Yellow antimony. Antimony is an extremely important industrial substance. Metal or non-metal
DEFINITION
Antimony located in the fifth period of the V group of the main (A) subgroup of the Periodic table.
Refers to elements p-families. Semi-metal. Designation - Sb. The serial number is 51. The relative atomic mass is 121.75 amu.
Electronic structure of antimony atom
The antimony atom consists of a positively charged nucleus (+51), inside which there are 51 protons and 71 neutrons, and 51 electrons move around in five orbits.
Fig. 1. Schematic structure of antimony atom.
The orbital distribution of electrons is as follows:
51Sb) 2) 8) 18) 18) 5;
1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 5p 3 .
The external energy level of the antimony atom contains 5 electrons, which are valence. The energy diagram of the ground state takes the following form:
The presence of three unpaired electrons indicates that antimony has an oxidation state of +3. Due to the presence of vacant orbitals 5 d-sublevel for antimony atom possibly excited state (oxidation state +5):
The valence electrons of an antimony atom can be characterized by a set of four quantum numbers: n (main quantum), l (orbital), m l (magnetic) and s (spin):
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Sublevel |
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Examples of problem solving
EXAMPLE 1
Antimony is a chemical element (French Antimoine, English Antimony, German Antimon, Latin Stibium, whence the symbol is Sb, or Regulus antimonii; atomic weight \u003d 120, if O \u003d 16) - a shiny silvery-white metal with a rough-lamellar crystalline fractured or grainy, depending on the speed of solidification from the molten state. Antimony crystallizes in obtuse rhombohedrons, very close to a cube, like bismuth (see), and has beats. weight 6.71-6.86. Native antimony occurs in the form of scaly masses, usually containing silver, iron and arsenic; beats its weight is 6.5-7.0. It is the most fragile of metals, easily powdery in an ordinary porcelain mortar. S. melts at 629.5 ° [According to the latest definitions (Heycock and Neville. 1895).] And is distilled under white heat; even its vapor density was determined, which at 1640 ° turned out to be somewhat higher than required for the adoption of two atoms in a particle - Sb 2 [It was V. Meyer and G. Biltz who found in 1889 the following for the vapor density of C. in relation to air values: 10.743 at 1572 ° and 9.781 at 1640 °, which indicates the ability of the particle to dissociate when heated. Since the density of 8.3 is calculated for the Sb 2 particle, the found densities speak, as it were, of the inability of this "metal" to be in the simplest state, in the form of a monoatomic particle of Sb 3, which distinguishes it from real metals. The same authors investigated the vapor densities of bismuth, arsenic and phosphorus. Only one bismuth was able to give a Bi 1 particle; the following densities were found for it: 10.125 at 1700 ° and 11.983 at 1600 °, and the densities calculated for Bi 1 and Bi 2 are 7.2 and 14.4. Particles of phosphorus P 4 (at 515 ° - 1040 °) and arsenic As 4 (at 860 °) are difficult to dissociate from heating, especially P 4: at 1700 ° from 3P 4 only one particle - one might think - turns into 2P 2, and As4 at the same time it undergoes an almost complete transformation into As2. Thus, the most metallic of these elements that make up one of the subgroups of the periodic table is bismuth, judging by the vapor density; properties of non-metal belong to the greatest extent to phosphorus, characterizing at the same time arsenic and to a lesser extent - S.]]. It is possible to distill S. in a stream of dry gas, for example. hydrogen, since it is easily oxidized not only in air, but also in water vapor at a high temperature, turning into oxide, or, what is the same, into antimony anhydride:
2Sb + 3H 2 O \u003d Sb2 O3 + 3H 2;
if you melt a piece of carbon on a coal in front of a blowpipe and drop it from a certain height onto a sheet of paper, you get a mass of red-hot balls that roll to form white oxide smoke. At ordinary temperatures, C. does not change in air. In terms of the forms of compounds and in all chemical relations, C. belongs to group V of the periodic table of elements, namely to its less metallic subgroup, which also contains phosphorus, arsenic, and bismuth; it refers to the last two elements in the same way as tin in group IV refers to germanium and lead. The most important types of compounds C. are two - SbX 3 and SbX 5, where it is trivalent and pentavalent; it is very likely that these types are unique at the same time. C. halide compounds in particular clearly confirm what has just been said about the forms of the compounds. Trichloride
Sb2 S3 + 3HgCl2 \u003d 2SbCl3 + 3HgS
moreover, volatile sulfurous mercury remains more difficult in the retort, while SbCl 3 is distilled in the form of a colorless liquid, which solidifies in a receiver into a mass similar to cow butter (Butyrum Antimonii). Before 1648, the volatile product was believed to contain mercury; Glauber this year showed that this assumption was wrong. On strong heating of the residue in the retort, it also volatilizes and gives a crystalline sublimation of cinnabar (Cinnabaris Antimonii) HgS. The easiest way is to prepare SbCl 3 from metallic sulfur, acting on it with a slow current of chlorine while heating Sb + 1 ½ Cl2 \u003d SbCl3, and after the disappearance of the metal, a liquid product is obtained containing a certain amount of pentachloride C., .:
3SbCl5 + 2Sb \u003d 5SbCl3;
finally, the SbCl 3 is distilled. By heating sulfurous sulfur with strong hydrochloric acid, an excess of SbCl3 is obtained, and hydrogen sulfide develops:
Sb2 S3 + 6HCl \u003d 2SbCl3 + 3H2 S.
The same solution is obtained by dissolving sulfur oxide in hydrochloric acid. When distilling an acidic solution, first of all, water and excess hydrochloric acid are distilled off, and then SbCl 3 is chased - usually yellowish in the first portions (due to the presence of ferric chloride) and after that colorless. S. trichloride is a crystalline mass that melts at 73.2 ° and boils at 223.5 °, forming a colorless vapor, the density of which fully corresponds to the formula SbCl 3, namely, 7.8 relative to air. It attracts moisture from the air, spreading out into a transparent liquid, from which it can be separated again in a crystalline form when standing in a desiccator over sulfuric acid. In terms of its ability to dissolve in water (in small amounts), SbCl 3 is quite similar to other, real salts of hydrochloric acid, but large amounts of water decompose SbCl 3, converting it into one or another oxychloride, according to the equation:
SbCl3 + 2H 2 O \u003d (HO) 2 SbCl + 2HCl \u003d OSbCl + H 2 O + 2HCl
and 4SbCl 3 + 5H 2 O \u003d O5 Sb4 Cl2 + 10HCl
which represent the extreme limits of incomplete action of water (there are intermediate composition chloroxides); a large excess of water leads to the complete removal of chlorine from the antimony compound. Water precipitates a white powder of similar C chloroxides, but some of the SbCl 3 may remain in solution and precipitate with a larger amount of water. By adding hydrochloric acid, you can dissolve the precipitate again, transform it into a solution of SbCl 3. Obviously, sulfur oxide (see below) is a weak base, like bismuth oxide, and therefore water, in excess, is capable of removing acid from it, converting average sulfur salts into basic salts, or, in this case, into chloroxides; the addition of hydrochloric acid is analogous to a decrease in the amount of reacting water, which is why oxychloride is converted to SbCl 3. The white precipitate resulting from the action of water on SbCl 3 is called algoroth powder by the name of the Verona physician who used it (at the end of the 16th century) for medical purposes.
If we saturate molten sulfuric trichloride with chlorine, we get sulfur pentachloride:
SbCl3 + Cl2 \u003d SbCl5
discovered by G. Rose (1835). It can also be obtained from metallic sulfur, the powder of which burns in it when poured into a container with chlorine:
Sb + 2 ½ Cl2 \u003d SbCl5.
It is a colorless or slightly yellowish liquid that smokes in the air and has a nasty odor; in the cold, it crystallizes in the form of needles and melts at -6 °; it is volatile SbCl 3, but partly decomposes during distillation:
SbCl5 \u003d SbCl3 + Cl2;
under a pressure of 22 mm it boils at 79 ° - without decomposition (under these conditions the boiling point of SbCl 3 \u003d 113.5 °). The vapor density at 218 ° and at a pressure of 58 mm is 10.0 relative to air, which corresponds to the above partial formula (for SbCl 5 the calculated vapor density is 10.3). With the calculated amount of water at 0 ° SbCl 5 gives a crystalline hydrate SbCl 5 + H 2 O, soluble in chloroform and melting at 90 °; with a large amount of water a clear solution is obtained, which upon evaporation over sulfuric acid gives another crystalline hydrate SbCl 5 + 4H 2 O, which is no longer soluble in chloroform (Anschutz and Evans, Weber). SbCl 5 refers to hot water as an acid chloride, giving its acidic hydrate in excess (see below). S. pentichloride easily transforms into trichloride if there are substances capable of attaching chlorine, as a result of which it is often used in organic chemistry for chlorination; it is a "chlorine transmitter". S. trichloride is capable of forming crystalline compounds and double salts with certain chloride metals; similar compounds are produced by antimony pentachloride with various compounds and oxides. Known compounds of antimony and other halogens, namely SbF 3 and SbF 5, SbBr3, SbJ3 and SbJ 5.
