Antimony

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Antimony, 51Sb
Antimony-4.jpg
Antimony
Pronunciation
Appearancesilvery lustrous gray
Standard atomic weight Ar°(Sb)
Antimony in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
As
↑
Sb
↓
Bi
tin ← antimony → tellurium
Atomic number (Z)51
Group group 15 (pnictogens)
Period period 5
Block   p-block
Electron configuration [ Kr ] 4d10 5s2 5p3
Electrons per shell2, 8, 18, 18, 5
Physical properties
Phase at  STP solid
Melting point 903.78  K ​(630.63 °C,​1167.13 °F)
Boiling point 1908 K​(1635 °C,​2975 °F)
Density (at 20° C)6.694 g/cm3 [3]
when liquid (at  m.p.)6.53 g/cm3
Heat of fusion 19.79  kJ/mol
Heat of vaporization 193.43 kJ/mol
Molar heat capacity 25.23 J/(mol·K)
Vapor pressure
P (Pa)1101001 k10 k100 k
at T (K)8078761011121914911858
Atomic properties
Oxidation states common: −3, +3, +5
−2, ? −1, ? 0, [4] +1, ? +2, ? +4 ?
Electronegativity Pauling scale: 2.05
Ionization energies
  • 1st: 834 kJ/mol
  • 2nd: 1594.9 kJ/mol
  • 3rd: 2440 kJ/mol
  • (more)
Atomic radius empirical:140  pm
Covalent radius 139±5 pm
Van der Waals radius 206 pm
Antimony spectrum visible.png
Spectral lines of antimony
Other properties
Natural occurrence primordial
Crystal structure ​ rhombohedral (hR2)
Lattice constants
Rhombohedral.svg
a = 0.45066 nm
α = 57.112°
ah = 0.43084 nm
ch = 1.12736 nm (at 20 °C) [3]
Thermal expansion 11.04×10−6/K (at 20 °C) [a]
Thermal conductivity 24.4 W/(m⋅K)
Electrical resistivity 417 nΩ⋅m(at 20 °C)
Magnetic ordering diamagnetic [5]
Molar magnetic susceptibility −99.0×10−6 cm3/mol [6]
Young's modulus 55 GPa
Shear modulus 20 GPa
Bulk modulus 42 GPa
Speed of sound thin rod3420 m/s(at 20 °C)
Mohs hardness 3.0
Brinell hardness 294–384 MPa
CAS Number 7440-36-0
History
Discovery Arabic alchemists (before AD 815)
Symbol"Sb": from Latin stibium 'stibnite'
Isotopes of antimony
Main isotopes [7] Decay
abun­dance half-life (t1/2) mode pro­duct
121Sb57.2% stable
123Sb42.8%stable
125Sb synth 2.7576 y β− 125Te
Symbol category class.svg  Category: Antimony
| references

Antimony is a chemical element; it has symbol Sb (from Latin stibium) and atomic number 51. A lustrous grey metal or metalloid, it is found in nature mainly as the sulfide mineral stibnite (Sb2S3). Antimony compounds have been known since ancient times and were powdered for use as medicine and cosmetics, often known by the Arabic name kohl. [8] The earliest known description of this metalloid in the West was written in 1540 by Vannoccio Biringuccio.

Contents

China is the largest producer of antimony and its compounds, with most production coming from the Xikuangshan Mine in Hunan. The industrial methods for refining antimony from stibnite are roasting followed by reduction with carbon, or direct reduction of stibnite with iron.

The most common applications for metallic antimony are in alloys with lead and tin, which have improved properties for solders, bullets, and plain bearings. It improves the rigidity of lead-alloy plates in lead–acid batteries. Antimony trioxide is a prominent additive for halogen-containing flame retardants. Antimony is used as a dopant in semiconductor devices.

Characteristics

Properties

A vial containing the metallic allotrope of antimony Antimon.PNG
A vial containing the metallic allotrope of antimony
Native antimony with oxidation products Antimony massive.jpg
Native antimony with oxidation products
Crystal structure common to Sb, AsSb and gray As SbAs lattice.png
Crystal structure common to Sb, AsSb and gray As

Antimony is a member of group 15 of the periodic table, one of the elements called pnictogens, and has an electronegativity of 2.05. In accordance with periodic trends, it is more electronegative than tin or bismuth, and less electronegative than tellurium or arsenic. Antimony is stable in air at room temperature but, if heated, it reacts with oxygen to produce antimony trioxide, Sb2O3. [9]

Antimony is a silvery, lustrous gray metalloid with a Mohs scale hardness of 3, which is too soft to mark hard objects. Coins of antimony were issued in China's Guizhou in 1931; durability was poor, and minting was soon discontinued because of its softness and toxicity. [10] Antimony is resistant to attack by acids.

The only stable allotrope of antimony under standard conditions [11] is metallic, brittle, silver-white, and shiny. It crystallises in a trigonal cell, isomorphic with bismuth and the gray allotrope of arsenic, and is formed when molten antimony is cooled slowly. Amorphous black antimony is formed upon rapid cooling of antimony vapor, and is only stable as a thin film (thickness in nanometres); thicker samples spontaneously transform into the metallic form. [12] It oxidizes in air and may ignite spontaneously. At 100 °C, it gradually transforms into the stable form. The supposed yellow allotrope of antimony, generated only by oxidation of stibine (SbH3) at −90 °C, is also impure and not a true allotrope; [13] [14] above this temperature and in ambient light, it transforms into the more stable black allotrope. [15] [16] [17] A rare explosive form of antimony can be formed from the electrolysis of antimony trichloride, but it always contains appreciable chlorine and is not really an antimony allotrope. [13] When scratched with a sharp implement, an exothermic reaction occurs and white fumes are given off as metallic antimony forms; when rubbed with a pestle in a mortar, a strong detonation occurs.

Elemental antimony adopts a layered structure (space group R3m No. 166) whose layers consist of fused, ruffled, six-membered rings. The nearest and next-nearest neighbors form an irregular octahedral complex, with the three atoms in each double layer slightly closer than the three atoms in the next. This relatively close packing leads to a high density of 6.697 g/cm3, but the weak bonding between the layers leads to the low hardness and brittleness of antimony. [9]

Isotopes

Antimony has two stable isotopes: 121Sb with a natural abundance of 57.36% and 123Sb with a natural abundance of 42.64%. It also has 35 radioisotopes, of which the longest-lived is 125Sb with a half-life of 2.75 years. In addition, 29 metastable states have been characterized. The most stable of these is 120m1Sb with a half-life of 5.76 days. Isotopes that are lighter than the stable 123Sb tend to decay by β+ decay, and those that are heavier tend to decay by β− decay, with some exceptions. [18] Antimony is the lightest element to have an isotope with an alpha decay branch, excluding 8Be and other light nuclides with beta-delayed alpha emission. [18]

Occurrence

Stibnite, China CM29287 Carnegie Museum of Natural History specimen on display in Hillman Hall of Minerals and Gems Stibnite.jpg
Stibnite, China CM29287 Carnegie Museum of Natural History specimen on display in Hillman Hall of Minerals and Gems

The abundance of antimony in the Earth's crust is estimated at 0.2 parts per million, [19] comparable to thallium at 0.5 ppm and silver at 0.07 ppm. It is the 63rd most abundant element in the crust. Even though this element is not abundant, it is found in more than 100 mineral species. [20] Antimony is sometimes found natively (e.g. on Antimony Peak), but more frequently it is found in the sulfide stibnite (Sb2S3) which is the predominant ore mineral. [19]

Compounds

Antimony compounds are often classified according to their oxidation state: Sb(III) and Sb(V). The +5 oxidation state is more common. [21]

Oxides and hydroxides

Antimony trioxide is formed when antimony is burnt in air. [22] In the gas phase, the molecule of the compound is Sb
4O
6, but it polymerizes upon condensing. [9] Antimony pentoxide (Sb
4O
10) can be formed only by oxidation with concentrated nitric acid. [23] Antimony also forms a mixed-valence oxide, antimony tetroxide (Sb
2O
4), which features both Sb(III) and Sb(V). [23] Unlike oxides of phosphorus and arsenic, these oxides are amphoteric, do not form well-defined oxoacids, and react with acids to form antimony salts.

