Stibnium | Article about Stibnium by The Free Dictionary Stibnium | Article about Stibnium by The Free Dictionary Also found in: Dictionary , Thesaurus , Medical , Legal , Wikipedia . antimony (ăn`tĭmō'nē) [Lat. antimoneum], semimetallic chemical element; symbol Sb [Lat. stibium,=a mark]; at. no. 51; at. wt. 121.760; m.p. 630.74&degC;; b.p. 1,750&degC;; sp. gr. (metallic form) 6.69 at 20&degC;; valence 0, +3, −3, or +5. Antimony exists in two allotropic forms (see allotropy allotropy [Gr.,=other form]. A chemical element is said to exhibit allotropy when it occurs in two or more forms in the same physical state; the forms are called allotropes. ..... Click the link for more information. ); the more common is silvery blue-white and has a rhombohedral crystalline structure.

It is a poor conductor of heat and electricity and is brittle and easily powdered. It is primarily used in alloys and chemical compounds. It is a member of Group 15 of the periodic table periodic table, chart of the elements arranged according to the periodic law discovered by Dmitri I. Mendeleev and revised by Henry G. J. Moseley. In the periodic table the elements are arranged in columns and rows according to increasing atomic number (see the table entitled ..... Click the link for more information. . Antimony rarely occurs free in nature, but its ores are widely distributed. The principal ore is stibnite stibnite , antimony sulfide, Sb2S3, a mineral, silvery gray in color, with a metallic luster. It crystallizes in the orthorhombic system. Found in many parts of the world, it is the most important ore of antimony. ..... Click the link for more information. , a sulfur compound known since early times; there are extensive deposits in China. Antimony is often found in other ores as well, e.g., silver, copper, and lead.

The pure element antimony is produced from the ore by roasting it to form the oxide, then reducing the oxide with carbon or iron; often a flux of sodium sulfate or sodium carbonate is used to prevent loss of molten antimony by evaporation. Antimony does not react with air or water at room temperature; it does react with fluorine, chlorine, or bromine and is soluble in hot nitric or sulfuric acid; at higher temperatures, antimony will ignite and burn in air. It unites with hydrogen to form stibine, a poisonous gas. In combination with metals antimony forms alloys that are hard and brittle and have low melting points. The alloys of antimony include britannia metal britannia metal, silvery-white alloy of tin with antimony, copper, and sometimes bismuth and zinc. It is very similar in appearance to pewter, but is harder. It is used widely for the manufacture of tableware. ..... Click the link for more information. , type metal type metal, alloy of lead with antimony, tin, and sometimes copper, so named because of its one time extensive use for making printing type.

Expanding upon solidification, the alloy takes a fine and clear impression of the mold in which it hardens. It has a low melting point. ..... Click the link for more information. , Babbitt metal Babbitt metal, an antifriction metal first produced by Isaac Babbitt in 1839. In present-day usage the term is applied to a whole class of silver-white bearing metals, or "white metals. ..... Click the link for more information. , and sometimes pewter pewter, any of a number of ductile, silver-white alloys consisting principally of tin. The properties vary with the percentage of tin and the nature of the added materials. ..... Click the link for more information. ; these alloys expand on cooling, thereby retaining fine details of a mold. Alloys and compounds of antimony are used in bearings, storage batteries, safety matches, and as a red pigment in paint. Although antimony and many of its compounds are toxic, tartar emetic tartar emetic, poisonous, odorless, transparent rhombic crystals or white powder with a metallic, sweetish taste.

Chemically, it is potassium antimony tartrate, KSbC4H4O7· 1-2H2O. It is used as a mordant in dyeing. ..... Click the link for more information. (potassium antimonyl tartrate), meglumine antimoniate, sodium stibogluconate, and other compounds are used as medicines. Small concentrations of antimony can be detected by a method similar to the Marsh test Marsh test, method for the detection of arsenic, so sensitive that it can be used to detect minute amounts of arsenic in foods (the residue of fruit spray) or in stomach contents. The sample is placed in a flask with arsenic-free zinc and sulfuric acid. ..... Click the link for more information. for arsenic. Antimony is mixed with soot and other substances to make kohl, used for centuries by women in some countries as an eye cosmetic. A method for the extraction of antimony from stibnite was first described c.1600 by Basilius Valentinus. Although known to the ancients, the element was first adequately described by Nicolas Lémery in 1707.

Antimony Sb, a chemical element in group V of Mendeleev’s periodic system. Atomic number, 51; atomic weight, 121.75. Antimony is a silvery white metal with a blue tinge. In nature, two stable isotopes are known: 121Sb (57.25 percent) and 123Sb (42.75 percent). The most important of the element’s artificial radioisotopes are 122Sb (half-life 2.8 days), 124Sb (half-life 60.2 days), and 125Sb (half-life two years). History. Antimony has been known since antiquity. In the Orient, it was used around 3000 B.C. in making various vessels. In Egypt, as early as the 19th century B.C. , powdered antimony glance (natural Sb2S3, called mesten or stem) was used for darkening eyebrows. In ancient Greece, the powder was known as stimi or stibi, hence the Latin stibium.

The name antimonium came into use sometime between the 12th and 14th centuries A.D. In 1789, A. Lavoisier included antimony in his list of chemical elements, using the French name antimoine (antimonio in Spanish and Italian, Antimon in German). The Russian name for the element, sur’ma, is derived from the Turkish sürme, the term for powdered lead glance (PbS), also used for darkening eyebrows. (According to some sources, sur’ma is derived from a Persian word meaning metal.) A detailed description of the properties and methods of obtaining antimony was first given by the alchemist Basil Valentine in 1604 in Germany. Distribution in nature. The average content of antimony in the earth’s crust (clarke) is 5 × 10–5 percent by weight. Antimony is dispersed in magma and in the biosphere. It is contained in hot groundwater, forming concentrations in hydrothermal deposits. Antimony deposits as such are known, as are antimony-mercury, antimony-lead, gold-antimony, and antimony-tungsten deposits.

Of the 27 antimony minerals, antimonite (Sb2S3) has the greatest industrial importance. Because of its affinity for sulfur, antimony is often encountered as an admixture in the sulfides of arsenic, bismuth, nickel, lead, mercury, silver, and other elements. Physical and chemical properties. Antimony is known in a crystalline form and in three amorphous forms—explosive, black, and yellow. Explosive antimony, with a density of 5.64–5.97 g/cm3, explodes upon contact; it is produced in the electrolysis of a solution of SbCl3. Black antimony, with a density of 5.3 g/cm3, is formed through the rapid cooling of antimony vapors, and yellow antimony is formed by passing oxygen through liquefied SbH3. The yellow and black forms are unstable and convert into the crystalline form at reduced temperatures.