, or antimony anhydride, belongs to the type C trichloride and therefore can be represented by the formula Sb 2 O3, but the determination of the vapor density (at 1560 °, V. Meyer, 1879), which is found to be 19.9 in relation to air, showed that this oxide should give the doubled Sb 4 O6 formula, similarly with arsenous and phosphorous anhydrides. S. oxide occurs in nature in the form of valentine, forming white, shiny prisms of the rhombic system, beats. weight 5.57, and less often - senarmontite - colorless or gray octahedra, with beats. the weight. 5,2-5,3, and sometimes also covers in the form of an earthy coating - antimony ocher - various ores of C. The oxide is also obtained by firing sulfurous C. and arises as the final product of the action of water on SbСl 3 in crystalline form and in amorphous form when processing of metallic or sulfurous sulfur with diluted nitric acid when heated. Sulfur oxide is white; it turns yellow when heated, melts at a higher temperature, and finally volatilizes with white heat. When the molten oxide is cooled, it is obtained in a crystalline form. If carbon oxide is heated in the presence of air, it absorbs oxygen, converting into the nonvolatile oxide SbO 2, or, more likely, into Sb 2 O4 (see below). The basic properties of sulfur dioxide are very weak, as already indicated above; its salts are most often basic. Of the mineral oxygen acids, almost one sulfuric acid is capable of producing C salts; the average salt Sb 2 (SO4) 3 is obtained when a metal or oxide is heated with concentrated sulfuric acid, in the form of a white mass and crystallizes from slightly diluted sulfuric acid in long, silky needles; water decomposes it into soluble acidic and insoluble basic salt. There are salts with organic acids, for example. basic antimony-potassium salt of tartaric acid, or emetic stone KO-CO-CH (OH) -CH (OH) -CO-O-SbO + ½ H2 O (Tartarus emeticus), rather soluble in water (at 12.5 wt. frequent at 21 °). On the other hand, sulfur oxide possesses weak anhydrite properties, as can be easily seen if a solution of caustic potassium or sodium hydroxide is poured into a solution of SbCl 3: the resulting white precipitate dissolves in an excess of the reagent, similar to the case for solutions of aluminum salts. Salts of antimony acid are known mainly for potassium and sodium, for example, crystallizes from a boiling solution of Sb 2 O3 in caustic soda antimony sodium NaSbO2 + 3H2 O, in shiny octahedra; such salts are also known - NaSbO 2 + 2HSbO2 and KSbO 2 + Sb2 O3 [Perhaps this salt can be considered as a basic double salt, potassium-antimony, ortho-antimony acid -
]. The corresponding acid, ie, metacid (by analogy with the names of phosphoric acids), HSbO 2, however, is unknown; ortho- and pyroacids are known: H 3 SbO3 is obtained in the form of a fine white powder by the action of nitric acid on a solution of the mentioned double salt of tartaric acid and has this composition after drying at 100 °; Н 4 Sb2 O5 is formed if an alkaline solution of trisulfurous sulfur is exposed to the action of copper sulfate in such an amount that the filtrate ceases to give an orange precipitate with acetic acid - the precipitate then turns white and has the specified composition.
The highest oxide of the type C pentachloride is antimony anhydride Sb2 O5. It is obtained by the action of vigorously boiling nitric acid on the sulfur powder or on its oxide; the resulting powder is then gently heated; it usually contains an admixture of a lower oxide. In pure form, the anhydride can be obtained from solutions of salts of antimony acid, decomposing them with nitric acid and subjecting the washed precipitate to heating until complete removal of water elements; it is a yellowish powder, insoluble in water, however, giving it the ability to dye a blue litmus paper red. In nitric acid, the anhydride is completely insoluble, in hydrochloric acid (strong) it dissolves, albeit slowly, completely; when heated with ammonia, it can evaporate. There are three known hydrates of antimony anhydride having a composition corresponding to hydrates of phosphoric anhydride. Ortho-antimic acid H3 SbO4 is obtained from potassium metastimic acid by treatment with dilute nitric acid and has the proper composition after washing and drying at 100 °; at 175 ° it turns into the metacid HSbO3; both hydrates are white powders, soluble in solutions of caustic potassium and difficult - in water; when heated, they turn into anhydride. Pyrostimonic acid(Fremy called it metacid) is obtained by the action of hot water on pentachloride C. in the form of a white precipitate, which, when dried in air, has the composition H 4 Sb2 O7 + 2H 2 O, and at 100 ° it turns into anhydrous acid, which at 200 ° ( and even just when standing under water - over time) turns into metacid. The pyro acid is more soluble in water than the ortho acid; it is also capable of dissolving in cold ammonia, which orthoacid is not capable of. Salts are known only for meta- and pyroacids, which probably gives the right to give the ortho-acid the formula HSbO 3 + H 2 O, to consider it a hydrate of metacid. Sodium and potassium metasalts are obtained by fusion of the powder of metallic sulfur (or from sulfurous sulfur) with the corresponding nitrate. With KNO 3, after washing with water, a white powder is obtained, which is soluble in an appreciable amount in water and is capable of crystallizing; the salt isolated from the solution and dried at 100 ° contains water 2KSbO3 + 3H2O; at 185 ° it loses one particle of water and turns into KSbO 3 + H2 O. The corresponding sodium salt has the composition 2NaSbO3 + 7H2 O, which at 200 ° loses 2H 2 O and becomes anhydrous only with red heat. Even carbonic acid is capable of decomposing these salts: if CO2 is passed through a solution of potassium salt, then a sparingly soluble precipitate of such an acid salt is obtained 2K 2 O ∙ 3Sb2 O5 + 7H2 O (this is after drying at 100 °, after drying at 350 ° there is still 2H 2 O). If you dissolve metacid in a hot ammonia solution, then on cooling, the ammonium salt (NH 4) SbO3 crystallizes, which is difficult to dissolve in the cold. Oxidizing sulfuric oxide, dissolved in caustic potassium (antimony-sour potassium), with a chameleon and then evaporating the filtrate, we obtain acid pyrosantimic acid potassiumK 2 H2 Sb2 O7 + 4H 2 O; this salt is quite soluble in water (at 20 ° - 2.81 hours of anhydrous salt in 160 hours of water) and serves as a reagent for qualitative analysis for sodium salts (in an average solution), since the corresponding crystalline salt is Na 2 H2 Sb2 O7 + 6H2 O is very difficult to dissolve in water. This can be said to be the most difficultly soluble sodium salt, especially in the presence of a certain amount of alcohol; when there is only 0.1% sodium salt in the solution, then a crystalline pyrosalt precipitate also appears. Since the antimony salts of lithium, ammonium and alkaline earth metals also form precipitates, it is clear that these metals must be removed beforehand. Salts of other metals are hardly soluble or insoluble in water; they can be obtained through double decomposition in the form of crystalline precipitates and are converted by weak acids into acidic salts, while strong acids displace antimonic acid completely. Almost all antimoniates are soluble in hydrochloric acid.
With strong heating in air of each of the described oxides of sulfur, another oxide is obtained, namely Sb 2 O4:
Sb2 O5 \u003d Sb2 O4 + ½O2 and Sb 2 O3 + ½O2 \u003d Sb2 O4.
This oxide can be considered to contain trivalent and pentavalent sulfur, ie, in this case, it would be the average salt of orthosantimonic acid Sb "" SbO4 or the basic salt of metacid OSb-SbO 3. This oxide is the most stable at high temperatures and represents an analogy with red lead (see Lead) and in particular with the corresponding bismuth oxide Bi 2 O4 (see Bismuth). Sb 2 O4 is a non-volatile white powder that is very difficult to dissolve in acids and is obtained together with Sb 2 O3 during the burning of natural sulfurous C. - Sb2 O4 has the ability to combine with alkalis; when fusion with potash, after washing with water, a white product is obtained, soluble in hot water and having the composition K 2 SbO5; this salt-like substance is, perhaps, the double antimony-potassium salt of orthosanbic acid (OSb) K 2 SbO4. Hydrochloric acid precipitates from the solution of such a salt the acidic salt K 2 Sb4 O9, which can be considered a double salt of pyrosantimic acid, namely (OSb) 2 K2 Sb2 O7. In nature, there are similar double (?) Salts for calcium and copper: romeite (OSb) CaSbO4 and ammyolite (OSb) CuSbO4. C. can be weighed in the form of Sb 2 O4 during quantitative analysis; it is only necessary to calcine the flushed oxygen compound of the metal with good air access (in an open crucible) and take great care that combustible gases from the flame do not enter the crucible.
