What is bromine? Chemical element bromine: formula, properties. Chemical and physical properties of bromine

DEFINITION

Bromine is the thirty-fifth element of the Periodic Table. Designation - Br from the Latin "bromum". Located in the fourth period, VIIA group. Refers to non-metals. The core charge is 35.

Like chlorine, bromine is found in nature mainly in the form of salts of potassium, sodium and magnesium. Metal bromides are found in sea ​​water, in some lakes and underground brines.

Under normal conditions, bromine is a red-brown liquid (Fig. 1), slightly soluble in water. When an aqueous solution of bromine is cooled, crystalline hydrates of the clarate type Br 2 × 8H 2 O are released. Let's dissolve well in organic solvents (alcohol, benzene, ether, carbon disulfide, etc.).

Rice. 1. Bromine. Appearance.

Atomic and molecular weight of bromine

DEFINITION

Relative atomic mass of an element called the ratio of the mass of an atom of a given element to 1/12 of the mass of a carbon atom.

The relative atomic mass is dimensionless and is denoted by A r (subscript "r" is the initial letter English word relative, which in translation means "relative"). The relative atomic mass of atomic bromine is 79.901 amu.

The masses of molecules, just like the masses of atoms, are expressed in atomic mass units.

DEFINITION

Relative molecular weight substances call the ratio of the mass of a molecule of a given substance to 1/12 of the mass of a carbon atom, the mass of which is 12 a.m.u.

The molecular weight of a substance is the mass of a molecule, expressed in atomic mass units. It is known that the bromine molecule is diatomic - Br 2 . The relative molecular weight of a hydrogen molecule will be equal to:

M r (Br 2) = 79.901 × 2 ≈160.

Isotopes of bromine

It is known that in nature bromine can be in the form of two stable isotopes 79 Br (50.56%) and 81 Br (49.44%). Their mass numbers are 79 and 81, respectively. The nucleus of the bromine isotope 79 Br contains thirty-five protons and forty-four neutrons, and the isotope 81 Br contains the same number of protons and forty-six neutrons.

There are artificial unstable isotopes of bromine with mass numbers from 67 to 97, as well as fourteen isomeric states of nuclei, among which the 82 Br isotope with a half-life of 35.282 hours is the longest-lived.

Bromine ions

On the outer energy level of the bromine atom, there are eight electrons that are valence:

1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 5 .

As a result of chemical interaction, bromine either gives up its valence electrons, i.e. is their donor, and turns into a positively charged ion, or accepts electrons from another atom, i.e. is their acceptor and turns into a negatively charged ion:

Br 0 +1e → Br 1- ;

Br 0 -1e → Br 1+;

Br 0 -3e → Br 3+;

Br 0 -5e → Br 5+;

Br 0 -7e → Br 7+.

Molecule and atom of bromine

The bromine molecule consists of two atoms - Br 2 . Here are some properties that characterize the atom and molecule of bromine:

Examples of problem solving

EXAMPLE 1

Bromine- element of the 17th group periodic table chemical elements (according to the outdated classification - an element of the main subgroup of group VII), of the fourth period, with atomic number 35. It is designated by the symbol Br (lat. Bromum). Reactive non-metal, belongs to the group of halogens. The simple substance bromine (CAS number: 7726-95-6) under normal conditions is a heavy, caustic red-brown liquid with a strong bad smell. The bromine molecule is diatomic (formula Br2).

Receipt

• Bromine is obtained chemically from brine brine:

Physical Properties

• Under normal conditions, bromine is a red-brown liquid with a sharp unpleasant odor, poisonous, and burns on contact with the skin. Bromine is one of only two simple substances (and the only non-metal), along with mercury, that is liquid at room temperature. Density at 0 °C - 3.19 g/cm³. The melting point of bromine is -7.2 ° C, the boiling point is 58.8 ° C, when boiling, bromine turns from a liquid into a brown-brown vapor, irritating the respiratory tract when inhaled. The standard electrode potential Br2/Br− in aqueous solution is +1.065 V.
• Natural bromine consists of two stable isotopes 79Br (50.56%) and 81Br (49.44%). Numerous radioactive isotopes of bromine have been artificially obtained.

