Jump to content

Tin

Edit links
From Wikipedia, the free encyclopedia
(Redirected from Gray tin)
This article is about the chemical element. For other uses, see Tin (disambiguation).
"Stannum" redirects here. For other uses, see Stannum (disambiguation).

Tin, 50Sn
Tin
Allotropessilvery-white, β (beta); gray, α (alpha)
Standard atomic weight Ar°(Sn)
Tin 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
Ge
↑
Sn
↓
Pb
indium ← tin → antimony
Atomic number (Z)50
Groupgroup 14 (carbon group)
Periodperiod 5
Block  p-block
Electron configuration[Kr] 4d10 5s2 5p2
Electrons per shell2, 8, 18, 18, 4
Physical properties
Phase at STPsolid
Melting point505.08 K ​(231.93 °C, ​449.47 °F)
Boiling point2875 K ​(2602 °C, ​4716 °F)
Density (at 20° C)white (β): 7.289 g/cm3
gray (α): 5.770 g/cm3[3]
when liquid (at m.p.)6.99 g/cm3
Heat of fusionwhite (β): 7.03 kJ/mol
Heat of vaporizationwhite (β): 296.1 kJ/mol
Molar heat capacitywhite (β): 27.112 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 1497 1657 1855 2107 2438 2893
Atomic properties
Oxidation states−4, −3, −2, −1, 0,[4] +1,[5] +2, +3,[6] +4 (an amphoteric oxide)
ElectronegativityPauling scale: 1.96
Ionization energies
  • 1st: 708.6 kJ/mol
  • 2nd: 1411.8 kJ/mol
  • 3rd: 2943.0 kJ/mol
Atomic radiusempirical: 140 pm
Covalent radius139±4 pm
Van der Waals radius217 pm
Color lines in a spectral range
Spectral lines of tin
Other properties
Natural occurrenceprimordial
Crystal structurewhite (β): ​body-centered tetragonal (tI4)
Lattice constants
Body-centered tetragonal crystal structure for white (β): tin
white (β):
a = 583.13 pm
c = 318.11 pm
(at 20 °C)[3]
Crystal structuregray (α): ​face-centered diamond-cubic (cF8)
Lattice constant
Diamond cubic crystal structure for gray (α): tin
gray (α):
a = 648.96 pm (at 20 °C)[3]
Thermal expansionwhite (β): 21.76×10−6/K (at 20 °C)[a]
gray (α): 5.20×10−6/K (at 20 °C)[3]
Thermal conductivity66.8 W/(m⋅K)
Electrical resistivity115 nΩ⋅m (at 0 °C)
Magnetic orderingwhite (β): paramagnetic
gray (α): diamagnetic[7]
Molar magnetic susceptibilitywhite (β): +3.1×10−6 cm3/mol (298 K)[8]
Young's modulus50 GPa
Shear modulus18 GPa
Bulk modulus58 GPa
Speed of sound thin rod2730 m/s (at r.t.) (rolled)
Poisson ratio0.36
Mohs hardness1.5
Brinell hardness50–440 MPa
CAS Number7440-31-5
History
Discoveryprotohistoric, around 35th century BC
Symbol"Sn": from Latin stannum
Isotopes of tin
Main isotopes[9] Decay
abun­dance half-life (t1/2) mode pro­duct
112Sn 0.970% stable
114Sn 0.66% stable
115Sn 0.34% stable
116Sn 14.5% stable
117Sn 7.68% stable
118Sn 24.2% stable
119Sn 8.59% stable
120Sn 32.6% stable
122Sn 4.63% stable
124Sn 5.79% stable
126Sn trace 2.3×105 y β− 126Sb
 Category: Tin
| references

Tin is a chemical element; it has symbol Sn (from Latin stannum) and atomic number 50. A silvery-colored metal, tin is soft enough to be cut with little force,[10] and a bar of tin can be bent by hand with little effort. When bent, the so-called "tin cry" can be heard as a result of twinning in tin crystals.[11]

Tin is a post-transition metal in group 14 of the periodic table of elements. It is obtained chiefly from the mineral cassiterite, which contains stannic oxide, SnO
2. Tin shows a chemical similarity to both of its neighbors in group 14, germanium and lead, and has two main oxidation states, +2 and the slightly more stable +4. Tin is the 49th-most abundant element on Earth and has, with 10 stable isotopes, the largest number of stable isotopes in the periodic table, due to its magic number of protons.

It has two main allotropes: at room temperature, the stable allotrope is β-tin, a silvery-white, malleable metal; at low temperatures it is less dense grey α-tin, which has the diamond cubic structure. Metallic tin does not easily oxidize in air and water.

The first tin alloy used on a large scale was bronze, made of 1⁄8 tin and 7⁄8 copper (12.5% and 87.5% respectively), from as early as 3000 BC. After 600 BC, pure metallic tin was produced. Pewter, which is an alloy of 85–90% tin with the remainder commonly consisting of copper, antimony, bismuth, and sometimes lead and silver, has been used for flatware since the Bronze Age. In modern times, tin is used in many alloys, most notably tin-lead soft solders, which are typically 60% or more tin, and in the manufacture of transparent, electrically conducting films of indium tin oxide in optoelectronic applications. Another large application is corrosion-resistant tin plating of steel. Because of the low toxicity of inorganic tin, tin-plated steel is widely used for food packaging as "tin cans". Some organotin compounds can be extremely toxic.

Characteristics

[edit]

Physical

[edit]
Droplet of solidified molten tin

Tin is a soft, malleable, ductile and highly crystalline silvery-white metal. When a bar of tin is bent a crackling sound known as the "tin cry" can be heard from the twinning of the crystals.[11] This trait is shared by indium, cadmium, zinc, and mercury in its solid state. Tin melts at about 232 °C (450 °F), the lowest in group 14. The melting point is further lowered to 177.3 °C (351.1 °F) for 11 nm particles.[12][13]

External videos
video icon β–α transition of tin at −40 °C (time lapse; one second of the video is one hour in real time)

β-tin, also called white tin, is the allotrope (structural form) of elemental tin that is stable at and above room temperature. It is metallic and malleable, and has body-centered tetragonal crystal structure. α-tin, or gray tin, is the nonmetallic form. It is stable below 13.2 °C (55.8 °F) and is brittle. α-tin has a diamond cubic crystal structure, as do diamond and silicon. α-tin does not have metallic properties because its atoms form a covalent structure in which electrons cannot move freely. α-tin is a dull-gray powdery material with no common uses other than specialized semiconductor applications.[11] γ-tin and σ-tin exist at temperatures above 161 °C (322 °F)  and pressures above several GPa.[14]

In cold conditions β-tin tends to transform spontaneously into α-tin, a phenomenon known as "tin pest" or "tin disease".[15] Some unverifiable sources also say that, during Napoleon's Russian campaign of 1812, the temperatures became so cold that the tin buttons on the soldiers' uniforms disintegrated over time, contributing to the defeat of the Grande Armée,[16] a persistent legend.[17][18][19]

