mineral Sulfur Native
Sulfur, unlike other native elements, has a molecular lattice, which determines its low hardness (1.5-2.5), lack of cleavage, fragility, uneven fracture and the resulting greasy splash; Only on the surface of the crystals is a glassy sheen observed. Specific gravity 2.07 g/cm3. Sulfur has poor electrical conductivity, weak thermal conductivity, low melting point (112.8°C) and ignition point (248°C). Sulfur is ignited by a match and burns with a blue flame; this produces sulfur dioxide, which has a pungent, suffocating odor. The color of native sulfur is light yellow, straw yellow, honey yellow, greenish; sulfur containing organic substances acquire a brown, gray, black color. Volcanic sulfur is bright yellow, orange, greenish. In some places it usually has a yellowish tint. Sulfur is found in the form of solid, dense, sintered, earthy, powdery masses; There are also overgrown crystals, nodules, plaques, crusts, inclusions and pseudomorphs of organic residues. Rhombic syngony.
Distinctive features: native sulfur is characterized by: a non-metallic luster and the fact that the sulfur ignites with a match and burns, releasing sulfur dioxide, which has a sharp suffocating odor. The most characteristic color of native sulfur is light yellow.
Variety
Vulcanite (selenium sulfur). Orange-red, red-brown color. The origin is volcanic.
Chemical properties
It ignites with a match and burns with a blue flame, which produces sulfur dioxide, which has a pungent, suffocating odor. Melts easily (melting point 112.8° C). Flash point 248° C. Sulfur dissolves in carbon disulfide.
Origin of sulfur
Native sulfur of natural and volcanic origin is found. Sulfur bacteria live in water basins enriched with hydrogen sulfide due to the decomposition of organic residues - at the bottom of swamps, estuaries, and shallow sea bays. The Black Sea estuaries and Sivash Bay are examples of such bodies of water. The concentration of sulfur of volcanic origin is confined to volcanic vents and to the voids of volcanic rocks. During volcanic eruptions, various sulfur compounds (H 2 S, SO 2) are released, which are oxidized in surface conditions, which leads to its reduction; in addition, sulfur is sublimated directly from the vapor.
Sometimes, during volcanic processes, sulfur is ejected in liquid form. This happens when sulfur, previously deposited on the walls of the craters, melts as the temperature rises. Sulfur is also deposited from hot aqueous solutions as a result of the decomposition of hydrogen sulfide and sulfur compounds released during one of the later phases of volcanic activity. These phenomena are now observed near the geyser vents of Yellowstone Park (USA) and Iceland. It is found together with gypsum, anhydrite, limestone, dolomite, rock and potassium salts, clays, bituminous deposits (oil, ozokerite, asphalt) and pyrite. It is also found on the walls of volcanic craters, in cracks in lavas and tuffs surrounding the vents of volcanoes, both active and extinct, near sulfur mineral springs.
Satellites. Among the sedimentary rocks: gypsum, anhydrite, calcite, dolomite, siderite, rock salt, sylvite, carnallite, opal, chalcedony, bitumens (asphalt, oil, ozokerite). In deposits formed as a result of sulfide oxidation, there is mainly pyrite. Among the products of volcanic sublimation: gypsum, realgar, orpiment.
Application
Sulfur is widely used in the chemical industry. Three quarters of sulfur production is used to produce sulfuric acid. It is also used to control agricultural pests, in addition, in the paper, rubber industries (rubber vulcanization), in the production of gunpowder, matches, pharmaceuticals, glass, and food industries.
Sulfur deposits
On the territory of Eurasia, all industrial deposits of native sulfur are of surface origin. Some of them are located in Turkmenistan, in the Volga region, etc. Rocks containing sulfur stretch along the left bank of the Volga from the city of Samara in a strip several kilometers wide to Kazan. Sulfur was probably formed in lagoons during the Permian period as a result of biochemical processes. Sulfur deposits are located in Razdol (Lviv region, Carpathian region), Yavorovsk (Ukraine) and in the Ural-Embinsky region. In the Urals (Chelyabinsk region) sulfur is found, formed as a result of the oxidation of pyrite. Sulfur of volcanic origin is found in Kamchatka and the Kuril Islands. The main sulfur reserves of capitalist countries are located in Iraq, the USA (Louisiana and Utah), Mexico, Chile, Japan and Italy (Sicily).
Properties of the mineral
- Specific gravity: 2 - 2,1
- Selection form: radial-radiant aggregates
- Selection form: radial-radiant aggregates
- USSR taxonomy classes: Metals
- Chemical formula: S
- Syngony: rhombic
- Color: Sulfur-yellow, yellow-orange, yellow-brown, grayish-yellow, grayish-brown.
- Trait color: Sulfur yellow, straw yellow
- Shine: fatty
- Transparency: translucent cloudy
- Cleavage: imperfect
- Kink: conchoidal
- Hardness: 2
- Fragility: Yes
- Additionally: It melts easily (at 119°C) and burns with a blue flame, turning into SO3. Behavior in acids. Insoluble (in water also), but soluble in CS2.
Photo of the mineral
Articles on the topic
- Characteristics of chemical element No. 16
History of the discovery of the element. 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. - Sulfur, Sulfur, S (16)
Man probably became familiar with the smell of burning sulfur, the suffocating effect of sulfur dioxide and the disgusting smell of hydrogen sulfide back in prehistoric times. - Native sulfur
About half of the world's sulfur comes from natural reserves
Deposits of the mineral Sulfur Native
- Vodinskoye field
- Alekseevskoye field
- Russia
- Samara Region
- Bolivia
- Ukraine
- Novoyavorovsk. Lviv region
Sulfur (from lat. sērum“serum”) is a mineral of the class of native elements, a non-metal. The Latin name is associated with Indo-European root swelp - “burn”. Chemical formula: S.
