Sulfur (English Sulfur, French Sufre, German Schwefel) in its native state, as well as in the form of sulfur compounds, has been known since ancient times. With the smell of burning sulfur, the suffocating effect of sulfur dioxide and the disgusting smell of hydrogen sulfide, people probably met in prehistoric times. It is because of these properties that sulfur was used by priests as part of sacred incense during religious rites. Sulfur was considered the product of superhuman beings from the world of spirits or underground gods. A very long time ago, sulfur began to be used as part of various combustible mixtures for military purposes. Homer already describes "sulphurous fumes", the deadly effect of the secretions of burning sulfur. Sulfur was probably part of the "Greek fire", which terrified opponents. Around the 8th century the Chinese began to use it in pyrotechnic mixtures, in particular, in mixtures such as gunpowder. The combustibility of sulfur, the ease with which it combines with metals to form sulfides (for example, on the surface of pieces of metal), explains that it was considered the "principle of combustibility" and an indispensable component of metal ores. Presbyter Theophilus (XI century) describes a method of oxidative roasting of sulfide copper ore, probably known in ancient Egypt. During the period of Arabic alchemy, the mercury-sulfur theory of the composition of metals arose, according to which sulfur was considered an obligatory constituent (father) of all metals. Later it became one of the three principles of alchemists, and later the "principle of combustibility" was the basis of the theory of phlogiston. The elementary nature of sulfur was established by Lavoisier in his combustion experiments. With the introduction of gunpowder in Europe, the development of the extraction of natural sulfur began, as well as the development of a method for obtaining it from pyrites; the latter was distributed in ancient Russia. For the first time in the literature, it is described by Agricola. Origin of lat. Sulfur is unclear. It is believed that this name is borrowed from the Greeks. Sulfur often appears in the literature of the alchemical period under various arcane names. In Ruland, one can find, for example, the names Zarnec (an explanation of "an egg with fire"), Thucios (living sulfur), Terra foetida, spiritus foetens, Scorith, Pater, and others. The Old Russian name "sulfur" has been used for a very long time. It meant various combustible and foul-smelling substances, resins, physiological secretions (wax in the ears, etc.). Apparently, this name comes from the Sanskrit sira (light yellow). The word "gray" is associated with it, that is, an indefinite color, which, in particular, refers to resins. The second old Russian name for sulfur - bogey (combustible sulfur) - also contains the concept of not only combustibility, but also a bad smell. As philologists explain, it. Schwefel comes from the Sanskrit root swep (sleep, Anglo-Saxon sweblan - to kill), which may be related to the poisonous properties of sulfur dioxide.

Sulfur takes an honorable 16th place in the periodic table, denoted "S" - sulfur, which in Latin means "fat, combustible substance." This substance has been known since ancient times.

We present interesting facts about sulfur.

It has a terrible smell and has a suffocating effect on humans. The priests used it for various rituals and sacred incense, and the military added it to various combustible mixtures.

Functions in the body

Not a single process in the body can do without sulfur. It is one of the main components of all existing proteins. The functions that are assigned to the work of sulfur in human body are huge. Starting from the stable functioning of nerve cells, balancing blood sugar and a general increase in immunity, ending with wound healing and anti-inflammatory effects.

Diseases. Sulfur is used necessarily for diseases:

• scabies
• allergy
• arthritis and osteoarthritis
• eczema

"Miracle" - sulfur is a part of medicines and is used in pure form for treatment.

Nutrition

It will seem strange to some, and someone has known about it for a long time, but sulfur is contained in the mass of products that we use daily, even without suspecting it. This number includes: all legumes, cereals and cereals, as well as bakery products (!); onions, garlic and cabbage; apples, grapes and gooseberries; milk products; a fish.

Not surprisingly, to date, recorded cases of sulfur deficiency are negligible. After all, some of the above we in any case use in the diet.

Here are some more interesting facts about sulfur. Something we don't know for sure.

• for example, when we cut onions and "cry" - we must say "thank you" to the sulfur that is absorbed into the soil where it grows.
• in the province of Indonesia there is a volcano completely filled with sulfur, which is called Kawa Ijen. It settles on the pipes, after which the workers knock it down with fittings and carry it for weighing. This is how they earn their living.

• hygienic "products" based on sulfur created specifically for cleaning problem skin from acne and rashes.
• earwax, which we have been taught to remove since childhood with cotton swabs, "poisons" our lives with noble intentions. It contains special lysozyme enzymes; it is they who "do not let" everything foreign - bacterial - into our body.