Crystalline antimony, which is the most stable form, crystallizes in the trigonal system (a = 4.5064 angstroms); this form has a density of 6.61–6.73 g/cm3 (liquid, 6.55 g/cm3), a melting point of 630.5°C, a boiling point of 1635°–1645°C, a specific heat at 20°–100°C of 0.210 kilojoule/kg· °K (0.0498 calorie/g· °C), and a thermal conductivity at 20°C of 17.6 watts/m· °K (0.042 calorie/cm· sec · °C).

The linear coefficient of expansion of polycrystalline antimony is 11.5 × 10–6 at 0°–100°C; for a single crystal in the temperature range 0°–400°C, α1 = 8.1 x 10–6 and α2 = 19.5 × 10–6, and the electrical resistivity of a single crystal of antimony at 20°C is 43.045 × 10–6 ohm·cm. Antimony is diamagnetic, with a magnetic susceptibility of –0.66 × 10–6. In contrast to most metals, antimony is brittle and is easily split along cleavage planes; it can be ground into a powder. It is not forgeable and consequently is sometimes classified as a semimetal. Mechanical properties depend on the purity of the metal.

The Brinell hardness of cast antimony is 325–340 meganewtons/m2 (32.5–34.0 kilograms-force/mm2), the modulus of elasticity is 285–300, and the ultimate strength is 86.0 meganewtons/m2 (8.6 kilograms-force/mm2). The configuration of the outer electrons of the antimony atom is 5s25p3. In compounds, antimony has oxidation states of +5, +3, and –3. Antimony has relatively low chemical reactivity. It does not undergo oxidation in the air at temperatures ranging up to its melting point, and it does not react with nitrogen and hydrogen. Carbon dissolves to only a slight extent in molten antimony. The metal reacts vigorously with chlorine and other halogens to form antimony halides. It reacts with oxygen at temperatures above 630°C, forming Sb2O3. Antimony sulfides are obtained when antimony is melted in the presence of sulfur; antimony reacts similarly with phosphorus and arsenic. Antimony is stable in relation to water and dilute acids.

Concentrated hydrochloric and sulfuric acids slowly dissolve antimony with the formation of the chloride SbCl3 and the sulfate Sb2(SO4)3; concentrated nitric acid oxidizes antimony to a higher oxide, which takes the form of the hydrate xSb2O5·yH2O. The difficultly soluble salts of antimonic acid have practical importance. They include antimonates (MSbO3·3H2O, where Me is Na or K) and the salts of meta-antimonous acid (not yet isolated in pure form), namely, meta-antimonates (MeSbO2·3H2O), which possess reducing properties. Antimony combines with metals to form antimonides. Production. Antimony is obtained by the pyrometallurgical and hydrometallurgical treatment of concentrates or from ore containing 20–60 percent Sb. The pyrometallurgical methods include precipitation smelting and reduction smelting.

Sulfide concentrates serve as the raw material for precipitation smelting, which is based on the replacement of antimony in the sulfide by iron: Sb2S3 + 3Fe ⇄ 2Sb + 3FeS. The iron is introduced into the charge as scrap, and the smelting is carried out in reverberatory or short rotating furnaces at 1300°–1400°C. The extraction of antimony in the form of crude metal exceeds 90 percent. The reduction smelting of antimony is based on the reduction of antimony oxides to the metal using charcoal or coal dust and on the slagging of waste rock. Reduction smelting is preceded by oxidative roasting at 550°C with an excess of air. The calcine contains the nonvolatile tetroxide of antimony. Electric furnaces can be used in both precipitation and reduction smelting.

The two stages involved in the hydrometallurgical process of obtaining antimony are the treatment of the raw material with an alkaline sulfide solution, which results in the entry of antimony into solution as sul-fosalts and salts of antimonic acids, and the separation of antimony by electrolysis. Depending on the composition of the raw material and the method of production, crude antimony contains 1.5 to 15 percent impurities, for the most part Fe, As, and S. Pyrometallurgical or electrolytic refining is used to produce pure antimony. In pyrometallurgical refining, impurities of iron and copper are removed as sulfur compounds by introducing antimonite (Sb2S3); arsenic (as sodium arsenate) and sulfur are then removed by passing air under the soda slag. In electrolytic refining with a soluble anode, crude antimony is purified of iron, copper, and other metals remaining in the electrolyte (with Cu, Ag, and Au remaining in the slurry. A solution consisting of SbF3, H2SO4, and HF serves as the electrolyte.

The content of impurities in refined antimony does not exceed 0.5–0.8 percent. To obtain high-purity antimony, zone refining is carried out in an atmosphere of inert gas, or antimony is obtained from previously purified antimony trioxide or antimony trichloride. Uses. Antimony is used mainly in lead- and tin-base alloys for battery grids, cable covering, and bearings (babbitt metal) and in alloys used in printing (type metal). These alloys have increased hardness, wear resistance, and corrosion resistance. In fluorescent lamps, calcium halophosphate is activated by antimony. Antimony is used in semiconductor materials as an alloying addition to germanium and silicon; it is also found in antimonides, for example, InSb. The radioisotope 122Sb is used as a source of gamma radiation and neutrons. O. E. K REIN In organisms. The content of antimony (per 100 g dry weight) is 0.006 mg in plants, 0.02 mg in marine animals, and 0.0006 mg in terrestrial animals.

Antimony enters animals and humans through the respiratory organs and the gastrointestinal tract. It leaves the body mainly in the feces and, in smaller quantities, urine. The biological role of antimony is unknown. Antimony is selectively concentrated in the thyroid gland, liver, and spleen. In accumulations in red blood cells, it displays the +3 oxidation state, while accumulations in blood plasma show the +5 state. The maximum permissible concentration of antimony is 10–5–10–7g per 100 g dry tissue. At high concentrations, the element inactivates a series of enzymes involved in lipid, carbohydrate, and protein metabolism, possibly as a result of the blocking of mercapto groups. In medicine, preparations of antimony (Solyusurmin) find use mainly in the treatment of leishmaniasis and certain forms of helminthiasis, for example, schistosomiasis. Antimony and its compounds are toxic. Poisoning can occur during the smelting of antimony ore concentrates and production of antimony alloys. With acute poisoning, there is irritation of the mucous membrane of the upper respiratory passages and of the eyes and skin.

Dermatitis and conjunctivitis may develop. Poisoning is treated with 2,3-dimercapto-1-propanol sodium sulfonate, as well as with diuretics and diaphoretics. The danger of poisoning can be reduced through adequate ventilation and the automation of certain production processes. REFERENCES Antimony, Chemical Element - reaction, water, uses, elements, metal, number, name, symbol PRONUNCIATION AN-ti-moh-nee Antimony is a metalloid. A metalloid is an element that has characteristics of both metals and non-metals. The metalloids can be found on either side of the staircase line on the right side of the periodic table (with the exception of aluminum, which is not considered a metalloid). Antimony is primarily used in alloys, ceramics and glass, plastics, and flame retardant materials. Flame retardant materials do not burn with an open flame. Instead, they smolder or do not burn at all. Discovery and naming Compounds of antimony were known to ancient cultures. They have been found, for example, in the colored glazes used on beads, vases, and other glassware.

