test (1843), aimed at determining nitrogen, sulfur and halogens (Beilstein test)

— Sodium chloride (table salt) is the oldest used flavoring and preservative.
— Sodium azide (Na 3 N) is used as a nitriding agent in metallurgy and in the production of lead azide.
— Sodium cyanide (NaCN) is used in the hydrometallurgical method of leaching gold from rocks, as well as in the nitrocarburization of steel and in electroplating (silvering, gilding).
— Sodium chlorate (NaClO 3) is used to destroy unwanted vegetation on railway tracks.

Biological role

Sodium is found in the body for the most part outside the cells (about 15 times more than in the cytoplasm). This difference is maintained by the sodium-potassium pump, which pumps out sodium trapped inside the cell.

Together withpotassiumsodium performs the following functions:
Creating conditions for the occurrence of membrane potential and muscle contractions.
Maintaining blood osmotic concentration.
Maintaining acid-base balance.
Normalization water balance.
Ensuring membrane transport.
Activation of many enzymes.

Sodium is found in almost all foods, although the body gets most of it from table salt. Absorption mainly occurs in the stomach and small intestine. Vitamin D improves the absorption of sodium, however, excessively salty foods and foods rich in protein interfere with normal absorption. The amount of sodium taken in from food shows the sodium content in the urine. Sodium-rich foods are characterized by accelerated excretion.

Sodium deficiency in the dieter balanced food does not occur in humans, however, some problems can arise with vegetarian diets. Temporary deficiency may be caused by diuretic use, diarrhea, excessive sweating, or excess water intake. Symptoms of sodium deficiency include weight loss, vomiting, gas in the gastrointestinal tract, and impaired absorption amino acids and monosaccharides. Long-term deficiency causes muscle cramps and neuralgia.

Excess sodium causes swelling of the legs and face, as well as increased excretion of potassium in the urine. Maximum amount salt that can be processed by the kidneys is approximately 20-30 grams, large quantity already life-threatening.

Sodium compounds

Sodium, Natrium, Na (11)
The name sodium - sodium, natrium comes from an ancient word common in Egypt, among the ancient Greeks (vixpov) and Romans. It is found in Pliny (Nitron) and other ancient authors and corresponds to the Hebrew neter. IN ancient Egypt natron, or nitron, was generally called an alkali obtained not only from natural soda lakes, but also from plant ash. It was used for washing, making glazes, and mummifying corpses. In the Middle Ages, the name nitron (nitron, natron, nataron), as well as boron (baurach), also applied to saltpeter (Nitrum). Arab alchemists called alkali alkali. With the discovery of gunpowder in Europe, saltpeter (Sal Petrae) began to be strictly distinguished from alkalis, and in the 17th century. already distinguished between non-volatile, or fixed alkalis, and volatile alkali (Alkali volatile). At the same time, a difference was established between vegetable (Alkali fixum vegetabile - potash) and mineral alkali (Alkali fixum minerale - soda).

IN late XVIII V. Klaproth introduced the name Natron, or soda, for the mineral alkali, and for the vegetable alkali, Kali. Lavoisier did not place alkalis in the “Table of Simple Bodies,” indicating in a note to it that these were probably complex substances that once Someday they will be decomposed. Indeed, in 1807 Davy, by electrolysis of slightly moistened solid alkalis, obtained free metals - potassium and sodium, calling them potassium and sodium. The following year, Gilbert, publisher of the famous Annals of Physics, proposed calling the new metals potassium and sodium (Natronium); Berzelius shortened the latter name to “sodium” (Natrium). IN early XIX V. in Russia sodium was called sodia (Dvigubsky, 182i; Solovyov, 1824); Strakhov proposed the name sod (1825). Sodium salts were called, for example, soda sulfate, hydrochloric soda, and at the same time acetic soda (Dvigubsky, 1828). Hess, following the example of Berzelius, introduced the name sodium.

Early 19th century sodium called sodium. This name was given to the element by Humphry Davy, who managed to isolate the metal from alkali. The chemist slightly moistened it and subjected it to electrolysis. Wilhelm Hilbert suggested changing the name of the element discovered by Humphrey.

This is the author of the famous “Annals of Physics”. The scientist began to call sodium sodium. The work was continued by Jens Berzelius. A chemist from Sweden introduced the abbreviation sodium. Our next material is about the properties and role of this metal in people’s lives.