Chemical properties

• It exists in free form in the form of diatomic Br2 molecules. A noticeable dissociation of molecules into atoms is observed at a temperature of 800 °C and rapidly increases with a further increase in temperature. The diameter of the Br2 molecule is 0.323 nm, the internuclear distance in this molecule is 0.228 nm.
• Bromine is slightly, but better than other halogens, soluble in water (3.58 g in 100 g of water at 20 ° C), the solution is called bromine water.
• With most organic solvents, bromine is miscible in all respects, and bromination of organic solvent molecules often occurs.
• Bromine is intermediate in chemical activity between chlorine and iodine. When bromine reacts with iodide solutions, free iodine is released. On the contrary, under the action of chlorine on bromides located in aqueous solutions, free bromine is released.
• The reaction of bromine with sulfur produces S2Br2, the reaction of bromine with phosphorus produces PBr3 and PBr5. Bromine also reacts with non-metals selenium and tellurium.
• The reaction of bromine with hydrogen proceeds when heated and leads to the formation of hydrogen bromide HBr. A solution of HBr in water is hydrobromic acid, close in strength to hydrochloric acid HCl.
• Bromine does not directly react with oxygen and nitrogen. Bromine forms big number various compounds with other halogens. For example, bromine forms unstable BrF3 and BrF5 with fluorine, and IBr with iodine. When interacting with many metals, bromine forms bromides, for example, AlBr3, CuBr2, MgBr2, etc. Tantalum and platinum are resistant to the action of bromine, and to a lesser extent silver, titanium and lead.
• Liquid bromine readily reacts with gold to form gold tribromide AuBr3.

In addition to the oxygen-free hydrobromic acid HBr, bromine forms a number of oxygen acids: bromine HBrO4, bromic HBrO3, bromine HBrO2, bromine HBrO.

Application

• In chemistry. Bromine-based substances are widely used in basic organic synthesis.
• "Bromine water" (an aqueous solution of bromine) is used as a reagent for the qualitative determination of unsaturated organic compounds.
• In engineering. Silver bromide AgBr is used in photography as a photosensitive substance.
• It is used to create flame retardants - additives that give fire resistance to plastics, wood, textile materials.
• Bromine pentafluoride is sometimes used as a very powerful propellant oxidizer.
• 1,2-dibromoethane is currently used as an antiknock additive in motor fuel, instead of tetraethyl lead.
• Bromide solutions are used in oil production.
• Solutions of heavy metal bromides are used as "heavy liquids" in the enrichment of minerals by the flotation method.
• Many organobromine compounds are used as insecticides and pesticides.
• In medicine. In medicine, sodium bromide and potassium bromide are used as sedatives.
• In the production of weapons. Since World War I, bromine has been used to manufacture chemical warfare agents.

Atom properties
Name, symbol, number	Bromine / Bromum (Br), 35
Atomic mass (molar mass)	a. e.m. (g/mol)
Electronic configuration	3d 10 4s 2 4p 5
Chemical properties
covalent radius	114 pm
Ion radius	(+5e)47 (-1e)196 pm
Electronegativity	2.96 (Pauling scale)
Electrode potential	0
Oxidation states	7, 5, 3, 1, 0, -1
Ionization energy (first electron)	1142.0 (11.84) kJ/mol (eV)
Thermodynamic properties a simple substance
Density (at n.a.)	3.102 (25 °C) g/cm³
Melting temperature	265.9K (-7.25°C)
Boiling temperature	331.9K
Melting heat	(Br-Br) 10.57 kJ/mol
Heat of evaporation	(Br-Br) 29.56 kJ/mol
Molar heat capacity	75.69 J/(K mol)
Molar volume	23.5 cm³/mol
Crystal cell a simple substance
Lattice structure	orthorhombic
Lattice parameters	a=6.67 b=4.48 c=8.72 Å
Other characteristics
Thermal conductivity	(300 K) 0.005 W/(m K)

The discovery of bromine took place in the first third of the 19th century, independently of each other, the German chemist Karl Jacob Loewich in 1825, and the Frenchman Antoine Jerome Balard - in 1826 introduced the world to a new chemical element. Interesting fact- originally Balar named his element murid(from Latin Muria- brine), because he made his discovery while studying the Mediterranean salt mines.

Bromine (from the ancient Greek βρῶμος, literally translated “stinky”, “stench”, “stinker”) is an element of the main subgroup of group VII of the fourth period of the periodic system of chemical elements of D.I. Mendeleev (in the new classification - an element of the 17th group). Bromine is a halogen, a reactive non-metal, with an atomic number of 35 and a molecular weight of 79.904. The symbol is used to designate Br(from Latin Bromum).