Antimonous acid Sb(OH)
3 is unknown, but the conjugate base sodium antimonite ([Na
3SbO
3]
4) forms upon fusing sodium oxide and Sb
4O
6. [24] Transition metal antimonites are also known. [25] : 122  Antimonic acid exists only as the hydrate HSb(OH)
6, forming salts as the antimonate anion Sb(OH)−
6. When a solution containing this anion is dehydrated, the precipitate contains mixed oxides. [25] : 143 

The most important antimony ore is stibnite (Sb
2S
3). Other sulfide minerals include pyrargyrite (Ag
3SbS
3), zinkenite, jamesonite, and boulangerite. [26] Antimony pentasulfide is non-stoichiometric, which features antimony in the +3 oxidation state and S–S bonds. [27] Several thioantimonides are known, such as [Sb
6S
10]2−
 and [Sb
8S
13]2−
. [28]

Halides

Antimony forms two series of halides: SbX
3 and SbX
5. The trihalides SbF
3, SbCl
3, SbBr
3, and SbI
3 are all molecular compounds having trigonal pyramidal molecular geometry.

The trifluoride SbF
3 is prepared by the reaction of Sb
2O
3 with HF: [29]

Sb
2O
3 + 6 HF → 2 SbF
3 + 3 H
2O

It is Lewis acidic and readily accepts fluoride ions to form the complex anions SbF−
4 and SbF2−
5. Molten SbF
3 is a weak electrical conductor. The trichloride SbCl
3 is prepared by dissolving Sb
2S
3 in hydrochloric acid: [30]

Sb
2S
3 + 6 HCl → 2 SbCl
3 + 3 H
2S

Arsenic sulfides are not readily attacked by the hydrochloric acid, so this method offers a route to As-free Sb.

Structure of gaseous SbF5 Antimony-pentafluoride-monomer-3D-balls.png
Structure of gaseous SbF5

The pentahalides SbF
5 and SbCl
5 have trigonal bipyramidal molecular geometry in the gas phase, but in the liquid phase, SbF
5 is polymeric, whereas SbCl
5 is monomeric. [31] SbF
5 is a powerful Lewis acid used to make the superacid fluoroantimonic acid ("H2SbF7").

Oxyhalides are more common for antimony than for arsenic and phosphorus. Antimony trioxide dissolves in concentrated acid to form oxoantimonyl compounds such as SbOCl and (SbO)
2SO
4. [32]

Antimonides, hydrides, and organoantimony compounds

Compounds in this class generally are described as derivatives of Sb3−. Antimony forms antimonides with metals, such as indium antimonide (InSb) and silver antimonide (Ag
3Sb). [33] The alkali metal and zinc antimonides, such as Na3Sb and Zn3Sb2, are more reactive. Treating these antimonides with acid produces the highly unstable gas stibine, SbH
3: [34]

Sb3−
 + 3 H+
 → SbH
3

Stibine can also be produced by treating Sb3+
 salts with hydride reagents such as sodium borohydride. Stibine decomposes spontaneously at room temperature. Because stibine has a positive heat of formation, it is thermodynamically unstable and thus antimony does not react with hydrogen directly. [35]

Organoantimony compounds are typically prepared by alkylation of antimony halides with Grignard reagents. [36] A large variety of compounds are known with both Sb(III) and Sb(V) centers, including mixed chloro-organic derivatives, anions, and cations. Examples include triphenylstibine (Sb(C6H5)3) and pentaphenylantimony (Sb(C6H5)5). [37]

History

One of the alchemical symbols for antimony Antimony symbol.svg
One of the alchemical symbols for antimony

Antimony(III) sulfide, Sb2S3, was recognized in predynastic Egypt as an eye cosmetic (kohl) as early as about 3100 BC, when the cosmetic palette was invented. [38]

An artifact, said to be part of a vase, made of antimony dating to about 3000 BC was found at Telloh, 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. [15] Austen, at a lecture by Herbert Gladstone in 1892, commented that "we only know of antimony at the present day as a highly brittle and crystalline metal, which could hardly be fashioned into a useful vase, and therefore this remarkable 'find' (artifact mentioned above) must represent the lost art of rendering antimony malleable." [39]

The British archaeologist Roger Moorey was unconvinced the artifact was indeed a vase, mentioning that Selimkhanov, after his analysis of the Tello object (published in 1975), "attempted to relate the metal to Transcaucasian natural antimony" (i.e. native metal) and that "the antimony objects from Transcaucasia are all small personal ornaments." [39] This weakens the evidence for a lost art "of rendering antimony malleable". [39]

The Roman scholar Pliny the Elder described several ways of preparing antimony sulfide for medical purposes in his treatise Natural History, around 77 AD. [40] Pliny the Elder also made a distinction between "male" and "female" forms of antimony; the male form is probably the sulfide, while the female form, which is superior, heavier, and less friable, has been suspected to be native metallic antimony. [41]

The Greek naturalist Pedanius Dioscorides mentioned that antimony sulfide could be roasted by heating by a current of air. It is thought that this produced metallic antimony. [40]

The Italian metallurgist Vannoccio Biringuccio described a procedure to isolate antimony. Specola, medaglione di vannoccio biringucci.JPG
The Italian metallurgist Vannoccio Biringuccio described a procedure to isolate antimony.

Antimony was frequently described in alchemical manuscripts, including the Summa Perfectionis of Pseudo-Geber, written around the 14th century. [42] A description of a procedure for isolating antimony is later given in the 1540 book De la pirotechnia by Vannoccio Biringuccio, [43] predating the more famous 1556 book by Agricola, De re metallica . In this context Agricola has been often incorrectly credited with the discovery of metallic antimony. The book Currus Triumphalis Antimonii (The Triumphal Chariot of Antimony), describing the preparation of metallic antimony, was published in Germany in 1604. It was purported to be written by a Benedictine monk, writing under the name Basilius Valentinus in the 15th century; if it were authentic, which it is not, it would predate Biringuccio. [b] [16] [46]

The metal antimony was known to German chemist Andreas Libavius in 1615 who obtained it by adding iron to a molten mixture of antimony sulfide, salt and potassium tartrate. This procedure produced antimony with a crystalline or starred surface. [40]

With the advent of challenges to phlogiston theory, it was recognized that antimony is an element forming sulfides, oxides, and other compounds, as do other metals. [40]

The first discovery of naturally occurring pure antimony in the Earth's crust was described by the Swedish scientist and local mine district engineer Anton von Swab in 1783; the type-sample was collected from the Sala Silver Mine in the Bergslagen mining district of Sala, Västmanland, Sweden. [47] [48]

Etymology

The medieval Latin form, from which the modern languages and late Byzantine Greek take their names for antimony, is antimonium. [49] The origin of that is uncertain, and all suggestions have some difficulty either of form or interpretation. The popular etymology, from ἀντίμοναχός anti-monachos or French antimoine, would mean "monk-killer", which is explained by the fact that many early alchemists were monks, and some antimony compounds were poisonous. [50]