As you can see, sulfur is present in human life and his body directly constantly. Deficiency, like excess, is always bad. Watch your lifestyle and then, such a macronutrient as " sulfur", that is, sulfur will benefit you, both externally and internally.

Well, of course, our standard method of obtaining fire is based on the same sulfur.

Sulfur - S, chemical element with atomic number 16, atomic mass 32.066. The chemical symbol for sulfur is S, pronounced "es".

Natural sulfur consists of four stable nuclides: 32S (content 95.084% by mass), 33S (0.74%), 34S (4.16%) and 36S (0.016%).

The radius of the sulfur atom is 0.104 nm. Ion radii: S2- ion 0.170 nm (coordination number 6), S4+ ion 0.051 nm (coordination number 6) and S6+ ion 0.026 nm (coordination number 4). The sequential ionization energies of a neutral sulfur atom from S0 to S6+ are 10.36, 23.35, 34.8, 47.3, 72.5, and 88.0 eV, respectively.

Sulfur is located in the VIA group of the periodic system of D. I. Mendeleev, in the 3rd period, and belongs to the number of chalcogens. The configuration of the outer electron layer is 3s23p4. The most characteristic oxidation states in compounds are -2, +4, +6 (valencies II, IV and VI, respectively). The electronegativity value of sulfur according to Pauling is 2.6.

Sulfur is one of the non-metals.

Physical properties of sulfur

Sulfur differs significantly from oxygen in its ability to form stable chains and cycles of atoms. The most stable are cyclic S8 molecules, which have the shape of a crown and form rhombic and monoclinic sulfur. This is crystalline sulfur - a brittle yellow substance. In addition, molecules with closed (S4, S6) chains and open chains are possible. Such a composition has plastic sulfur, a brown substance, which is obtained by sharp cooling of the sulfur melt (plastic sulfur becomes brittle after a few hours, turns yellow and gradually turns into a rhombic one). The formula for sulfur is most often written simply as S, since, although it has a molecular structure, it is a mixture of simple substances with different molecules. Sulfur is insoluble in water, some of its modifications dissolve in organic solvents, such as carbon disulfide, turpentine. The melting of sulfur is accompanied by a noticeable increase in volume (about 15%). Molten sulfur is a yellow, highly mobile liquid, which above 160 °C turns into a very viscous dark brown mass. The sulfur melt acquires the highest viscosity at a temperature of 190 °C; a further increase in temperature is accompanied by a decrease in viscosity, and above 300 °C the molten sulfur becomes mobile again. This is due to the fact that when sulfur is heated, it gradually polymerizes, increasing the chain length with increasing temperature. When sulfur is heated above 190 °C, the polymer units begin to break down. Sulfur is the simplest example of an electret. When rubbed, sulfur acquires a strong negative charge.

Chalcogens are a group of elements to which sulfur belongs. Its chemical symbol is S, the first letter of the Latin name Sulfur. The composition of a simple substance is written using this symbol without an index. Consider the main points regarding the structure, properties, production and use of this element. The characterization of sulfur will be presented in as much detail as possible.

Common features and differences of chalcogens

Sulfur belongs to the oxygen subgroup. This is the 16th group in the modern long-period form of the Periodic Table (PS). An obsolete version of the number and index is VIA. Titles chemical elements groups, chemical signs:

• oxygen (O);
• sulfur (S);
• selenium (Se);
• tellurium (Te);
• polonium (Po).

The outer electron shell of the above elements has the same structure. In total, it contains 6 which can participate in the formation of a chemical bond with other atoms. Hydrogen compounds correspond to the composition H 2 R, for example, H 2 S is hydrogen sulfide. The names of the chemical elements that form two types of compounds with oxygen: sulfur, selenium and tellurium. The general formulas of the oxides of these elements are RO 2, RO 3.

Chalcogens correspond to simple substances that differ significantly in physical properties. The most common chalcogens in the earth's crust are oxygen and sulfur. The first element forms two gases, the second - solids. Polonium, a radioactive element, is rarely found in the earth's crust. In the group from oxygen to polonium, non-metallic properties decrease and metallic properties increase. For example, sulfur is a typical non-metal, while tellurium has a metallic luster and electrical conductivity.

Element No. 16 of the D.I. Mendeleev

The relative atomic mass of sulfur is 32.064. Of the natural isotopes, 32 S is the most common (more than 95% by weight). Nuclides with atomic masses of 33, 34 and 36 are found in smaller quantities. Characteristics of sulfur by position in PS and atomic structure:

• serial number - 16;
• the charge of the nucleus of an atom is +16;
• atomic radius - 0.104 nm;
• ionization energy -10.36 eV;
• relative electronegativity - 2.6;
• oxidation state in compounds - +6, +4, +2, -2;
• valency - II (-), II (+), IV (+), VI (+).