Finding bromine in nature

Bromine is a widespread chemical element external environment found almost everywhere. Especially a lot of bromine is found in salt water - seas and lakes, where it is available in the form of potassium bromide, sodium bromide and magnesium bromide. The largest number bromine is formed by the evaporation of sea water, it is also found in some rocks and also in plants.

In the human body are up to 300 mg of bromine, mainly in thyroid gland, also bromine contains blood, kidneys and pituitary gland, muscles and bone tissue.

Physical and chemical properties of bromine

Bromine is usually a caustic heavy liquid, has a red-brown color and a sharp, very unpleasant (fetid) odor. It is the only non-metal that is in a liquid state at room temperature.

Bromine (as well as - bromine vapor) - toxic and poisonous substance, when working with it, it is necessary to use chemical protection means, because bromine forms burns when it comes into contact with the skin and mucous membranes of a person.

The composition of natural bromine is two stable isotopes (79 Br and 81 Br), the bromine molecule consists of two atoms and has the chemical formula Br 2.

Daily requirement of the body for bromine

Need healthy body in bromine - no more than 0.8-1 g.

Along with what is available in the body, a person receives bromine from food products. The main suppliers of bromine are nuts ( , ), legumes ( , and ), and pasta from, dairy products, algae and almost all types of marine fish.

The danger and harm of bromine

Elemental bromine is a potent poison; it is strictly forbidden to take it orally. Bromine vapors can cause pulmonary edema, especially in those who are prone to allergic reactions or has lung disease and respiratory tract(bromine vapors are very dangerous for asthmatics).

Signs of excess bromine

An excess of this substance usually occurs when an overdose of bromine preparations is categorically undesirable for people, because it can pose a real health hazard. The main signs of an excess of bromine in the body are inflammation and rashes on the skin, malfunctions digestive system, general lethargy and depression, persistent bronchitis and rhinitis, not associated with colds and viruses.

Bromine deficiency symptoms

The lack of bromine in the body is manifested by insomnia, growth retardation in children and adolescents, a decrease in the level of hemoglobin in the blood, but these symptoms are not always associated with an insufficient amount of bromine, therefore, to confirm suspicions, you need to visit a doctor and pass necessary tests. Often, due to a lack of bromine, the risk of spontaneous abortion increases (miscarriage on different terms until the third trimester).

Useful properties of bromine and its effect on the body

Bromine (in the form of bromides) is used for various diseases, its main action is sedative, so bromine preparations are often prescribed for nervous disorders and sleep disorders. Bromine salts are effective tool for the treatment of diseases that cause seizures (especially epilepsy), as well as disorders of activity of cardio-vascular system and some gastrointestinal ailments (stomach and duodenal ulcers).

Bromine digestibility

The absorption of bromine is slowed down by aluminum, and therefore it is necessary to take preparations containing bromine salts only after consulting a doctor.

Contrary to unsubstantiated rumors (more like anecdotes), bromine does not have a depressing effect on men's sexual desire and potency. Allegedly, bromine in the form of a white powder is added to the food of young soldiers in the army, as well as male patients in psychiatric dispensaries and prisoners in prisons and colonies. There is not a single scientific confirmation of this, and rumors can be explained by the ability of bromine (its preparations) to have a calming effect.

According to some sources, bromine promotes the activation of sexual function in men and an increase in both the volume of the ejaculant and the number of spermatozoa contained in it.

The use of bromine in life

Bromine is used not only in medicine (potassium bromide and sodium bromide), but also in other areas, such as photography, oil production, and the production of motor fuel. Bromine is used in the manufacture of chemical warfare agents, which once again emphasizes the need for careful handling of this element.

Red-brown liquid, with a sharp specific odor, poorly soluble in water, but soluble in benzene, chloroform, carbon disulfide and other organic solvents. Such an answer can be given to the question: "What is bromine?" The compound belongs to the group of the most active non-metals, reacting with many simple substances. It is highly toxic: inhalation of its vapors irritates the respiratory tract, and contact with the skin causes severe burns that do not heal for a long time. In our article we will study it physical properties, and also consider the chemical reactions characteristic of bromine.

