Who discovered sulfur. Physical and chemical properties of sulfur. Common signs and differences chalcogen.

It is widely distributed in nature, in the free state or in combination. In its free state it mixes with gypsum and pumice in volcanic areas in Iceland, Sicily, Mexico and Japan. Free sulfur can be formed by the natural decay of pyrite precipitated by hot sulfur waters, in which hydrogen sulfide has been oxidized in the atmosphere.

When ordinary sulfur is melted, it forms a straw liquid, which darkens when heated and then boils. When molten sulfur cools slowly, its physical properties change depending on temperature, pressure, and precipitation regime. Thus, sulfur exists in various forms, called allotropic varieties, which consist of liquids.

It is moderately soluble in alcohol and ether and moderately soluble in oil. The temperature at which rhombic and monoclinic sulfur are in equilibrium, i.e. 94, 5 ° C, is the transition temperature. Sulfur is chemically similar to oxygen and can be substituted in many combinations, but sulfur is less electronic.

In Sicily, sulphurous rocks are piled on the ground and burned. The resulting liquid sulfur is poured into a series of wooden forms in which it solidifies. Then it can be purified by distillation. Sulfur is mainly used in the production of compounds such as sulfuric acid, sulphides, sulphates and sulfur dioxide. Sulfur is widely used in sulfamide-based preparations and in many dermatological ointments. Sulfur is also used in the manufacture of matches, vulcanized rubber, dyes and gunpowder. In a finely divided state and often mixed with lime, it is used as a fungicide for plants.

Potassium and ammonium sulfates are used as fertilizers, and together with various inert mineral charges, sulfur forms a special cement used to anchor metal objects, such as fences and chains made of stone. Sulfuric acid is one of the most important industrial chemicals, since it is used not only for the synthesis of sulfur-containing molecules, but also for the production of many other compounds.

At a time when everyone talks about microelements, sulfur is often forgotten. It is important to recall some common facts and evidence of sulfur. Fumaroles that are mainly deposited in volcanic zones, precipitating sulfur crystals, are very fragrant, highly flammable, therefore its use in the production of gunpowder, sulfur is demographic culturally, and yet we find that sulfur is of paramount importance to life.

Some very original chemical communities. Sulfur is a simple chemical non-metallic, acidic, light yellow. After its crystallization, it has an aspect. Glossy and translucent matte and opaque. . Very loose, it has several melting points with amazing features.

Sulfur reacts with most other elements to form sulfates or sulphides. It is mixed with carbon hydrocarbons and natural gas. Sulfur due to its acidic nature is ideal for the production of various acids: sulfuric acid, sulfuric acid, widely used in all industries.

Sulfur at the beginnings of life. Sulfur is vital, it, besides the origin of life, on the other hand, its derivatives can be very toxic or even mortal. Sulfur - acid, life too. Present in all proteins of living organisms, thanks to sulfur in albumin, the water of our body remains structured. Without sulfur, we would be only a meadow.

There is more sulfur in the blood than iron, and when you know very specific chemical relationships between these two elements, it would be interesting to use sulfur in case of anemia or hemochromatosis. The effect of a gray stone massage on the liver should quickly resolve this disorder around the iron.

Sulfur, regulator of the skin and lungs. Due to its acidic nature, sulfur contained in the skin provides the boundary between the internal environment of the body and the external environment, which can be subjected to various types of attacks. We find sulfur in abundance in keratin, the main protective protein of the skin.

Similarly, sulfur will be "protective" from the lungs. However, this is not about sulfur inhalation. A simple daily massage of the chest will relieve many chronic respiratory problems. Moreover, people with chronic epidermal or pulmonary disorders do not regularly go to sanatorium-resort treatment, where they have very sulfuric water treatment to get rid of their sufferings.

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One solid body, not metallic, of lemon yellow color. Sulfur exists in two crystalline forms. The resulting cold by evaporation of its solutions is represented in the octahedra of the orthorhombic system, the density is 2. 06; by melting molten sulfur, it crystallizes in the needles of the monoclinic density system 1.