The α-β transformation temperature is 13.2 °C (55.8 °F), but impurities (e.g. Al, Zn, etc.) lower it well below 0 °C (32 °F). With the addition of antimony or bismuth the transformation might not occur at all, increasing durability.[20]

Commercial grades of tin (99.8% tin content) resist transformation because of the inhibiting effect of small amounts of bismuth, antimony, lead, and silver present as impurities. Alloying elements such as copper, antimony, bismuth, cadmium, and silver increase the hardness of tin.[21] Tin easily forms hard, brittle intermetallic phases that are typically undesirable. It does not mix into a solution with most metals and elements so tin does not have much solid solubility. Tin mixes well with bismuth, gallium, lead, thallium and zinc, forming simple eutectic systems.[20]

Tin becomes a superconductor below 3.72 K[22] and was one of the first superconductors to be studied.[23] The Meissner effect, one of the characteristic features of superconductors, was first discovered in superconducting tin crystals.[23]

Chemical

[edit]

Tin resists corrosion from water, but can be corroded by acids and alkalis. Tin can be highly polished and is used as a protective coat for other metals,[11] a protective oxide (passivation) layer prevents further oxidation.[24] Tin acts as a catalyst triggering a chemical reaction of a solution containing oxygen and helps to increase the speed of the chemical reaction that results.[25]

Isotopes

[edit]
Main article: Isotopes of tin

Tin has ten stable isotopes, the greatest number of any element. Their mass numbers are 112, 114, 115, 116, 117, 118, 119, 120, 122, and 124. Tin-120 makes up almost a third of all tin. Tin-118 and tin-116 are also common. Tin-115 is the least common stable isotope. The isotopes with even mass numbers have no nuclear spin, while those with odd mass numbers have a nuclear spin of 1/2. It is thought that tin has such a great multitude of stable isotopes because of tin's atomic number being 50, which is a "magic number" in nuclear physics.

Tin is one of the easiest elements to detect and analyze by NMR spectroscopy, which relies on molecular weight and its chemical shifts are referenced against tetramethyltin (SnMe
4).[b][26]

Of the stable isotopes, tin-115 has a high neutron capture cross section for fast neutron energies, at 30 barns. Tin-117 has a cross section of 2.3 barns, one order of magnitude smaller, while tin-119 has a slightly smaller cross section of 2.2 barns.[27] Before these cross sections were well known, it was proposed to use tin-lead solder as a reactor coolant for fast reactors because of its low melting point. Current studies are for lead or lead-bismuth reactor coolants because both heavy metals are nearly transparent to fast neutrons, with very low capture cross sections.[28] In order to use a tin or tin-lead coolant, the tin would first have to go through isotopic separation to remove the isotopes with odd mass number. Combined, these three isotopes make up about 17% of natural tin but represent nearly all of the capture cross section. Of the remaining seven isotopes tin-112 has a capture cross section of 1 barn. The other six isotopes forming 82.7% of natural tin have capture cross sections of 0.3 barns or less, making them effectively transparent to neutrons.

Tin has 31 unstable isotopes, ranging in mass number from 99 to 139. The unstable tin isotopes have half-lives of less than a year except for tin-126, which has a half-life of about 230,000 years. Tin-100 and tin-132 are two of the very few nuclides with a "doubly magic" nucleus which despite being unstable, as they have very uneven neutron–proton ratios, are the endpoints beyond which tin isotopes lighter than tin-100 and heavier than tin-132 are much less stable.[29] Another 30 metastable isomers have been identified for tin isotopes between 111 and 131, the most stable being tin-121m, with a half-life of 43.9 years.[30]

The relative differences in the abundances of tin's stable isotopes can be explained by how they are formed during stellar nucleosynthesis. Tin-116 through tin-120, along with tin-122, are formed in the s-process (slow neutron capture) in most stars which leads to them being the most common tin isotopes, while tin-124 is only formed in the r-process (rapid neutron capture) in supernovae and neutron star mergers. Tin isotopes 115, 117 through 120, and 122 are produced via both the s-process and the r-process,[31] The two lightest stable isotopes, tin-112 and tin-114, cannot be made in significant amounts in the s- or r-processes and are among the p-nuclei whose origins are not well understood. Some theories about their formation include proton capture and photodisintegration. Tin-115 might be partially produced in the s-process, both directly and as the daughter of long-lived indium-115, and also from the decay of indium-115 produced via the r-process.[31][32]

Etymology

[edit]

The word tin is shared among Germanic languages and can be traced back to reconstructed Proto-Germanic *tin-om; cognates include German Zinn, Swedish tenn and Dutch tin. It is not found in other branches of Indo-European, except by borrowing from Germanic (e.g., Irish tinne from English).[33][34]

The Latin name for tin, stannum, originally meant an alloy of silver and lead, and came to mean 'tin' in the fourth century[35]—the earlier Latin word for it was plumbum candidum, or "white lead". Stannum apparently came from an earlier stāgnum (meaning the same substance),[33] the origin of the Romance and Celtic terms for tin, such as French étain, Spanish estaño, Italian stagno, and Irish stán.[33][36] The origin of stannum/stāgnum is unknown; it may be pre-Indo-European.[37]

The Meyers Konversations-Lexikon suggests instead that stannum came from Cornish stean, and is evidence that Cornwall in the first centuries AD was the main source of tin.[citation needed]

History

[edit]
Main article: Tin sources and trade in ancient times
Ceremonial giant bronze dirk of the Plougrescant-Ommerschans type, Plougrescant, France, 1500–1300 BC

Tin extraction and use can be dated to the beginnings of the Bronze Age around 3000 BC, when it was observed that copper objects formed of polymetallic ores with different metal contents had different physical properties.[38] The earliest bronze objects had a tin or arsenic content of less than 2% and are believed to be the result of unintentional alloying due to trace metal content in the copper ore.[39] The addition of a second metal to copper increases its hardness, lowers the melting temperature, and improves the casting process by producing a more fluid melt that cools to a denser, less spongy metal.[39] This was an important innovation that allowed for the much more complex shapes cast in closed molds of the Bronze Age. Arsenical bronze objects appear first in the Near East where arsenic is commonly found with copper ore, but the health risks were quickly realized and the quest for sources of the much less hazardous tin ores began early in the Bronze Age.[40] This created the demand for rare tin metal and formed a trade network that linked the distant sources of tin to the markets of Bronze Age cultures.[citation needed]

Cassiterite (SnO
2), the oxide form of tin, was most likely the original source of tin. Other tin ores are less common sulfides such as stannite that require a more involved smelting process. Cassiterite often accumulates in alluvial channels as placer deposits because it is harder, heavier, and more chemically resistant than the accompanying granite.[39] Cassiterite is usually black or dark in color, and these deposits can be easily seen in river banks. Alluvial (placer) deposits may incidentally have been collected and separated by methods similar to gold panning.[41]

Compounds and chemistry

[edit]
See also: Category:Tin compounds

In the great majority of its compounds, tin has the oxidation state II or IV. Compounds containing bivalent tin are called stannous while those containing tetravalent tin are termed stannic.