Sulfur is in the third period; electrons in an atom are located on three energy levels: on the first - 2, on the second - 8, on the third - 6. All external electrons are valence. When interacting with more electronegative elements, sulfur gives up 4 or 6 electrons, acquiring typical oxidation states of +6, +4. In reactions with hydrogen and metals, the atom attracts the missing 2 electrons until the octet is filled and a steady state is reached. in this case it drops to -2.

Physical properties of rhombic and monoclinic allotropic forms

Under normal conditions, sulfur atoms are connected to each other at an angle into stable chains. They can be closed in rings, which allows us to speak about the existence of cyclic sulfur molecules. Their composition reflect the formulas S 6 and S 8 .

The characterization of sulfur should be supplemented by a description of the differences between allotropic modifications with different physical properties.

Rhombic or α-sulfur is the most stable crystalline form. These are bright yellow crystals composed of S 8 molecules. The density of rhombic sulfur is 2.07 g/cm3. Light yellow monoclinic crystals are formed by β-sulfur with a density of 1.96 g/cm3. The boiling point reaches 444.5°C.

Obtaining amorphous sulfur

What color is sulfur in the plastic state? It is a dark brown mass, completely different from yellow powder or crystals. To obtain it, you need to melt rhombic or monoclinic sulfur. At temperatures above 110°C, a liquid is formed, with further heating it darkens, at 200°C it becomes thick and viscous. If you quickly pour molten sulfur into cold water, then it will solidify with the formation of zigzag chains, the composition of which is reflected by the formula S n.

Solubility of sulfur

Some modifications in carbon disulfide, benzene, toluene and liquid ammonia. If organic solutions are cooled slowly, needle-like crystals of monoclinic sulfur are formed. When liquids evaporate, transparent lemon-yellow crystals of rhombic sulfur are released. They are brittle and can be easily ground into powder. Sulfur does not dissolve in water. The crystals sink to the bottom of the vessel, and the powder can float on the surface (not wetted).

Chemical properties

The reactions show the typical non-metallic properties of element No. 16:

• sulfur oxidizes metals and hydrogen, is reduced to the S 2- ion;
• when burned in air and oxygen, di- and sulfur trioxide are formed, which are acid anhydrides;
• in a reaction with another more electronegative element - fluorine - sulfur also loses its electrons (is oxidized).

Free sulfur in nature

In terms of prevalence in the earth's crust, sulfur is in 15th place among the chemical elements. The average content of S atoms in is 0.05% of the mass of the earth's crust.

What color is sulfur in nature (native)? It is a light yellow powder with a characteristic odor or yellow crystals with a glassy luster. Deposits in the form of placers, crystalline layers of sulfur are found in areas of ancient and modern volcanism: in Italy, Poland, Central Asia, Japan, Mexico, and the USA. Often, when mining, beautiful druze and giant single crystals are found.

Hydrogen sulfide and oxides in nature

In areas of volcanism, gaseous sulfur compounds come to the surface. The Black Sea at a depth of over 200 m is lifeless due to the release of hydrogen sulfide H 2 S. The formula of sulfur oxide is divalent - SO 2, trivalent - SO 3. The listed gaseous compounds are present in some oil, gas, and natural water deposits. Sulfur is part of coal. It is necessary for the construction of many organic compounds. When egg whites rot, hydrogen sulfide is released, which is why it is often said that this gas has the smell of rotten eggs. Sulfur is a biogenic element, it is necessary for the growth and development of humans, animals and plants.

Importance of natural sulfides and sulfates

The characterization of sulfur will be incomplete, if not to say that the element occurs not only in the form of a simple substance and oxides. The most common natural compounds are salts of hydrosulfide and sulfuric acids. Sulfides of copper, iron, zinc, mercury, lead are found in the minerals sphalerite, cinnabar and galena. Sulfates include sodium, calcium, barium and magnesium salts, which form minerals and rocks in nature (mirabilite, gypsum, selenite, barite, kieserite, epsomite). All these compounds are used in various sectors of the economy, used as raw materials for industrial processing, fertilizers, building materials. The medical value of some crystalline hydrates is great.