By the method of formation of sulfur compounds, sulfur, like arsenic, can be ranked among real metals with greater justification than, for example, chromium. All compounds of trivalent sulfur in acidic solutions (best of all in the presence of hydrochloric acid) under the action of hydrogen sulfide are transformed into an orange-red precipitate of trisulfurous sulfur, Sb 2 S3, which, in addition, contains water. Compounds of pentavalent C., also in the presence of hydrochloric acid, with hydrogen sulfide give a yellowish-red powder of pentavalent C. Sb 2 S5, which usually contains an admixture of Sb 2 S3 and free sulfur; pure Sb 2 S5 is obtained when, at ordinary temperature, an excess of hydrogen sulfide water is added to an acidified solution of antimony salt (Bunsen); in a mixture with Sb 2 S3 and sulfur, it is obtained if hydrogen sulfide is passed into a heated acidic solution; the lower the temperature of the precipitated solution and the faster the flow of hydrogen sulfide, the less Sb 2 S3 and sulfur are obtained and the cleaner the precipitated Sb 2 S5 (Bosêk, 1895). On the other hand, Sb 2 S3 and Sb 2 S5, like the corresponding arsenic compounds, have the properties of anhydrides; these are thioanhydrides; combining with ammonium sulfide or with potassium sulfide, sodium, barium, etc., they give thiosalts, for example. Na 3 SbS4 and Ba 3 (SbS4) 2 or KSbS 2, etc. These salts are apparently analogous to the oxygen salts of elements of the phosphorus group; they contain bivalent sulfur instead of oxygen and are usually called sulfosalts, which leads to confusion of concepts, recalling the salts of organic sulfonic acids, which would always be best called sulfonic acids [Similarly, the names of sulfonic anhydrides (SnS 2, As2 S5, etc.) and sulfo bases (N 2 S, BaS, etc.) should be replaced with thio anhydrides and thio bases.]. Trisulfur C. Sb 2 S3 under the name antimony luster represents the most important ore C .; it is quite common among crystalline and older layered rocks; found in Cornwallis, Hungary, Transylvania, Westphalia, Black Forest, Bohemia, Siberia; in Japan it is found in the form of especially large, well-formed crystals, and in Borneo, significant deposits are found. Sb 2 S3 crystallizes in prisms and usually forms radiant-crystalline, grayish-black masses with a metallic sheen; beats weight 4.62; fusible and easily crushed into a powder that stains fingers like graphite and has long been used (Bible, Book of the Prophet Ezekiel, XXIII, 40) as a cosmetic agent for eyeliner; under the name "antimony" it was used and, probably, is still used for this purpose in our country. Black sulphurous S. in trade (Antimonium crudum) is smelted ore; this material at fracture presents gray color, metallic luster and crystalline addition. In addition, in nature, there are numerous salt-like compounds Sb 2 S3 with various sulfur metals (thio bases), for example: berthierite Fe (SbS2) 2, wolfsbergite CuSbS2, boulangerite Pb3 (SbS3) 2, pyrargyrite, or red silver ore, Ag 3 SbS3, etc. Ores containing, in addition to Sb 2 S3, sulphurous zinc, copper, iron and arsenic, are the so-called. faded ores. If molten trisulfide sulfur is rapidly cooled to solidification (poured into water), then it is obtained in an amorphous form and then has a lower beats. weight, namely 4.15, has a lead-gray color, in thin layers it shines through with hyacinth-red and in the form of a powder has a red-brown color; it does not conduct electricity, which is characteristic of crystalline modification. From the so-called. antimony liver (hepar antimontii), which is obtained by fusing crystalline Sb 2 S3 with caustic potash or potash and contains a mixture of thioantimoniite and potassium antimoniite [Solutions of such a liver are very capable of absorbing atmospheric oxygen. Another variety of liver, which is prepared from a powdery mixture of Sb 2 S3 and nitrate (in equal amounts), and the reaction starts from a hot coal thrown into the mixture, and proceeds very vigorously with the gradual addition of the mixture, contains, in addition to KSbS 2 and KSbO 2, also K 2 SO4, as well as a certain amount of antimony acid (K-salt).]:
2Sb2 S3 + 4KOH \u003d 3KSbS2 + KSbO2 + 2H2 O
in the same way, amorphous trisulfurous sulfur can be obtained, for which the liver is removed with water and the filtered solution is decomposed with sulfuric acid, or crystalline Sb 2 S3 is treated with a boiling solution of KOH (or K 2 CO 3), and then the filtrate is decomposed with acid; in both cases, the precipitate is washed with highly diluted acid (tartaric at the end) and water and dried at 100 °. The result is a light red-brown, easily soiled powder of sulfurous sulfur, which is soluble in hydrochloric acid, caustic and carbonic alkalis much easier than crystalline Sb 2 S3. Similar preparations of sulfurous S., only not completely pure, have long been known under the name of "mineral kermes" and have been used in medicine and as a paint. The orange-red precipitate of Sb 2 S3 hydrate, which is obtained by the action of hydrogen sulfide on acidic solutions of C. oxide, loses (washed) water at 100 ° -130 ° and turns into a black transformation at 200 °; under a layer of dilute hydrochloric acid in a stream of carbon dioxide, this transformation takes place already during boiling (Mitchell's lecture experiment, 1893). If you add hydrogen sulphide water to a solution of emetic stone, you get an orange-red (in transmitted light) solution of colloidal Sb 2 S3, which precipitates when calcium chloride and some other salts are added. Heating in a stream of hydrogen leads Sb 2 S3 to the complete reduction of the metal, while in a nitrogen atmosphere it only sublimes. Crystalline Sb 2 S3 is used for the preparation of other C. compounds, and is also used as a combustible substance mixed with berthollet's salt and other oxidants for pyrotechnic purposes; it is a part of Swedish match heads and is used for other ignition devices; it also has medicinal value as a laxative for animals (horses). Pentasulphurous sulfur can be obtained as indicated above or by decomposition with dilute acid of the above-mentioned soluble thiosalts:
2K З SbS4 + 6HCl \u003d Sb2 S5 + 6KCl + 3H2 S.
It does not occur in nature, but has been known for a long time; Glauber described (in 1654) obtaining it from the slag that is formed during the preparation of metallic S. from the antimony luster by fusing it with tartar and saltpeter by the action of acetic acid and recommended it as a laxative (panacea antimonialis seu sulfur purgans universale). This sulphurous compound has to be dealt with in analysis: hydrogen sulfide precipitates metals of the 4th and 5th analytical groups from the acidified solution; among the latter is S .; it is usually precipitated in the form of a mixture of Sb 2 S5 and Sb 2 S3 (see above) or only in the form of Sb 2 S 3 (when there were no SbX 5 compounds in the precipitated solution) and then separated by the action of ammonium polysulfide from the sulfurous metals 4th groups that remain in the sediment; Sb 2 S3 is converted by polysulphurous ammonium to Sb 2 S5, and then all of the sulfur is in solution in the form of a higher type ammonium thiosalt, from which, after filtration, it precipitates with acid together with each other. sulfide metals of the 5th group, if any were in the test substance. Pentasulfuric sulfur is insoluble in water, readily soluble in aqueous solutions of caustic alkalis, their carbonate salts, and sulphurous alkali metals, also in ammonium sulphide and in a hot solution of ammonia, but not ammonium carbonate. When Sb 2 S5 is exposed to sunlight or heated under water at 98 °, and also without water, but in the absence of air, then it decomposes according to the equation:
Sb2 S5 \u003d Sb2 S3 + 2S
as a result of which, when heated with strong hydrochloric acid, it gives sulfur, hydrogen sulfide and SbCl 3. Thiosantimic acid nampium, or "Schlippe salt", which crystallizes in large regular tetrahedra, colorless or yellowish, of the composition Na 3 SbS4 + 9H 2 O, can be obtained by dissolving a mixture of Sb 2 S3 and sulfur in a solution of caustic soda of a certain concentration or by fusing anhydrous sodium sulfate and Sb 2 S3 with coal and then boiling an aqueous solution of the resulting alloy with sulfur. Solutions of this salt have an alkaline reaction and a salt, cooling and at the same time bitter-metallic taste. The potassium salt can be obtained in the same way, and the barium salt appears when Sb 2 S5 dissolves in a BaS solution; these salts form crystals of the composition K3 SbS4 + 9H2 O and Ba 3 (SbS4) 2 + 6H 2 O. Penta-sulfuric sulfur is used in the vulcanization of rubber (see) and gives it a well-known brown-red color. Antimony hydrogen
2SbH3 + 6S \u003d Sb2 S З + 3H2 S
whereby an orange-red modification of Sb 2 S3 is obtained; acts in a decomposing manner, even in the dark, and hydrogen sulfide, which itself decomposes during this:
2SbH3 + 3H 2 S \u003d Sb2 S3 + 6H 2.
If SbH 3 (with H 2) is passed into a solution of silver nitrate, a black precipitate is obtained, which is antimony silver with an admixture of metallic silver:
SbH3 + 3AgNO3 \u003d Ag3 Sb + 3HNO3;
this S.'s compound also occurs in nature - discrasite. Solutions of caustic alkalis dissolve SbH 3, acquiring a brown color and the ability to absorb oxygen from the air. Arsenous hydrogen is characterized by similar relationships; both hydrogen compounds do not show the slightest ability to give derivatives of the ammonium type; they are more reminiscent of hydrogen sulfide and exhibit acidic properties. Other hydrogen compounds of hydrogen, which are poorer in hydrogen, are not known with certainty, judging by analogies; metallic sulfur, obtained by electrolysis and capable of exploding, contains hydrogen; perhaps a similar hydrogen compound is present here, which is explosive, like acetylene or hydrazoic acid, poor in hydrogen. The existence of a volatile, even gaseous, hydrogenous compound for sulfur makes it possible, in particular, to classify it as a nonmetal; and its non-metallicity is probably in connection with the ability to give various alloys with metals. Organometallic compounds
FROM . find very significant application; the presence of sulfur in them causes an increase in gloss and hardness, and with significant amounts - and the fragility of metals fused with it. An alloy consisting of lead and sulfur (usually 4 hours and 1 hour) is used for casting typographic letters, for which alloys are often prepared containing, in addition, a significant amount of tin (10-25%), and sometimes also a little copper (about 2%). The so-called. "British metal" is an alloy of 9 parts of tin, 1 part of S. and contains copper (up to 0.1%); it is used for making teapots, coffee pots, etc. utensils. "White, or anti-friction metal" - alloys used for bearings; such alloys contain about 10% sulfur and up to 85% tin, which is sometimes replaced by almost half of lead (Babbit's metall), in addition, up to 5% copper, the amount of which drops in favor of sulfur to 1.5%, if the alloy is lead; 7 hours C. with 3 hours of iron, on white heat, form a "Reaumur alloy", which is very hard and gives sparks when filing.Two crystalline compounds with zinc (Cooke jr.) Zn3 Sb2 and Zn 2 Sb2 are known and a purple alloy with copper of the composition Cu 2 Sb (Regulus Veneris) .Alloys with sodium or potassium, which are prepared by fusing sulfur with carbon dioxide alkali metals and coal, and also by heating sulfur oxide with tartar, are fairly constant in the continuous state in air. but in the form of powders and with a significant content of alkali metal, they can spontaneously ignite in air, and hydrogen is released with water, giving a caustic alkali in solution and antimony powder in the sediment. , contains up to 12% ka lium and is used to obtain organometallic compounds of C. (see. (See also Alloys.)