Inorganic compounds

[edit]

Halide compounds are known for both oxidation states. For Sn(IV), all four halides are well known: SnF4, SnCl4, SnBr4, and SnI4. The three heavier members are volatile molecular compounds, whereas the tetrafluoride is polymeric. All four halides are known for Sn(II) also: SnF2, SnCl
2, SnBr2, and SnI2. All are polymeric solids. Of these eight compounds, only the iodides are colored.[42]

Tin(II) chloride (also known as stannous chloride) is the most important commercial tin halide. Illustrating the routes to such compounds, chlorine reacts with tin metal to give SnCl4 whereas the reaction of hydrochloric acid and tin produces SnCl
2 and hydrogen gas. Alternatively SnCl4 and Sn combine to stannous chloride by a process called comproportionation:[43]

SnCl4 + Sn → 2 SnCl
2

Tin can form many oxides, sulfides, and other chalcogenide derivatives. The dioxide SnO
2 (cassiterite) forms when tin is heated in the presence of air.[42] SnO
2 is amphoteric, which means that it dissolves in both acidic and basic solutions.[44] Stannates with the structure [Sn(OH)
6]2−, like K
2[Sn(OH)
6], are also known, though the free stannic acid H
2[Sn(OH)
6] is unknown.

Sulfides of tin exist in both the +2 and +4 oxidation states: tin(II) sulfide and tin(IV) sulfide (mosaic gold).

Ball-and-stick models of the structure of solid stannous chloride (SnCl
2)[45]

Hydrides

[edit]

Stannane (SnH
4), with tin in the +4 oxidation state, is unstable. Organotin hydrides are however well known, e.g. tributyltin hydride (Sn(C4H9)3H).[11] These compounds release transient tributyl tin radicals, which are rare examples of compounds of tin(III).[46]

Organotin compounds

[edit]

Organotin compounds, sometimes called stannanes, are chemical compounds with tin–carbon bonds.[47] Of the tin compounds, the organic derivatives are commercially the most useful.[48] Some organotin compounds are highly toxic and have been used as biocides. The first organotin compound to be reported was diethyltin diiodide ((C2H5)2SnI2), reported by Edward Frankland in 1849.[49]

Most organotin compounds are colorless liquids or solids that are stable to air and water. They adopt tetrahedral geometry. Tetraalkyl- and tetraaryltin compounds can be prepared using Grignard reagents:[48]

SnCl
4 + 4 RMgBr → R
4Sn + 4 MgBrCl

The mixed halide-alkyls, which are more common and more important commercially than the tetraorgano derivatives, are prepared by redistribution reactions:

SnCl
4 + R
4Sn → 2 SnCl
2R2

Divalent organotin compounds are uncommon, although more common than related divalent organogermanium and organosilicon compounds. The greater stabilization enjoyed by Sn(II) is attributed to the "inert pair effect". Organotin(II) compounds include both stannylenes (formula: R2Sn, as seen for singlet carbenes) and distannylenes (R4Sn2), which are roughly equivalent to alkenes. Both classes exhibit unusual reactions.[50]

Occurrence

[edit]
See also: Category:Tin minerals
Sample of cassiterite, the main ore of tin

Tin is generated via the long s-process in low-to-medium mass stars (with masses of 0.6 to 10 times that of the Sun), and finally by beta decay of the heavy isotopes of indium.[51]

Tin is the 49th most abundant element in Earth's crust, representing 2 ppm compared with 75 ppm for zinc, 50 ppm for copper, and 14 ppm for lead.[52]

Tin does not occur as the native element but must be extracted from various ores. Cassiterite (SnO
2) is the only commercially important source of tin, although small quantities of tin are recovered from complex sulfides such as stannite, cylindrite, franckeite, canfieldite, and teallite. Minerals with tin are almost always associated with granite rock, usually at a level of 1% tin oxide content.[53]

Because of the higher specific gravity of tin dioxide, about 80% of mined tin is from secondary deposits found downstream from the primary lodes. Tin is often recovered from granules washed downstream in the past and deposited in valleys or the sea. The most economical ways of mining tin are by dredging, hydraulicking, or open pits. Most of the world's tin is produced from placer deposits, which can contain as little as 0.015% tin.[54]

World tin mine reserves (tonnes, 2011)[55]
Country Reserves
 China 1,500,000
 Malaysia 250,000
 Peru 310,000
 Indonesia 800,000
 Brazil 590,000
 Bolivia 400,000
 Russia 350,000
 Australia 180,000
 Thailand 170,000
  Other 180,000
  Total 4,800,000
Economically recoverable tin reserves[53]
Year Million tonnes
1965 4,265
1970 3,930
1975 9,060
1980 9,100
1985 3,060
1990 7,100
2000 7,100[55]
2010 5,200[55]

About 253,000 tonnes of tin were mined in 2011, mostly in China (110,000 t), Indonesia (51,000 t), Peru (34,600 t), Bolivia (20,700 t) and Brazil (12,000 t).[55] Estimates of tin production have historically varied with the market and mining technology. It is estimated that, at current consumption rates and technologies, the Earth will run out of mine-able tin in 40 years.[56] In 2006 Lester Brown suggested tin could run out within 20 years based on conservative estimates of 2% annual growth.[57]

Scrap tin is an important source of the metal. Recovery of tin through recycling is increasing rapidly as of 2019.[58] Whereas the United States has neither mined (since 1993) nor smelted (since 1989) tin, it was the largest secondary producer, recycling nearly 14,000 tonnes in 2006.[55]

New deposits are reported in Mongolia,[59] and in 2009, new deposits of tin were discovered in Colombia.[60]

Production

[edit]

Tin is produced by carbothermic reduction of the oxide ore with carbon or coke. Both reverberatory furnace and electric furnace can be used:[61][62][63]

SnO2 + C Arc furnace→ Sn + CO2↑

Mining and smelting

[edit]
Main article: Tin mining

Industry

[edit]
Further information: List of countries by tin production

The ten largest tin-producing companies produced most of the world's tin in 2007.