Sulfur, unlike other native elements, has a molecular lattice, which determines its low hardness (1.5-2.5), lack of cleavage, fragility, uneven fracture and the resulting greasy splash; Only on the surface of the crystals is a glassy sheen observed. Specific gravity 2.07 g/cm3. It has poor electrical conductivity, weak thermal conductivity, low melting point (112.8°C) and ignition point (248°C). Lights easily with a match and burns with a blue flame; this produces sulfur dioxide, which has a pungent, suffocating odor. The color of native sulfur is light yellow, straw yellow, honey yellow, greenish; sulfur containing organic substances acquire a brown, gray, black color. Volcanic sulfur is bright yellow, orange, greenish. In some places it usually has a yellowish tint. The mineral is found in the form of continuous dense, sintered, earthy, powdery masses; There are also overgrown crystals, nodules, plaques, crusts, inclusions and pseudomorphs of organic residues. Rhombic syngony.
Features: native sulfur is characterized by: a non-metallic luster and the fact that it ignites with a match and burns, releasing sulfur dioxide, which has a sharp suffocating odor. The most characteristic color of native sulfur is light yellow.
Variety:
Vulcanite(selenium sulfur). Orange-red, red-brown color. The origin is volcanic.
Monoclinic sulfur Crystalline sulfur Crystalline sulfur Selenous sulfur - vulcanite
Chemical properties of sulfur
It ignites with a match and burns with a blue flame, which produces sulfur dioxide, which has a pungent, suffocating odor. Melts easily (melting point 112.8° C). Ignition temperature 248°C. Sulfur dissolves in carbon disulfide.
Origin of sulfur
Native sulfur of natural and volcanic origin is found. Sulfur bacteria live in water basins enriched with hydrogen sulfide due to the decomposition of organic residues - at the bottom of swamps, estuaries, and shallow sea bays. The Black Sea estuaries and Sivash Bay are examples of such bodies of water. The concentration of sulfur of volcanic origin is confined to volcanic vents and to the voids of volcanic rocks. During volcanic eruptions, various sulfur compounds (H 2 S, SO 2) are released, which are oxidized in surface conditions, which leads to its reduction; in addition, sulfur is sublimated directly from the vapor.
Sometimes, during volcanic processes, sulfur is ejected in liquid form. This happens when sulfur, previously deposited on the walls of the craters, melts as the temperature rises. Sulfur is also deposited from hot aqueous solutions as a result of the decomposition of hydrogen sulfide and sulfur compounds released during one of the later phases of volcanic activity. These phenomena are now observed near the geyser vents of Yellowstone Park (USA) and Iceland. It is found together with gypsum, anhydrite, limestone, dolomite, rock and potassium salts, clays, bituminous deposits (oil, ozokerite, asphalt) and pyrite. It is also found on the walls of volcanic craters, in cracks in lavas and tuffs surrounding the vents of volcanoes, both active and extinct, near sulfur mineral springs.
Satellites. Among the sedimentary rocks: gypsum, anhydrite, calcite, dolomite, siderite, rock salt, sylvite, carnallite, opal, chalcedony, bitumens (asphalt, oil, ozokerite). In deposits formed as a result of sulfide oxidation, there is mainly pyrite. Among the products of volcanic sublimation: gypsum, realgar, orpiment.
Application
Widely used in the chemical industry. Three quarters of sulfur production is used to produce sulfuric acid. It is also used to control agricultural pests, in addition, in the paper, rubber industries (rubber vulcanization), in the production of gunpowder, matches, pharmaceuticals, glass, and food industries.
Sulfur deposits
On the territory of Eurasia, all industrial deposits of native sulfur are of surface origin. Some of them are located in Turkmenistan, in the Volga region, etc. Rocks containing sulfur stretch along the left bank of the Volga from the city of Samara in a strip several kilometers wide to Kazan. Sulfur was probably formed in lagoons during the Permian period as a result of biochemical processes. Sulfur deposits are located in Razdol (Lviv region, Carpathian region), Yavorovsk (Ukraine) and in the Ural-Embinsky region. In the Urals (Chelyabinsk region) sulfur is found, formed as a result of the oxidation of pyrite. Sulfur of volcanic origin is found in Kamchatka and the Kuril Islands. The main reserves are located in Iraq, the USA (Louisiana and Utah), Mexico, Chile, Japan and Italy (Sicily).
Sulfur is an element of the sixth group of the third period of the main subgroup of the periodic system of chemical elements, with atomic number 16. It exhibits non-metallic properties. Denoted by the symbol S (Latin Sulfur). In hydrogen and oxygen compounds it is found in various ions and forms many acids and salts. Many sulfur-containing salts are poorly soluble in water.