But these compounds were not widely used until the Middle Ages when they became popular among alchemists. They thought that antimony could be used to convert lead into gold. It was during this period that records about the properties of antimony begin to appear. The element was probably first named by Roman scholar Pliny ( A.D. 23-79), who called it stibium. Muslim alchemist Abu Musa Jabir Ibn Hayyan (c. 721-c. 815) probably first called it antimony— anti ("not") and monos ("alone"). The name comes from the fact that antimony does not occur alone in nature. Alchemists used secret codes to write about much of their work, so modern scholars do not know a great deal about how antimony was used. The first detailed reports about antimony were published in 1707 when French chemist Nicolas Lemery (1645-1715) published his famous book, Treatise on Antimony. Physical properties Antimony is a silvery-white, shiny element that looks like a metal. It has a scaly surface and is hard and brittle like a non-metal.

It can also be prepared as a black powder with a shiny brilliance to it. The melting point of antimony is 630°C (1,170°F) and its boiling point is 1,635°C (2,980°F). It is a relatively soft material that can be scratched by glass. Its density is 6.68 grams per cubic centimeter. A metalloid is an element that has characteristics of both metals and non-metals. Chemical properties Antimony is a moderately active element. It does not combine with oxygen in the air at room temperature. It also does not react with cold water or with most cold acids. It does dissolve in some hot acids, however, and in aqua regia. Aqua regia is a mixture of hydrochloric and nitric acids. It often reacts with materials that do not react with either acid separately. Occurrence in nature Antimony is rarely found in its native (as an element) state. Instead, it usually occurs as a compound. The most common minerals of antimony are stibnite, tetrahedrite, bournonite, boulangerite, and jamesonite.

In most of these minerals, antimony is combined with sulfur to produce some form of antimony sulfide (Sb 2 S 3 ). The largest producers of antimony are China, Russia, Bolivia, South Africa, and Kyrgyzstan, in that order. The United States produces antimony as a by-product at only one silver mine in Idaho. The abundance of antimony is estimated to be about 0.2 parts per million, placing it in the bottom fifth among the chemical elements found in the Earth's crust. It is more abundant than silver or mercury, but less abundant than iodine. Isotopes There are two naturally occurring isotopes of antimony, antimony-121 and antimony-123. Isotopes are two or more forms of an element. Isotopes differ from each other according to their mass number. The number written to the right of the element's name is the mass number. The mass number represents the number of protons plus neutrons in the nucleus of an atom of the element. The number of protons determines the element, but the number of neutrons in the atom of any one element can vary. Each variation is an isotope.

About 20 radioactive isotopes of antimony are also known. A radioactive isotope is one that breaks apart and gives off some form of radiation. Radioactive isotopes are produced when very small particles are fired at atoms. These particles stick in the atoms and make them radioactive. Two of antimony's radioactive isotopes are used commercially as tracers. These isotopes are antimony-124 and antimony-125. A tracer is an isotope injected into a living or non-living system. The movement of the isotope can then be followed as it moves through the system. For example, a small amount of antimony-124 could be injected into an oil pipeline. The presence of the isotope can be detected by means of an instrument held above the pipeline. The radiation given off by the isotope causes a light to flash or a sound to occur in the Antimony samples. instrument. The movement of the isotope through the pipeline can be followed in this way. If the pipeline has a leak, the tracer will escape from it. Its movement through the soil can be detected.

Extraction Antimony can be recovered from stibnite with hot iron: About half the antimony produced in the United States is recycled from old lead storage batteries used in cars and trucks. Uses Antimony is used to make alloys with a number of different metals. An alloy is made by melting and mixing two or more metals. The properties of the mixture are different than those of the individual metals. One of the most common of these Lead-antimony alloys are used for fishing tackle. alloys is one made with lead. Lead-antimony alloys are used for solder, ammunition, fishing tackle, covering for electrical cables, alloys that melt at low temperatures, and batteries. The manufacture of lead storage batteries, like the ones used in cars and trucks, account for about one-fifth of all the antimony used each year. A small amount of antimony is also used in making transistors, which are found in such consumer electrical devices as computer games, pocket calculators, and portable stereos. A transistor is a solid-state (using special properties of solids, rather than electron tubes) electronic device used to control the flow of an electric current. Other minor uses of antimony include the manufacture of glass and ceramics and the production of plastics.

In glass and ceramics, a small amount of antimony insures that the final product will be clear and colorless. In the production of plastics, antimony is used as a catalyst. A catalyst is a substance used to speed up or slow down a chemical reaction. The catalyst does not undergo any change itself during the reaction. Compounds The most important use of antimony is in making compounds used in the manufacture of flame-retardant materials. Slightly more than half of all antimony goes to this use. These include antimony oxychloride (SbOCl), antimony pentoxide (Sb 2 O 5 ), antimony trichloride (SbCl 3 ), and antimony trioxide (Sb 2 O 3 ). These compounds are sprayed on or added to a fabric to make it flame retardant. Health effects Antimony and its compounds are dangerous to human health. In low levels, these materials can irritate the eyes and lungs. They may also cause stomach pain, diarrhea, vomiting, and stomach ulcers. At higher doses, antimony and its compounds can cause lung, heart, liver, and kidney damage. At very high doses, they can cause death.

Also read article about Antimony from Wikipedia User Contributions: Chemical Elements.com - Antimony (Sb) Bentor, Yinon. Chemical Element.com - Antimony. < For more information about citing online sources, please visit the MLA's Website . This page was created by Yinon Bentor. Use of this web site is restricted by this site's license agreement . Copyright © 1996-2012 Yinon Bentor. All Rights Reserved. Antimony - Wikipedia, the free encyclopedia Antimony This article is about the element. For the town in Utah, see Antimony, Utah . Not to be confused with antinomy , a type of paradox . 51 1491 1858 Sb is stable with 70 neutrons 123Sb Sb is stable with 72 neutrons 125Sb References Antimony ( IPA : 'æntəməʊni) is a chemical element in the periodic table that has the symbol Sb ( Latin : stibium, meaning "mark") and atomic number 51. A metalloid , antimony has four allotropic forms. The stable form of antimony is a blue-white metalloid.

Yellow and black antimony are unstable non-metals. Antimony is used in flame-proofing, paints , ceramics , enamels , a wide variety of alloys , electronics , and rubber . Contents [ edit ] Notable characteristics Antimony in its elemental form is a silvery white, brittle , fusible , crystalline solid that exhibits poor electrical and heat conductivity properties and vaporizes at low temperatures . A metalloid , antimony resembles a metal in its appearance and in many of its physical properties, but does not chemically react as a metal. It is also attacked by oxidizing acids and halogens . Antimony and some of its alloys are unusual in that they expand on cooling. According to New Scientist ( 26 May 2007 ) the earth has an estimated thirty years supply left of this element. Estimates of the abundance of antimony in the Earth 's crust range from 0.2 to 0.5 ppm . Antimony is geochemically categorized as a chalcophile , occurring with sulfur and the heavy metals lead , copper , and silver . [ edit ] Applications Antimony is increasingly being used in the semiconductor industry in the production of diodes , infrared detectors, and Hall-effect devices.