Another popular etymology is the hypothetical Greek word ἀντίμόνος antimonos, "against aloneness", explained as "not found as metal", or "not found unalloyed". [15] However, ancient Greek would more naturally express the pure negative as α- ("not"). [51] Edmund Oscar von Lippmann conjectured a hypothetical Greek word ανθήμόνιον anthemonion, which would mean "floret", and cites several examples of related Greek words (but not that one) which describe chemical or biological efflorescence. [52]

The early uses of antimonium include the translations, in 1050–1100, by Constantine the African of Arabic medical treatises. [52] Several authorities believe antimonium is a scribal corruption of some Arabic form; Meyerhof derives it from ithmid; [53] other possibilities include athimar, the Arabic name of the metalloid, and a hypothetical as-stimmi, derived from or parallel to the Greek. [54] : 28 

The standard chemical symbol for antimony (Sb) is credited to Jöns Jakob Berzelius, who derived the abbreviation from stibium. [55]

The ancient words for antimony mostly have, as their chief meaning, kohl, the sulfide of antimony. [56]

The Egyptians called antimony mśdmt [57] : 230  [58] : 541  or stm. [59]

The Arabic word for the substance, as opposed to the cosmetic, can appear as إثمدithmid, athmoud, othmod, or uthmod. Littré suggests the first form, which is the earliest, derives from stimmida, an accusative for stimmi. [54] [60] The Greek word στίμμι (stimmi) is used by Attic tragic poets of the 5th century BC, and is possibly a loan word from Arabic or from Egyptian stm. [59]

Production

Process

The extraction of antimony from ores depends on the quality and composition of the ore. Most antimony is mined as the sulfide; lower-grade ores are concentrated by froth flotation, while higher-grade ores are heated to 500–600 °C, the temperature at which stibnite melts and separates from the gangue minerals. Antimony can be isolated from the crude antimony sulfide by reduction with scrap iron: [61]

Sb
2S
3 + 3 Fe → 2 Sb + 3 FeS

The sulfide is converted to an oxide by roasting. The product is further purified by vaporizing the volatile antimony(III) oxide, which is recovered. [30] This sublimate is often used directly for the main applications, impurities being arsenic and sulfide. [62] [63] Antimony is isolated from the oxide by a carbothermal reduction: [61] [62]

2 Sb
2O
3 + 3 C → 4 Sb + 3 CO
2

The lower-grade ores are reduced in blast furnaces while the higher-grade ores are reduced in reverberatory furnaces. [61]

World antimony output in 2010 World Antimony Production 2010.svg
World antimony output in 2010
World production trend of antimony Antimony - world production trend.svg
World production trend of antimony

Top producers and production volumes

In 2022, according to the US Geological Survey, China accounted for 54.5% of total antimony production, followed in second place by Russia with 18.2% and Tajikistan with 15.5%. [64]

Antimony mining in 2022 [64]
CountryTonnes % of total
Flag of the People's Republic of China.svg  China 60,00054.5
Flag of Russia.svg  Russia 20,00018.2
Flag of Tajikistan.svg  Tajikistan 17,00015.5
Flag of Myanmar.svg  Myanmar 4,0003.6
Flag of Australia (converted).svg  Australia 4,0003.6
Top 5105,00095.5
Total world110,000100.0

Chinese production of antimony is expected to decline in the future as mines and smelters are closed down by the government as part of pollution control. Especially due to an environmental protection law having gone into effect in January 2015 [65] and revised "Emission Standards of Pollutants for Stanum, Antimony, and Mercury" having gone into effect, hurdles for economic production are higher.

Reported production of antimony in China has fallen and is unlikely to increase in the coming years, according to the Roskill report. No significant antimony deposits in China have been developed for about ten years, and the remaining economic reserves are being rapidly depleted. [66]

Reserves

World antimony reserves in 2022 [64]
CountryReserves
(tonnes)
Flag of the People's Republic of China.svg  China 350,000
Flag of Russia.svg  Russia 350,000
Flag of Bolivia.svg  Bolivia 310,000
Flag of Kyrgyzstan.svg  Kyrgyzstan 260,000
Flag of Myanmar.svg  Myanmar 140,000
Flag of Australia (converted).svg  Australia 120,000
Flag of Turkey.svg  Turkey 100,000
Flag of Canada (Pantone).svg  Canada 78,000
Flag of the United States.svg  United States 60,000
Flag of Slovakia.svg  Slovakia 60,000
Flag of Tajikistan.svg  Tajikistan 50,000
Total world>1,800,000

Supply risk

For antimony-importing regions, such as Europe and the U.S., antimony is considered to be a critical mineral for industrial manufacturing that is at risk of supply chain disruption. With global production coming mainly from China (74%), Tajikistan (8%), and Russia (4%), these sources are critical to supply. [67] [68]

Applications

Approximately 48% of antimony is consumed in flame retardants, 33% in lead–acid batteries, and 8% in plastics. [61]

Flame retardants

Antimony is mainly used as the trioxide for flame-proofing compounds, always in combination with halogenated flame retardants except in halogen-containing polymers. The flame retarding effect of antimony trioxide is produced by the formation of halogenated antimony compounds, [73] which react with hydrogen atoms, and probably also with oxygen atoms and OH radicals, thus inhibiting fire. [74] Markets for these flame-retardants include children's clothing, toys, aircraft, and automobile seat covers. They are also added to polyester resins in fiberglass composites for such items as light aircraft engine covers. The resin will burn in the presence of an externally generated flame, but will extinguish when the external flame is removed. [30] [75]

Alloys

Antimony forms a highly useful alloy with lead, increasing its hardness and mechanical strength. When casting it increases fluidity of the melt and reduces shrinkage during cooling. [76] For most applications involving lead, varying amounts of antimony are used as alloying metal. In lead–acid batteries, this addition improves plate strength and charging characteristics. [30] [77] For sailboats, lead keels are used to provide righting moment, ranging from 600 lbs to over 200 tons for the largest sailing superyachts; to improve hardness and tensile strength of the lead keel, antimony is mixed with lead between 2% and 5% by volume. Antimony is used in antifriction alloys (such as Babbitt metal), [78] in bullets and lead shot, electrical cable sheathing, type metal (for example, for linotype printing machines [79] ), solder (some "lead-free" solders contain 5% Sb), [80] in pewter, [81] and in hardening alloys with low tin content in the manufacturing of organ pipes.

Other applications

InSb infrared detector manufactured by Mullard in the 1960s InSb IR detector.jpg
InSb infrared detector manufactured by Mullard in the 1960s

Three other applications consume nearly all the rest of the world's supply. [61] One application is as a stabilizer and catalyst for the production of polyethylene terephthalate. [61] Another is as a fining agent to remove microscopic bubbles in glass, mostly for TV screens [82] – antimony ions interact with oxygen, suppressing the tendency of the latter to form bubbles. [83] The third application is pigments. [61]

In the 1990s antimony was increasingly being used in semiconductors as a dopant in n-type silicon wafers [84] for diodes, infrared detectors, and Hall-effect devices. In the 1950s, the emitters and collectors of n-p-n alloy junction transistors were doped with tiny beads of a lead-antimony alloy. [85] Indium antimonide (InSb) is used as a material for mid-infrared detectors. [86] [87] [88]

The material Ge2Sb2Te5 is used as for phase-change memory, a type of computer memory.