Most of the world's tin is traded on LME, from 8 countries, under 17 brands.[64]

Largest tin producing companies (tonnes)[65]
Company Polity 2006 2007 2017[66] 2006–2017
% change
Yunnan Tin China 52,339 61,129 74,500 42.3
PT Timah Indonesia 44,689 58,325 30,200 −32.4
Malaysia Smelting Corp Malaysia 22,850 25,471 27,200 19.0
Yunnan Chengfeng China 21,765 18,000 26,800 23.1
Minsur Peru 40,977 35,940 18,000 −56.1
EM Vinto Bolivia 11,804 9,448 12,600 6.7
Guangxi China Tin China / / 11,500 /
Thaisarco Thailand 27,828 19,826 10,600 −61.9
Metallo-Chimique Belgium 8,049 8,372 9,700 20.5
Gejiu Zi Li China / / 8,700 /

International Tin Council was established in 1947 to control the price of tin. It collapsed in 1985. In 1984, Association of Tin Producing Countries was created, with Australia, Bolivia, Indonesia, Malaysia, Nigeria, Thailand, and Zaire as members.[67]

Price and exchanges

[edit]
World production and price (US exchange) of tin

Tin is unique among mineral commodities because of the complex agreements between producer countries and consumer countries dating back to 1921. Earlier agreements tended to be somewhat informal and led to the "First International Tin Agreement" in 1956, the first of a series that effectively collapsed in 1985. Through these agreements, the International Tin Council (ITC) had a considerable effect on tin prices. ITC supported the price of tin during periods of low prices by buying tin for its buffer stockpile and was able to restrain the price during periods of high prices by selling from the stockpile. This was an anti-free-market approach, designed to assure a sufficient flow of tin to consumer countries and a profit for producer countries. However, the buffer stockpile was not sufficiently large, and during most of those 29 years tin prices rose, sometimes sharply, especially from 1973 through 1980 when rampant inflation plagued many world economies.[68]

During the late 1970s and early 1980s, the U.S. reduced its strategic tin stockpile, partly to take advantage of historically high tin prices. The 1981–82 recession damaged the tin industry. Tin consumption declined dramatically. ITC was able to avoid truly steep declines through accelerated buying for its buffer stockpile; this activity required extensive borrowing. ITC continued to borrow until late 1985 when it reached its credit limit. Immediately, a major "tin crisis" ensued—tin was delisted from trading on the London Metal Exchange for about three years. ITC dissolved soon afterward, and the price of tin, now in a free-market environment, fell to $4 per pound and remained around that level through the 1990s.[68] The price increased again by 2010 with a rebound in consumption following the 2007–2008 economic crisis, accompanying restocking and continued growth in consumption.[55]

Tin Prices 2008–2022
See also: 2020s commodities boom

London Metal Exchange (LME) is tin's principal trading site.[55] Other tin contract markets are Kuala Lumpur Tin Market (KLTM) and Indonesia Tin Exchange (INATIN).[69]

Due to factors involved in the 2021 global supply chain crisis, tin prices almost doubled during 2020–21 and have had their largest annual rise in over 30 years. Global refined tin consumption dropped 1.6 percent in 2020 as the COVID-19 pandemic disrupted global manufacturing industries.[70]

Applications

[edit]
World consumption of refined tin by end-use, 2006

In 2018, just under half of all tin produced was used in solder. The rest was divided between tin plating, tin chemicals, brass and bronze alloys, and niche uses.[71]

Pigments

[edit]

Pigment Yellow 38, tin(IV) sulfide, is known as mosaic gold.[72]

Purple of Cassius, Pigment Red 109, a hydrous double stannate of gold, was mainly, in terms of painting, restricted to miniatures due to its high cost. It was widely used to make cranberry glass. It has also been used in the arts to stain porcelain.[73]

Lead-tin yellow (which occurs in two yellow forms — a stannate and a silicate) was a pigment that was historically highly important for oil painting and which had some use in fresco in its silicate form.[74] Lead stannate is also known in orange form but has not seen wide use in the fine arts. It is available for purchase in pigment form from specialist artists' suppliers. There is another minor form, in terms of artistic usage and availability, of lead-tin yellow known as Lead-tin Antimony Yellow.

Cerulean blue, a somewhat dull cyan chemically known as cobalt stannate, continues to be an important artists' pigment. Its hue is similar to that of Manganese blue, Pigment Blue 33, although it lacks that pigment's colorfulness and is more opaque.[75] Artists typically must choose between cobalt stannate and manganese blue imitations made with phthalocyanine blue green shade (Pigment Blue 15:3), as industrial production of manganese blue pigment ceased in the 1970s.[76] Cerulean blue made with cobalt stannate, however, was popular with artists prior to the production of Manganese blue.

Pigment Red 233, commonly known as Pinkcolor or Potter's Pink and more precisely known as Chrome Tin Pink Sphene, is a historically important pigment in watercolor.[77] However, it has enjoyed a large resurgence in popularity due to Internet-based word-of-mouth. It is fully lightfast and chemically stable in both oil paints and watercolors. Other inorganic mixed metal complex pigments, produced via calcination, often feature tin as a constituent. These pigments are known for their lightfastness, weatherfastness, chemical stability, lack of toxicity, and opacity. Many are rather dull in terms of colorfulness. However, some possess enough colorfulness to be competitive for use cases that require more than a moderate amount of it. Some are prized for other qualities. For instance, Pinkcolor is chosen by many watercolorists for its strong granulation, even though its chroma is low. Recently, NTP Yellow (a pyrochlore) has been brought to market as a non-toxic replacement for lead(II) chromate with greater opacity, lightfastness, and weathering resistance than proposed organic lead chromate replacement pigments possess.[78] NTP Yellow possesses the highest level of color saturation of these contemporary inorganic mixed metal complex pigments. More examples of this group include Pigment Yellow 158 (Tin Vanadium Yellow Cassiterite),[79] Pigment Yellow 216 (Solaplex Yellow),[80] Pigment Yellow 219 (Titanium Zinc Antimony Stannate),[81] Pigment Orange 82 (Tin Titanium Zinc oxide, also known as Sicopal Orange),[82] Pigment Red 121 (also known as Tin Violet and Chromium stannate),[83] Pigment Red 230 (Chrome Alumina Pink Corundum),[84] Pigment Red 236 (Chrome Tin Orchid Cassiterite),[85] and Pigment Black 23 (Tin Antimony Grey Cassiterite).[86] Another blue pigment with tin and cobalt is Pigment Blue 81, Cobalt Tin Alumina Blue Spinel.

Pigment White 15, tin(IV) oxide, is used for its iridescence, most commonly as a ceramic glaze.[87] There are no green pigments that have been used by artists that have tin as a constituent and purplish pigments with tin are classified as red, according to the Colour Index International.