The main subgroup of the seventh group is the position of the element in the periodic table of chemical elements. The last energy layer of an atom contains two s-electrons and five p-electrons. Like all halogens, bromine has a significant electron affinity. This means that it easily attracts negative particles of other chemical elements into its electron shell, becoming an anion. The molecular formula of bromine is Br 2 . Atoms are connected to each other with the help of a joint pair of electrons, this type of bond is called covalent. It is also non-polar, located at the same distance from the nuclei of atoms. Due to the rather large radius of the atom - 1.14A °, the oxidizing properties of the element, its electronegativity and non-metallic properties become less than those of fluorine and chlorine. The boiling point, on the contrary, rises and is 59.2 ° C, the relative molecular weight of bromine is 180. In the free state, due to the high activity, the element as a simple substance does not occur. In nature, it can be found in a bound state in the form of salts of sodium, magnesium, potassium, their content is especially high in sea water. Some types of brown and red algae: sargassum, fucus, batrachospermum, contain a large amount of bromine and iodine.

Reactions with simple substances

The element is characterized by interaction with many non-metals: sulfur, phosphorus, hydrogen:

Br 2 + H 2 \u003d 2HBr

However, bromine does not directly react with nitrogen, carbon and oxygen. Most metals are easily oxidized by bromine. Only some of them are passive to the action of halogen, for example, lead, silver and platinum. Reactions with bromine of more active halogens, such as fluorine and chlorine, are fast:

Br 2 +3 F 2 \u003d 2 BrF 3

In the last reaction, the oxidation state of the element is +3, it acts as a reducing agent. In industry, bromine is produced by the oxidation of hydrogen bromide with a stronger halogen, such as chlorine. The main sources of raw materials for obtaining the compound are underground drilling waters, as well as a highly concentrated solution of salt lakes. The halogen can interact with complex substances from the class of medium salts. So, under the action of bromine water, which has a red-brown color, on a solution of sodium sulfite, we observe a discoloration of the solution. This is due to the oxidation of the middle salt, sulfite, to sodium sulfate by bromine. The halogen itself is reduced, turning into the form of hydrogen bromide, which has no color.

Interaction with organic compounds

Br 2 molecules are capable of interacting not only with simple but also with complex substances. For example, the substitution reaction takes place between the aromatic hydrocarbon benzene and bromine when heated, in the presence of a catalyst - ferric bromide. It ends with the formation of a colorless compound, insoluble in water - bromobenzene:

C 6 H 6 + Br 2 \u003d C 6 H 5 Br + HBr

The simple substance bromine, dissolved in water, is used as an indicator to determine the presence of unsaturated bonds between carbon atoms in a molecule of organic substances. Such a qualitative reaction is found in the molecules of alkenes or alkynes, pi bonds, on which the main chemical reactions specified hydrocarbons. The compound enters into substitution reactions with saturated hydrocarbons, while forming derivatives of methane, ethane and other alkanes. A well-known reaction is the addition of bromine particles, the formula of which is Br2, to unsaturated substances with one or two double or triple bonds in molecules, for example, to such as ethene, acetylene or butadiene.

CH 2 \u003d CH 2 + Br 2 \u003d CH 2 Br - CH 2 Br

With these hydrocarbons, not only a simple substance can react, but also its hydrogen compound - HBr.

Features of the interaction of halogen with phenol

An organic substance consisting of a benzene ring associated with a hydroxyl group is phenol. In its molecule, the mutual influence of groups of atoms on each other is traced. Therefore, substitution reactions with halogens in it proceed much faster than in benzene. Moreover, the process does not require heating and the presence of a catalyst. Immediately three hydrogen atoms in the phenol molecule are replaced by bromine radicals. As a result of the reaction, tribromophenol is formed.

Oxygen compounds of bromine

Let's continue studying the question of what bromine is. The interaction of the halogen with cold water leads to the production of hypochlorous acid HBrO. It is weaker than the chlorine compound by reducing its oxidizing properties. Another compound, bromic acid, can be obtained by oxidizing bromine water with chlorine. Earlier in chemistry, it was believed that bromine could not have compounds in which it could exhibit an oxidation state of +7. However, by oxidation of potassium bromate, a salt was obtained - potassium bromate, and from it - and the corresponding acid - HBrO 4. Halogen ions have reducing properties: when HBr molecules act on metals, the latter are oxidized by hydrogen cations. Therefore, only those metallic elements that are in the activity series up to hydrogen interact with the acid. As a result of the reaction, medium salts are formed - bromides, and free hydrogen is released.