Biology and medicine have few uses for antimony. Treatments containing antimony, known as antimonials, are used as emetics. [89] Antimony compounds are used as antiprotozoan drugs. Potassium antimonyl tartrate, or tartar emetic, was once used as an anti-schistosomal drug from 1919 on. It was subsequently replaced by praziquantel. [90] Antimony and its compounds are used in several veterinary preparations, such as anthiomaline and lithium antimony thiomalate, as a skin conditioner in ruminants. [91] Antimony has a nourishing or conditioning effect on keratinized tissues in animals.

Antimony-based drugs, such as meglumine antimoniate, are also considered the drugs of choice for treatment of leishmaniasis. Early treatments used antimony(III) species (trivalent antimonials), but in 1922 Upendranath Brahmachari invented a much safer antimony(V) drug, and since then so-called pentavalent antimonials have been the standard first-line treatment. However, Leishmania strains in Bihar and neighboring regions have developed resistance to antimony. [92] Elemental antimony as an antimony pill was once used as a medicine. It could be reused by others after ingestion and elimination. [93]

Antimony(III) sulfide is used in the heads of some safety matches. [94] [95] Antimony sulfides help to stabilize the friction coefficient in automotive brake pad materials. [96] Antimony is used in bullets, bullet tracers, [97] paint, glass art, and as an opacifier in enamel. Antimony-124 is used together with beryllium in neutron sources; the gamma rays emitted by antimony-124 initiate the photodisintegration of beryllium. [98] [99] The emitted neutrons have an average energy of 24 keV. [100] Natural antimony is used in startup neutron sources.

The powder derived from crushed antimony sulfide ( kohl ) has been used for millennia as an eye cosmetic. Historically it was applied to the eyes with a metal rod and with one's spittle, and was thought by the ancients to aid in curing eye infections. [101] The practice is still seen in Yemen and in other Muslim countries. [102]

Precautions

Antimony
Hazards
GHS labelling:
GHS-pictogram-skull.svg GHS-pictogram-exclam.svg GHS-pictogram-silhouette.svg GHS-pictogram-pollu.svg
Danger
H301, H332, H351, H373, H411
P203, P260, P264, P270, P273, P280, P301+P316, P304+P340, P318, P321, P330, P391, P405

Antimony and many of its compounds are toxic, and the effects of antimony poisoning are similar to arsenic poisoning. The toxicity of antimony is far lower than that of arsenic; this might be caused by the significant differences of uptake, metabolism and excretion between arsenic and antimony. The uptake of antimony(III) or antimony(V) in the gastrointestinal tract is at most 20%. Antimony(V) is not quantitatively reduced to antimony(III) in the cell (in fact antimony(III) is oxidised to antimony(V) instead [103] ).

Since methylation of antimony does not occur, the excretion of antimony(V) in urine is the main way of elimination. [104] Like arsenic, the most serious effect of acute antimony poisoning is cardiotoxicity and the resulting myocarditis; however, it can also manifest as Adams–Stokes syndrome, which arsenic does not. Reported cases of intoxication by antimony equivalent to 90 mg antimony potassium tartrate dissolved from enamel has been reported to show only short term effects. An intoxication with 6 g of antimony potassium tartrate was reported to result in death after three days. [105]

Inhalation of antimony dust is harmful and in certain cases may be fatal; in small doses, antimony causes headaches, dizziness, and depression. Larger doses such as prolonged skin contact may cause dermatitis, or damage the kidneys and the liver, causing violent and frequent vomiting, leading to death in a few days. [106]

Antimony is incompatible with strong oxidizing agents, strong acids, halogen acids, chlorine, or fluorine. It should be kept away from heat. [107]

Antimony leaches from polyethylene terephthalate (PET) bottles into liquids. [108] While levels observed for bottled water are below drinking water guidelines, [109] fruit juice concentrates (for which no guidelines are established) produced in the UK were found to contain up to 44.7 μg/L of antimony, well above the EU limits for tap water of 5 μg/L. [110] The guidelines are:

The tolerable daily intake (TDI) proposed by WHO is 6 μg antimony per kilogram of body weight. [111] The immediately dangerous to life or health (IDLH) value for antimony is 50 mg/m3. [114]

Toxicity

Certain compounds of antimony appear to be toxic, particularly antimony trioxide and antimony potassium tartrate. [115] Effects may be similar to arsenic poisoning. [116] Occupational exposure may cause respiratory irritation, pneumoconiosis, antimony spots on the skin, gastrointestinal symptoms, and cardiac arrhythmias. In addition, antimony trioxide is potentially carcinogenic to humans. [117]

Adverse health effects have been observed in humans and animals following inhalation, oral, or dermal exposure to antimony and antimony compounds. [115] Antimony toxicity typically occurs either due to occupational exposure, during therapy or from accidental ingestion. It is unclear if antimony can enter the body through the skin. [115] The presence of low levels of antimony in saliva may also be associated with dental decay. [118]

Notes

  1. ↑ The thermal expansion is anisotropic: the parameters (at 20 °C) for each crystal axis are αah = 8.24×10−6/K, αch = 16.62×10−6/K, and αaverage = αV/3 = 11.04×10−6/K. [3]
  2. ↑ Already in 1710 Wilhelm Gottlob Freiherr von Leibniz, after careful inquiry, concluded the work was spurious, there was no monk named Basilius Valentinus, and the book's author was its ostensible editor, Johann Thölde (c. 1565 – c. 1624). Professional historians now agree the Currus Triumphalis ... was written after the middle of the 16th century and Thölde was likely its author. [44] Harold Jantz was perhaps the only modern scholar to deny Thölde's authorship, but he too agrees the work dates from after 1550. [45]

Related Research Articles

A metalloid is a chemical element which has a preponderance of properties in between, or that are a mixture of, those of metals and nonmetals. The word metalloid comes from the Latin metallum ("metal") and the Greek oeides. There is no standard definition of a metalloid and no complete agreement on which elements are metalloids. Despite the lack of specificity, the term remains in use in the literature.

<span class="mw-page-title-main">Pnictogen</span> Group 15 elements of the periodic table with valency 5

The pnictogens are the chemical elements in group 15 of the periodic table. This group is also known as the nitrogen group or nitrogen family. Group 15 consists of the elements nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), bismuth (Bi), and moscovium (Mc). This is also the only group in the periodic table in which only one element ends in the common suffix -ium.

<span class="mw-page-title-main">Marsh test</span> Method for detecting arsenic

The Marsh test is a highly sensitive method in the detection of arsenic, especially useful in the field of forensic toxicology when arsenic was used as a poison. It was developed by the chemist James Marsh and first published in 1836. The method continued to be used, with improvements, in forensic toxicology until the 1970s.

Sulfide (also sulphide in British English) is an inorganic anion of sulfur with the chemical formula S2− or a compound containing one or more S2− ions. Solutions of sulfide salts are corrosive. Sulfide also refers to large families of inorganic and organic compounds, e.g. lead sulfide and dimethyl sulfide. Hydrogen sulfide (H2S) and bisulfide (SH−) are the conjugate acids of sulfide.

<span class="mw-page-title-main">Stibnite</span> Sulfide mineral

Stibnite, sometimes called antimonite, is a sulfide mineral with the formula Sb2S3. This soft grey material crystallizes in an orthorhombic space group. It is the most important source for the metalloid antimony. The name is derived from the Greek στίβι stibi through the Latin stibium as the former name for the mineral and the element antimony.

In chemistry, antimonite refers to a salt of antimony(III), such as NaSb(OH)4 and NaSbO2 (meta-antimonite), which can be prepared by reacting alkali with antimony trioxide, Sb2O3. These are formally salts of antimonous acid, Sb(OH)3, whose existence in solution is dubious. Attempts to isolate it generally form Sb2O3·xH2O, antimony(III) oxide hydrate, which slowly transforms into Sb2O3.