History of discovery
Sulfur (English Sulfur, French Soufre, German Schwefel) in its native state, as well as in the form of sulfur compounds, has been known since ancient times. Man probably became familiar with the smell of burning sulfur, the suffocating effect of sulfur dioxide and the disgusting smell of hydrogen sulfide back in prehistoric times. It was because of these properties that sulfur was used by priests as part of sacred incense during religious rites. Sulfur was considered the work 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 flammable mixtures for military purposes. Homer already described “sulphurous fumes,” the deadly effect of burning sulfur emissions. Sulfur was probably part of the “Greek fire” that terrified opponents. Around the 8th century The Chinese began to use it in pyrotechnic mixtures, in particular, in mixtures such as gunpowder. The flammability of sulfur, the ease with which it combines with metals to form sulfides (for example, on the surface of pieces of metal), explains why it was considered the “principle of flammability” and an essential component of metal ores. Presbyter Theophilus (12th century) describes a method of oxidative roasting of sulfide copper ore, probably known in ancient Egypt. During the period of Arab alchemy, the mercury-sulfur theory of the composition of metals arose, according to which sulfur was revered as an essential component (father) of all metals. Later it became one of the three principles of alchemists, and later the “principle of flammability” became the basis of the theory of phlogiston. The elemental nature of sulfur was established by Lavoisier in his combustion experiments. With the introduction of gunpowder in Europe, the development of natural sulfur mining began, as well as the development of a method for obtaining it from pyrites; the latter was common in ancient Rus'. It was first described in literature by Agricola. Thus, the exact origin of sulfur has not been established, but, as stated above, this element was used before the birth of Christ, and therefore has been familiar to people since ancient times.
origin of name
The Russian name for sulfur goes back to the Proto-Slavic *sěra, which is associated with Lat. serum "serum".
The Latin sulfur (a Hellenized spelling of the older sulpur) comes from the Indo-European root *swelp, “to burn.”
Receipt
In ancient times and in the Middle Ages, sulfur was mined by digging a large clay pot into the ground, on which another was placed, with a hole in the bottom. The latter was filled with rock containing sulfur and then heated. The sulfur melted and flowed into the lower pot.
Currently, sulfur is obtained mainly by smelting native sulfur directly in places where it occurs underground. Sulfur ores are mined in different ways, depending on the conditions of occurrence. Sulfur deposits are almost always accompanied by accumulations of toxic gases - sulfur compounds. In addition, we must not forget about the possibility of its spontaneous combustion.
Open pit mining of ore occurs like this. Walking excavators remove layers of rock under which ore lies. The ore layer is crushed by explosions, after which the ore blocks are sent to a sulfur smelter, where sulfur is extracted from the concentrate.
In 1890, Hermann Frasch proposed melting sulfur underground and pumping it to the surface through oil wells. The relatively low (113 °C) melting point of sulfur confirmed the reality of Frasch’s idea. In 1890, tests began that led to success.
There are several known methods for obtaining sulfur from sulfur ores: steam-water, filtration, thermal, centrifugal and extraction.
Physical properties
Sulfur differs significantly from oxygen in its ability to form stable chains and cycles of atoms. The most stable are cyclic S8 molecules, having the shape of a crown, forming orthorhombic and monoclinic sulfur. This is crystalline sulfur - a brittle yellow substance. In addition, molecules with closed (S 4, S 6) chains and open chains are possible. This composition has plastic sulfur, a brown substance, which is obtained by sharp cooling of molten sulfur (plastic sulfur becomes brittle after a few hours, acquires a yellow color and gradually turns into rhombic). The formula for sulfur is most often written simply 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 and turpentine. The melting of sulfur is accompanied by a noticeable increase in volume (approximately 15%). Molten sulfur is a yellow, easily 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 again becomes mobile. This is because when sulfur is heated, it gradually polymerizes, increasing the length of the chain as the temperature increases. When sulfur is heated above 190 °C, the polymer units begin to collapse. Sulfur can serve as the simplest example of an electret. When rubbed, sulfur acquires a strong negative charge.
Sulfur is used for the production of sulfuric acid, rubber vulcanization, as a fungicide in agriculture and as colloidal sulfur - a medicinal product. Also, sulfur in sulfur bitumen compositions is used to produce sulfur asphalt, and as a substitute for Portland cement to produce sulfur concrete.
Natural Sulfur Minerals
Sulfur is the sixteenth most abundant element in the earth's crust. It is found in a free (native) state and bound form.
The most important natural sulfur compounds: FeS 2 - iron pyrite or pyrite, ZnS - zinc blende or sphalerite (wurtzite), PbS - lead luster or galena, HgS - cinnabar, Sb 2 S 3 - stibnite. In addition, sulfur is present in petroleum, natural coal, natural gases and shale. Sulfur is the sixth most abundant element in natural waters; it is found mainly in the form of sulfate ions and causes the “constant” hardness of fresh water. A vital element for higher organisms, an integral part of many proteins, is concentrated in the hair.
What areas of application of sulfur you will learn from this article.
Application areas of sulfur
Sulfur occurs in nature in a free state and in various compounds. It is obtained from native ores. It is also a by-product of the processing of polymetallic ores, complex processing of sulfates, and purification of fossil fuels.
Application of sulfur in industry
The main consumer of sulfur is the chemical industry, which absorbs approximately half of the sulfuric acid produced. It is used to produce black powder, carbon disulfide, various dyes, sparklers and luminous compounds. A significant portion of sulfur is consumed by the paper industry.
In the rubber industry, sulfur is used to turn rubber into rubber. The material acquires the properties of rubber, such as elasticity and resilience, only after mixing with sulfur and heating. This process is called vulcanization. There are two types: hot and cold. During hot vulcanization, rubber with sulfur is heated to 130-160°C. Cold vulcanization takes place without heating; the rubber is treated with sulfur chloride (S 2 C 12).
When 0.5-5% sulfur is added to rubber, soft rubber is obtained, from which car tubes, tires, tubes, and balls are made. If you add 30-50% sulfur to the material, you get a hard, inelastic material - ebonite. It is a solid and an electrical insulator.