2SbCl3 + 3ZnR2 \u003d 2SbR З + 3ZnCl2,
where R \u003d CH 3 or C 2 H5, etc., as well as in the interaction of RJ, iodide alcohol radicals, with the above-mentioned alloy of C. with potassium. Trimethylstibine Sb (CH3) 3 boils at 81 °, sp. weight 1.523 (15 °); triethylstibine boils at 159 °, beats. weight 1.324 (16 °). They are almost water-insoluble, onion-smelling liquids that ignite spontaneously in air. Connecting with RJ, stibins give iodide stibonia R4 Sb-J, from which - completely analogous to tetrasubstituted hydrocarbon radicals ammonium iodide, phosphonium and arsonium - it is possible to obtain basic hydrates of substituted stibonium oxides R 4 Sb-OH, which have the properties of caustic alkalis. But, in addition, stibines are very similar in their relations to bivalent electropositive metals; they not only easily combine with chlorine, sulfur and oxygen, forming salt-like compounds, for example. (CH 3) 3 Sb \u003d Cl2 and (CH 3) 3 Sb \u003d S, and oxides, for example (CH 3) 3 Sb \u003d O, but even displace hydrogen from acids, like zinc, for example:
Sb (C2 Н 5) 3 + 2СlH \u003d (С 2 H5) 3 Sb \u003d Сl 2 + Н 2.
Sulphurous stibines precipitate sulphurous metals from salt solutions, turning into the corresponding salts, for example:
(C2 H5) 3 Sb \u003d S + CuSO4 \u003d CuS + (C2 H5) 3 Sb \u003d SO4.
A solution of its oxide can be obtained from stibine sulfate by precipitating sulfuric acid with caustic barite:
(C2 H5) 3 Sb \u003d SO 4 + Ba (OH) 2 \u003d (C 2 H5) 3 Sb \u003d O + BaSO 4 + H 2 O.
Such oxides are also obtained by careful action of air on stibines; they are soluble in water, neutralize acids and precipitate real metal oxides. In composition and structure, the oxides of stibines are completely analogous to the oxides of phosphines and arsines, but differ from them in strongly expressed basic properties. Triphenylstibine Sb (C6 H5) 3, which is obtained by the action of sodium on a benzene solution of a mixture of SbCl 3 with phenyl chloride and crystallizes in transparent plates melting at 48 °, is capable of combining with halogens, but not with sulfur or CH 3 J: presence of negative phenyls lowers, next, the metallic properties of stibins; this is all the more interesting because the corresponding ratios of analogous compounds of more metallic bismuth are completely reversed: bismuthines Β iR3 containing limiting radicals are not capable of addition at all, a Β i (C6 Η 5) 3 gives (C 6 H5) 3 Bi \u003d Cl2 and (C 6 H5) 3 Bi \u003d Br 2 (see Bismuth). As if the electropositive character of Bi must be weakened by electronegative phenyls to form a compound like a metal divalent atom. S. S. Kolotov.
Encyclopedic Dictionary of F.A. Brockhaus and I.A. Efron. - S.-Pb .: Brockhaus-Efron... - GOLD (lat. Aurum), Au (read "aurum"), a chemical element with atomic number 79, atomic mass 196.9665. It has been known since ancient times. In nature, there is one stable isotope, 197Au. Configuration of external and pre-external electronic enclosures ... ... encyclopedic Dictionary
- (French Chlore, German Chlor, English Chlorine) an element from the group of halogens; sign it Cl; atomic weight 35.451 [According to Clarke's calculation of Stas data.] at O \u200b\u200b\u003d 16; particle Cl 2, to which the densities found by Bunsen and Regno correspond well with respect to ... ...
- (chem.; Phosphore French, Phosphor German, Phosphorus English and Latin, whence the designation P, sometimes Ph; atomic weight 31 [In modern times, the atomic weight of F. is found (van der Plaats) as follows: 30.93 by restoration with a certain weight of F. metal ... ... Encyclopedic Dictionary of F.A. Brockhaus and I.A. Efron
Encyclopedic Dictionary of F.A. Brockhaus and I.A. Efron
- (Soufre French, Sulfur or Brimstone English, Schwefel German, θετον Greek, Latin Sulfur, whence the symbol S; atomic weight 32.06 at O \u200b\u200b\u003d 16 [Determined by Stas by the composition of silver sulfide Ag 2 S]) belongs to among the most important non-metallic elements. ... ... Encyclopedic Dictionary of F.A. Brockhaus and I.A. Efron
- (Platine fr., Platina or um English, Platin German; Pt \u003d 194.83, if O \u003d 16 according to K. Seibert). P. is usually accompanied by other metals, and those of these metals that are adjacent to it in their chemical properties are called ... ... Encyclopedic Dictionary of F.A. Brockhaus and I.A. Efron
- (Soufre French, Sulfur or Brimstone English, Schwefel German, θετον Greek, Latin Sulfur, whence the symbol S; atomic weight 32.06 at O \u200b\u200b\u003d 16 [Determined by Stas by the composition of silver sulfide Ag2S]) belongs to the number the most important non-metallic elements. She… … Encyclopedic Dictionary of F.A. Brockhaus and I.A. Efron
S; g. [Persian. surma metal] 1. Chemical element (Sb), bluish white metal (used in various alloys in technology, in printing). Smelting antimony. Antimony-sulfur compound. 2. In the old days: dye for blackening hair, eyebrows, eyelashes. ... ... encyclopedic Dictionary
- (pers. sourme). A metal naturally occurring in conjunction with sulfur; used in medicine as an emetic. Dictionary of foreign words included in the Russian language. Chudinov AN, 1910. ANTIMONY, gray metal; beats in. 6.7; ... ... Dictionary of foreign words of the Russian language
DEFINITION
Antimony - the fifty-first element of the Periodic Table. Designation - Sb from Latin "stibium". Located in the fifth period, VA group. Refers to semimetals. The nuclear charge is 51.
Antimony occurs naturally in combination with sulfur - in the form of antimony luster] 6 or antimonite, Sb 2 S 3. Despite the fact that the content of antimony in the earth's crust is relatively low, antimony was known in ancient times. This is due to the prevalence of antimony luster in nature and the ease of obtaining antimony from it.
In a free state, antimony forms silvery-white crystals (Fig. 1) with a metallic luster and a density of 6.68 g / cm 3. Resembling a metal in appearance, crystalline antimony is fragile and conducts heat and electric current much worse than ordinary metals. In addition to crystalline antimony, other allotropic modifications are also known.
Figure: 1. Antimony. Appearance.
Atomic and molecular weight of antimony
The relative molecular weight of the substance (M r) is a number showing how many times the mass of a given molecule is greater than 1/12 of the mass of a carbon atom, and relative atomic mass of an element (A r) - how many times the average mass of atoms of a chemical element is more than 1/12 of the mass of a carbon atom.
Since in a free state antimony exists in the form of monatomic Sb molecules, the values \u200b\u200bof its atomic and molecular masses coincide. They are equal to 121,760.
Antimony isotopes
It is known that in nature antimony can be found in the form of two stable isotopes 121 Sb (57.36%) and 123 Sb (42.64%). Their mass numbers are 121 and 123, respectively. The nucleus of the antimony isotope 121 Sb contains fifty-one protons and seventy neutrons, and the 123 Sb isotope contains that number of protons and seventy-two neutrons.
There are artificial unstable isotopes of antimony with mass numbers from 103 to 139, as well as more than twenty isomeric states of nuclei, among which the longest-lived isotope 125 Sb with a half-life of 2.76 years.
Antimony ions
At the external energy level of the antimony atom, there are five electrons, which are valence:
1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2 5p 3.
As a result of chemical interaction, antimony gives up its valence electrons, i.e. is their donor, and turns into a positively charged ion or accepts electrons from another atom, i.e. is their acceptor and turns into a negatively charged ion:
Sb 0 -3e → Sb 3+;
Sb 0 -5e → Sb 5+;
Sb 0 + 3e → Sb 3-.
Molecule and atom of antimony
In the free state, antimony exists in the form of monatomic Sb molecules. Here are some properties that characterize antimony atom and molecule:
Antimony alloys
Antimony is added to some alloys to harden them. An alloy consisting of antimony, lead and a small amount of tin is called typographic metal, or garte, and is used to make typographic type. From an alloy of antimony with lead (from 5 to 15% Sb), lead-acid battery plates, sheets and pipes for the chemical industry are made.
Examples of problem solving
EXAMPLE 1
Antimony is a poisonous metal (semi-metal),
used in metallurgy, medicine and engineering
Toxic and poisonous stones and minerals
Antimony (Latin Stibium, denoted by the symbol Sb) is an element with atomic number 51 and atomic weight 121.75. It is an element of the main subgroup of the fifth group, the fifth period of the periodic system of chemical elements of D.I. Mendeleev. Antimony is a metal (semi-metal) of silvery-white color with a bluish tint, coarse-grained structure. In its usual form, it forms crystals with a metallic luster and a density of 6.68 g / cm3.
Resembling metal in appearance, crystalline antimony is fragile and conducts heat and electric current worse than conventional metals. In nature, two stable isotopes are known, 121Sb (isotopic abundance 57.25%) and 123Sb (42.75%). In the photo - Antimony. Tulare District, pcs. California. USA. Photo: A.A. Evseev.