<span class="mw-page-title-main">Antimony trisulfide</span> Chemical compound

Antimony trisulfide is found in nature as the crystalline mineral stibnite and the amorphous red mineral metastibnite. It is manufactured for use in safety matches, military ammunition, explosives and fireworks. It also is used in the production of ruby-colored glass and in plastics as a flame retardant. Historically the stibnite form was used as a grey pigment in paintings produced in the 16th century. In 1817, the dye and fabric chemist, John Mercer discovered the non-stoichiometric compound Antimony Orange, the first good orange pigment available for cotton fabric printing.

<span class="mw-page-title-main">Arsenic trioxide</span> Chemical compound (industrial chemical and medication)

Arsenic trioxide is an inorganic compound with the formula As
2O
3. As an industrial chemical, its major uses include the manufacture of wood preservatives, pesticides, and glass. It is sold under the brand name Trisenox among others when used as a medication to treat a type of cancer known as acute promyelocytic leukemia. For this use it is given by injection into a vein.

<span class="mw-page-title-main">Antimony trioxide</span> Chemical compound

Antimony(III) oxide is the inorganic compound with the formula Sb2O3. It is the most important commercial compound of antimony. It is found in nature as the minerals valentinite and senarmontite. Like most polymeric oxides, Sb2O3 dissolves in aqueous solutions with hydrolysis. A mixed arsenic-antimony oxide occurs in nature as the very rare mineral stibioclaudetite.

<span class="mw-page-title-main">Arsenic acid</span> Chemical compound

Arsenic acid or arsoric acid is the chemical compound with the formula H3AsO4. More descriptively written as AsO(OH)3, this colorless acid is the arsenic analogue of phosphoric acid. Arsenate and phosphate salts behave very similarly. Arsenic acid as such has not been isolated, but is only found in solution, where it is largely ionized. Its hemihydrate form (2H3AsO4·H2O) does form stable crystals. Crystalline samples dehydrate with condensation at 100 °C.

<span class="mw-page-title-main">Antimony triiodide</span> Chemical compound

Antimony triiodide is the chemical compound with the formula SbI3. This ruby-red solid is the only characterized "binary" iodide of antimony, i.e. the sole compound isolated with the formula SbxIy. It contains antimony in its +3 oxidation state. Like many iodides of the heavier main group elements, its structure depends on the phase. Gaseous SbI3 is a molecular, pyramidal species as anticipated by VSEPR theory. In the solid state, however, the Sb center is surrounded by an octahedron of six iodide ligands, three of which are closer and three more distant. For the related compound BiI3, all six Bi—I distances are equal.

<span class="mw-page-title-main">Selenium compounds</span> Chemical compounds containing selenium

Selenium compounds are compounds containing the element selenium (Se). Among these compounds, selenium has various oxidation states, the most common ones being −2, +4, and +6. Selenium compounds exist in nature in the form of various minerals, such as clausthalite, guanajuatite, tiemannite, crookesite etc., and can also coexist with sulfide minerals such as pyrite and chalcopyrite. For many mammals, selenium compounds are essential. For example, selenomethionine and selenocysteine are selenium-containing amino acids present in the human body. Selenomethionine participates in the synthesis of selenoproteins. The reduction potential and pKa (5.47) of selenocysteine are lower than those of cysteine, making some proteins have antioxidant activity. Selenium compounds have important applications in semiconductors, glass and ceramic industries, medicine, metallurgy and other fields.

Antimony pentasulfide is an inorganic compound of antimony and sulfur, also known as antimony red. It is a nonstoichiometric compound with a variable composition. Its structure is unknown. Commercial samples are contaminated with sulfur, which may be removed by washing with carbon disulfide in a Soxhlet extractor.

<span class="mw-page-title-main">Bismuth</span> Chemical element with atomic number 83 (Bi)

Bismuth is a chemical element with the symbol Bi and atomic number 83. It is a post-transition metal and one of the pnictogens, with chemical properties resembling its lighter group 15 siblings arsenic and antimony. Elemental bismuth occurs naturally, and its sulfide and oxide forms are important commercial ores. The free element is 86% as dense as lead. It is a brittle metal with a silvery-white color when freshly produced. Surface oxidation generally gives samples of the metal a somewhat rosy cast. Further oxidation under heat can give bismuth a vividly iridescent appearance due to thin-film interference. Bismuth is both the most diamagnetic element and one of the least thermally conductive metals known.

Organoantimony chemistry is the chemistry of compounds containing a carbon to antimony (Sb) chemical bond. Relevant oxidation states are SbV and SbIII. The toxicity of antimony limits practical application in organic chemistry.

Gallium compounds are compounds containing the element gallium. These compounds are found primarily in the +3 oxidation state. The +1 oxidation state is also found in some compounds, although it is less common than it is for gallium's heavier congeners indium and thallium. For example, the very stable GaCl2 contains both gallium(I) and gallium(III) and can be formulated as GaIGaIIICl4; in contrast, the monochloride is unstable above 0 °C, disproportionating into elemental gallium and gallium(III) chloride. Compounds containing Ga–Ga bonds are true gallium(II) compounds, such as GaS (which can be formulated as Ga24+(S2−)2) and the dioxan complex Ga2Cl4(C4H8O2)2. There are also compounds of gallium with negative oxidation states, ranging from -5 to -1, most of these compounds being magnesium gallides (MgxGay).

<span class="mw-page-title-main">Arsenic compounds</span> Chemical compounds containing arsenic

Compounds of arsenic resemble in some respects those of phosphorus which occupies the same group (column) of the periodic table. The most common oxidation states for arsenic are: −3 in the arsenides, which are alloy-like intermetallic compounds, +3 in the arsenites, and +5 in the arsenates and most organoarsenic compounds. Arsenic also bonds readily to itself as seen in the square As3−
4 ions in the mineral skutterudite. In the +3 oxidation state, arsenic is typically pyramidal owing to the influence of the lone pair of electrons.

<span class="mw-page-title-main">Bismuth compounds</span>

Bismuth forms mainly trivalent and a few pentavalent compounds. Many of its chemical properties are similar to those of arsenic and antimony, although much less toxic.

<span class="mw-page-title-main">Bismuthyl (ion)</span> Chemical compound

Bismuthyl is an inorganic oxygen-containing singly charged ion with the chemical formula BiO+, and is an oxycation of bismuth in the +3 oxidation state. Most often it is formed during the hydrolysis of trivalent bismuth salts, primarily nitrate, chloride and other halides. In chemical compounds, bismuthyl plays the role of a monovalent cation.