Application of sulfur in agriculture carried out in elementary form and in the form of compounds. Plants need sulfur, so sulfur fertilizers are made that increase the quality and quantity of the crop. Sulfur fertilizers help increase the frost resistance of cereals and the formation of organic matter. Sulfur is also used to fight diseases of cotton and grape plants. It is used to fumigate infected granaries, fruit and vegetable stores, and scabies-infected animals.
Use of sulfur in medicine
Sulfur is the basis of ointments that cure fungal skin diseases - scabies, psoriasis, seborrhea. Sulfamide preparations are made from organic sulfur compounds - sulfazole, sulfidine, norsulfazole, streptocide and sulfodimezine. They are also used internally as a laxative and expectorant.
Section 1. Determination of sulfur.
Section 2. Natural minerals sulfur.
Section 3. History of discoverysulfur.
Section 4. Origin of the name sulfur.
Section 5. Origin of sulfur.
Section 6. Receiptsulfur.
Section 7. Manufacturerssulfur.
Section 8. Propertiessulfur.
- Subsection 1. Physicalproperties.
- Subsection2. Chemicalproperties.
Section 10. Fire hazardous properties of sulfur.
- Subsection1. Fires in sulfur warehouses.
Section 11. Being in nature.
Section 12. Biological rolesulfur.
Section 13. Applicationsulfur.
Definitionsulfur
sulfur is element of the sixth group of the third period of the periodic table of chemical elements of D.I. Mendeleev, with atomic number 16. Exhibits non-metallic properties. Denoted by the symbol S (Latin Sulfur). In hydrogen and oxygen compounds it is found in various ions and forms many acids and salts. Many sulfur-containing salts are poorly soluble in water.
Sulfur - S, chemical element with atomic number 16, atomic mass 32.066. The chemical symbol for sulfur S is pronounced "es". Natural sulfur consists of four stable nuclides: 32S (content 95.084% by weight), 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 the neutral sulfur atom from S0 to S6+ are, respectively, 10.36, 23.35, 34.8, 47.3, 72.5 and 88.0 eV. Sulfur is located in the VIA group of D.I. Mendeleev’s periodic table, in the 3rd period, and belongs to the chalcogens. The configuration of the outer electronic layer is 3s23p4. The most characteristic oxidation states in compounds are -2, +4, +6 (valency II, IV and VI, respectively). The Pauling electronegativity value of sulfur is 2.6. Sulfur is a non-metal.
In its free form, sulfur appears as yellow, brittle crystals or yellow powder.
Sulfur is
Natural minerals sulfur
Sulfur is the sixteenth most abundant element in the earth's crust. It is found in a free (native) state and bound form.
The most important natural sulfur compounds: FeS2 - iron pyrite or pyrite, ZnS - zinc blende or sphalerite (wurtzite), PbS - lead luster or galena, HgS - cinnabar, Sb2S3 - stibnite. In addition, sulfur is present in black gold, natural coal, natural gases and shale. Sulfur is the sixth most abundant element in natural waters; it is found mainly in the form of sulfate ions and causes the “constant” hardness of fresh water. A vital element for higher organisms, an integral part of many proteins, is concentrated in the hair.
Sulfur is
History of discoverysulfur
sulfur in its native state, as well as in the form of sulfur compounds, has been known since ancient times. Man probably became familiar with the smell of burning sulfur, the suffocating effect of sulfur dioxide and the disgusting smell of hydrogen sulfide back in prehistoric times. It was because of these properties that sulfur was used by priests as part of sacred incense during religious rites. Sulfur was considered the work 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 flammable mixtures for military purposes. Homer already described “sulphurous fumes,” the deadly effect of burning sulfur emissions. Sulfur was probably part of the “Greek fire” that terrified opponents. Around the 8th century The Chinese began to use it in pyrotechnic mixtures, in particular, in mixtures such as gunpowder. The flammability of sulfur, the ease with which it combines with metals to form sulfides (for example, on the surface of pieces metal), explain the fact that it was considered the “principle of flammability” and an essential component of metal ores. Presbyter Theophilus (12th century) describes a method of oxidative roasting of sulfide copper ore, probably known in ancient Egypt. IN period Arabian alchemy arose the mercury-sulfur theory of composition metals, according to which sulfur was revered as an essential component (father) of all metals. Later it became one of the three principles of alchemists, and later the “principle of flammability” became the basis of the theory of phlogiston. The elemental nature of sulfur was established by Lavoisier in his combustion experiments. With the introduction of gunpowder in Europe, the development of natural sulfur mining began, as well as the development of a method for obtaining it from pyrites; the latter was common in ancient Rus'. It was first described in literature by Agricola. Thus, the exact origin of sulfur has not been established, but, as stated above, this element was used before the birth of Christ, and therefore has been familiar to people since ancient times.
Sulfur occurs in nature in a free (native) state, so it was known to man already in ancient times. Sulfur attracted attention due to its characteristic color, blue flame and specific smell that occurs during combustion (the smell of sulfur dioxide). It was believed that burning sulfur drove away evil spirits. The Bible talks about the use of sulfur to cleanse sinners. For medieval people, the smell of “sulfur” was associated with the underworld. The use of burning sulfur for disinfection is mentioned by Homer. In ancient Rome, fabrics were bleached using sulfur dioxide.
Sulfur has long been used in medicine - patients were fumigated with its flame, it was included in various ointments for the treatment of skin diseases. In the 11th century Avicenna (Ibn Sina), and then European alchemists believed that metals, including silver, consist of sulfur and mercury in different proportions. Therefore, sulfur played an important role in alchemists' attempts to find the "philosopher's stone" and transform base metals into precious ones. In the 16th century Paracelsus considered sulfur, along with mercury and “salt,” one of the main “principles” of nature, the “soul” of all bodies.