Solder

[edit]
A coil of lead-free solder wire

Tin has long been used in alloys with lead as solder, in amounts of 5 to 70% w/w. Tin with lead forms a eutectic mixture at the weight proportion of 61.9% tin and 38.1% lead (the atomic proportion: 73.9% tin and 26.1% lead), with melting temperature of 183 °C (361.4 °F). Such solders are primarily used for joining pipes or electric circuits. Since the European Union Waste Electrical and Electronic Equipment Directive (WEEE Directive) and Restriction of Hazardous Substances Directive came into effect on 1 July 2006, the lead content in such alloys has decreased. While lead exposure is associated with serious health problems, lead-free solder is not without its challenges, including a higher melting point, and the formation of tin whiskers that cause electrical problems. Tin pest can occur in lead-free solders, leading to loss of the soldered joint. Replacement alloys are being found, but the problems of joint integrity remain.[88] A common lead-free alloy is 99% tin, 0.7% copper, and 0.3% silver, with melting temperature of 217 °C (422.6 °F).[89]

Tin plating

[edit]
Tin plated metal from a can

Tin bonds readily to iron and is used for coating lead, zinc, and steel to prevent corrosion. Tin-plated (or tinned) steel containers are widely used for food preservation, and this forms a large part of the market for metallic tin. A tinplate canister for preserving food was first manufactured in London in 1812.[90] Speakers of British English call such containers "tins", while speakers of U.S. English call them "cans" or "tin cans". One derivation of such use is the slang term "tinnie" or "tinny", meaning "can of beer" in Australia. The tin whistle is so called because it was mass-produced first in tin-plated steel.[91][92]

Copper cooking vessels such as saucepans and frying pans are frequently lined with a thin plating of tin, by electroplating or by traditional chemical methods, since use of copper cookware with acidic foods can be toxic.

Specialized alloys

[edit]
Pewter plate
Artisans working with tin sheets

Tin in combination with other elements forms a wide variety of useful alloys. Tin is most commonly alloyed with copper. Pewter is 85–99% tin,[93] and bearing metal has a high percentage of tin as well.[94][95] Bronze is mostly copper with 12% tin, while the addition of phosphorus yields phosphor bronze. Bell metal is also a copper–tin alloy, containing 22% tin. Tin has sometimes been used in coinage; it once formed a single-digit percentage (usually five percent or less) of American[96] and Canadian[97] pennies. Because copper is often the major metal in such coins, sometimes including zinc, these could be called bronze, or brass alloys.

The niobium–tin compound Nb3Sn is commercially used in coils of superconducting magnets for its high critical temperature (18 K) and critical magnetic field (25 T). A superconducting magnet weighing as little as two kilograms is capable of producing the magnetic field of a conventional electromagnet weighing tons.[98]

A small percentage of tin is added to zirconium alloys for the cladding of nuclear fuel.[99]

Most metal pipes in a pipe organ are of a tin/lead alloy, with 50/50 as the most common composition. The proportion of tin in the pipe defines the pipe's tone, since tin has a desirable tonal resonance. When a tin/lead alloy cools, the lead phase solidifies first, then when the eutectic temperature is reached, the remaining liquid forms the layered tin/lead eutectic structure, which is shiny; contrast with the lead phase produces a mottled or spotted effect. This metal alloy is referred to as spotted metal. Major advantages of using tin for pipes include its appearance, workability, and resistance to corrosion.[100][101]

Manufacturing of chemicals

[edit]

Tin compounds are used in the production of various chemicals, including stabilizers for PVC and catalysts for industrial processes. Tin in form of ingots provide the raw material necessary for these chemical reactions, ensuring consistent quality and performance.[102]

Optoelectronics

[edit]

The oxides of indium and tin are electrically conductive and transparent, and are used to make transparent electrically conducting films with applications in optoelectronics devices such as liquid crystal displays.[103]

Other applications

[edit]
A 21st-century reproduction barn lantern made of punched tin

Punched tin-plated steel, also called pierced tin, is an artisan technique originating in central Europe for creating functional and decorative housewares. Decorative piercing designs exist in a wide variety, based on local tradition and the artisan. Punched tin lanterns are the most common application of this artisan technique. The light of a candle shining through the pierced design creates a decorative light pattern in the room where it sits. Lanterns and other punched tin articles were created in the New World from the earliest European settlement. A well-known example is the Revere lantern, named after Paul Revere.[104]

In America, pie safes and food safes were in use in the days before refrigeration. These were wooden cupboards of various styles and sizes – either floor standing or hanging cupboards meant to discourage vermin and insects and to keep dust from perishable foodstuffs. These cabinets had tinplate inserts in the doors and sometimes in the sides, punched out by the homeowner, cabinetmaker, or a tinsmith in varying designs to allow for air circulation while excluding flies. Modern reproductions of these articles remain popular in North America.[105]

Window glass is most often made by floating molten glass on molten tin (float glass), resulting in a flat and flawless surface. This is also called the "Pilkington process".[106]

Tin is used as a negative electrode in advanced Li-ion batteries. Its application is somewhat limited by the fact that some tin surfaces[which?] catalyze decomposition of carbonate-based electrolytes used in Li-ion batteries.[107]

Tin(II) fluoride is added to some dental care products[108] as stannous fluoride (SnF2). Tin(II) fluoride can be mixed with calcium abrasives while the more common sodium fluoride gradually becomes biologically inactive in the presence of calcium compounds.[109] It has also been shown to be more effective than sodium fluoride in controlling gingivitis.[110]

Tin is used as a target to create laser-induced plasmas that act as the light source for extreme ultraviolet lithography.[111]

Organotin compounds

[edit]
Main article: Organotin chemistry

Worldwide industrial production of organotin compounds probably exceeds 50,000 tonnes.[112]

PVC stabilizers

[edit]

The major commercial application of organotin compounds is in the stabilization of PVC plastics. In the absence of such stabilizers, PVC would rapidly degrade under heat, light, and atmospheric oxygen, resulting in discolored, brittle products. Tin scavenges labile chloride ions (Cl−), which would otherwise strip HCl from the plastic material.[113] Typical tin compounds are carboxylic acid derivatives of dibutyltin dichloride, such as dibutyltin dilaurate.[114]

Biocides

[edit]

Some organotin compounds are relatively toxic, with both advantages and problems. They are used for biocidal properties as fungicides, pesticides, algaecides, wood preservatives, and antifouling agents.[113] Tributyltin oxide is used as a wood preservative.[115] Tributyltin is used for various industrial purposes such as slime control in paper mills and disinfection of circulating industrial cooling waters.[116] Tributyltin was used as additive for ship paint to prevent growth of fouling organisms on ships, with use declining after organotin compounds were recognized as persistent organic pollutants with high toxicity for some marine organisms (the dog whelk, for example).[117] The EU banned the use of organotin compounds in 2003,[118] while concerns over the toxicity of these compounds to marine life and damage to the reproduction and growth of some marine species[113] (some reports describe biological effects to marine life at a concentration of 1 nanogram per liter) have led to a worldwide ban by the International Maritime Organization.[119] Many nations now restrict the use of organotin compounds to vessels greater than 25 m (82 ft) long.[113] The persistence of tributyltin in the aquatic environment is dependent upon the nature of the ecosystem.[120] Because of this persistence and its use as an additive in ship paint, high concentrations of tributyltin have been found in marine sediments located near naval docks.[121] Tributyltin has been used as a biomarker for imposex in neogastropods, with at least 82 known species.[122] With the high levels of TBT in the local inshore areas, due to shipping activities, the shellfish had an adverse effect.[120] Imposex is the imposition of male sexual characteristics on female specimens where they grow a penis and a pallial vas deferens.[122][123] A high level of TBT can damage mammalian endocrine glands, reproductive and central nervous systems, bone structure and gastrointestinal tract.[123] Not only does tributyltin affect mammals, it affects sea otters, whales, dolphins, and humans.[123]