Chemical and physical properties sodium

The element is included in the main subgroup of the 1st group, occupying the 11th position. All metals in the column are alkaline, so sodium. Water reacts with him. A caustic alkali is formed. Another one general feature group metals - the presence of only 1 electron in the outer orbit of the atom.

This makes sodium a powerful reducing agent. An element readily donates an outer-level electron, increasing its oxidation state. The atom comes to the completed shell of the previous level.

Reducing activity is the reason for the absence of pure metal in nature. You can only find connections. So, sodium chloride- This is table salt. Sodium carbonate- baking soda. So, it was not for nothing that the metal was originally called sodium.

It could also be called neter. It is under this name that the substance appears in Old Testament. As for, people began to use it back in Paleolithic times, that is, about 6,000 years ago.

Most energetic sodium interacts not only with water, but also with all non-metals. To obtain a delicate one from an active reducing agent, the 11th element is combined with. An amalgam is formed.

If, on the contrary, it is necessary to increase the aggression of sodium, oxygen is added to it. The result is peroxide, a powerful oxidizing agent. In its atmosphere, most substances ignite.

Difficulty and “character” sodium hydroxide. It is called caustic. The compound corrodes fabrics, skin, and other organics and materials made on its basis. True, in the air sodium hydroxide captures carbon dioxide and is neutralized, turning into carbonate.

When Humphry Davy managed to isolate pure sodium, the world learned what he was like externally. The metal is silvery white. Thin sections have a purple tint. Sodium formula makes it soft and pliable.

It can be cut with a regular knife and shines on the sliding surface of the blade. The element has a low melting point - 97 degrees. Sodium boils at 883 on the Celsius scale.

Pure metal conducts current and heat well, does not differ high density. Its indicator for the 11th element is less than one. This does not discount the weight of sodium in biological processes.

Metal is found in both plants and animal tissues. Yes, in the human body sodium solution– part of blood plasma, digestive and lymph.

Osmotic pressure, for example, is maintained precisely by the 11th element. It was used not only by nature, but also by man. Mass of sodium goes, for example, for industrial purposes. Which? We'll talk about this in the next chapter.

Applications of sodium

In nature, the element is represented by only one stable isotope. Its mass number is 23. Another 15 isotopes have been created under artificial conditions. They are not stable, most are destroyed in a couple of minutes. Exception: - 22nd and 24th Na.

The half-lives of these isotopes are significant. The first one lasts for 2.5 years, actively emits positrons, which serves science. The half-life of the second is 15 hours. Enough to serve medicine and help leukemia patients.

In the field of nuclear energy, sodium has become a coolant. The “run-up” between the melting and boiling points of the element was useful. An interval of 800 degrees Celsius allows, for example, to fill the energy circuits of nuclear submarines with alkali metal. Sodium takes heat from the reactor without boiling.

It is possible to keep the temperature within reasonable limits due to the circulation of liquid metal between the reactor and the steam generator. In the latter happens sodium cooling, water evaporates. So it turns out to rotate the turbine with the energy of high-pressure steam.

The pure element is also useful in metallurgy. What role does it play in it? sodium? Instructions The application is as follows: the metal strengthens lead-based alloys. About 1.5% of the 11th element is sufficient. Sodium is also added to alloys of other metals. It is no longer strength that is achieved, but the refractoriness of the mixtures.

Wires are worth mentioning among the products. Buy sodium for their manufacture is more profitable than the usual one. The 11th element conducts electricity 3 times worse. But alkali metal is 9 times lighter.

This argument forced industrialists to switch to sodium buses for high currents. Thin wires continued to be made from the usual copper and.

Now, about the role sodium compounds. Peroxide not only ignites substances, but can also bleach fabrics. The 11th metal hydroxide is needed by oil workers. The compound purifies liquid processing products. Hydroxide is also purchased for the production of hard grades detergents. Without a caustic substance it is impossible to saponify the fats in them.

In parallel, the odorless white powder is also used in the production of textiles. Here the bet is on sodium chloride solution. The product can lighten both writing sheets and fabrics. The reagent is popularly called bleach.

Sodium tetraborate has become a cure for candidiasis and other vaginal infections. Sulfacyp sodium– a drug that helps with conjunctivitis and others inflammatory process in the eyes. An antidote for salt poisoning and general intoxication of the body is sodium thiosulfate.