The practical importance of sulfur increased sharply after the invention of black gunpowder (which necessarily includes sulfur). In 673, the Byzantines, defending Constantinople, burned the enemy fleet with the help of so-called Greek fire - a mixture of saltpeter, sulfur, resin and other substances - the flame of which was not extinguished by water. In the Middle Ages Europe Black gunpowder was used, the composition of which was close to a mixture of Greek fire. Since then, sulfur has been widely used for military purposes.
The most important sulfur compound, sulfuric acid, has long been known. One of the creators of iatrochemistry, monk Vasily Valentin, in the 15th century described in detail the production of sulfuric acid by calcining iron sulfate (the ancient name for sulfuric acid is oil of vitriol).
The elemental nature of sulfur was established in 1789 by A. Lavoisier. The names of chemical compounds containing sulfur often contain the prefix “thio” (for example, the Na2S2O3 reagent used in photography is called sodium thiosulfate). The origin of this prefix is related to the Greek name for sulfur - theion.
Origin of the name sulfur
The Russian name for sulfur goes back to the Proto-Slavic *sěra, which is associated with Lat. serum "serum".
Latin sulfur (a Hellenized spelling of the older sulpur) comes from the Indo-European root *swelp- “to burn.”
Origin of sulfur
Large accumulations of native sulfur are not very common. It is more often present in some ores. Native sulfur ore is a rock interspersed with pure sulfur.
When were these inclusions formed - simultaneously with the accompanying rocks or later? The direction of prospecting and exploration work depends on the answer to this question. But, despite thousands of years of communication with sulfur, humanity still does not have a clear answer. There are several theories whose authors hold opposing views.
The theory of syngenesis (that is, the simultaneous formation of sulfur and host rocks) suggests that the formation of native sulfur occurred in shallow basins. Special bacteria reduced sulfates dissolved in water to hydrogen sulfide, which rose upward, entered the oxidation zone, and here, chemically or with the participation of other bacteria, was oxidized to elemental sulfur. The sulfur settled to the bottom, and subsequently the sulfur-containing silt formed ore.
The theory of epigenesis (sulfur inclusions formed later than the main rocks) has several options. The most common of them assumes that groundwater, penetrating through rock strata, is enriched with sulfates. If such waters come into contact with deposits black gold or Natural gas, then sulfate ions are reduced by hydrocarbons to hydrogen sulfide. Hydrogen sulfide rises to the surface and, when oxidized, releases pure sulfur in the voids and cracks of rocks.
In recent decades, one of the varieties of the theory of epigenesis has found more and more confirmation - the theory of metasomatosis (translated from Greek “metasomatosis” means replacement). According to it, the transformation of gypsum CaSO4-H2O and anhydrite CaSO4 into sulfur and calcite CaCO3 constantly occurs in the depths. This theory was created in 1935 by Soviet scientists L. M. Miropolsky and B. P. Krotov. In particular, this fact speaks in its favor.
Mishraq was discovered in Iraq in 1961. The sulfur here is contained in carbonate rocks, which form an arch supported by pillars going deep (in geology they are called wings). These wings consist mainly of anhydrite and gypsum. The same picture was observed at the domestic Shor-Su field.
The geological originality of these deposits can only be explained from the standpoint of the theory of metasomatism: primary gypsum and anhydrites turned into secondary carbonate ores interspersed with native sulfur. It's not just the neighborhood that matters minerals— the average sulfur content in the ore of these deposits is equal to the content of chemically bound sulfur in anhydrite. And studies of the isotopic composition of sulfur and carbon in the ore of these deposits gave supporters of the theory of metasomatism additional arguments.
But there is one “but”: the chemistry of the process of converting gypsum into sulfur and calcite is not yet clear, and therefore there is no reason to consider the theory of metasomatism the only correct one. There are still lakes on earth (in particular, Sernoye Lake near Sernovodsk), where syngenetic deposition of sulfur occurs and the sulfur-bearing silt contains neither gypsum nor anhydrite.
All this means that the variety of theories and hypotheses about the origin of native sulfur is the result not only and not so much of the incompleteness of our knowledge, but of the complexity of the phenomena occurring in subsoil. We all know from elementary school mathematics that different paths can lead to the same result. This extends to geochemistry as well.
Receiptsulfur
sulfur is obtained mainly by smelting native sulfur directly in places where it occurs underground. Sulfur ores are mined in different ways, depending on the conditions of occurrence. Sulfur deposits are almost always accompanied by accumulations of poisonous gases - sulfur compounds. In addition, we must not forget about the possibility of its spontaneous combustion.
Open pit mining of ore occurs like this. Walking excavators remove layers of rock under which ore lies. The ore layer is crushed by explosions, after which the ore blocks are sent to a sulfur smelter, where sulfur is extracted from the concentrate.
In 1890, Hermann Frasch proposed melting sulfur underground and pumping it to the surface through oil wells. The relatively low (113°C) melting point of sulfur confirmed the reality of Frasch’s idea. In 1890, tests began that led to success.
There are several known methods for obtaining sulfur from sulfur ores: steam-water, filtration, thermal, centrifugal and extraction.
Sulfur is also found in large quantities in Natural gas in a gaseous state (in the form of hydrogen sulfide, sulfur dioxide). During mining, it is deposited on the walls of pipes and equipment, rendering them inoperable. Therefore, it is recovered from the gas as quickly as possible after production. The resulting chemically pure fine sulfur is an ideal raw material for the chemical and rubber industries.