Mankind has been familiar with antimony since ancient times: in the countries of the East, it was used about 3000 years BC. e. for the manufacture of vessels. Antimony compound - antimony gloss (natural Sb2S3) was used for dyeing eyebrows and eyelashes black. In ancient Egypt, the powder from this mineral was called mesten or stem, for the ancient Greeks, antimony was known as stími and stíbi, hence the Latin stibium.
Metallic antimony, in view of its fragility, is rarely used, however, due to the fact that it increases the hardness of other metals (tin, lead) and does not oxidize under normal conditions, metallurgists often introduce it as an alloying element in various alloys. Alloys using the fifty-first element are widely used in a wide variety of fields: for battery plates, typographic fonts, bearings (babbits), screens for working with sources of ionizing radiation, dishes, artistic casting, etc.
Pure metallic antimony is mainly used in the semiconductor industry to obtain antimonides (antimony salts) with semiconducting properties. Antimony is a part of synthetic medicinal preparations. Antimony compounds are also widely used: antimony sulfides are used in the manufacture of matches and in the rubber industry. Antimony oxides are used in the production of refractory compounds, ceramic enamels, glass, paints and ceramic products.
Antimony belongs to trace elements (content in the human body is 10–6% by weight). It is known that antimony forms bonds with sulfur atoms, which causes its high toxicity. Antimony exhibits an irritating and cumulative effect, accumulates in the thyroid gland, inhibiting its function and causing endemic goiter... Dust and vapors cause nosebleeds, antimony "foundry fever", pneumosclerosis, affect the skin, and interfere with sexual functions. Nevertheless, since ancient times, antimony compounds have been used in medicine as valuable medicines.
Biological properties
Antimony belongs to trace elements, it is found in many living organisms. It was found that the content of the fifty-first element (per one hundred grams of dry matter) is 0.006 mg in plants, 0.02 mg in marine animals, 0.0006 mg in terrestrial animals. In the human body, the content of antimony is only 10–6% by weight. The entry of the fifty-first element into the body of animals and humans occurs through the respiratory organs (with inhaled air) or the gastrointestinal tract (with food, water, medicines), the average daily intake is about 50 μg. The main depots of antimony accumulation are thyroid, liver, spleen, kidneys, bone tissue, accumulation also occurs in the blood (in erythrocytes mainly antimony accumulates in the oxidation state +3, in the blood plasma - in the oxidation state +5).
The metal is excreted from the body rather slowly, mainly with urine (80%), in small amounts - with feces. However, the physiological and biochemical role of antimony is still unknown and poorly studied; therefore, there are no data on the clinical manifestations of antimony deficiency.
However, there are data on the maximum permissible concentrations of the element for the human body: 10-5-10-7 grams per 100 grams of dry tissue. At a higher concentration, antimony inactivates (interferes with work) a number of enzymes of lipid, carbohydrate and protein metabolism (possibly as a result of blocking sulfhydryl groups).
The fact is that antimony and its derivatives are toxic - Sb forms bonds with sulfur (for example, reacts with the SH-groups of enzymes), which leads to its high toxicity. Accumulating in excess in the thyroid gland, antimony inhibits its function and causes endemic goiter. When entering the digestive tract, antimony and its compounds do not cause poisoning, since Sb (III) salts are hydrolyzed to form poorly soluble products that are excreted from the body: irritation of the gastric mucosa occurs, reflex vomiting occurs, and almost all the amount of antimony taken is thrown out along with the emetics masses.
However, after taking significant amounts of antimony or with its prolonged use, lesions of the gastrointestinal tract can be observed: ulcers, hyperemia, swelling of the mucous membrane. Antimony (III) compounds are more toxic than antimony (V) - they are bioavailable. The taste threshold in water is 0.5 mg / l. The lethal dose for an adult is 100 mg, for children - 49 mg. Maximum concentration limit for Sb in soil is 4.5 mg / kg.
In water, antimony belongs to the second hazard class, has an MPC of 0.005 mg / l, established by the sanitary-toxicological LPV. In natural waters, the standard is 0.05 mg / l. In industrial waste waters discharged to treatment facilities with biofilters, the antimony content should not exceed 0.2 mg / l.
Dust and vapors cause nosebleeds, antimony "foundry fever", pneumosclerosis, affect the skin, and interfere with sexual functions. For antimony aerosols the maximum permissible concentration in the air of the working area is 0.5 mg / m3, in the atmospheric air is 0.01 mg / m3. When rubbed into the skin, antimony causes irritation, erythema, and smallpox-like pustules.
This kind of damage can be observed in professions dealing with antimony: among enamelists (using antimony oxide), among printers (working with printed alloys, British metal). In case of chronic intoxication of the body with antimony, it is necessary to take preventive measures, limit its intake, carry out symptomatic treatment, it is possible to use complexing agents.
Nevertheless, despite the negative factors associated with the toxicity of antimony, it, like its compounds, is used in medicine. Back in the XV-XVI centuries. antimony preparations were used as medicines, mainly as expectorants and emetics. To induce vomiting, the patient was given wine aged in an antimony vessel. One of the antimony compounds, KC4H4O6 (SbO) * H2O, is called vomit. The mechanism of action of such a drug is described by us above.
Antimony. Monarch district (Sb), Gravelott, Limpopo prov. South Africa. Photo: A.A. Evseev.
Interesting Facts
One of the most modern methods of "using" antimony has entered the arsenal of criminologists. The fact is that a bullet from a rifled weapon leaves behind a (tracer) vortex flow - a "trace", in which there are fractions of a number of elements - lead, antimony, barium, copper. When they settle, they leave an invisible "imprint" on the surface.
However, these particles were invisible only until recently, modern developments make it possible to determine the presence of particles and the direction of flight of a bullet. It happens as follows: strips of wet filter paper are applied to the surface, then they are placed in an elementary particle accelerator (synchrophasatron) and bombarded with neutrons. As a result of the "shelling", some of the atoms that have passed to the paper (including antimony atoms) are converted into unstable radioactive isotopes, and the degree of their activity makes it possible to judge the content of these elements in the samples and thus determine the trajectory and length of the bullet flight, the characteristics of the bullet, weapons and ammunition.
Many semiconductor materials containing antimony have been obtained in zero gravity aboard the Salyut-6 and Skylab near-Earth space orbital scientific stations.
The author of "The Adventures of the Gallant Soldier Schweik" in the story "The Stone of Life" presents one of the versions of the origin of the name "antimony". In 1460, the abbot of the Stalhausen monastery in Bavaria, the father of one monastery, was looking for a philosopher's stone (an amalgam of gold and ruti - "white gold", evaporated to gold). In those distant times, it would hardly have been possible to find at least one monastery, in whose cells and basements alchemical work would not have taken place (Spain, Almaden, the world's largest deposit of industrial red cinnabar - mercury sulfide, a satellite of antimony deposits, dry volcanic sublimation on incandescent batholiths). The photo below shows deposits of the "cinnabar" type and cinnabar - a companion of antimony in the deposits.
Black antimonite - antimony sulfide, with companions - gray chalcedony
and red cinnabar in druze, Nikitovka, Donetsk region, south-east of Ukraine
In one of the experiments, the abbot mixed the ashes of Jeanne D "Arcs (" The Orleans Virgin "- the pride of France) in a crucible with ashes and double the amount of earth taken from the place of burning (cinnabar). The monk began to heat this" infernal mixture ". After evaporation with coal the result was a heavy dark substance with a metallic luster (mercury) The result upset the abbot - the book said that the cherished "philosopher's stone" should be weightless and transparent (translation errors - expensive and golden).
Disappointed in the "heretical science", Leonardus threw the resulting substance into the monastery courtyard (with stubs - antimonite). He soon noticed that the pigs willingly lick the "stone" (stub) thrown out by him and quickly grow fat. Deciding that a nutrient was discovered for them, which can feed the hungry, the monk prepared a new portion of the "stone of life", pounded it and added this powder to the porridge that his skinny brothers in Christ ate. The next day, forty monks of the monastery died in terrible agony. Repenting of his deed, the abbot cursed the experiments, and renamed the "stone of life" antimonium, that is, a means "against monks." It is not worth vouching for the reliability of the story, as well as for the author of this version.
Chemists of the Middle Ages in Western Europe (Spain) found that almost all metals are often dissolved in molten antimony (an element of the "philosopher's stone-II" - after mercury and its amalgams). Antimony, a metal that devours other metals, is a "chemical predator". Perhaps such reasoning led to the symbolic depiction of antimony in the form of a wolf with an open (gaping) mouth (burns of the chemical production of antimony - "Infernal or Devil's Mouths" Almaden, Spain, Catholic Church of His Majesty the King of Spain).
In Arabic literature, lead and antimony shine was called al-kahkhal (make-up), alko (g) ol, alcofol. It was believed that cosmetic and medical products for the eyes contain a mysterious spirit (genie), hence, probably, volatile liquids began to be called alcohol.
Everyone is familiar with the expression "scorching eyebrows" (applying make-up on the face), which previously denoted a cosmetic operation using antimony sulphide powder Sb2S3. The fact is that antimony compounds have different colors: some are black, others are orange-red. Even in time immemorial, the Arabs traded in the countries of the East eyebrow dye, which contained antimony. The author of the novel "Samvel" describes in detail the technique of this cosmetic operation: "The young man took out a leather bag from his bosom, took a thin pointed gold stick, held it to his lips, breathed on it to make it wet, and dipped it into powder. The stick was covered with a thin layer. black dust. He began to put antimony on his eyes. " During archaeological excavations of ancient burials on the territory of Armenia, all the above-described cosmetic accessories were discovered: a thin pointed gold stick and a tiny casket made of polished marble (theft on Vake in Spain, Middle Ages, Western Europe).