References

  1. ↑ "Standard Atomic Weights: Antimony". CIAAW. 1993.
  2. ↑ Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (4 May 2022). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN   1365-3075.
  3. 1 2 3 Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. ISBN   978-1-62708-155-9.
  4. ↑ Anastas Sidiropoulos (2019). "Studies of N-heterocyclic Carbene (NHC) Complexes of the Main Group Elements" (PDF). p. 39. doi:10.4225/03/5B0F4BDF98F60. S2CID   132399530.
  5. ↑ Lide, D. R., ed. (2005). "Magnetic susceptibility of the elements and inorganic compounds". CRC Handbook of Chemistry and Physics (PDF) (86th ed.). Boca Raton (FL): CRC Press. ISBN   0-8493-0486-5.
  6. ↑ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN   0-8493-0464-4.
  7. ↑ Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
  8. ↑ David Kimhi's Commentary on Isaiah 4:30 and I Chronicles 29:2; Hebrew: פוך/כְּחֻל, Aramaic: כּוּחְלִי/צדידא; Arabic: كحل, and which can also refer to antimony trisulfide. See also Z. Dori, Antimony and Henna (Heb. הפוך והכופר), Jerusalem 1983 (Hebrew).
  9. 1 2 3 Wiberg and Holleman, p. 758
  10. ↑ "Metals Used in Coins and Medals". ukcoinpics.co.uk. Archived from the original on 26 December 2010. Retrieved 16 October 2009.
  11. ↑ Ashcheulov, A. A.; Manyk, O. N.; Manyk, T. O.; Marenkin, S. F.; Bilynskiy-Slotylo, V. R. (2013). "Some Aspects of the Chemical Bonding in Antimony". Inorganic Materials. 49 (8): 766–769. doi:10.1134/s0020168513070017. S2CID   54954678.
  12. ↑ Shen, Xueyang; Zhou, Yuxing; Zhang, Hanyi; Derlinger, Volker L.; Mazzarello, Riccardo; Zhang, Wei (2023). "Surface effects on the crystallization kinetics of amorphous antimony". Nanoscale. 15 (37): 15259–15267. doi:10.1039/D3NR03536K. PMID   37674458. S2CID   261552619.
  13. 1 2 Lide, D. R., ed. (2001). CRC Handbook of Chemistry and Physics (82nd ed.). Boca Raton, FL: CRC Press. p. 4-4. ISBN   0-8493-0482-2.
  14. ↑ Krebs, H.; Schultze-Gebhardt, F.; Thees, R. (1955). "Über die Struktur und die Eigenschaften der Halbmetalle. IX: Die Allotropie des Antimons". Zeitschrift für anorganische und allgemeine Chemie (in German). 282 (1–6): 177–195. doi:10.1002/zaac.19552820121.
  15. 1 2 3 "Antimony" in Kirk-Othmer Encyclopedia of Chemical Technology, 5th ed. 2004. ISBN   978-0-471-48494-3
  16. 1 2 Wang, Chung Wu (1919). "The Chemistry of Antimony" (PDF). Antimony: Its History, Chemistry, Mineralogy, Geology, Metallurgy, Uses, Preparation, Analysis, Production and Valuation with Complete Bibliographies. London, United Kingdom: Charles Geiffin and Co. Ltd. pp. 6–33. Archived (PDF) from the original on 9 October 2022.
  17. ↑ Norman 1998, pp. 50–51
  18. 1 2 Audi, Georges; Bersillon, Olivier; Blachot, Jean; Wapstra, Aaldert Hendrik (2003). "The NUBASE evaluation of nuclear and decay properties". Nuclear Physics A. 729: 3–128. Bibcode:2003NuPhA.729....3A. doi:10.1016/j.nuclphysa.2003.11.001.
  19. 1 2 Greenwood and Earnshaw, p. 548
  20. ↑ Antimony minerals. mindat.org
  21. ↑ Greenwood and Earnshaw, p. 553
  22. ↑ Reger, Daniel L.; Goode, Scott R. & Ball, David W. (2009). Chemistry: Principles and Practice (3rd ed.). Cengage Learning. p. 883. ISBN   978-0-534-42012-3.
  23. 1 2 House, James E. (2008). Inorganic chemistry. Academic Press. p. 502. ISBN   978-0-12-356786-4.
  24. ↑ Wiberg and Holleman, p. 763
  25. 1 2 Godfrey, S. M.; McAuliffe, C. A.; Mackie, A. G. & Pritchard, R. G. (1998). Norman, Nicholas C. (ed.). Chemistry of arsenic, antimony, and bismuth. Springer. ISBN   978-0-7514-0389-3.
  26. ↑ Wiberg and Holleman, p. 757
  27. ↑ Long, G.; Stevens, J. G.; Bowen, L. H.; Ruby, S. L. (1969). "The oxidation number of antimony in antimony pentasulfide". Inorganic and Nuclear Chemistry Letters. 5: 21. doi:10.1016/0020-1650(69)80231-X.
  28. ↑ Lees, R.; Powell, A.; Chippindale, A. (2007). "The synthesis and characterisation of four new antimony sulphides incorporating transition-metal complexes". Journal of Physics and Chemistry of Solids. 68 (5–6): 1215. Bibcode:2007JPCS...68.1215L. doi:10.1016/j.jpcs.2006.12.010.
  29. ↑ Wiberg and Holleman, pp. 761–762
  30. 1 2 3 4 Grund, Sabina C.; Hanusch, Kunibert; Breunig, Hans J.; Wolf, Hans Uwe (2006) "Antimony and Antimony Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim. doi : 10.1002/14356007.a03_055.pub2
  31. ↑ Wiberg and Holleman, p. 761
  32. ↑ Wiberg and Holleman, p. 764
  33. ↑ Wiberg and Holleman, p. 760
  34. ↑ Kahlenberg, Louis (2008). Outlines of Chemistry – A Textbook for College Students. READ BOOKS. pp. 324–325. ISBN   978-1-4097-6995-8.
  35. ↑ Greenwood and Earnshaw, p. 558
  36. ↑ Elschenbroich, C. (2006) "Organometallics". Wiley-VCH: Weinheim. ISBN   3-527-29390-6
  37. ↑ Greenwood and Earnshaw, p. 598
  38. ↑ Shortland, A. J. (2006). "Application of Lead Isotope Analysis to a Wide Range of Late Bronze Age Egyptian Materials". Archaeometry. 48 (4): 657. doi:10.1111/j.1475-4754.2006.00279.x.
  39. 1 2 3 Moorey, P. R. S. (1994). Ancient Mesopotamian Materials and Industries: the Archaeological Evidence. New York: Clarendon Press. p. 241. ISBN   978-1-57506-042-2.
  40. 1 2 3 4 Mellor, Joseph William (1964). "Antimony". A comprehensive treatise on inorganic and theoretical chemistry. Vol. 9. p. 339.
  41. ↑ Pliny, Natural history , 33.33; W.H.S. Jones, the Loeb Classical Library translator, supplies a note suggesting the identifications.
  42. ↑ Montserrat Filella, ed. (2021). Antimony. De Gruyter. p. 4. ISBN   9783110668711.
  43. ↑ Vannoccio Biringuccio, De la Pirotechnia (Venice (Italy): Curtio Navo e fratelli, 1540), Book 2, chapter 3: Del antimonio & sua miniera, Capitolo terzo (On antimony and its ore, third chapter), pp. 27–28. [Note: Only every second page of this book is numbered, so the relevant passage is to be found on the 74th and 75th pages of the text.] (in Italian)
  44. ↑ Priesner, Claus; Figala, Karin, eds. (1998). Alchemie. Lexikon einer hermetischen Wissenschaft (in German). München: C.H. Beck. ISBN   3406441068.
  45. ↑ Harold Jantz Collection of German Baroque Literature Reel Listing.
  46. ↑ Weeks, Mary Elvira (1932). "The discovery of the elements. II. Elements known to the alchemists". Journal of Chemical Education. 9 (1): 11. Bibcode:1932JChEd...9...11W. doi:10.1021/ed009p11.
  47. ↑ "Native antimony". Mindat.org.