Soft sulfur is a brown, pasty and elastic solid obtained by pouring molten sulfur into cold water at its boiling point. Sulfur is in a natural state near ancient volcanoes, which is 0.06% of the lithosphere. Most often it is combined with metals, and sulphides of iron, copper, lead, zinc are important minerals of these metals. Purified, it is used in the production of black powder and fireworks.

It is also used for making matches, curing rubber and making ebonite. Sulfur is used internally as a mild laxative and in external applications for its antiparasitic, keratolytic and antiseborrheic properties. An element with a sulphurous reputation?

Sulfur is in the standard state of a yellow solid, odorless, tasteless, insoluble in water, with poor mechanical properties, a very poor conductor and diamagnetic. Sulfur exists in molecular form. It is in a state of powder: a flower of sulfur, which is obtained by sublimation.

Molded block: sulfur in the barrel; as well as in aggregate. It is possible to obtain colloidal sulfur or sulfuric milk, as well as plastic sulfur and various amorphous forms of sulfur by quenching molten sulfur. Sulfur has a wide range of allotropic forms.

The place of sulfur in the periodic classification is the electronic configuration. Its atomic number is 16; It is classified as non-metal. Column 16 Representation: Oxygen Family. Sulfur reacts quite easily with many elements of the periodic table, both with metals and non-metals.

Like oxygen, sulfur has an oxidation state of -2 and gives sulfides. Since sulfur is less electronegative than oxygen, it also has oxidation states 4, 6 with more electronegative elements. Other oxidation states are possible: for example, 1, but also 2, 2 and 3 in the case of tetrathionate ion 3, 5, 7. Frost diagram. However, many of these compounds can be considered to be formed by combinations of sulfur atoms in oxidation states of 4 or 6 and sulfur atoms in the 0, -2, or -1 oxidation stages.

For example: a thiosulfate ion, in which one of the sulfate oxygen atoms is replaced by a sulfur atom, has two sulfur atoms, the oxidation numbers of which are different - "4, 0" or 6, -2 depending on how the electrons are counted. The property of concatenation of sulfur makes it difficult to determine the amount of oxidation of the sulfur atom in molecules and formed ions.

Sulfur has many compounds where the byte rule no longer applies. Sulfur, which is more voluminous than oxygen, can accommodate more neighbors. Atomic properties, isotopes. There are four natural isotopes, all stable. Several artificial sulfur isotopes are known.

Appearance and abundance and achievement. Sulfur is in its natural state, near volcanoes or in natural sediments in the open air or underground. But also in the form of sulphides and sulphates of metals: cinnabar, galena, opium, barite, gypsum, etc. Removal of natural gas and oil desulfurization.

Exploitation of sulfur deposits in a natural state. The most important use of sulfur is the production of sulfuric acid. Sulfur is a fungicide used for viticulture and horticulture. Vulcanization of natural rubber always uses a significant amount of sulfur.

Carbon disulfide is produced by the interaction of sulfur with methane. We also mention the sulfur-sodium electrochemical cells, the storage capacity of which is the main event today. Basic sulfur compounds and some of their uses. Sulphuric acid: neutralization, leaching, production of hydrofluoric acid, production of titanium dioxide, lead batteries, metal etching, dehydration of alcohols, paraffin paper, etc.

Ferrous sulfate or green vitriol. Calcium hydrogen sulfite. Organic compounds containing sulfur: thiols, thioethers, and the like; They are widely used in the pharmaceutical and agrochemical industry. The element is gray and alive. Sulfur is one of the indispensable elements in life.

It is found in two essential amino acids: cysteine ​​and methionine, but also in homocysteine ​​and taurine. Enzymes owe their configuration to "disulfide" bridges, which lead to protein bending on themselves. When the bread “rises”, it is obliged to them to “disulfide” bridges of the cysteine-cystine pair, also responsible for the undulation of the hair.

They are still found in the oceans near volcanic faults. The history of the discovery of the element sulfur. Sulfur is one of the nine known elements from antiquity. This is cited in the Old Testament. It is used for cosmetic, therapeutic purposes. Sulfur is also mentioned in Homer's Odyssey upon returning to Ithaca; Sulfur had the ability to remove pests!