The use of bromine compounds

The high oxidizing ability of bromine, whose mass is quite large, is widely used in analytical chemistry, as well as in the chemistry of organic synthesis. AT agriculture preparations containing bromine are used in the fight against weeds and insect pests. Flame retardants - substances that prevent spontaneous combustion, are used to impregnate building materials, plastics, fabrics. In medicine, the inhibitory effect of salts: potassium and sodium bromide - on the passage of bioelectric impulses along nerve fibers has long been known. They are used in the treatment of disorders nervous system: hysteria, neurasthenia, epilepsy. Given the strong toxicity of the compounds, the dosage of the drug should be controlled by a doctor.

In our article, we found out what bromine is, and what physical and chemical properties are characteristic of it.

atomic number	35
Appearance of a simple substance	red-brown liquid with a strong unpleasant odor
Atom properties
Atomic mass (molar mass)	79.904 a. e.m. (g/mol)
Atom radius	n/a pm
Ionization energy (first electron)	1142.0 (11.84) kJ/mol (eV)
Electronic configuration	3d 10 4s 2 4p 5
Chemical properties
covalent radius	114 pm
Ion radius	(+5e)47 (-1e)196 pm
Electronegativity (according to Pauling)	2,96
Electrode potential	0
Oxidation states	7, 5, 3, 1, -1
Thermodynamic properties of a simple substance
Density	3.12 g/cm³
Molar heat capacity	75.69 J/(K mol)
Thermal conductivity	0.005 W/(m K)
Melting temperature	265.9K
Melting heat	(Br—Br) 10.57 kJ/mol
Boiling temperature	331.9K
Heat of evaporation	(Br—Br) 29.56 kJ/mol
Molar volume	23.5 cm³/mol
The crystal lattice of a simple substance
Lattice structure	orthorhombic
Lattice parameters	a=6.67 b=4.48 c=8.72 Å
c/a ratio	—
Debye temperature	n/a K

Br	35
79,904
3d 10 4s 2 4p 5

- an element of the main subgroup of the seventh group of the fourth period of the periodic system of chemical elements of D. I. Mendeleev, atomic number 35. It is designated by the symbol Br (lat. Bromum). Reactive non-metal, belongs to the group of halogens. The simple substance bromine (CAS number: 7726-95-6) under normal conditions is a heavy red-brown liquid with a strong unpleasant odor. The bromine molecule is diatomic (formula Br2).

Story

Bromine was discovered in 1826 by A. J. Balar, a young college teacher in the city of Montpellier. The discovery of Balar made his name known to the whole world. From one popular book to another, the assertion wanders that, distressed by the fact that the unknown Antoine Balard was ahead of Justus Liebig himself in the discovery of bromine, Liebig exclaimed that, they say, it was not Balar who discovered bromine, but bromine discovered Balar. However, this is not true, or, more precisely, not entirely true. There was a phrase, but it did not belong to J. Liebig, but to Charles Gerard, who really wanted Auguste Laurent to take the chair of chemistry at the Sorbonne, and not A. Balard, who was elected to the post of professor.

origin of name

The name of the element is βρῶμος — stench.

Receipt

Bromine is obtained chemically from brine brine -:

Physical Properties

Under normal conditions, bromine is a red-brown liquid with a sharp unpleasant odor, poisonous, and burns on contact with the skin. Density at 0 ° C - 3.19 g / cm³. The melting point (solidification) of bromine is -7.2 ° C, the boiling point is 58.8 ° C, when boiling, bromine turns from a liquid into a brown-brown vapor, irritating the respiratory tract when inhaled. The standard electrode potential Br² / Br - in an aqueous solution is +1.065 V.

Ordinary bromine consists of the isotopes 79 Br (50.56%) and 81 Br (49.44%). Artificially obtained radioactive isotopes.

Chemical properties

It exists in free form in the form of diatomic molecules Br 2 . A noticeable dissociation of molecules into atoms is observed at a temperature of 800 °C and rapidly increases with a further increase in temperature. The diameter of the Br 2 molecule is 0.323 nm, the internuclear distance in this molecule is 0.228 nm.

Bromine is slightly, but better than other halogens, soluble in water (3.58 g in 100 g of water at 20 ° C), the solution is called bromine water. In bromine water, a reaction proceeds with the formation of hydrobromic and unstable hypobromous acids:

Br 2 + H 2 O → HBr + HBrO.

With most organic solvents, bromine is miscible in all respects, and bromination of organic solvent molecules often occurs.

Bromine is intermediate in chemical activity between chlorine and iodine. When bromine reacts with iodide solutions, free iodine is released:

Br 2 + 2KI → I 2 ↓ + 2KBr.