  48. ↑ Klaproth, M. (1803). "XL. Extracts from the third volume of the analyses". Philosophical Magazine. Series 1. 17 (67): 230. doi:10.1080/14786440308676406.
  49. ↑ "antimony". Britannica.com. 22 May 2024 [July 20, 1998]. Retrieved 10 June 2024.
  50. ↑ Fernando, Diana (1998). Alchemy: an illustrated A to Z. Blandford. ISBN   9780713726688. Fernando connects the proposed etymology to the story of "Basil Valentine", although antimonium is found two centuries before Valentine's time.
  51. ↑ "Antimony" . Oxford English Dictionary (Online ed.). Oxford University Press.(Subscription or participating institution membership required.), which considers the derivation a "popular etymology".
  52. 1 2 von Lippmann, Edmund Oscar (1919) Entstehung und Ausbreitung der Alchemie, teil 1. Berlin: Julius Springer (in German). pp. 642–5
  53. ↑ Meyerhof as quoted in Sarton 1935, asserts that ithmid or athmoud became corrupted in the medieval "traductions barbaro-latines". The OED asserts some Arabic form is the origin, and if ithmid is the root, posits athimodium, atimodium, atimonium as intermediates.
  54. 1 2 Endlich, F. M. (1888). "On Some Interesting Derivations of Mineral Names". The American Naturalist. 22 (253): 21–32. Bibcode:1888ANat...22...21E. doi: 10.1086/274630 . JSTOR   2451020.
  55. ↑ Jöns Jacob Berzelius, "Essay on the cause of chemical proportions, and on some circumstances relating to them: together with a short and easy method of expressing them," Annals of Philosophy, vol. 2, pages 443–454 (1813) and vol. 3, pages 51–62, 93–106, 244–255, 353–364 (1814). On p. 52, Berzelius lists the symbol for antimony as "St"; however, starting from p. 248, Berzelius consistently uses the symbol "Sb" instead.
  56. ↑ Helmenstine, Anne (9 July 2024). "Antimony Facts - Symbol, Definition, Uses". Science Notes and Projects. Retrieved 30 October 2024.
  57. ↑ Albright, W. F. (1918). "Notes on Egypto-Semitic Etymology. II". The American Journal of Semitic Languages and Literatures. 34 (4): 215–255. doi:10.1086/369866. JSTOR   528157. S2CID   170203738.
  58. ↑ Sarton, George (1935). "Review of Al-morchid fi'l-kohhl, ou Le guide d'oculistique (Translated by Max Meyerhof)". Isis (in French). 22 (2): 539-542. doi:10.1086/346926. JSTOR   225136.
  59. 1 2 Harper, Douglas. "antimony". Online Etymology Dictionary .
  60. ↑
    • LSJ, s.v., vocalisation, spelling, and declension vary
    • Celsus, 6.6.6 ff
    • Pliny Natural History 33.33
    • Lewis and Short: Latin Dictionary
    • OED, s. "antimony"
  61. 1 2 3 4 5 6 7 Klochko, Kateryna (2021). "2017 Minerals Yearbook: Antimony" (PDF). United States Geological Survey.
  62. 1 2 Norman 1998, p. 45
  63. ↑ Wilson, N. J.; Craw, D.; Hunter, K. (2004). "Antimony distribution and environmental mobility at an historic antimony smelter site, New Zealand". Environmental Pollution. 129 (2): 257–66. Bibcode:2004EPoll.129..257W. doi:10.1016/j.envpol.2003.10.014. PMID   14987811.
  64. 1 2 3 4 "Antimony Statistics and Information" (PDF). National Minerals Information Center. USGS.
  65. ↑ "Environmental Protection Law of the People's Republic of China" (PDF). 24 April 2014. Archived from the original (PDF) on 2 June 2014. Retrieved 14 October 2016.
  66. ↑ "Study of the antimony market by Roskill Consulting Group" (PDF). Archived from the original (PDF) on 18 October 2012. Retrieved 9 April 2012.
  67. 1 2 "Critical Raw Materials Resilience: Charting a Path towards greater Security and Sustainability". European Commission. 2020. Retrieved 2 February 2022.
  68. 1 2 Nassar, Nedal T.; et al. (21 February 2020). "Evaluating the mineral commodity supply risk of the U.S. manufacturing sector". Sci. Adv. 6 (8): eaay8647. Bibcode:2020SciA....6.8647N. doi:10.1126/sciadv.aay8647. PMC   7035000 . PMID   32128413.
  69. ↑ "MineralsUK Risk List 2015". BGS.
  70. ↑ "British Geological Survey Risk list 2015" (PDF). Minerals UK. BGS. Archived (PDF) from the original on 9 October 2022. Retrieved 2 February 2022.
  71. ↑ "Interior Releases 2018's Final List of Critical Minerals". United States Geological Survey . Retrieved 1 February 2022.
  72. ↑ "Antimony". U.S. Geological Survey, Mineral Commodity Summaries, January 2022 (PDF). Archived (PDF) from the original on 9 October 2022. Retrieved 1 February 2022.
  73. ↑ Weil, Edward D.; Levchik, Sergei V. (4 June 2009). "Antimony trioxide and Related Compounds". Flame retardants for plastics and textiles: Practical applications. Hanser. ISBN   978-3-446-41652-9.
  74. ↑ Hastie, John W. (1973). "Mass spectrometric studies of flame inhibition: Analysis of antimony trihalides in flames". Combustion and Flame. 21 (1): 49. Bibcode:1973CoFl...21...49H. doi:10.1016/0010-2180(73)90006-0.
  75. ↑ Weil, Edward D.; Levchik, Sergei V. (4 June 2009). Flame retardants for plastics and textiles: Practical applications. Hanser. pp. 15–16. ISBN   978-3-446-41652-9.
  76. ↑ Butterman, W.C.; Carlin, Jr., J.F. (2004). "Mineral Commodity Profiles - Antimony" (PDF). U.S. Geological Survey. Archived (PDF) from the original on 24 March 2024. Retrieved 18 July 2024.
  77. ↑ Kiehne, Heinz Albert (2003). "Types of Alloys". Battery Technology Handbook. CRC Press. pp. 60–61. ISBN   978-0-8247-4249-2.
  78. ↑ Williams, Robert S. (2007). Principles of Metallography. Read books. pp. 46–47. ISBN   978-1-4067-4671-6.
  79. ↑ Holmyard, E. J. (2008). Inorganic Chemistry – A Textbook for Colleges and Schools. Read Books. pp. 399–400. ISBN   978-1-4437-2253-7.
  80. ↑ Ipser, H.; Flandorfer, H.; Luef, Ch.; Schmetterer, C.; Saeed, U. (2007). "Thermodynamics and phase diagrams of lead-free solder materials". Journal of Materials Science: Materials in Electronics. 18 (1–3): 3–17. doi:10.1007/s10854-006-9009-3. S2CID   85452380.
  81. ↑ Hull, Charles (1992). Pewter. Osprey Publishing. pp. 1–5. ISBN   978-0-7478-0152-8.
  82. ↑ De Jong, Bernard H. W. S.; Beerkens, Ruud G. C.; Van Nijnatten, Peter A. (2000). "Glass". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a12_365. ISBN   978-3-527-30673-2.
  83. ↑ Yamashita, H.; Yamaguchi, S.; Nishimura, R.; Maekawa, T. (2001). "Voltammetric Studies of Antimony Ions in Soda-lime-silica Glass Melts up to 1873 K". Analytical Sciences. 17 (1): 45–50. doi: 10.2116/analsci.17.45 . PMID   11993676.
  84. ↑ O'Mara, William C.; Herring, Robert B.; Hunt, Lee Philip (1990). Handbook of semiconductor silicon technology. William Andrew. p. 473. ISBN   978-0-8155-1237-0.