As an alloy , this metalloid greatly increases lead 's hardness and mechanical strength. The most important use of antimony is as a hardener in lead for storage batteries. Uses include: soldering - some "lead-free" solders contain 5% Sb main and big-end bearings in internal combustion engines (as alloy) used in the past to treat Schistosomiasis ; today Praziquantel is universally used used in linotype printing machines Antimony compounds in the form of oxides , sulfides , sodium antimonate, and antimony trichloride are used in the making of flame-proofing compounds, ceramic enamels, glass , paints , and pottery . Antimony trioxide is the most important of the antimony compounds and is primarily used in flame-retardant formulations. These flame-retardant applications include such markets as children's clothing, toys, aircraft and automobile seat covers. Also, antimony sulfide is one of the ingredients of safety matches . The natural sulfide of antimony, stibnite , was known and used in Biblical times as medicine and as a cosmetic . Stibnite is still used in some developing countries as medicine .

Antimony has been used for the treatment of schistosomiasis . Antimony attaches itself to sulfur atoms in certain enzymes which are used by both the parasite and human host. Small doses can kill the parasite without causing damage to the patient. Antimony and its compounds are used in several veterinary preparations like Anthiomaline or Lithium antimony thiomalate, which is used as a skin conditioner in ruminants. Antimony has a nourishing or conditioning effect on keratinized tissues, at least in animals. Tartar emetic is another antimony preparation which is used as an anti-schistosomal drug. Treatments chiefly involving antimony have been called antimonials . A coin made of antimony was issued in the Keichow Province of China in 1931. The coins were not popular, being too soft and they wore quickly when in circulation. After the first issue no others were produced.[ citation needed ] [ edit ] Names of antimony The ancient words for antimony mostly have, as their chief meaning, kohl , the sulfide of antimony.

Pliny the Elder , however, distinguishes between male and female forms of antimony; his male form is probably the sulfide, the female form, which is superior, heavier, and less friable, is probably native metallic antimony. [1] The Egyptians called antimony mśdmt; in hieroglyphics, the vowels are uncertain, but there is an Arabic tradition that the word is mesdemet. [2] The Greek word, stimmi, is probably a loan word from Arabic or Egyptian, and is used by the Attic tragic poets of the 5th century BC; later Greeks also used stibi, as did Celsus and Pliny, writing in Latin, in the first century AD. Pliny also gives the names stimi [sic], larbaris, alabaster , and the "very common" platyophthalmos, "wide-eye" (from the effect of the cosmetic). Later Latin authors adapted the word to Latin as stibium. The Arabic word for the substance, as opposed to the cosmetic, can appear as ithmid, athmoud, othmod, or uthmod.

Littré suggests the first form, which is the earliest, derives from stimmida, (one) accusative for stimmi. [3] The use of Sb as the standard chemical symbol for antimony is due to the 18th century chemical pioneer, Jöns Jakob Berzelius , who used this abbreviation of the name stibium. The medieval Latin form, from which the modern languages, and late Byzantine Greek, take their names, is antimonium. The origin of this is uncertain; all suggestions have some difficulty either of form or interpretation. The popular etymology, from anti-monachos or French antimoine, still has adherents; this would mean "monk-killer", and is explained by many early alchemists being monks, and antimony being poisonous. [4] So does the hypothetical Greek word antimonos, "against one", explained as "not found as metal", or "not found unalloyed". [5] Lippmann conjectured a Greek word, anthemonion, which would mean "floret", and he cites several examples of related Greek words (but not that one) which describe chemical or biological efflorescence .

[6] The early uses of antimonium include the translations, in 1050-1100, by Constantine the African of Arabic medical treatises. [7] Several authorities believe that antimonium is a scribal corruption of some Arabic form; Meyerhof derives it from ithmid; [8] other possibilities include Athimar, the Arabic name of the metal, and a hypothetical *as-stimmi, derived from or parallel to, the Greek. [9] [ edit ] History Antimony's sulfide compound, antimony (III) trisulfide, Sb2S3 was recognized in antiquity, at least as early as 3000 BC . Pastes of Sb2S3 powder in fat [10] or in other materials have been used since that date as eye cosmetics in the Middle East and farther afield; in this use, Sb2S3 is called "kohl". It was used to darken the brows and lashes, or to draw a line around the perimeter of the eye.

An artefact made of antimony dating to about 3000 BC was found at Tello, Chaldea (part of present day Iraq), and a copper object plated with antimony dating between 2500 BC and 2200 BC has been found in Egypt. [11] There is some uncertainty as to the description of the artefact from Tello. Although it is sometimes reported to be a vase, a recent detailed discussion of it reports it to be rather a fragment of indeterminate purpose. [12] According to the history of metallurgy, the first description of a procedure for isolating antimony is in the book " De la pirotechnia " of 1540 of Vannoccio Biringuccio , written in Italian. This book precedes the more famous 1556 book in Latin by Agricola , " De re metallica ", even though Agricola has been often incorrectly credited with the discovery of metallic antimony.

Alchemical symbol for antimony According to the traditional history of western alchemy , metallic antimony was described (previous to Biringuccio) by the putative Prior Basilius Valentinus in a Latin manuscript, "Currus Triumphalis Antimonii", supposedly circa 1450. This manuscript was published in 1604 in English translation as "The triumphal chariot of antimony", by Johann Thölde (1565-1614). The marvelous discovery of a complete set of Valentinus' manuscripts, including the alchemical tales, is fully described by Jean-Jacques Manget in his Bibliotheca chemica curiosa (1702): the manuscripts had been enclosed for more than a century in a pillar of St. Peter's Abbey, at Erfurt , until the pillar was shattered by a thunderbolt. Many scholars have considered Basilius Valentinus a mythological personage.

Gottfried Wilhelm Leibniz (1646-1716) declared, after careful enquiry, that no Prior Valentinus ever existed in the Abbey of Erfurt, rather that the name was only a pseudonym -- probably of Thölde himself -- used to merge poorly translated materials of various origins. According to the traditional history of Middle Eastern alchemy, pure antimony was well known to Geber , sometimes called "the Father of Chemistry", in the 8th century. Here there is still an open controversy: Marcellin Berthelot , who translated a number of Geber's books, stated that antimony is never mentioned in them, but other authors claim that Berthelot translated only some of the less important books, while the more interesting ones (some of which might describe antimony) are not yet translated, and their content is completely unknown. Native massive antimony with oxidation products Antimony output in 2005 World production trend of antimony Even though this element is not abundant, it is found in over 100 mineral species.