The food is popularly known as a remedy for heartburn. Sodium bicarbonate– an alkali that neutralizes stomach acid. The 11th element is also used for constipation. Helps out sodium sulfate.

In addition to the medical field itself, the element is also valued in cosmetology. Sodium acid- nothing more than hyaluronic acid. It maintains youthful skin. Injections are usually given into nasolabial folds and wrinkles. Acid fills them. In youth, hyaluronate is produced by the body, but with age the process slows down. You have to administer the drug from outside.

Pictured are foods containing sodium

Humanity was the first to appreciate sodium salts. But, in the 21st century, they learned the charm of the cyanide form of the metal. She helps mine. The jewel is melted in sodium cyanide. True, some other composite ores also pass into liquid form.

However, it is already easier to isolate gold from a complex melt than from solid masses. At the final stage they “connect” and... the precious metal is mined.

Sodium extraction

If a pure element is needed, it is extracted from ordinary table salt. Its deposits are found on all continents. If there are not enough resources, the waters of the seas are a storehouse of salt. Select from sodium chloride succeeds by melting it and subsequent electrolysis. Cathodes are made of iron or copper. Anodes are purchased from.

Sodium fluoride and potassium chloride are added to the salt. They reduce the softening temperature of raw materials from 800 to 500 degrees Celsius. This reduces sodium loss through evaporation. The method is doubly beneficial, because simultaneously with the 11th element, pure chlorine is also extracted.

Sodium price

The cost of the item depends on what is purchased sodium hydroxide solution, pure metal, its sulfate or other compound. The price tag also depends on whether it is purchased, for example, as part of a drug, or separately. There are many areas of use of sodium, hundreds and thousands of manufacturers.

Everyone has their own needs. Some substances are easily obtained practically in finished form, the same salt. It costs about 10-20 rubles per kilogram. Other sodium compounds must be synthesized, which increases their cost.

One way or another, humanity is ready to pay for the benefits brought to it by the 11th element. Its mining is active and, apparently, is not going to subside.

Sodium

SODIUM-I; m. Chemical element (Na), a soft, silvery-white metal that oxidizes quickly in air.

◁ Sodium, oh, oh. N-th connections. Nth saltpeter.

(lat. Natrium), chemical element Group I of the periodic table; refers to alkali metals. The name (from the Arabic natrun) originally referred to natural soda. Silver-white metal, soft, light (density 0.968 g/cm3), fusible ( t mp 97.86°C). In air it oxidizes quickly. Interaction with water may result in an explosion. Ranks 6th in prevalence in earth's crust(minerals halite, mirabilite, etc.) and 1st among metallic elements in the World Ocean. They are used to produce pure metals (K, Zr, Ta, etc.), as a coolant in nuclear reactors (an alloy with potassium) and as a source of luminescence in sodium lamps. Sodium is involved in mineral metabolism all living organisms.