The largest deposit of native sulfur of volcanic origin is located on the island of Iturup with reserves of category A+B+C1 - 4227 thousand tons and category C2 - 895 thousand tons, which is enough to build an enterprise with a capacity of 200 thousand tons of granulated sulfur per year.
Manufacturerssulfur
The main producers of sulfur in the Russian Federation are enterprises OJSC Gazprom: LLC Gazprom Dobycha Astrakhan and LLC Gazprom Dobycha Orenburg, receiving it as a by-product during gas purification.
Propertiessulfur
1) Physical
sulfur differs significantly from oxygen in its ability to form stable chains and cycles of atoms. The most stable are the crown-shaped cyclic S8 molecules, which form orthorhombic and monoclinic sulfur. This is crystalline sulfur - a brittle yellow substance. In addition, molecules with closed (S4, S6) chains and open chains are possible. This composition has plastic sulfur, a brown substance, which is obtained by sharp cooling of molten sulfur (plastic sulfur becomes brittle after a few hours, acquires a yellow color and gradually turns into rhombic). The formula for sulfur is most often written simply 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 and turpentine. The melting of sulfur is accompanied by a noticeable increase in volume (approximately 15%). Molten sulfur is a yellow, easily 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 again becomes mobile. This is because when sulfur is heated, it gradually polymerizes, increasing the length of the chain as the temperature increases. When sulfur is heated above 190 °C, the polymer units begin to collapse. Sulfur can serve as the simplest example of an electret. When rubbed, sulfur acquires a strong negative charge.
Sulfur is used for the production of sulfuric acid, rubber vulcanization, as a fungicide in agriculture and as colloidal sulfur - a medicinal product. Also, sulfur in sulfur bitumen compositions is used to produce sulfur asphalt, and as a substitute for Portland cement to produce sulfur concrete.
2) Chemical
Burning sulfur
In air, sulfur burns, forming sulfur dioxide - a colorless gas with a pungent odor:
Using spectral analysis, it was established that in fact process The oxidation of sulfur into dioxide is a chain reaction and occurs with the formation of a number of intermediate products: sulfur monoxide S2O2, molecular sulfur S2, free sulfur atoms S and free radicals sulfur monoxide SO.
In addition to oxygen, sulfur reacts with many non-metals, however, at room temperature, sulfur reacts only with fluorine, exhibiting reducing properties:
Molten sulfur reacts with chlorine, and the formation of two lower chlorides is possible:
2S + Cl2 = S2Cl2
When heated, sulfur also reacts with phosphorus, apparently forming a mixture of phosphorus sulfides, among which is the higher sulfide P2S5:
In addition, when heated, sulfur reacts with hydrogen, carbon, silicon:
S + H2 = H2S (hydrogen sulfide)
C + 2S = CS2 (carbon disulfide)
When heated, sulfur interacts with many metals, often quite violently. Sometimes a mixture of metal and sulfur ignites when ignited. This interaction produces sulfides:
2Al + 3S = Al2S3
Solutions of alkali metal sulfides react with sulfur to form polysulfides:
Na2S + S = Na2S2
Of the complex substances, noteworthy first of all is the reaction of sulfur with molten alkali, in which sulfur is disproportionately similar to chlorine:
3S + 6KOH = K2SO3 + 2K2S + 3H2O
The resulting melt is called sulfur liver.
Sulfur reacts with concentrated oxidizing acids (HNO3, H2SO4) only during prolonged heating, oxidizing:
S + 6HNO3(conc.) = H2SO4 + 6NO2 + 2H2O
S + 2H2SO4(conc.) = 3SO2 + 2H2O
Sulfur is
Sulfur is
Fire hazardous properties of sulfur
Finely ground sulfur is prone to chemical spontaneous combustion in the presence of moisture, upon contact with oxidizing agents, and also in a mixture with coal, fats, and oils. Sulfur forms explosive mixtures with nitrates, chlorates and perchlorates. Spontaneously ignites on contact with bleach.
Extinguishing agents: sprayed water, air-mechanical foam.
According to V. Marshall, sulfur dust is classified as explosive, but for an explosion a sufficiently high concentration of dust is required - about 20 g/m3 (20,000 mg/m3), this concentration is many times higher than the maximum permissible concentration for humans in the air of a working area - 6 mg /m3.
Vapors form an explosive mixture with air.
The combustion of sulfur occurs only in a molten state, similar to the combustion of liquids. The top layer of burning sulfur boils, creating vapors that form a dimly luminous flame up to 5 cm high. The flame temperature when burning sulfur is 1820 °C.
Since air by volume consists of approximately 21% oxygen and 79% nitrogen, and when sulfur burns, one volume of oxygen produces one volume of SO2, the maximum theoretically possible SO2 content in the gas mixture is 21%. In practice, combustion occurs with some excess air, and the volumetric SO2 content in the gas mixture is less than theoretically possible, usually amounting to 14...15%.
Detection of sulfur combustion by fire automatics is a difficult problem. The flame is difficult to detect with the human eye or a video camera; the spectrum of blue flame lies mainly in the ultraviolet range. Combustion occurs at low temperature. To detect combustion with a heat detector, it must be placed directly close to the sulfur. Sulfur flame does not emit infrared radiation. Thus, it will not be detected by common infrared detectors. They will only detect secondary fires. A sulfur flame does not release water vapor. Therefore, UV flame detectors that use nickel compounds will not work.