Antimony is sometimes found native, but more frequently it is found in the sulfide stibnite (Sb2S3) which is the predominant ore mineral . Commercial forms of antimony are generally ingots, broken pieces, granules, and cast cake. Other forms are powder, shot, and single crystals. In 2005, China was the top producer of antimony with about 84% world share followed at a distance by South Africa, Bolivia and Tajikistan, reports the British Geological Survey . Country Chiffres de 2003 , métal contenue dans les minerais et concentrés, source : L'état du monde 2005 The largest mine in China is Xikuangshan mine in Hunan Province. [ edit ] Precautions Antimony and many of its compounds are toxic . Clinically, antimony poisoning is very similar to arsenic poisoning. In small doses, antimony causes headache , dizziness , and depression . Larger doses cause violent and frequent vomiting, and will lead to death in a few days. See also arsenic poisoning .

[ edit ] Leaching from PET A study found that antimony is leaching from PET bottles (reported for some acidic fruit drinks),[ citation needed ] but at levels below drinking water guidelines. The guidelines are: WHO, 20 µg l–1 Japan, 15 µg l–1 [13] US EPA, Health Canada and the Ontario Ministry of Environment, 6 µg l–1 German Federal Ministry of Environment, 5 µg l–1 [14] The acidic nature of the drink is sufficient to dissolve small amounts of antimony oxide contained in the packaging of the drink;[ citation needed ] modern manufacturing methods prevent this occurrence.[ citation needed ] However, researchers are concerned that antimony levels correspond to duration the bottle is left to stand - the longer the beverage has been bottled, the higher the antimony leached.[ citation needed ] [ edit ] Bibliography W. F. Albright "Notes on Egypto-Semitic Etymology. II", The American Journal of Semitic Languages and Literatures, Vol. 34, No. 4. (Jul., 1918), pp. 215-255. JSTOR link .

esp p.230 Endlich, F.M. "On Some Interesting Derivations of Mineral Names", The American Naturalist, Vol. 22, No. 253. (Jan., 1888), pp. 21-32. JSTOR link . p.28 Kirk-Othmer Encyclopedia of Chemical Technology, 5th ed. 2004. Entry for antimony. Lippmann, E O von [Edmund Oscar]. 1919. Entstehung und Ausbreitung der Alchemie, teil 1. Berlin: Julius Springer. In German. Moorey, PRS. 1994. Ancient Mesopotamian Materials and Industries: the Archaeological Evidence. New York: Clarendon Press. Priesner, Claus and Figala, Karin, eds. 1998. Alchemie. Lexikon einer hermetischen Wissenschaft. München: C.H. Beck. 412 p. In German. Sarton, George. 1935. Review of Al-morchid fi'l-kohhl, ou Le guide d'oculistique, translated by Max Meyerhof . Isis (Feb.

1935), 22(2):539-542 (The journal Isis is in the JSTOR archive.) In French. Antimony - Element information, properties and uses | Periodic Table Chemistry in its element: antimony (Promo) You're listening to Chemistry in its element brought to you by Chemistry World, the magazine of the Royal Society of Chemistry. (End promo) Chris Smith Hello, this week we meet the chemical that's maimed and murdered, but often with the best intentions. To tell the story of the element that can't quite make up its mind if it's a metal or not here's Phil Ball. Phil Ball Many wars have been fought over territory, some over pride or love or money. But in the 1600s a long and bitter war was waged over antimony. What, you might ask, is there to fight about in this apparently unremarkable element, a soft, greyish metal that doesn't even conduct electricity well enough to qualify as a true metal? It has its uses, but they are mundane: as an alloy component of battery electrodes and of pewter, and as a flame retardant.

But at the heart of the Antimony War, which raged in France and Germany throughout much of the seventeenth century, was a more unlikely use of antimony. Some doctors of that age believed that it was a vital ingredient in medicine. The advocates and opponents of this point of view didn't actually take up arms: they fought with pen in hand, sometimes denouncing one another in terms far more vitriolic than we'll find in the academic literature today. It's very curious that the subject of this dispute should be antimony, because this element is actually rather toxic, causing liver damage in large enough doses. But pharmaceutical uses of antimony have a long history. In the ancient world it was known primarily in the form of its black sulphide ore, called stibnite, which the Greek physician Dioscorides recommended for skin complaints in the first century AD. The Egyptians, meanwhile, used stibnite as a cosmetic, applying it as a form of mascara. They called it kuhl, meaning 'eye-paint', and to the later Islamic alchemical physicians this became al-kohl. From its original meaning of powdered stibnite, this term came to designate any powder, and then a potent extract of any substance.

In the early sixteenth century the Swiss alchemical physician Paracelsus called a distilled extract of wine alcool vini, from where we get the modern word alcohol: a long and strange road from eye make-up to intoxicating liquor. Paracelsus was particularly fond of antimony compounds as medicines. After his death, Paracelsus's chemical medicine was championed by many doctors in Europe, especially in France, and some of these made antimony their most prized remedy. One, a German salt-maker who wrote under the false persona of a fifteenth-century monk called Basil Valentine, published an entire book advertising antimony remedies in 1604 called The Triumphal Chariot of Antimony. Valentine admitted that antimony was poisonous - in fact he offered an apocryphal explanation for the name, saying that it derives from anti-monachos, meaning 'anti-monk' in Latin, because he once unintentionally poisoned several of his fellow monks by adding it secretly to their food in an attempt to improve their health. But he claimed that alchemy could be used to free the metal of its toxic effects and make it "a most salutary Medicine".

The Paracelsian chemical physicians were opposed by traditionalists who preferred the medical theories of the ancient doctors like Hippocrates, based on the idea that our health is controlled by a balance of four humours. This was partly a battle for academic power, but the rival camps were also split along religious and political lines. So there was a lot riding on the struggle, and for a time it crystallized around the medical value of antimony. The toxicity of antimony can cause vomiting - but to its supporters, this was seen as a good thing. They would administer the salt antimony tartrate as a so-called emetic, a vomit-inducer that was believed to purge the body of other bad substances. Some doctors continued to prescribe antimony freely after the inconclusive Antimony War, and it has been suggested that a fondness for antimony remedies was what actually killed Mozart in 1791. By the nineteenth century it had become a favourite slow poison for murderers eager to conceal their crimes - a chemical villain almost as notorious as lead. Chris Smith But would Mozart have been the maestro that he was without the help of antimony? Well I guess we will never know. Thank you very much to science writer and author Phil Ball.

Next week we'll be telling the tale of the element that at one time quite literally kept the world going, but not quite in the way you might think. John Emsley The summer of 1618 saw England gripped by drought, but as Henry Wicker walked across Epsom Common he came across a pool of water from which thirsty cattle refused to drink. He found that the water tasted bitter and on evaporation it yielded a salt which had remarkable effects: it acted as a laxative. This became the famous Epsom's salt (magnesium sulfate, MgSO4) and became a treatment for constipation for the next 350 years. Chris Smith 350 years, certainly sounds like a bad case of constipation. Thankfully John Emsley will be running smoothly through the element with atomic number 12 and that's magnesium in next week's Chemistry in its element, I hope you can join us. I'm Chris Smith, thank you for listening, see you next time. (Promo) Chemistry in its element is brought to you by the Royal Society of Chemistry and produced by thenakedscientists.com .