Story
The name of the discoverer of antimony is unknown, since this metal has been known to man since prehistoric times. Articles made of antimony and its alloys (in particular, antimony with copper) have been used by man for many millennia, antimony bronze, used during the Babylonian kingdom, consisted of copper and additives of tin, lead and antimony. Archaeological finds have confirmed the assumption that in Babylon as early as 3 thousand years BC. (together with its geological companion - red cinnabar) vessels were made from antimony, for example, a well-known description of fragments of a vase made of metallic antimony found in Tello (southern Babylonia). Other objects made of antimony were also found, in particular in Georgia, dating back to the 1st millennium BC. e. For the manufacture of products, alloys of antimony with lead were also used, and it should be noted that in ancient times metallic antimony was not considered an independent metal, and it was taken for lead (an imitator of a transitional chemical industrial form of mercury - an aphrodisiac for women).
With regard to compounds of antimony, the most famous "antimony luster" - antimony sulphide Sb2S3, which was known in many countries. In India, Mesopotamia, Egypt, Central Asia and other Asian countries, a fine shiny black powder was made from this mineral, which was used for cosmetic purposes, especially for making up the eyes "eye ointment". Pliny the Elder calls antimony stimmi and stibi - cosmetic and pharmaceutical products for making up and treating eyes. In the Greek literature of the Alexandrian period, these words mean a black cosmetic (black powder).
As for the Russian word "antimony", then, most likely, it has a Turkic origin - surme. The original meaning of this term was - ointment, make-up, rubbing. This is confirmed by the preservation of this word to our time in many oriental languages: Turkish, Persian, Uzbek, Azerbaijani and others. According to other sources, "antimony" comes from the Persian "surme" - metal. In Russian literature of the early 19th century, the words antimyak (Zakharov, 1810), surma, surma, surma kinglet and antimony are used.
Being in nature
Despite the fact that the content of antimony in the earth's crust is relatively low - the average content (clarke) is 5 ∙ 10-5% (500 mg / t) - it was known in ancient times. This is not surprising, because antimony is part of about a hundred minerals, the most common of which is the antimony luster Sb2S3 - a lead-gray mineral with a metallic luster (aka antimonite, aka stibnite), containing more than 70% antimony and serving as the main industrial raw material for receiving it. The bulk of the antimony luster is formed in hydrothermal deposits, where its accumulations create deposits of antimony ore in the form of veins and sheet-like bodies. In the upper parts of the ore bodies, near the surface of the earth, the antimony luster undergoes oxidation, forming a number of minerals, namely: senarmontite and valentite Sb2O3 (both minerals of the same chemical composition, contain 83.32% antimony and 16.68% oxygen); servantite (antimony ocher) Sb2O4; stibiocanite Sb2O4 ∙ nH2O; kermesite Sb2S2O. In rare cases, antimony ores (due to their affinity with sulfur) are represented by complex sulfides of antimony, copper, mercury, lead, iron (berthierite FeSbS4, jamesonite Pb4FeSb6S14, tetrahedrite Cu12Sb4S13, livingstonite HgSb4Sb and others), oxychlorite Sb and others antimony.
The content of antimony in igneous effusive rocks is lower than in sedimentary rocks (volcanic sublimation along cracks from hot magma on a catalyst from the caldera - water). In sedimentary, the highest concentrations of antimony are found in shales (1.2 g / t), bauxite and phosphorites (2 g / t) and the lowest in limestones and sandstones (0.3 g / t). Increased amounts of antimony are found in coal ash (it conflicts with cinnabar with water - cinnabar is formed on arsenic).
In natural compounds, antimony, on the one hand, exhibits the properties of a metal and is a typical chalcophilic element, forming antimonite. At the same time, antimony has metalloid properties, manifested in the formation of various sulfosalts - boulangerite, tetrahedrite, bournonite, pyrargyrite and others. With a number of metals (palladium, arsenic), antimony is capable of creating intermetallic compounds. In addition, isomorphic substitution of antimony and arsenic is observed in nature in fahlores and geocronite Pb5 (Sb, As) 2S8, and antimony and bismuth in cobellite Pb6FeBi4Sb2S16, etc.
It should be noted that antimony is also found in its native state. Native antimony is a Sb mineral, sometimes with an insignificant admixture of silver, arsenic, bismuth (up to 5%). It occurs in the form of granular masses (crystallizing in a trigonal system), drip formations and rhombohedral lamellar crystals.
Native antimony has a metallic luster, a tin-white color with a yellow tarnish. It is formed with a deficiency of sulfur in low-temperature antimony, antimony-gold-silver and copper-lead-zinc-antimony-silver-arsenic, as well as high-temperature pneumatolytic-hydrothermal antimony-silver-tungsten deposits (in the latter, the antimony content in the latter can reach Finland - antimony crystal shield).
The content of antimony in the bed ore bodies is from 1 to 10%, in the veins - from 3 to 50%, the average content is from 5 to 20%, sometimes more. Bed ore bodies are formed by means of low-temperature hydrothermal solutions by filling cracks in rocks, as well as by replacing the latter with antimony minerals. Two types of deposits are of major industrial importance: stratal bodies, lenses, nests and stockworks in mature mantle-like deposits formed as a result of metasomatic replacement of limestones with silica and antimony compounds under the shale screen (in China - Sikuanshan, in the CIS - Kadamjay, Tereksay Sredney, Jizhikrut Asia). The second type of deposits is a system of steeply dipping intersecting quartz-antimonite veins in shales (in the CIS - Turgayskoye, Razdolninskoye, Sarylakh, etc.; in South Africa - Gravelot, etc.). The third is vertical cracks (Donetsk region, south-east of Ukraine, Nikitovka). Rich deposits of antimony minerals have been found in China, Bolivia, Japan, USA, Mexico, and a number of African countries.
Application
Due to its fragility, metallic antimony is rarely used, but since it increases the hardness of other metals (for example, tin and lead) and does not oxidize under normal conditions, metallurgists introduce it into various alloys. The total number of alloys containing the fifty-first element is close to two hundred. Alloying a number of alloys with antimony was known back in the Middle Ages: "If by fusion a certain portion of antimony is added to the tin, a typographic alloy is obtained ( garth), from which the font used by those who receive the books is made. "
It's incredible, but such an alloy - garth (in Ukrainian - " hardening", - antimony, tin and lead), containing from 5 to 30% Sb - an indispensable attribute of typography! What is the uniqueness of the alloy that has passed through the centuries? Molten antimony, unlike other metals (except bismuth and gallium), expands during solidification Thus, when the type is cast, the typographic alloy containing antimony, solidifying in the casting matrix, expands, due to which it tightly fills it and reproduces a mirror image, which is transferred to the paper. In addition, antimony gives the typographic alloy hardness and wear resistance, which is important when reusing a template (matrix, typographic form).
Lead-antimony alloys used in chemical engineering (for lining baths and other acid-resistant equipment) have high hardness and corrosion resistance. The most famous alloy of gartbles (Sb content from 5 to 15%) is used for the manufacture of pipes, through which corrosive liquids are transported. Sheaths of telegraph, telephone and electric cables, electrodes, battery plates, bullet cores, shot, shrapnel are made of the same alloy. Bearing alloys (babbits) containing tin, copper, lead and antimony (Sb from 4 to 15%) have found wide application (machine-tool building, rail and road transport); they have sufficient hardness, high abrasion resistance, and high corrosion resistance. Antimony is also added to metals intended for thin and brittle castings.
Pure antimony is used to obtain antimonides (AlSb, CaSb, InSb), as well as an additive in the production of semiconductor compounds. The most important semiconductor metal, germanium, is alloyed with such antimony (only 0.000001%) in order to improve its quality. A number of its compounds (in particular, with gallium and indium) are semiconductors. Antimony is used in the semiconductor industry not only as a legend. Antimony is also used in the production of diodes (AlSb and CaSb), infrared detectors, and Hall-effect devices. Indium antimonide is used to build Hall sensors, to convert non-electrical quantities into electrical ones, in calculating devices, as a filter and recorder of infrared radiation. Due to its large band gap, AlSb is used to build solar cells.
The "activity" of antimony compounds is also diverse. For example, antimony trioxide (oxide) (Sb2O3) is mainly used as a pigment for paints, a muffler for enamel, mordant in the textile industry, in the production of refractory compounds and paints, it is also used for the manufacture of optical (anti-reflective) glass, ceramic enamels.
Antimony pentoxide (Sb2O5) is widely used in the manufacture of pharmaceuticals, in the production of glass, ceramics, paints, in the textile and rubber industries, as a component of fluorescent fluorescent lamps (in fluorescent lamps, calcium halophosphate is activated by Sb). Antimony trisulfide is used in the manufacture of matches and in pyrotechnics. Antimony five-sulfur is used for vulcanization of rubber (for "medical" rubber, which contains Sb2S5, a characteristic red color and high elasticity). Antimony trichloride (SbCl3) is used for bluing steel, blackening zinc, in medicine, as a mordant in the textile industry and as a reagent in analytical chemistry.
Poisonous stibine or antimony hydrogen SbH3 - used as a fumigant to fight insect pests of agricultural plants. Many antimony compounds can serve as pigments in paints, for example, potassium antimony (K2O * 2Sb2O5) is widely used in the production of ceramics, antimony paint, which is based on antimony trioxide, is used to paint underwater parts and above-deck buildings of ships. Sodium metastimonic acid (NaSbO3) called "leukonin" is used to coat kitchen utensils, as well as in the production of enamel and white milk glass.