To comply with fire safety requirements at sulfur warehouses, it is necessary:
Structures and technological equipment must be regularly cleaned of dust;
The warehouse premises must be constantly ventilated by natural ventilation with the doors open;
Crushing sulfur lumps on the bunker grate should be done with wooden sledgehammers or tools made of non-sparking material;
Conveyors for supplying sulfur to production premises must be equipped with metal detectors;
In places where sulfur is stored and used, it is necessary to provide devices (sides, thresholds with a ramp, etc.) that ensure in an emergency the prevention of the spreading of molten sulfur outside the room or open area;
At the sulfur warehouse it is prohibited:
Production of all types works using open fire;
Store and store oily rags and rags;
When making repairs, use tools made of non-sparking material.
Fires in sulfur warehouses
In December 1995, at an open sulfur warehouse enterprises, located in the city of Somerset in the Western Cape Province of the Republic of South Africa, a large fire occurred, killing two people.
On January 16, 2006, at about five in the evening, a warehouse with sulfur caught fire at the Cherepovets enterprise “Ammofos”. The total area of the fire is about 250 square meters. It was possible to completely eliminate it only at the beginning of the second night. There are no casualties or injuries.
On March 15, 2007, early in the morning at Balakovo Fiber Materials Plant LLC, a fire occurred in a closed sulfur warehouse. The fire area was 20 sq.m. There were 4 fire crews with 13 personnel working on the fire. After about half an hour, the fire was extinguished. No harm done.
On March 4 and 9, 2008, a sulfur fire occurred in the Atyrau region in the TCO sulfur storage facility at the Tengiz field. In the first case, the fire was extinguished quickly; in the second case, the sulfur burned for 4 hours. The volume of burned oil refining waste, which according to Kazakhstan laws attributed to sulfur, amounted to more than 9 thousand kilograms.
In April 2008, not far from the village of Kryazh, Samara region, a warehouse in which 70 tons of sulfur was stored caught fire. The fire was assigned the second category of complexity. 11 fire brigades and rescuers went to the scene of the incident. At that moment, when firefighters found themselves near the warehouse, not all of the sulfur was burning, but only a small part of it - about 300 kilograms. The area of the fire, including areas of dry grass adjacent to the warehouse, amounted to 80 square meters. Firefighters managed to quickly put out the flames and localize the fire: the fires were covered with earth and filled with water.
In July 2009, sulfur burned in Dneprodzerzhinsk. A fire occurred at one of the coke-chemical plants in the Bagleysky district of the city. The fire consumed more than eight tons of sulfur. None of the plant employees were injured.
Being in naturesulfur
WITH The era is quite widespread in nature. In the earth's crust its content is estimated at 0.05% by mass. In nature there are often significant deposits native sulfur (usually near volcanoes); V Europe they are located in the south of Italy, in Sicily. Even bigger deposits native sulfur is available in the USA (in the states of Louisiana and Texas), as well as in Central Asia, Japan, and Mexico. In nature, sulfur is found both in bulk and in the form of crystalline layers, sometimes forming amazingly beautiful groups of translucent yellow crystals (the so-called druses).
In volcanic areas, hydrogen sulfide gas H2S is often released from the ground; in these same regions, hydrogen sulfide is found dissolved in sulfuric waters. Volcanic gases often also contain sulfur dioxide SO2.
Deposits of various sulfide compounds are widespread on the surface of our planet. The most common among them are: iron pyrite (pyrite) FeS2, copper pyrite (chalcopyrite) CuFeS2, lead luster PbS, cinnabar HgS, sphalerite ZnS and its crystalline modification wurtzite, stibnite Sb2S3 and others. Numerous deposits of various sulfates are also known, for example, calcium sulfate (gypsum CaSO4 2H2O and anhydrite CaSO4), magnesium sulfate MgSO4 (bitter salt), barium sulfate BaSO4 (barite), strontium sulfate SrSO4 (celestine), sodium sulfate Na2SO4 10H2O (mirabilite ) and etc.
Hard coals contain an average of 1.0-1.5% sulfur. Sulfur may also be part of black gold. A number of natural combustible gas fields (for example, Astrakhan) contain hydrogen sulfide as an impurity.
Sulfur is one of the elements that are essential for living organisms, as it is an essential component of proteins. Proteins contain 0.8-2.4% (by weight) of chemically bound sulfur. Plants obtain sulfur from sulfates found in the soil. Unpleasant odors arising from rotting animal corpses are mainly explained by the release of sulfur compounds (hydrogen sulfide and mercaptans) formed during the decomposition of proteins. Sea water contains about 8.7·10-2% sulfur.
Receiptsulfur
WITH Sulfur is obtained mainly by smelting it from rocks containing native (elemental) sulfur. The so-called geotechnological method makes it possible to obtain sulfur without raising ore to the surface. This method was proposed at the end of the 19th century by the American chemist G. Frasch, who was faced with the task of extracting sulfur from the deposits of the south to the surface of the earth USA, where the sandy soil greatly complicated its extraction using the traditional mine method.
Frasch proposed using superheated water vapor to lift sulfur to the surface. Superheated steam is fed through a pipe into an underground layer containing sulfur. The sulfur melts (its melting point is slightly below 120°C) and rises to the top through a pipe located inside the one through which water vapor is pumped underground. In order to ensure the rise of liquid sulfur, compressed air is pumped through the thinnest inner tube.
According to another (thermal) method, which became especially widespread at the beginning of the 20th century in Sicily, sulfur is smelted, or sublimated, from crushed rock in special clay ovens.
There are other methods for separating native sulfur from rock, for example, by extraction with carbon disulfide or flotation methods.
Due to the fact that the need industry in sulfur is very high, methods have been developed for its production from hydrogen sulfide H2S and sulfates.