There's more information and other episodes of Chemistry in its element on our website at chemistryworld.org/elements . (End promo) Element 51 | Article about Element 51 by The Free Dictionary Element 51 | Article about Element 51 by The Free Dictionary Related to Element 51: Element 56 , Element 52 , Element 53 antimony (ăn`tĭmō'nē) [Lat. antimoneum], semimetallic chemical element; symbol Sb [Lat. stibium,=a mark]; at. no. 51; at. wt. 121.760; m.p. 630.74&degC;; b.p. 1,750&degC;; sp. gr. (metallic form) 6.69 at 20&degC;; valence 0, +3, −3, or +5. Antimony exists in two allotropic forms (see allotropy allotropy [Gr.,=other form]. A chemical element is said to exhibit allotropy when it occurs in two or more forms in the same physical state; the forms are called allotropes. .....

Click the link for more information. ); the more common is silvery blue-white and has a rhombohedral crystalline structure. It is a poor conductor of heat and electricity and is brittle and easily powdered. It is primarily used in alloys and chemical compounds. It is a member of Group 15 of the periodic table periodic table, chart of the elements arranged according to the periodic law discovered by Dmitri I. Mendeleev and revised by Henry G. J. Moseley. In the periodic table the elements are arranged in columns and rows according to increasing atomic number (see the table entitled ..... Click the link for more information. . Antimony rarely occurs free in nature, but its ores are widely distributed. The principal ore is stibnite stibnite , antimony sulfide, Sb2S3, a mineral, silvery gray in color, with a metallic luster. It crystallizes in the orthorhombic system. Found in many parts of the world, it is the most important ore of antimony. ..... Click the link for more information. , a sulfur compound known since early times; there are extensive deposits in China.

Antimony is often found in other ores as well, e.g., silver, copper, and lead. The pure element antimony is produced from the ore by roasting it to form the oxide, then reducing the oxide with carbon or iron; often a flux of sodium sulfate or sodium carbonate is used to prevent loss of molten antimony by evaporation. Antimony does not react with air or water at room temperature; it does react with fluorine, chlorine, or bromine and is soluble in hot nitric or sulfuric acid; at higher temperatures, antimony will ignite and burn in air. It unites with hydrogen to form stibine, a poisonous gas. In combination with metals antimony forms alloys that are hard and brittle and have low melting points. The alloys of antimony include britannia metal britannia metal, silvery-white alloy of tin with antimony, copper, and sometimes bismuth and zinc. It is very similar in appearance to pewter, but is harder. It is used widely for the manufacture of tableware. ..... Click the link for more information.

, type metal type metal, alloy of lead with antimony, tin, and sometimes copper, so named because of its one time extensive use for making printing type. Expanding upon solidification, the alloy takes a fine and clear impression of the mold in which it hardens. It has a low melting point. ..... Click the link for more information. , Babbitt metal Babbitt metal, an antifriction metal first produced by Isaac Babbitt in 1839. In present-day usage the term is applied to a whole class of silver-white bearing metals, or "white metals. ..... Click the link for more information. , and sometimes pewter pewter, any of a number of ductile, silver-white alloys consisting principally of tin. The properties vary with the percentage of tin and the nature of the added materials. ..... Click the link for more information. ; these alloys expand on cooling, thereby retaining fine details of a mold. Alloys and compounds of antimony are used in bearings, storage batteries, safety matches, and as a red pigment in paint.

Although antimony and many of its compounds are toxic, tartar emetic tartar emetic, poisonous, odorless, transparent rhombic crystals or white powder with a metallic, sweetish taste. Chemically, it is potassium antimony tartrate, KSbC4H4O7· 1-2H2O. It is used as a mordant in dyeing. ..... Click the link for more information. (potassium antimonyl tartrate), meglumine antimoniate, sodium stibogluconate, and other compounds are used as medicines. Small concentrations of antimony can be detected by a method similar to the Marsh test Marsh test, method for the detection of arsenic, so sensitive that it can be used to detect minute amounts of arsenic in foods (the residue of fruit spray) or in stomach contents. The sample is placed in a flask with arsenic-free zinc and sulfuric acid. ..... Click the link for more information. for arsenic. Antimony is mixed with soot and other substances to make kohl, used for centuries by women in some countries as an eye cosmetic.

A method for the extraction of antimony from stibnite was first described c.1600 by Basilius Valentinus. Although known to the ancients, the element was first adequately described by Nicolas Lémery in 1707. Antimony Sb, a chemical element in group V of Mendeleev’s periodic system. Atomic number, 51; atomic weight, 121.75. Antimony is a silvery white metal with a blue tinge. In nature, two stable isotopes are known: 121Sb (57.25 percent) and 123Sb (42.75 percent). The most important of the element’s artificial radioisotopes are 122Sb (half-life 2.8 days), 124Sb (half-life 60.2 days), and 125Sb (half-life two years). History. Antimony has been known since antiquity. In the Orient, it was used around 3000 B.C. in making various vessels. In Egypt, as early as the 19th century B.C.

, powdered antimony glance (natural Sb2S3, called mesten or stem) was used for darkening eyebrows. In ancient Greece, the powder was known as stimi or stibi, hence the Latin stibium. The name antimonium came into use sometime between the 12th and 14th centuries A.D. In 1789, A. Lavoisier included antimony in his list of chemical elements, using the French name antimoine (antimonio in Spanish and Italian, Antimon in German). The Russian name for the element, sur’ma, is derived from the Turkish sürme, the term for powdered lead glance (PbS), also used for darkening eyebrows. (According to some sources, sur’ma is derived from a Persian word meaning metal.) A detailed description of the properties and methods of obtaining antimony was first given by the alchemist Basil Valentine in 1604 in Germany. Distribution in nature. The average content of antimony in the earth’s crust (clarke) is 5 × 10–5 percent by weight. Antimony is dispersed in magma and in the biosphere.

It is contained in hot groundwater, forming concentrations in hydrothermal deposits. Antimony deposits as such are known, as are antimony-mercury, antimony-lead, gold-antimony, and antimony-tungsten deposits. Of the 27 antimony minerals, antimonite (Sb2S3) has the greatest industrial importance. Because of its affinity for sulfur, antimony is often encountered as an admixture in the sulfides of arsenic, bismuth, nickel, lead, mercury, silver, and other elements. Physical and chemical properties. Antimony is known in a crystalline form and in three amorphous forms—explosive, black, and yellow. Explosive antimony, with a density of 5.64–5.97 g/cm3, explodes upon contact; it is produced in the electrolysis of a solution of SbCl3. Black antimony, with a density of 5.3 g/cm3, is formed through the rapid cooling of antimony vapors, and yellow antimony is formed by passing oxygen through liquefied SbH3. The yellow and black forms are unstable and convert into the crystalline form at reduced temperatures.