Production
Antimony is a rather rare element, in the earth's crust there is no more than 5 ∙ 10-5%, however, more than a hundred minerals are known to contain this element. A widespread and semi-industrial value antimony mineral (not sulfide) is antimony luster, or stibnite, Sb2S3, containing over 70% antimony. The rest of the antimony ores differ sharply from each other in their metal content - from 1 to 60%. It is impractical to obtain metallic antimony from ores containing less than 10% Sb. For this reason, poor ores are beneficiated.
Sulfide (the richest), as well as complex ores are enriched by flotation, and sulphide-oxidized ones - by combined methods. After beneficiation, the ore concentrate contains from 30 to 60% Sb, such raw material is suitable for processing into antimony, which is produced by pyrometallurgical or hydrometallurgical methods. In the first version, the transformations take place in the melt under the influence of high temperature, in the second - in aqueous solutions of antimony compounds and other elements. Pyrometallurgical methods for producing antimony include: precipitation, reduction and direct smelting in shaft furnaces. Precipitation smelting, the raw material for which is sulfide concentrate, is based on the displacement of antimony from its sulfide by iron:
Sb2S3 + 3Fe → 2Sb + 3FeS
The process takes place in reflective or rotary drum furnaces as follows: iron in the form of cast iron or steel shavings is introduced directly into the furnace, then, to form a reducing atmosphere, which prevents losses with the release of volatile antimony (III) oxide, charcoal (coal fines or coke). For slagging waste rock, fluxes - sodium sulfate or soda - are introduced into the charge. The charge is melted at a constant temperature of 1,300-1,400 o C. As a result of precipitation smelting, rough antimony is formed, containing from 95 to 97% Sb (depending on the initial content in the concentrate) and from 3 to 5% of impurities - iron, gold, lead , copper, arsenic and other metals that were contained in the feedstock. The recovery of antimony from the original concentrate ranges from 77 to 92%.
Reduction smelting is based on the reduction of antimony oxides to metal with solid carbon:
Sb2O4 + 4C → 2Sb + 4CO
It is produced in reflective or short drum furnaces at a temperature of 800-1,000 o C. The charge is made up of oxidized ore, charcoal (possibly coal dust) and flux (soda, potash). It turns out that rough antimony is more pure than in precipitation smelting (more than 99% Sb), the metal recovery from the concentrate is 80-90%.
Direct smelting in shaft furnaces is used to smelt metal from oxidized or sulphide lumpy raw materials. The maximum temperature of 1,300-1,500 o C is achieved by combustion of coke - a component of the charge, limestone, pyrite cinders or iron ore act as a flux. The metal is obtained both by reduction with carbon (coal) with Sb2O3 coke, and as a result of the interaction of unoxidized antimonite with Sb2O3 with constant removal of SO2 from the melt with furnace gases. The smelting products (crude metal and slag) flow into the lower part of the furnace and are discharged from it into a settling tank.
Another method of obtaining antimony, hydrometallurgical, has been increasingly used lately. It consists of two stages: the processing of raw materials with the transfer of antimony compounds into a solution and the separation of antimony from these solutions. The complexity of the method lies in the fact that it is problematic to transfer antimony into a solution: most natural antimony compounds do not dissolve in water. However, the desired solvent was found - an aqueous solution of sodium sulfide (120 g / l) and caustic soda (30 g / l). Sulfide and antimony oxide goes into solution in the form of sulfasalts and salts of antimony acids. Antimony is isolated from the resulting solution by electrolysis. The rough antimony obtained by the hydrometallurgical method does not differ in purity and contains from 1.5 to 15% of impurities.
To obtain antimony with a smaller amount of impurities, pyrometallurgical (fire) or electrolytic refining is used. The most widespread fire refining in industry is carried out in reverberatory furnaces. When stibnite is added to the molten rough antimony, impurities of iron and copper form sulfur compounds and pass into matte. Arsenic is removed in the form of sodium arsenate by melting in an oxidizing atmosphere (blowing with air) with soda or potash, while sulfur is also removed.
In the presence of noble metals, anodic electrolytic refining is used to concentrate noble metals in the sludge. Refined antimony no longer contains more than 0.5-0.8% of foreign impurities. However, even such a metal does not satisfy all consumers - for the semiconductor industry, for example, antimony of 99.999% purity is required. In this case, the crystallophysical method of purification is used - zone melting in an argon atmosphere, in especially critical cases, zone melting is repeated several times.
Physical properties
Antimony is known in crystalline form and three amorphous modifications (explosive, black and yellow). In appearance, crystalline, or gray, antimony (its main modification) is a shiny silver-white metal with a bluish tint, which is thinner the more impurities (a pure element in a free state forms needle-like crystals resembling the shape of stars).
Many mechanical properties depend on the purity of the metal. Gray antimony crystallizes in the trigonal (rhombohedral) system (a \u003d 0.45064 nm, z \u003d 2, space group R3m), its density is 6.61-6.73 g / cm3 (in the liquid state - 6.55 g / cm3) ... At a pressure of ~ 5.5 GPa, the rhombohedral lattice of sulfur antimony transforms into the cubic SbII modification. At a pressure of 8.5 GPa - into hexagonal SbIII. Above 28 GPa, SbIV is formed. Crystalline antimony melts at a low temperature - 630.5 o C, molten antimony begins to boil at 1 634 o C.
The specific heat of antimony at temperatures of 20-100 o C is 0.210 kJ / (kg * K) or 0.0498 cal / (g * o C), the thermal conductivity at 20 o C is 17.6 W / (m * K) or 0.042 cal / (cm * sec * o С). The temperature coefficient of linear expansion for polycrystalline antimony is 11.5 * 10-6 at a temperature from 0 to 100 o C; for a single crystal a1 \u003d 8.1 * 10-6, a2 \u003d 19.5 * 10-6 at 0-400 o C, the electrical resistivity at 20 o C is 43.045 * 10-6 cm * cm.
Antimony is diamagnetic, its specific magnetic susceptibility is -0.66 * 10-6. The Brinell hardness for cast metal is 325-340 Mn / m2 (32.5-34.0 kgf / mm2); modulus of elasticity 285-300; tensile strength 86.0 Mn / m2 (8.6 kgf / mm2). The temperature of the transition of antimony to the superconducting state is 2.7 K. Gray antimony has a layered structure, where each Sb atom is pyramidal linked to three neighbors in the layer (interatomic distance 0.288 nm) and has three nearest neighbors in another layer (interatomic distance 0.338 nm). It is this form of antimony that is stable under normal conditions.
With a sharp cooling of the vapors of sulfur antimony, black antimony is formed (density 5.3 g / cm3), which, when heated to 400 o C without access to air, turns into gray antimony. Black antimony has semiconducting properties. Yellow antimony is formed by the action of oxygen on liquid stibine SbH3 and contains small amounts of chemically bound hydrogen. When heated, as well as when illuminated with visible light, yellow antimony transforms into black antimony.
Explosive antimony looks like graphite (density 5.64-5.97 g / cm3) explodes upon impact and friction. This modification is formed during the electrolysis of a SbCl3 solution in hydrochloric acid at a low current density, and contains bound chlorine. Explosive antimony, when rubbed or struck with an explosion, turns into metallic antimony.
It is impossible to say unequivocally that antimony is a metal. Even medieval alchemists ranked it (however, like some true metals: zinc and bismuth, for example) to the group of "semimetals", because they were worse forged, and malleability was considered the main sign of a metal, in addition, according to alchemical ideas, each metal was associated with any heavenly body. By that time, all the known celestial bodies had already been distributed (the Sun was associated with gold, the Moon personified silver, Mercury - mercury, Venus - copper, Mars - iron, Jupiter - tin and Saturn - lead), therefore, independent metals, according to alchemists, no longer existed.
Unlike most metals, antimony, firstly, is fragile and abrades into powder (this can be done in a porcelain mortar with a porcelain pestle), and secondly, it conducts electricity and heat worse (at 0 o C its electrical conductivity is only 3.76 % electrical conductivity of silver). At the same time, crystalline antimony has a characteristic metallic luster, above 310 o C it becomes plastic, in addition, high-purity single crystals are plastic. With sulfuric acid, antimony forms sulfate Sb2 (SO4) 3 and asserts itself in a metallic quality, and nitric acid oxidizes antimony to a higher oxide formed in the form of a hydrated compound xSb2O5 * yH2O, proving its nature as a non-metal. It turns out that the metallic properties of antimony are rather weak, however, the properties of a non-metal are not inherent to it in full.
Chemical properties
The configuration of the outer electrons of the antimony atom is 5s25p3. In compounds, antimony shows similarities with arsenic, but differs from it in pronounced metallic properties, exhibits oxidation states of +5, +3 and -3. Chemically, the fifty-first element is inactive - in air at room temperature, metallic antimony is stable, begins to oxidize at temperatures close to the melting point (~ 600 o C) with the formation of antimony (III) oxide, or antimony anhydride - Sb2O3:
4Sb + 3O2 → 2Sb2O3
above the melting point, antimony ignites. Antimony (III) oxide is an amphoteric oxide with a predominance of basic properties, insoluble, forms minerals. Reacts with alkalis and acids, and in strong acids, for example sulfuric and hydrochloric, antimony (III) oxide dissolves to form antimony (III) salts, in alkalis to form antimony salts H3SbO3 or metantimony HSbO2 acid:
Sb2O3 + 2NaOH → 2NaSbO2 + H2O
Sb2O3 + 6HCl → 2SbCl3 + 3H2O
When Sb2O3 is heated above 700 o C in oxygen, an oxide of the composition Sb2O4 is formed:
2Sb2O3 + O2 → 2Sb2O4
Sb2O4 simultaneously contains tri- and pentavalent antimony. In its structure, octahedral groups and are connected to each other. This antimony oxide is the most stable.