On the contrary, under the action of chlorine on bromides in aqueous solutions, free bromine is released:

When bromine reacts with sulfur, S 2 Br 2 is formed; when bromine reacts with phosphorus, PBr 3 and PBr 5 are formed. Bromine also reacts with non-metals selenium and tellurium.

The reaction of bromine with hydrogen proceeds when heated and leads to the formation of hydrogen bromide HBr. A solution of HBr in water is hydrobromic acid, similar in strength to hydrochloric acid HCl. Salts of hydrobromic acid - bromides (NaBr, MgBr 2, AlBr 3, etc.). A qualitative reaction to the presence of bromide ions in solution is the formation with Ag + ions of a light yellow precipitate of silver bromide AgBr, which is practically insoluble in water.

Bromine does not directly react with oxygen and nitrogen. Bromine forms a large number of different compounds with other halogens. For example, bromine forms unstable BrF 3 and BrF 5 with fluorine, and IBr with iodine. When interacting with many metals, bromine forms bromides, for example, AlBr 3, CuBr 2, MgBr 2, etc. Tantalum and platinum are resistant to the action of bromine, to a lesser extent - silver, titanium and lead.

Bromine is a strong oxidizing agent, it oxidizes the sulfite ion to sulfate, the nitrite ion to nitrate, etc.

When interacting with organic compounds containing a double bond, bromine is added, giving the corresponding dibromo derivatives:

C 2 H 4 + Br 2 → C 2 H 4 Br 2.

Bromine also joins organic molecules, which contain a triple bond. The discoloration of bromine water when a gas is passed through it or a liquid is added to it indicates that an unsaturated compound is present in the gas or liquid.

When heated in the presence of a catalyst, bromine reacts with benzene to form bromobenzene C 6 H 5 Br (substitution reaction).

When bromine interacts with alkali solutions and with solutions of sodium or potassium carbonates, the corresponding bromides and bromates are formed, for example:

3Br 2 + 3Na 2 CO 3 → 5NaBr + NaBrO 3 + 3CO 2.

Brominated acids

In addition to the oxygen-free hydrobromic acid HBr, bromine forms a number of oxygen acids: bromine HBrO 4, bromine HBrO 3, bromine HBrO 2, bromine HBrO.

Application

In chemistry

Bromine-based substances are widely used in basic organic synthesis.

In engineering

- Silver bromide AgBr is used in photography as a photosensitive substance.
- Used to create flame retardants - additives that give fire resistance to plastics, wood, textile materials.
- Bromine pentafluoride is sometimes used as a very powerful propellant oxidizer.
- 1,2-dibromoethane is currently used as an antiknock additive in motor fuel, instead of tetraethyl lead.
— Bromide solutions are used in oil production.

In medicine

In medicine, sodium bromide and potassium bromide are used as sedatives.

In the production of weapons

Since the First World War, bromine has been used to produce chemical warfare agents.

Physiological action

Already at a bromine content in the air at a concentration of about 0.001% (by volume), irritation of the mucous membranes, dizziness, and at more high concentrations- spasms of the respiratory tract, suffocation. MPC of bromine vapor is 0.5 mg/m³. When ingested toxic dose is 3 g, lethal - from 35 g. In case of poisoning with bromine vapor, the victim must be immediately removed to fresh air; to restore breathing, you can use a swab moistened with ammonia for a short time, periodically bringing it to the victim’s nose for a short time. Further treatment should be done under medical supervision. Liquid bromine on contact with the skin causes painful burns.

Features of work

When working with bromine, protective clothing, a gas mask, and special gloves should be used. Due to the high reactivity and toxicity of both bromine vapor and liquid bromine, it should be stored in a glass, tightly sealed thick-walled container. Vials with bromine are placed in containers with sand, which protects the flasks from destruction when shaken. Because of high density bromine bottles with him in no case should not be taken only by the throat (the throat can come off, and then the bromine will be on the floor).

To neutralize the spilled bromine, the surface with it must be filled with a solution of sodium sulfite Na 2 SO 3

Myths and legends

There is a widespread legend that in the army they allegedly add bromine to food to reduce sexual desire. This myth has no basis - attraction is successfully reduced physical exercise, while additives actually added to food most often turn out to be ascorbic acid to prevent avitaminosis. In addition, bromine preparations are salty in taste and do not affect either attraction or potency. They have a sedative and sedative effect.