Organic chemistry

[edit]

Some tin reagents are useful in organic chemistry. In the largest application, stannous chloride is a common reducing agent for the conversion of nitro and oxime groups to amines. The Stille reaction couples organotin compounds with organic halides or pseudohalides.[124]

Li-ion batteries

[edit]
Main article: Lithium-ion battery

Tin forms several inter-metallic phases with lithium metal, making it a potentially attractive material for battery applications. Large volumetric expansion of tin upon alloying with lithium and instability of the tin-organic electrolyte interface at low electrochemical potentials are the greatest challenges to employment in commercial cells.[125] Tin inter-metallic compound with cobalt and carbon was implemented by Sony in its Nexelion cells released in the late 2000s. The composition of the active material is approximately Sn0.3Co0.4C0.3. Research showed that only some crystalline facets of tetragonal (beta) Sn are responsible for undesirable electrochemical activity.[126]

Precautions

[edit]
Main article: Tin poisoning

Cases of poisoning from tin metal, its oxides, and its salts are almost unknown. On the other hand, certain organotin compounds are almost as toxic as cyanide.[48]

Exposure to tin in the workplace can occur by inhalation, skin contact, and eye contact. The US Occupational Safety and Health Administration (OSHA) set the permissible exposure limit for tin exposure in the workplace as 2 mg/m3 over an 8-hour workday. The National Institute for Occupational Safety and Health (NIOSH) determined a recommended exposure limit (REL) of 2 mg/m3 over an 8-hour workday. At levels of 100 mg/m3, tin is immediately dangerous to life and health.[127]

See also

[edit]

Notes

[edit]
  1. ^ The thermal expansion of β-Sn is anisotropic: the parameters (at 20 °C) for each crystal axis are αa = 16.19×10−6/K, αc = 32.89×10−6/K, and αaverage = αV/3 = 21.76×10−6/K.[3]
  2. ^ Only hydrogen, fluorine, phosphorus, thallium and xenon are easier to use NMR analysis with for samples containing isotopes at their natural abundance.