Crystalline antimony, which is the most stable form, crystallizes in the trigonal system (a = 4.5064 angstroms); this form has a density of 6.61–6.73 g/cm3 (liquid, 6.55 g/cm3), a melting point of 630.5°C, a boiling point of 1635°–1645°C, a specific heat at 20°–100°C of 0.210 kilojoule/kg· °K (0.0498 calorie/g· °C), and a thermal conductivity at 20°C of 17.6 watts/m· °K (0.042 calorie/cm· sec · °C).

The linear coefficient of expansion of polycrystalline antimony is 11.5 × 10–6 at 0°–100°C; for a single crystal in the temperature range 0°–400°C, α1 = 8.1 x 10–6 and α2 = 19.5 × 10–6, and the electrical resistivity of a single crystal of antimony at 20°C is 43.045 × 10–6 ohm·cm. Antimony is diamagnetic, with a magnetic susceptibility of –0.66 × 10–6. In contrast to most metals, antimony is brittle and is easily split along cleavage planes; it can be ground into a powder. It is not forgeable and consequently is sometimes classified as a semimetal. Mechanical properties depend on the purity of the metal.

The Brinell hardness of cast antimony is 325–340 meganewtons/m2 (32.5–34.0 kilograms-force/mm2), the modulus of elasticity is 285–300, and the ultimate strength is 86.0 meganewtons/m2 (8.6 kilograms-force/mm2). The configuration of the outer electrons of the antimony atom is 5s25p3. In compounds, antimony has oxidation states of +5, +3, and –3. Antimony has relatively low chemical reactivity. It does not undergo oxidation in the air at temperatures ranging up to its melting point, and it does not react with nitrogen and hydrogen. Carbon dissolves to only a slight extent in molten antimony. The metal reacts vigorously with chlorine and other halogens to form antimony halides. It reacts with oxygen at temperatures above 630°C, forming Sb2O3. Antimony sulfides are obtained when antimony is melted in the presence of sulfur; antimony reacts similarly with phosphorus and arsenic. Antimony is stable in relation to water and dilute acids.

Concentrated hydrochloric and sulfuric acids slowly dissolve antimony with the formation of the chloride SbCl3 and the sulfate Sb2(SO4)3; concentrated nitric acid oxidizes antimony to a higher oxide, which takes the form of the hydrate xSb2O5·yH2O. The difficultly soluble salts of antimonic acid have practical importance. They include antimonates (MSbO3·3H2O, where Me is Na or K) and the salts of meta-antimonous acid (not yet isolated in pure form), namely, meta-antimonates (MeSbO2·3H2O), which possess reducing properties. Antimony combines with metals to form antimonides. Production. Antimony is obtained by the pyrometallurgical and hydrometallurgical treatment of concentrates or from ore containing 20–60 percent Sb. The pyrometallurgical methods include precipitation smelting and reduction smelting.

Sulfide concentrates serve as the raw material for precipitation smelting, which is based on the replacement of antimony in the sulfide by iron: Sb2S3 + 3Fe ⇄ 2Sb + 3FeS. The iron is introduced into the charge as scrap, and the smelting is carried out in reverberatory or short rotating furnaces at 1300°–1400°C. The extraction of antimony in the form of crude metal exceeds 90 percent. The reduction smelting of antimony is based on the reduction of antimony oxides to the metal using charcoal or coal dust and on the slagging of waste rock. Reduction smelting is preceded by oxidative roasting at 550°C with an excess of air. The calcine contains the nonvolatile tetroxide of antimony. Electric furnaces can be used in both precipitation and reduction smelting.

The two stages involved in the hydrometallurgical process of obtaining antimony are the treatment of the raw material with an alkaline sulfide solution, which results in the entry of antimony into solution as sul-fosalts and salts of antimonic acids, and the separation of antimony by electrolysis. Depending on the composition of the raw material and the method of production, crude antimony contains 1.5 to 15 percent impurities, for the most part Fe, As, and S. Pyrometallurgical or electrolytic refining is used to produce pure antimony. In pyrometallurgical refining, impurities of iron and copper are removed as sulfur compounds by introducing antimonite (Sb2S3); arsenic (as sodium arsenate) and sulfur are then removed by passing air under the soda slag. In electrolytic refining with a soluble anode, crude antimony is purified of iron, copper, and other metals remaining in the electrolyte (with Cu, Ag, and Au remaining in the slurry. A solution consisting of SbF3, H2SO4, and HF serves as the electrolyte.

The content of impurities in refined antimony does not exceed 0.5–0.8 percent. To obtain high-purity antimony, zone refining is carried out in an atmosphere of inert gas, or antimony is obtained from previously purified antimony trioxide or antimony trichloride. Uses. Antimony is used mainly in lead- and tin-base alloys for battery grids, cable covering, and bearings (babbitt metal) and in alloys used in printing (type metal). These alloys have increased hardness, wear resistance, and corrosion resistance. In fluorescent lamps, calcium halophosphate is activated by antimony. Antimony is used in semiconductor materials as an alloying addition to germanium and silicon; it is also found in antimonides, for example, InSb. The radioisotope 122Sb is used as a source of gamma radiation and neutrons. O. E. K REIN In organisms. The content of antimony (per 100 g dry weight) is 0.006 mg in plants, 0.02 mg in marine animals, and 0.0006 mg in terrestrial animals.

Antimony enters animals and humans through the respiratory organs and the gastrointestinal tract. It leaves the body mainly in the feces and, in smaller quantities, urine. The biological role of antimony is unknown. Antimony is selectively concentrated in the thyroid gland, liver, and spleen. In accumulations in red blood cells, it displays the +3 oxidation state, while accumulations in blood plasma show the +5 state. The maximum permissible concentration of antimony is 10–5–10–7g per 100 g dry tissue. At high concentrations, the element inactivates a series of enzymes involved in lipid, carbohydrate, and protein metabolism, possibly as a result of the blocking of mercapto groups. In medicine, preparations of antimony (Solyusurmin) find use mainly in the treatment of leishmaniasis and certain forms of helminthiasis, for example, schistosomiasis. Antimony and its compounds are toxic. Poisoning can occur during the smelting of antimony ore concentrates and production of antimony alloys. With acute poisoning, there is irritation of the mucous membrane of the upper respiratory passages and of the eyes and skin.