SODIUM (Latin Natrium, from Arabic natrun, Greek nitron - natural soda), Na (read “sodium”), a chemical element with atomic number 11, atomic mass 22.98977. One stable isotope, 23 Na, occurs in nature. Belongs to the alkali metals. Located in the third period in group IA in the periodic table of elements. Outer electron layer 3 configuration s 1 . Oxidation state +1 (valency I).
The radius of the atom is 0.192 nm, the radius of the Na + ion is 0.116 nm (coordination number 6). The sequential ionization energies are 5.139 and 47.304 eV. Electronegativity according to Pauling (cm. PAULING Linus) 1,00.
Historical reference
Salt(sodium chloride NaCl), caustic alkali (sodium hydroxide NaOH) and soda (sodium carbonate Na 2 CO 3) were used back in Ancient Greece.
Na metal was first obtained in 1807 by G. Davy (cm. DAVY Humphrey) using electrolysis of molten caustic soda.
Being in nature
Content in the earth's crust is 2.64% by weight. Main minerals: halite (cm. HALITE) NaCl, mirabilite (cm. MIRABILIT) Na 2 SO 4 10H 2 O, thenardite (cm. THENARDITIS) Na 2 SO 4, Chilean saltpeter NaNO 3 , throne (cm. TRON) NaHCO 3 Na 2 CO 3 2H 2 O, borax (cm. BORA) Na 2 B 4 O 7 10H 2 O and natural silicates, for example, nepheline (cm. NEPHELIN) Na.
The water of the World Ocean contains 1.5 10 16 tons of sodium salts.
Receipt
Na is obtained by electrolysis of molten sodium chloride NaCl, with the addition of NaCl 2, KCl and NaF to reduce the melting point of the electrolyte to 600°C. Anodes are made of graphite, cathodes are made of copper or iron. Electrolysis of the melt is carried out in a steel electrolyzer with a diaphragm. In parallel with Na electrolysis, Cl 2 is obtained:
2NaCl=2Na+Cl2
The resulting Na is purified by vacuum distillation or treatment with titanium or a titanium-zirconium alloy.
Physical and chemical properties
Sodium is a soft, silvery-white metal that quickly tarnishes when exposed to air.
Na is soft, easy to cut with a knife, and can be pressed and rolled. Above -222°C the cubic modification is stable, A= 0.4291 nm. Below is the hexagonal modification. Density 0.96842 kg/dm3. Melting point 97.86°C, boiling point 883.15°C. Sodium vapor consists of Na and Na 2 .
Na is chemically very active. At room temperature it interacts with O 2 air, water vapor and CO 2 with the formation of a loose crust. When Na burns in oxygen, Na 2 O 2 peroxide and Na 2 O oxide are formed:
4Na+O 2 =2Na 2 O and 2Na+O 2 =Na 2 O 2
When heated in air, Na burns with a yellow flame, yellow Many sodium salts also color flames. Sodium reacts violently with water and dilute acids:
2Na+H 2 O=2NaOH+H 2
When Na and alcohol interact, H2 is released and sodium alkoxide is formed. For example, interacting with ethanol C 2 H 5 OH, Na forms sodium ethanolate C 2 H 5 OHa:
C 2 H 5 OH + 2Na = 2 C 2 H 5 ONa + H 2
Oxygen-containing acids, interacting with Na, are reduced:
2Na+2H 2 SO 4 =SO 2 +Na 2 SO 4 +2H 2 O
When heated to 200°C, Na reacts with H2 to form NaH hydride:
2Na+H 2 =2NaH
Sodium spontaneously ignites in a fluorine atmosphere (cm. FLUORINE) or chlorine (cm. CHLORINE), with iodine (cm. IOD) reacts when heated. When ground in a mortar, Na reacts with S to form sulfides of variable composition. With N 2 the reaction occurs in an electric discharge, sodium nitride Na 3 N or azide NaN 3 are formed. Na reacts with liquid ammonia to form blue solutions, where Na is present as Na+ ions.
Sodium oxide Na 2 O exhibits pronounced basic properties, easily reacts with water to form a strong base - sodium hydroxide NaOH:
Na 2 O+H 2 O=2NaOH
Sodium peroxide Na 2 O 2 reacts with water to release oxygen:
2Na 2 O 2 +2H 2 O=4NaOH+O 2
Sodium hydroxide is a very strong base, an alkali, ( cm. ALKALI) are highly soluble in water (108 g of NaOH dissolves in 100 g of water at 20 °C). NaOH interacts with acidic and amphoteric (cm. AMPHOTERIC) oxides:
CO 2 +2NaOH=Na 2 CO 3 +H 2 O,
Al 2 O 3 +2NaOH+3H 2 O=2Na (in solution),
Al 2 O 3 +2NaOH=2NaAlO 2 +H 2 O (when fused)
In industry, sodium hydroxide NaOH is produced by electrolysis of aqueous solutions of NaCl or Na 2 CO 3 using ion exchange membranes and diaphragms:
2NaCl+2H 2 O=2NaOH+Cl 2 +H 2
Contact of solid NaOH or drops of its solution on the skin causes severe burns. Aqueous solutions of NaOH during storage destroy glass, and melts destroy porcelain.
Sodium carbonate Na 2 CO 3 is obtained by saturation aqueous solution NaCl with ammonia and CO 2. The solubility of the resulting sodium bicarbonate NaHCO 3 is less than 10 g in 100 g of water at 20°C, the main part of NaHCO 3 precipitates:
NaCl+NH 3 +CO 2 =NaHCO 3,
which is separated by filtration. When NaHCO 3 is calcined, soda ash is formed:
2NaHCO 3 =Na 2 CO 3 +CO 2 +H 2 O
For most Na salts, the solubility does not increase as much with increasing temperature; for potassium salts (cm. POTASSIUM).
Na is a strong reducing agent:
TiCl 4 +4Na=4NaCl+Ti
Application
Sodium is used as a reducing agent for active metals; its melt mixed with potassium is a coolant in nuclear reactors, since it does not absorb neutrons well. Na vapor is used in incandescent lamps.
NaCl is used in Food Industry, sodium hydroxide NaOH - in the production of paper, soap, artificial fibers, as an electrolyte. Sodium carbonate Na 2 CO 3 and bicarbonate NaHCO 3 - used in the food industry, is a component fire extinguishing agents, medicine. Sodium phosphate Na 3 PO 4 is a component of detergents, used in the production of glass and paints, in the food industry, and in photography. Silicates m Na 2 O n SiO 2 - charge components in glass production, for the production of aluminosilicate catalysts, heat-resistant, acid-resistant concrete.
Physiological role
Sodium ions Na + are necessary for the normal functioning of the body; they are involved in metabolic processes. In human blood plasma the content of Na + ions is 0.32% by weight, in bones - 0.6%, in muscle tissue - 1.5%. To replenish natural loss, a person must consume 4-5 g of Na with food daily.
Features of handling sodium metal
Store sodium in hermetically sealed iron containers under a layer of dehydrated kerosene or mineral oil. The ignited Na is poured with mineral oil or covered with a mixture of talc and NaCl. The resulting Na metal waste is destroyed in containers with ethyl or propyl alcohol.