References

[edit]
  1. ^ "Standard Atomic Weights: Tin". CIAAW. 1983.
  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. ^ a b c d e Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. ISBN 978-1-62708-155-9.
  4. ^ "New Type of Zero-Valent Tin Compound". Chemistry Europe. 27 August 2016.
  5. ^ "HSn". NIST Chemistry WebBook. National Institute of Standards and Technology. Retrieved 2013-01-23.
  6. ^ "SnH3". NIST Chemistry WebBook. National Institure of Standards and Technology. Retrieved 2013-01-23.
  7. ^ 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.
  8. ^ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
  9. ^ 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.
  10. ^ Gray, Theodore (2007). "Tin Images". The Elements. Black Dog & Leventhal.
  11. ^ a b c d e Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (1985). "Tin". Lehrbuch der Anorganischen Chemie (in German) (91–100 ed.). Walter de Gruyter. pp. 793–800. ISBN 978-3-11-007511-3.
  12. ^ "Ink with tin nanoparticles could print future circuit boards". Phys.org. 12 April 2011. Archived from the original on 16 September 2011.
  13. ^ Jo, Yun Hwan; Jung, Inyu; Choi, Chung Seok; Kim, Inyoung; Lee, Hyuck Mo (2011). "Synthesis and characterization of low temperature Sn nanoparticles for the fabrication of highly conductive ink". Nanotechnology. 22 (22): 225701. Bibcode:2011Nanot..22v5701J. doi:10.1088/0957-4484/22/22/225701. PMID 21454937. S2CID 25202674.
  14. ^ Molodets, A.M.; Nabatov, S.S. (2000). "Thermodynamic potentials, diagram of state, and phase transitions of tin on shock compression". High Temperature. 38 (5): 715–721. Bibcode:2000HTemp..38..715M. doi:10.1007/BF02755923. S2CID 120417927.
  15. ^ "Tin Pests | Center for Advanced Life Cycle Engineering". calce.umd.edu. Retrieved 2022-11-04.
  16. ^ Le Coureur, Penny; Burreson, Jay (2004). Napoleon's Buttons: 17 molecules that changed history. New York: Penguin Group, USA.
  17. ^ Öhrström, Lars (2013). The Last Alchemist in Paris. Oxford: Oxford University Press. ISBN 978-0-19-966109-1.
  18. ^ Cotton, Simon (29 April 2014). "Book review: The last alchemist in Pari". Chemistry World. Royal Society of Chemistry. Archived from the original on 10 August 2014. Retrieved 22 November 2019.
  19. ^ Emsley, John (1 October 2011) [2001]. Nature's Building Blocks: an A-Z Guide to the Elements (New ed.). New York, United States: Oxford University Press. p. 552. ISBN 978-0-19-960563-7. Only officers had metal buttons, and those were made of brass.
  20. ^ a b Schwartz, Mel (2002). "Tin and alloys, properties". Encyclopedia of Materials, Parts and Finishes (2nd ed.). CRC Press. ISBN 978-1-56676-661-6.
  21. ^ "Tin Alloys – Characteristics and Uses". Nuclear Power. Retrieved 2022-11-04.
  22. ^ Dehaas, W.; Deboer, J.; Vandenberg, G. (1935). "The electrical resistance of cadmium, thallium and tin at low temperatures". Physica. 2 (1–12): 453. Bibcode:1935Phy.....2..453D. doi:10.1016/S0031-8914(35)90114-8.
  23. ^ a b Meissner, W.; R. Ochsenfeld (1933). "Ein neuer effekt bei eintritt der Supraleitfähigkeit". Naturwissenschaften. 21 (44): 787–788. Bibcode:1933NW.....21..787M. doi:10.1007/BF01504252. S2CID 37842752.
  24. ^ Craig, Bruce D.; Anderson, David S.; International, A. S. M. (January 1995). Handbook of corrosion data. ASM International. p. 126. ISBN 978-0-87170-518-1. Archived from the original on 2016-05-11.
  25. ^ Crutchlow, Charlotte (25 June 2021). "Tin-Formation About the Element Tin | Periodic Table". ChemTalk. Retrieved 2022-11-04.
  26. ^ "Interactive NMR Frequency Map". Archived from the original on 2011-06-04. Retrieved 2009-05-05.
  27. ^ "Neutron Scattering Lengths and cross sections".
  28. ^ "Westinghouse Nuclear > Energy Systems > Lead-cooled Fast Reactor".
  29. ^ Walker, Phil (1994). "Doubly Magic Discovery of Tin-100". Physics World. 7 (June): 28. doi:10.1088/2058-7058/7/6/24.
  30. ^ 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
  31. ^ a b Bragagni, Alessandro; Wombacher, Frank; Kirchenbaur, Maria; Braukmüller, Ninja; Münker, Carsten (2023). "Mass-independent Sn isotope fractionation and radiogenic 115Sn in chondrites and terrestrial rocks". Geochimica et Cosmochimica Acta. 344: 40–58. doi:10.1016/j.gca.2023.01.014.
  32. ^ Cameron, A. G. W. (1973). "Abundance of the Elements in the Solar System" (PDF). Space Science Reviews. 15 (1): 121–146. Bibcode:1973SSRv...15..121C. doi:10.1007/BF00172440. S2CID 120201972. Archived from the original (PDF) on 2011-10-21.
  33. ^ a b c "tin". Oxford English Dictionary (Online ed.). Oxford University Press. (Subscription or participating institution membership required.)
  34. ^ Harper, Douglas. "tin". Online Etymology Dictionary.
  35. ^ Encyclopædia Britannica, 11th Edition, 1911, s.v. 'tin', citing H. Kopp
  36. ^ "The Ancient Mining of Tin". oxleigh.freeserve.co.uk. Archived from the original on 2009-04-03. Retrieved 2009-07-07.
  37. ^ American Heritage Dictionary
  38. ^ Cierny, J.; Weisgerber, G. (2003). "The "Bronze Age tin mines in Central Asia". In Giumlia-Mair, A.; Lo Schiavo, F. (eds.). The Problem of Early Tin. Oxford: Archaeopress. pp. 23–31. ISBN 978-1-84171-564-3.
  39. ^ a b c Penhallurick, R. D. (1986). Tin in Antiquity: its Mining and Trade Throughout the Ancient World with Particular Reference to Cornwall. London: The Institute of Metals. ISBN 978-0-904357-81-3.
  40. ^ Lamberg-Karlovsky, C. C.; Franklin, Alan D.; Olin, Jacqueline S.; Wertime, Theodore A., eds. (July 1980). "The development of the usage of tin and tin-bronze: some problems". The Search for Ancient Tin. Vol. 21. Washington D.C.: A seminar organized by Theodore A. Wertime and held at the Smithsonian Institution and the National Bureau of Standards, Washington D.C. March 14–15, 1977. p. 474. doi:10.2307/3103162. JSTOR 3103162. {{cite book}}: |journal= ignored (help)
  41. ^ Dube, RK (September 2006). "Interrelation between gold and tin: A historical perspective". Gold Bulletin. 39 (3): 103–113. doi:10.1007/BF03215537.
  42. ^ a b Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils (ed.), Inorganic Chemistry, translated by Eagleson, Mary; Brewer, William, San Diego/Berlin: Academic Press/De Gruyter, ISBN 0-12-352651-5
  43. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.[page needed]
  44. ^ Taylor, F. Sherwood (1942). Inorganic & Theoretical Chemistry (6th ed.). Heineman.
  45. ^ Leger, J. M.; Haines, J.; Atouf, A. (1996). "The high pressure behaviour of the cotunnite and post-cotunnite phases of PbCl2 and SnCl
    2    ". J. Phys. Chem. Solids. 57 (1): 7–16. Bibcode:1996JPCS...57....7L. doi:10.1016/0022-3697(95)00060-7.
  46. ^ Gaur, D. P.; Srivastava, G.; Mehrotra, R. C. (1973). "Organic Derivatives of Tin. III. Reactions of Trialkyltin Ethoxide with Alkanolamines". Zeitschrift für Anorganische und Allgemeine Chemie. 398: 72. doi:10.1002/zaac.19733980109.
  47. ^ Elschenbroich, Christoph (2006). Organometallics (3rd, completely rev. and extended ed.). Weinheim: Wiley-VCH. ISBN 3-527-29390-6. OCLC 64305455.
  48. ^ a b c Graf, G. G. (2000) "Tin, Tin Alloys, and Tin Compounds" in Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH, Weinheim doi:10.1002/14356007.a27_049
  49. ^ Thoonen, Sander H. L.; Deelman, Berth-Jan; van Koten, Gerard (2004). "Synthetic aspects of tetraorganotins and organotin(IV) halides" (PDF). Journal of Organometallic Chemistry. 689 (13): 2145–2157. doi:10.1016/j.jorganchem.2004.03.027. hdl:1874/6594. S2CID 100214292. Archived from the original (PDF) on 2011-08-07. Retrieved 2009-07-31.
  50. ^ Peng, Yang; Ellis, Bobby D.; Wang, Xinping; Fettinger, James C.; Power, P. P. (2009). "Reversible Reactions of Ethylene with Distannynes Under Ambient Conditions". Science. 325 (5948): 1668–1670. Bibcode:2009Sci...325.1668P. doi:10.1126/science.1176443. PMID 19779193. S2CID 3011002.