Dermatitis and conjunctivitis may develop. Poisoning is treated with 2,3-dimercapto-1-propanol sodium sulfonate, as well as with diuretics and diaphoretics. The danger of poisoning can be reduced through adequate ventilation and the automation of certain production processes. REFERENCES Element 51 | definition of Element 51 by Medical dictionary Element 51 | definition of Element 51 by Medical dictionary antimony (Sb) [an´tĭ-mo″ne] a chemical element, atomic number 51, atomic weight 121.75. (See Appendix 6.) Several of its salts are used in tropical medicine as treatments for schistosomiasis ; however, they must be used with caution because they are potentially poisonous, causing symptoms similar to those of arsenic poisoning . adj., adj antimo´�nial. antimony potassium tartrate a compound used in treatment of schistosomiasis , especially infection with Schistosoma japonicum. antimony sodium tartrate a compound used in treating schistosomiasis .

an·ti·mo·ny (Sb), (an'-ti-mō'nē), Do not confuse this word with antinomy. A metallic element, atomic no. 51, atomic wt. 121.757, valences 0, -3, +3, +5; used in alloys; toxic and irritating to the skin and mucous membranes. [G. anti + monos, not found alone] antimony /an·ti·mo·ny/ (Sb) (an´tĭ-mo″ne) a chemical element, at. no. 51, forming various medicinal and poisonous salts; ingestion of antimony compounds, and rarely industrial exposure to them, may produce symptoms similar to those of acute arsenic poisoning. A. potassium tartrate and a. sodium tartrate have been used as antischistosomals .antimo´nial antimony (Sb) [an′təmō′nē] Etymology: L, antimonium a bluish, crystalline metallic element occurring in nature.

Various antimony compounds are used in the treatment of filariasis, leishmaniasis, lymphogranuloma, schistosomiasis, and trypanosomiasis. They are also used as emetics. antimony Toxicology A metallic element–atomic number 51; atomic weight 121.75 Clinical-acute N&V, bloody diarrhea, hepatitis, kidney failure Clinical-chronic Itching, conjunctivitis, laryngitis, headache, anorexia, weight loss, anemia, jaundice, kidney failure Lethal dose 100 to 200 mg Management Supportive; gastric lavage/activated charcoal; dimercaprol to accelerate excretion; transfusions for hemolysis Ref range < 10 µg/L an·ti·mo·ny (Sb) (an'ti-mō-nē) A metallic element; atomic no. 51, atomic wt. 121.757; valences 0, -3, +3, +5; used in alloys; toxic and irritating to the skin and mucous membranes. [G.

anti + monos, not found alone] antimony A brittle, flaky metal, many of the compounds of which are poisonous. antimony, n a toxic metal sometimes found in alloys, semiconductors, and local pollution. Exposure has been linked to anemia, bleeding gums, conjunctivitis, headaches, laryngitis, skin disease, and weight loss. an·ti·mo·ny (an'ti-mō-nē) Do not confuse this word with antinomy. A metallic element used in alloys; toxic and irritating to the skin and mucous membranes. [G. anti + monos, not found alone] antimony, n a bluish crystalline metallic element occurring in nature both free and as salts. Antimony compounds are used in the treatment of filariasis, leishmaniasis, and other parasitic diseases. Antimony is also used as an emetic. antimony a chemical element, atomic number 51, atomic weight 121.75, symbol Sb. See Table 6. Trivalent and pentavalent antimony compounds are used in medicine as anti-infective agents in the treatment of tropical diseases, especially those of protozoan origin.

All antimony compounds are potentially poisonous and must be used with caution. See also stibogluconate, meglumine . antimony poisoning Antimony | Define Antimony at Dictionary.com antimony noun, Chemistry. 1. a brittle, lustrous, white metallic element occurring in nature free or combined, used chiefly in alloys and in compounds in medicine. Symbol: Sb; atomic number: 51; atomic weight: 121.75. Origin of antimony 1375-1425; late Middle English antimonie < Medieval Latin antimōnium, perhaps < dialectal Arabic uthmud Related forms Examples from the Web for antimony Expand British Dictionary definitions for antimony Expand noun 1. a toxic metallic element that exists in two allotropic forms and occurs principally in stibnite. The stable form is a brittle silvery-white crystalline metal that is added to alloys to increase their strength and hardness and is used in semiconductors.

Symbol: Sb; atomic no: 51; atomic wt: 121.757; valency: 0, –3, +3, or +5; relative density: 6.691; melting pt: 630.76°C; boiling pt: 1587°C Word Origin C15: from Medieval Latin antimōnium, of uncertain origin Collins English Dictionary - Complete & Unabridged 2012 Digital Edition © William Collins Sons & Co. Ltd. 1979, 1986 © HarperCollins Publishers 1998, 2000, 2003, 2005, 2006, 2007, 2009, 2012 Word Origin and History for antimony Expand n. brittle metallic element, early 15c., from Old French antimoine and directly from Medieval Latin antimonium, an alchemist's term (used 11c.

by Constantinus Africanus), origin obscure, probably a Latinization of Greek stimmi "powdered antimony, black antimony" (a cosmetic used to paint the eyelids), from some Arabic word (cf. al 'othmud), unless the Arabic word is from the Greek or the Latin is from Arabic; probably ultimately from Egyptian stm "powdered antimony." In French folk etymology, anti-moine "monk's bane" (from moine). As the name of a pure element, it is attested in English from 1788. Its chemical symbol Sb is for Stibium, the Latin name for "black antimony," which word was used also in English for "black antimony." Online Etymology Dictionary, © 2010 Douglas Harper ANTIMONY – Tri-Star Resources CONTACT US Antimony is a chemical element with symbol Sb and atomic number 51. It is one of the oldest elements in usage with the Ancient Egyptians having used it for make-up (kohl for the dramatic eye effects). The ancient Romans called it stibium, hence its chemical symbol Sb.

A lustrous gray metalloid, it is found in nature mainly as the sulfide mineral stibnite (Sb2S3). It was established to be an element around the 17th century. The first natural occurrence of pure antimony in the Earth’s crust was described by the Swedish scientist and local mine district engineer Anton von Swab in 1783. The abundance of antimony in the Earth’s crust is estimated at 0.2 to 0.5 parts per million, comparable to thallium at 0.5 parts per million and silver at 0.07 ppm. Even though Sb is not abundant, it is found in over 100 mineral species. Antimony is sometimes found natively, but more frequently it is found in the sulfide stibnite (Sb2S3) which is the predominant ore mineral. The principle use of antimony is in flame retardants as antimony trioxide (ATO). ATO is most commonly used as a synergist to improve the performance of other flame retardants such as aluminium hydroxide, magnesium hydroxide and halogenated compounds.

ATO is used in this way in many products including plastics, textiles, rubber, adhesives and plastic covers for aircrafts and automobiles. The largest applications for metallic antimony are as alloying material for lead and tin and for lead antimony plates in lead-acid batteries. Alloying lead and tin with antimony improves the properties of the alloys which are used in solders, bullets and plain bearings. The second most common use of antimony alloy is as a hardener for lead electrodes in lead acid batteries. This use is in decline as the antimony content of typical automotive battery alloys has declined by weight as calcium, aluminium and tin alloys are expected to replace it over time. An emerging application is the use of antimony in microelectronics. SONY DSC

Question: Which chemical element, atomic number 51, used to be called Stibium?
Answer: Antimony