Receipt

A yellow substance in a free state occurs in nature at different depths. If necessary, sulfur is smelted from rocks, without raising them to the surface, but by forcing superheated rocks to a depth. Another method is associated with sublimation from crushed rocks in special furnaces. Other methods involve dissolution with carbon disulfide or flotation.

The needs of industry for sulfur are great, therefore, its compounds are used to obtain elemental matter. In hydrogen sulfide and sulfides, sulfur is in reduced form. The oxidation state of the element is -2. Sulfur is oxidized, increasing this value to 0. For example, according to the Leblanc method, sodium sulfate is reduced with coal to sulfide. Then calcium sulfide is obtained from it, treated with carbon dioxide and water vapor. The resulting hydrogen sulfide is oxidized with atmospheric oxygen in the presence of a catalyst: 2H 2 S + O 2 = 2H 2 O + 2S. The determination of sulfur obtained by various methods sometimes gives low purity values. Refining or purification is carried out by distillation, rectification, treatment with mixtures of acids.

The use of sulfur in modern industry

Sulfur granulated is used for various production needs:

1. Obtaining sulfuric acid in the chemical industry.
2. Production of sulfites and sulfates.
3. Production of preparations for plant nutrition, control of diseases and pests of agricultural crops.
4. Sulfur-containing ores are processed at mining and chemical plants to obtain non-ferrous metals. Accompanying production is sulfuric acid.
5. Introduction to the composition of some grades of steels to impart special properties.
6. Thanks get rubber.
7. Manufacture of matches, pyrotechnics, explosives.
8. Use for the preparation of paints, pigments, artificial fibers.
9. Bleaching fabrics.

Toxicity of sulfur and its compounds

Dust-like particles with an unpleasant odor irritate the mucous membranes of the nasal cavity and respiratory tract, eyes, and skin. But the toxicity of elemental sulfur is not considered particularly high. Inhalation of hydrogen sulfide and dioxide can cause severe poisoning.

If, during the roasting of sulfur-containing ores at metallurgical plants, exhaust gases are not captured, then they enter the atmosphere. Combining with drops and water vapor, sulfur and nitrogen oxides give rise to the so-called acid rain.

Sulfur and its compounds in agriculture

Plants absorb sulfate ions along with the soil solution. A decrease in sulfur content leads to a slowdown in the metabolism of amino acids and proteins in green cells. Therefore, sulfates are used for fertilizing crops.

To disinfect poultry houses, basements, vegetable stores, a simple substance is burned or the premises are treated with modern sulfur-containing preparations. Sulfur oxide has antimicrobial properties, which has long been used in the production of wines, in the storage of vegetables and fruits. Sulfur preparations are used as pesticides to control diseases and pests of agricultural crops ( powdery mildew and spider mites).

Application in medicine

Great value to study medicinal properties yellow powder was given by the great healers of antiquity Avicenna and Paracelsus. Later it was found that a person who does not receive enough sulfur with food becomes weaker, experiences health problems (these include itching and flaking of the skin, weakening of hair and nails). The fact is that without sulfur, the synthesis of amino acids, keratin, and biochemical processes in the body is disrupted.

Medical sulfur is included in ointments for the treatment of skin diseases: acne, eczema, psoriasis, allergies, seborrhea. Sulfur baths can relieve the pain of rheumatism and gout. For better absorption by the body, water-soluble sulfur-containing preparations have been created. This is not a yellow powder, but a white crystalline substance. When used externally, this compound is incorporated into a skin care cosmetic.

Gypsum has long been used in the immobilization of injured parts of the human body. prescribed as a laxative. Magnesia lowers blood pressure, which is used in the treatment of hypertension.

Sulfur in history

Even in ancient times, a non-metallic yellow substance attracted the attention of a person. But it wasn't until 1789 that the great chemist Lavoisier established that powders and crystals found in nature were composed of sulfur atoms. It was believed that the unpleasant smell that occurs when it is burned, repels all evil spirits. The formula for sulfur oxide, which is obtained during combustion, is SO 2 (dioxide). It is a toxic gas and is hazardous to health if inhaled. Several cases of mass extinction of people by entire villages on the coasts, in the lowlands, scientists explain the release of hydrogen sulfide or sulfur dioxide from the earth or water.

The invention of black powder increased military interest in yellow crystals. Many battles have been won thanks to the ability of craftsmen to combine sulfur with other substances during the manufacturing process. Critical Connection- sulfuric acid - also learned to use a very long time ago. In the Middle Ages, this substance was called vitriol oil, and salts were called vitriol. Copper sulphate CuSO 4 and ferrous sulphate FeSO 4 still have not lost their importance in industry and agriculture.