Crushed powdered antimony burns in an atmosphere of chlorine, the fifty-first element actively reacts with other halogens, forming antimony halides. Metallic antimony does not react with nitrogen and hydrogen, just as with silicon and boron, carbon is slightly dissolved in molten antimony. Antimony combines with sulfur, phosphorus, arsenic and many metals during fusion. Combining with metals, antimony forms antimonides, for example, tin antimonide SnSb, nickel Ni2Sb3, NiSb, Ni5Sb2 and Ni4Sb. Antimonides can be considered as products of the replacement of hydrogen in stibine (SbН3) by metal atoms. Some antimonides, in particular AlSb, GaSb, InSb, have semiconducting properties.
Antimony is resistant to water and dilute acids. So, for example, antimony does not dissolve in hydrochloric acid and dilute sulfuric acid. It does not react with hydrofluoric and hydrofluoric acids either. However, concentrated hydrochloric and sulfuric acids slowly dissolve antimony to form chloride SbCl3 and sulfate Sb2 (SO4) 3. Poorly soluble β-antimonic acid HSbO3 is formed with concentrated nitric acid:
3Sb + 5HNO3 → 3HSbO3 + 5NO + H2O
Antimony dissolves in aqua regia - in a mixture of nitric and tartaric acids. Solutions of alkalis and NH3 have no effect on antimony; molten alkalis dissolve antimony to form antimonates.
When heated with nitrates or chlorates of alkali metals, powdered antimony with flash forms antimonic acid salts. Of practical interest are sparingly soluble salts of antimony acid - antimonates (MeSbO3 * 3H2O, where Me - Na, K) and salts of unselected metastimonic acid - metaantimonites (MeSbO2 * 3H2O), which have reducing properties. Antimonates (III) of alkali metals, especially potassium, are soluble in water, unlike other antimonates.
When heated in air, they oxidize to antimonates (V). Known metaantimonates (III), for example KSbO2, orthoantimonates (III), such as Na3SbO3, and polyantimonates, for example NaSb5O8, Na2Sb4O7. Rare earth elements are characterized by the formation of orthoantimonates LnSbO3 and Ln3Sb5O12. Antimonates of nickel, manganese are catalysts in organic synthesis (oxidation and polycondensation reactions), antimonates of rare earth elements are luminophores.
Of the important compounds of antimony, in addition to oxide (III), the following are also isolated: hydride (stibine) SbН3 - a colorless poisonous gas formed by the action of HCl on magnesium or zinc antimonides or a hydrochloric acid solution of SbCl3 on NaBH4. Stibine decomposes slowly at room temperature into antimony and hydrogen, the process is significantly accelerated when heated to 150 o C; it oxidizes, burns in air; slightly soluble in water; used to obtain high purity antimony. Another important compound of the fifty-first element is antimony (V) oxide or antimony anhydride, Sb2O5 (yellow crystals, dissolves in water, forming antimonic acid) has mainly acidic properties.
Interestingly, the lower antimony oxide (Sb2O3) is called antimony anhydride, although this statement is incorrect, because the anhydride is an acid-forming oxide, and in Sb (OH) 3, a Sb2O3 hydrate, the basic properties clearly prevail over acidic ones. Thus, the properties of the lower antimony oxide indicate that antimony is a metal. However, the higher antimony oxide Sb2O5 is indeed an anhydride with clearly pronounced acidic properties, which speaks in favor of the fact that antimony is still a non-metal. It turns out that the dualism observed in the physical characteristics of antimony is also traced in its chemical properties of antimony.
Antimonite. White Caps Mine County Nevada, USA. Photo: A.A. Evseev.
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ADR 6.1
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Risk of poisoning by inhalation, skin contact or swallowing. Are hazardous to the aquatic environment or sewer system
Use a mask for emergency vehicle abandonment
White rhombus, ADR number, black skull and crossbones
ADR 8
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White upper half of a rhombus, black - lower, equal size, ADR number, test tubes, hands
| Name of especially dangerous cargo during transportation | room UN | Class ADR |
| ANTIMONY - POWDER | 2871 | 6.1 |
| Antimony pentafluoride ANTIMONY PENTAFLUORIDE | 1732 | 8 |
| ANTIMONY LACTATE | 1550 | 6.1 |
| Antimony pentafluoride | 1732 | 8 |
| ANTIMONY PENTACHLORIDE LIQUID | 1730 | 8 |
| ANTIMONY PENTACHLORIDE SOLUTION | 1731 | 8 |
| ANTIMONY INORGANIC LIQUID COMPOUND, N.Z.K. | 3141 | 6.1 |
| ANTIMONY COMPOUND, INORGANIC SOLID, N.Z.K. | 1549 | 6.1 |
| ANTIMONY TRICHLORIDE SOLID | 1733 | 8 |
| ANTIMONY-POTASSIUM TARTRATE | 1551 | 6.1 |
Antimony (English Antimony, French Antimoine, German Antimon) has long been known both in the form of metal and in the form of certain compounds. Berthelot describes a fragment of a vase of metal antimony found in Tello (southern Babylonia) and dating back to the early 3rd century. BC e. Other objects made of metallic antimony were also found, in particular in Georgia, dating back to the 1st millennium BC. h. Antimony bronze is well known and was used during the period of the ancient Babylonian kingdom; bronze contained copper and additives - tin, lead and significant amounts of antimony. Alloys of antimony with lead were used for the manufacture of various products. It should be noted, however, that in ancient times, metallic antimony, apparently, was not considered an individual metal, it was taken for lead. Of the compounds of antimony in Mesopotamia, India, Central Asia and other Asian countries, sulphurous antimony (Sb 2 S 3), or the mineral "antimony luster", was known. The mineral was made into a fine, shiny black powder, which was used for cosmetic purposes, especially for eye makeup "eye ointment". However, contrary to all this information about the long-term distribution of antimony and its compounds, the famous researcher in the field of archaeological chemistry Lucas claims that antimony was almost unknown in ancient Egypt. There, he writes, only one case of the use of metallic antimony and a few cases of the use of antimony compounds has been established. In addition, according to Lucas, antimony is present only in the form of impurities in all archaeological metal objects; sulphurous antimony, at least until the time of the New Kingdom, was not used at all for makeup, as evidenced by the coloring of mummies. Meanwhile, back in the III millennium BC. e. in Asian countries and in Egypt itself, there was a cosmetic product called stem, place or stimmi; in the II millennium BC. e. the Indian word for antimony appears; but all these names were used, however, mainly for lead sulphide (lead luster). In Syria and Palestine, long before the beginning of our era. black make-up was called not only stimmi, but also kahkhal or kogol, which in all three cases meant any fine dry or powdered powder in the form of an ointment. Later writers (around the beginning of our era), for example Pliny, call stimmi and stibi - cosmetic and pharmaceutical means for making up and treating eyes. In the Greek literature of the Alexandrian period, these words also mean a black cosmetic (black powder). These names pass into Arabic literature with some variations. So, in Avicenna's "Canon of Medicine", along with stimmy, itmid appears, or atemid - a powder or sediment (paste) of lead. Later, the words al-kakhkhal (grim), alcohol, alcohol, referring mainly to lead luster, appear in the literature. It was believed that cosmetic and medical products for the eyes contain a certain mysterious spirit, hence, probably, volatile liquids began to be called alcohol. Alchemists called the antimony, as well as lead, the brilliance of Antimonium. In the dictionary of Ruland (1612), this word is explained as alcofol, a stone made of lead ore veins, marcasite, saturn, antimony (Stibium), and stibium, or stimmy, as black sulfur or a mineral that the Germans call Spiesglas, later Bpiesglanz (probably derived from stibium). However, despite such confusion in names, it was during the alchemical period in Western Europe that antimony and its compounds were finally distinguished from lead and its compounds. Already in alchemical literature, as well as in the writings of the Renaissance, metallic and sulfurous antimony is usually described quite accurately. Since the XVI century. antimony began to be used for a variety of purposes, in particular in gold metallurgy, for polishing mirrors, and later in printing and medicine. The origin of the word "antimony", which appeared after 1050, is explained in different ways. The story of Vasily Valentine is known about how one monk, who discovered the strong laxative effect of antimony sulphurous on a pig, recommended it to his brothers. The result of this medical advice turned out to be deplorable - after taking the remedy, all the monks died. Therefore, as if antimony received the name derived from "anti-monachium" (a remedy against monks). But all this is more of an anecdote. The word "antimony" is most likely simply a transformed itmid, or atemid, of the Arabs. There are, however, other explanations. So, some authors believe that "antimony" is the result of the reduction of the Greek. anthos ammonos, or the flower of the god Amun (Jupiter); so the antimony luster was allegedly called. Others produce "antimony" from the Greek. anti-monos (opponent of privacy), emphasizing that natural antimony is always combined with other minerals. The Russian word for antimony is of Turkic origin; the original meaning of this word is makeup, ointment, rubbing. This name has been preserved in many oriental languages \u200b\u200b(Persian, Uzbek, Azerbaijani, Turkish, etc.) to our times. Lomonosov considered the element a "semimetal" and called it antimony. Along with antimony, the name antimony also occurs. In Russian literature of the early 19th century. the words antimony are used (Zakharov, 1810), surma, syurma, surma kinglet and antimony.