  85. ↑ Maiti, C. K. (2008). Selected Works of Professor Herbert Kroemer. World Scientific, 2008. p. 101. ISBN   978-981-270-901-1.
  86. ↑ Committee on New Sensor Technologies: Materials And Applications, National Research Council (U.S.) (1995). Expanding the vision of sensor materials. National Academies Press. p. 68. ISBN   978-0-309-05175-0.
  87. ↑ Kinch, Michael A (2007). Fundamentals of infrared detector materials. SPIE Press. p. 35. ISBN   978-0-8194-6731-7.
  88. ↑ Willardson, Robert K & Beer, Albert C (1970). Infrared detectors. Academic Press. p. 15. ISBN   978-0-12-752105-3.
  89. ↑ Russell, Colin A. (2000). "Antimony's Curious History". Notes and Records of the Royal Society of London. 54 (1): 115–116. doi:10.1098/rsnr.2000.0101. JSTOR   532063. PMC   1064207 .
  90. ↑ Harder, A. (2002). "Chemotherapeutic approaches to schistosomes: Current knowledge and outlook". Parasitology Research. 88 (5): 395–7. doi:10.1007/s00436-001-0588-x. PMID   12049454. S2CID   28243137.
  91. ↑ Kassirsky, I. A.; Plotnikov, N. N. (1 August 2003). Diseases of Warm Lands: A Clinical Manual. The Minerva Group. pp. 262–265. ISBN   978-1-4102-0789-0.
  92. ↑ Control of the leishmaniases: report of a meeting of the WHO Expert Committee on the Control of Leishmaniases, Geneva, 22-26 March 2010. World Health Organization. 2010. p. 1–2, 55, 67–68. ISBN   978-92-4-120949-6.
  93. ↑ McCallum, R. I. (1999). Antimony in medical history: an account of the medical uses of antimony and its compounds since early times to the present. Pentland Press. ISBN   978-1-85821-642-3.
  94. ↑ Stellman, Jeanne Mager (1998). Encyclopaedia of Occupational Health and Safety: Chemical, industries and occupations. International Labour Organization. p. 109. ISBN   978-92-2-109816-4.
  95. ↑ Jang, H & Kim, S. (2000). "The effects of antimony trisulfide (Sb2S3) and zirconium silicate (ZrSiO4) in the automotive brake friction material on friction". Journal of Wear. 239 (2): 229. doi:10.1016/s0043-1648(00)00314-8.
  96. ↑ Randich, Erik; Duerfeldt, Wayne; McLendon, Wade; Tobin, William (2002). "A metallurgical review of the interpretation of bullet lead compositional analysis". Forensic Science International. 127 (3): 174–91. doi:10.1016/S0379-0738(02)00118-4. PMID   12175947. S2CID   22272775.
  97. ↑ Lalovic, M.; Werle, H. (1970). "The energy distribution of antimonyberyllium photoneutrons". Journal of Nuclear Energy. 24 (3): 123. Bibcode:1970JNuE...24..123L. doi:10.1016/0022-3107(70)90058-4.
  98. ↑ Ahmed, Syed Naeem (2007). Physics and engineering of radiation detection. Academic Press. p. 51. Bibcode:2007perd.book.....A. ISBN   978-0-12-045581-2.
  99. ↑ Schmitt, H (1960). "Determination of the energy of antimony-beryllium photoneutrons". Nuclear Physics. 20: 220. Bibcode:1960NucPh..20..220S. doi:10.1016/0029-5582(60)90171-1.
  100. ↑ Rabbeinu Hananel (1995). "Rabbeinu Hananel's Commentary on Tractate Shabbat". In Metzger, David (ed.). Perushe Rabenu Ḥananʼel Bar Ḥushiʼel la-Talmud (in Hebrew). Jerusalem: Mekhon 'Lev Sameaḥ'. p. 215 (Shabbat 109a). OCLC   319767989.
  101. ↑ "Sunan an-Nasa'i 5113 – The Book of Adornment – كتاب الزينة من السنن – Sunnah.com – Sayings and Teachings of Prophet Muhammad (صلى الله عليه و سلم)". sunnah.com. Retrieved 18 February 2021.
  102. ↑ Foster, S.; Maher, W.; Krikowa, F.; Telford, K.; Ellwood, M. (2005). "Observations on the measurement of total antimony and antimony species in algae, plant and animal tissues". Journal of Environmental Monitoring. 7 (12): 1214–1219. doi:10.1039/b509202g. PMID   16307074.
  103. ↑ Gebel, T (1997). "Arsenic and antimony: Comparative approach on mechanistic toxicology". Chemico-Biological Interactions. 107 (3): 131–44. Bibcode:1997CBI...107..131G. doi:10.1016/S0009-2797(97)00087-2. PMID   9448748.
  104. ↑ McCallum, RI (1977). "President's address. Observations upon antimony". Proceedings of the Royal Society of Medicine. 70 (11): 756–63. doi:10.1177/003591577707001103. PMC   1543508 . PMID   341167.
  105. ↑ Sundar, S.; Chakravarty, J. (2010). "Antimony Toxicity". International Journal of Environmental Research and Public Health. 7 (12): 4267–4277. doi: 10.3390/ijerph7124267 . PMC   3037053 . PMID   21318007.
  106. ↑ Antimony MSDS [ dead link ]. Baker
  107. ↑ Westerhoff, P; Prapaipong, P; Shock, E; Hillaireau, A (2008). "Antimony leaching from polyethylene terephthalate (PET) plastic used for bottled drinking water". Water Research. 42 (3): 551–6. Bibcode:2008WatRe..42..551W. doi:10.1016/j.watres.2007.07.048. PMID   17707454.
  108. 1 2 Shotyk, W.; Krachler, M.; Chen, B. (2006). "Contamination of Canadian and European bottled waters with antimony from PET containers". Journal of Environmental Monitoring. 8 (2): 288–92. doi:10.1039/b517844b. PMID   16470261. S2CID   9416637.
  109. ↑ Hansen, Claus; Tsirigotaki, Alexandra; Bak, Søren Alex; Pergantis, Spiros A.; Stürup, Stefan; Gammelgaard, Bente; Hansen, Helle Rüsz (2010). "Elevated antimony concentrations in commercial juices". Journal of Environmental Monitoring. 12 (4): 822–4. doi:10.1039/b926551a. PMID   20383361.
  110. 1 2 Guidelines for Drinking-water Quality (PDF) (4th ed.). World Health Organization. 2011. p. 314. ISBN   978-92-4-154815-1. Archived (PDF) from the original on 9 October 2022.
  111. ↑ Wakayama, Hiroshi (2003) "Revision of Drinking Water Standards in Japan", Ministry of Health, Labor and Welfare (Japan); Table 2, p. 84
  112. ↑ Screening assessment antimony-containing substances. Health Canada. July 2020. ISBN   978-0-660-32826-3
  113. ↑ NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  114. 1 2 3 "Toxicological Profile for Antimony and Compounds" (PDF). U.S. Department of Health and Human Services. Archived (PDF) from the original on 9 October 2022. Retrieved 19 May 2022.
  115. ↑ "Antimony poisoning". Encyclopedia Britannica.
  116. ↑ Sundar, S; Chakravarty, J (2010). "Antimony Toxicity". International Journal of Environmental Research and Public Health. 7 (12): 4267–4277. doi: 10.3390/ijerph7124267 . PMC   3037053 . PMID   21318007.
  117. ↑ Davis, E.; Bakulski, K. M.; Goodrich, J. M. (2020). "Low levels of salivary metals, oral microbiome composition and dental decay". Scientific Reports. 10 (1): 14640. Bibcode:2020NatSR..1014640D. doi: 10.1038/s41598-020-71495-9 . PMC   7474081 . PMID   32887894.

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