The method of oxidizing hydrogen sulfide to elemental sulfur was first developed in Great Britain, where they learned to obtain significant amounts of sulfur from the Na2CO3 remaining after the production of soda using the method of the French chemist N. Leblanc of calcium sulfide CaS. Leblanc's method is based on the reduction of sodium sulfate with coal in the presence of limestone CaCO3.
Na2SO4 + 2C = Na2S + 2CO2;
Na2S + CaCO3 = Na2CO3 + CaS.
The soda is then leached with water, and the aqueous suspension of poorly soluble calcium sulfide is treated with carbon dioxide:
CaS + CO2 + H2O = CaCO3 + H2S
The resulting hydrogen sulfide H2S mixed with air is passed in a furnace over a catalyst bed. In this case, due to the incomplete oxidation of hydrogen sulfide, sulfur is formed:
2H2S + O2 = 2H2O +2S
A similar method is used to obtain elemental sulfur from hydrogen sulfide accompanying natural gases.
Since modern technology requires high-purity sulfur, effective methods for refining sulfur have been developed. In this case, in particular, differences in the chemical behavior of sulfur and impurities are used. Thus, arsenic and selenium are removed by treating sulfur with a mixture of nitric and sulfuric acids.
Using methods based on distillation and rectification, it is possible to obtain high-purity sulfur with an impurity content of 10-5 - 10-6% by weight.
Applicationsulfur
ABOUT about half of the sulfur produced is used for the production of sulfuric acid, about 25% is spent to produce sulfites, 10-15% is used to control pests of agricultural crops (mainly grapes and cotton) (the solution of copper sulfate CuSO4 5H2O is of greatest importance here), about 10% used rubber industry for rubber vulcanization. Sulfur is used in the production of dyes and pigments, explosives (it is still part of gunpowder), artificial fibers, and phosphors. Sulfur is used in the production of matches, as it is part of the composition from which match heads are made. Some ointments that are used to treat skin diseases still contain sulfur. To give steels special properties, small additions of sulfur are introduced into them (although, as a rule, an admixture of sulfur in steels undesirable).
Biological rolesulfur
WITH era is constantly present in all living organisms, being an important biogenic element. Its content in plants is 0.3-1.2%, in animals 0.5-2% (marine organisms contain more sulfur than terrestrial ones). The biological significance of sulfur is determined primarily by the fact that it is part of the amino acids methionine and cysteine and, consequently, in the composition of peptides and proteins. Disulfide bonds -S-S- in polypeptide chains are involved in the formation of the spatial structure of proteins, and sulfhydryl groups (-SH) play an important role in the active centers of enzymes. In addition, sulfur is included in the molecules of hormones and important substances. A lot of sulfur is contained in the keratin of hair, bones, and nervous tissue. Inorganic sulfur compounds are necessary for the mineral nutrition of plants. They serve as substrates for oxidative reactions carried out by sulfur bacteria common in nature.
The body of an average person (body weight 70 kg) contains about 1402 g of sulfur. The daily requirement of an adult for sulfur is about 4.
However, in terms of its negative impact on the environment and humans, sulfur (more precisely, its compounds) is one of the first places. The main source of sulfur pollution is the combustion of coal and other fuels containing sulfur. At the same time, about 96% of the sulfur contained in the fuel enters the atmosphere in the form of sulfur dioxide SO2.
In the atmosphere, sulfur dioxide is gradually oxidized to sulfur oxide (VI). Both oxides - sulfur oxide (IV) and sulfur oxide (VI) - react with water vapor to form an acidic solution. These solutions then fall out in the form of acid rain. Once in the soil, acidic water inhibits the development of soil fauna and plants. As a result, unfavorable conditions are created for the development of vegetation, especially in the northern regions, where chemical pollution is added to the harsh climate. As a result, forests are dying, grass cover is being destroyed, and the condition of water bodies is deteriorating. Acid rain destroys monuments made of marble and other materials; moreover, they cause the destruction of even stone buildings and trade items from metals. Therefore, it is necessary to take various measures to prevent the release of sulfur compounds from fuel into the atmosphere. To do this, petroleum products are purified from sulfur compounds and the gases generated during fuel combustion are purified.
Sulfur itself in the form of dust irritates mucous membranes and respiratory organs and can cause serious illnesses. The maximum permissible concentration of sulfur in the air is 0.07 mg/m3.
Many sulfur compounds are toxic. Particularly noteworthy is hydrogen sulfide, inhalation of which quickly dulls the reaction to its unpleasant odor and can lead to severe poisoning, even death. The maximum permissible concentration of hydrogen sulfide in the air of working premises is 10 mg/m3, in atmospheric air 0.008 mg/m3.
Sources Great Medical Encyclopedia
SULFUR- chem. element, symbol S (lat. Sulfur), at. n. 16, at. m. 32.06. Exists in the form of several allotropic modifications; among them are sulfur of the monoclinic modification (density 1960 kg/m3, tmelt = 119°C) and orthorhombic sulfur (density 2070 kg/m3, ίπι = 112.8... ... Big Polytechnic Encyclopedia
SULFUR- (denoted S), a chemical element of group VI of the PERIODIC TABLE, a non-metal, known since antiquity. Occurs in nature both as a separate element and in the form of sulfide minerals such as GALENITE and PYRITE, and sulfate minerals,... ... Scientific and technical encyclopedic dictionary
sulfur- In the mythology of the Irish Celts, Sera is the father of Parthalon (see chapter 6). According to some sources, it was Sera, and not Parthalon, who was Dilgneid's husband. (