encyclopedic Dictionary. 2009 .

See what “sodium” is in other dictionaries:

SODIUM- SODIUM. Natrium, chemical element, symbol Na, a silvery-white, shiny, monatomic metal with a waxy density at ordinary temperatures, becoming brittle in the cold and distilling in bright red-hot heat; discovered by De.wi (1807) by electrolysis... ... Big medical encyclopedia

- (Greek nitron, Latin natrum). White metal that forms part of table salt, soda, saltpeter, etc. Dictionary foreign words, included in the Russian language. Chudinov A.N., 1910. SODIUM is a white shiny soft metal that quickly oxidizes into... ... Dictionary of foreign words of the Russian language

Sodium breakdown diagram 22 ... Wikipedia

- (Natrium), Na, chemical element of group I of the periodic table, atomic number 11, atomic mass 22.98977; soft alkali metal, melting point 97.86°C. Sodium and its alloys with potassium are coolants in nuclear reactors. Sodium component of alloys for... ... Modern encyclopedia

- (symbol Na), a common silvery-white metallic element, one of the ALKALI METALS, first isolated by Humphry Davy (1807). It is found in salts in sea ​​water and in many minerals. Its main source is CHLORIDE... ... Scientific and technical encyclopedic Dictionary

Sodium- (Natrium), Na, chemical element of group I of the periodic table, atomic number 11, atomic mass 22.98977; soft alkali metal, melting point 97.86°C. Sodium and its alloys with potassium are coolants in nuclear reactors. Sodium is a component of alloys for... ... Illustrated Encyclopedic Dictionary

- (lat. Natrium) Na, chemical element of group I of the periodic system of Mendeleev, atomic number 11, atomic mass 22.98977; refers to alkali metals. The name (from Arabic natrun) originally referred to natural soda. Silvery white... ... Big Encyclopedic Dictionary

Na (Latin Natrium, from Arabic natrun, Greek nitron, originally natural soda * a. sodium, natrium; n. Natrium; f. sodium; i. sodio), chemical. element of group I periodic. Mendeleev's system; at.s. 11, at. m. 22.98977; belongs to alkaline... ... Geological encyclopedia

Na is a chemical element of group I of the periodic system, atomic number 11, atomic mass 22.99; alkali metal; Due to its high thermal conductivity and relatively small cross section for capturing slow neutrons, metallic sodium (sometimes alloyed with... ... Nuclear energy terms

SODIUM- chem. element, symbol Na (lat. Natrium), at. n. 11, at. m. 22.98; belongs to alkali metals, silvery-white color, density 968 kg/m3, t = 97.83°C, very soft, has high thermal and electrical conductivity. N. easily interacts with... ... Big Polytechnic Encyclopedia

SODIUM, sodium, pl. no, husband (lat. natrium) (chemical). A soft and white lightweight alkali metal. Table salt is a chemical compound of chlorine and sodium. Dictionary Ushakova. D.N. Ushakov. 1935 1940 ... Ushakov's Explanatory Dictionary

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