  51. ^ Shu, Frank H. (1982). The physical universe: An introduction to astronomy. University Science Books. pp. 119–121. ISBN 978-0-935702-05-7.
  52. ^ Emsley 2001, pp. 124, 231, 449 and 503.
  53. ^ a b "Tin: From Ore to Ingot". International Tin Research Institute. 1991. Archived from the original on 2009-03-22. Retrieved 2009-03-21.
  54. ^ Sutphin, David M.; Sabin, Andrew E.; Reed, Bruce L. (1 June 1992). Tin – International Strategic Minerals Inventory Summary Report. DIANE. p. 9. ISBN 978-0-941375-62-7. Archived from the original on 2016-04-28.
  55. ^ a b c d e f g Carlin, James F. Jr. "Tin: Statistics and Information" (PDF). United States Geological Survey. Archived from the original on 2008-12-06. Retrieved 2008-11-23.
  56. ^ Reilly, Michael (26 May 2007). "How Long Will it Last?". New Scientist. 194 (2605): 38–39. Bibcode:2007NewSc.194...38R. doi:10.1016/S0262-4079(07)61508-5.
  57. ^ Brown, Lester (2006). Plan B 2.0. New York: W.W. Norton. p. 109. ISBN 978-0-393-32831-8.
  58. ^ Alves, Bruna (15 February 2024). "U.S. annual tin recycling 2023". Statista. Retrieved 2024-06-23.
  59. ^ Kovalenko, V. I.; Yarmolyuk, V. V. (1995). "Endogenous rare metal ore formations and rare metal metallogeny of Mongolia". Economic Geology. 90 (3): 520. Bibcode:1995EcGeo..90..520K. doi:10.2113/gsecongeo.90.3.520.
  60. ^ "Seminole Group Colombia Discovers High Grade Tin Ore in the Amazon Jungle". FreePR101 PressRelease. Archived from the original on 2014-08-26.
  61. ^ Schrader, George F.; Elshennawy, Ahmad K.; Doyle, Lawrence E. (July 2000). Manufacturing processes and materials. Society of Manufacturing Engineers. ISBN 978-0-87263-517-3. Archived from the original on 2016-05-11.
  62. ^ Louis, Henry (1911). Metallurgy of tin. McGraw-Hill book Company.
  63. ^ Knorr, Klaus (1945). Tin Under Control. Stanford University Press. ISBN 978-0-8047-2136-3. Archived from the original on 2016-05-19.
  64. ^ "LME Tin Brands". ITRI.co.uk. International Tin Research Institute. Archived from the original on 2008-12-07. Retrieved 2009-05-05.
  65. ^ "Top Ten Tin Producing Companies". itri.co.uk. International Tin Research Institute. Archived from the original on 2008-12-07. Retrieved 2009-05-05.
  66. ^ "The World's Biggest Tin Producers". The Balance. 13 January 2019.
  67. ^ "Agreement establishing the Association of Tin Producing Countries [1984] ATS 10". Australasian Legal Information Institute, Australian Treaties Library.
  68. ^ a b Carlin, James F. Jr. (1998). "Significant events affecting tin prices since 1958" (PDF). USGS. Archived from the original (PDF) on 2011-10-28.
  69. ^ "12 Januari Pemasaran Perdana INATIN". 15 December 2011. Archived from the original on 2012-04-26.
  70. ^ Daly, Tom (5 December 2021). "Tin surge worsens supply chain woes for electronics, solar and auto firms". Reuters. Retrieved 2021-12-07.
  71. ^ "Tin demand to decline – International Tin Association". Mining.com. 18 October 2019. Retrieved 2021-07-03.
  72. ^ "The Color of Art Pigment Database – Pigment Yellow – PY". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  73. ^ "The Color of Art Pigment Database – Pigment Red – PR". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  74. ^ "The Color of Art Pigment Database – Pigment Yellow – PY". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  75. ^ "The Color of Art Pigment Database – Pigment Blue – PB". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  76. ^ "The Color of Art Pigment Database – Pigment Blue – PB". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  77. ^ "The Color of Art Pigment Database – Pigment Red – PR". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  78. ^ "The Color of Art Pigment Database – Pigment Yellow – PY". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  79. ^ "The Color of Art Pigment Database – Pigment Yellow – PY". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  80. ^ "The Color of Art Pigment Database – Pigment Yellow – PY". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  81. ^ "The Color of Art Pigment Database – Pigment Yellow – PY". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  82. ^ "The Color of Art Pigment Database – Pigment Orange – PO". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  83. ^ "The Color of Art Pigment Database – Pigment Red – PR". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  84. ^ "The Color of Art Pigment Database – Pigment Red – PR". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  85. ^ "The Color of Art Pigment Database – Pigment Red – PR". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  86. ^ "The Color of Art Pigment Database – Pigment Black – PBk". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  87. ^ "The Color of Art Pigment Database – Pigment White – PW". artiscreation. 2024. Retrieved 2024-08-17.{{cite web}}: CS1 maint: url-status (link)
  88. ^ Black, Harvey (2005). "Getting the Lead Out of Electronics". Environmental Health Perspectives. 113 (10): A682–5. doi:10.1289/ehp.113-a682. PMC 1281311. PMID 16203230.
  89. ^ "Technical data Sheet - Lead free alloy" (PDF). RS Online. Retrieved 2023-06-18.
  90. ^ Childs, Peter (July 1995). "The tin-man's tale". Education in Chemistry. Vol. 32, no. 4. Royal Society of Chemistry. p. 92. Retrieved 2018-06-19.
  91. ^ Control, Tin Under (1945). Tin Under Control. pp. 10–15. ISBN 978-0-8047-2136-3. Archived from the original on 2016-05-31.
  92. ^ Panel On Tin, National Research Council (U.S.). Committee on Technical Aspects of Critical and Strategic Materials (1970). Trends in the use of tin. pp. 10–22. Archived from the original on 2016-05-22.
  93. ^ Hull, Charles (1992). Pewter. Osprey Publishing. pp. 1–5. ISBN 978-0-7478-0152-8.
  94. ^ Brakes, James (2009). "Introduction". Analysis of Babbit. BiblioBazaar, LLC. pp. 1–2. ISBN 978-1-110-11092-6.
  95. ^ Williams, Robert S. (2007). Principles of Metallography. Read books. pp. 46–47. ISBN 978-1-4067-4671-6.
  96. ^ "The Composition of the Cent". US Mint. Archived from the original on 2011-10-25. Retrieved 2011-10-28.
  97. ^ "Composition of canadian coins" (PDF). Canadian Mint. Archived (PDF) from the original on 2012-01-13. Retrieved 2011-10-28.
  98. ^ Geballe, Theodore H. (October 1993). "Superconductivity: From Physics to Technology". Physics Today. 46 (10): 52–56. Bibcode:1993PhT....46j..52G. doi:10.1063/1.881384.
  99. ^ Campbell, Flake C. (2008). "Zirconium". Elements of Metallurgy and Engineering Alloys. ASM International. p. 597. ISBN 978-0-87170-867-0. Archived from the original on 2016-05-28.
  100. ^ Robert Palmieri, ed. (2006). "Pipe Metal". Encyclopedia of keyboard instruments. New York: Garland. p. 411. ISBN 978-0-415-94174-7.
  101. ^ George Ashdown Audsley (1988). "Metal Pipes: And the Materials used in their Construction". The Art of Organ Building Audsley, George Ashdown. Courier Dover Publications. p. 501. ISBN 978-0-486-21315-6.
  102. ^ Gupta, Yash. "Tin Ingots". Rikayaa.
  103. ^ Kim, H.; Gilmore, C.; Pique, A.; Horwitz, J.; Mattoussi, H.; Murata, H.; Kafafi, Z.; Chrisey, D. (1999). "Electrical, optical, and structural properties of indium tin oxide thin films for organic light-emitting devices". Journal of Applied Physics. 86 (11): 6451. Bibcode:1999JAP....86.6451K. doi:10.1063/1.371708.
  104. ^ Bridge, Janet (September 1996). Making & decorating picture frames. North Light Books. ISBN 978-0-89134-739-2.
  105. ^ "Tin punching". Archived from the original on 2011-08-11. Retrieved 2011-08-15.
  106. ^ Pilkington, L. A. B. (1969). "Review Lecture. The Float Glass Process". Proceedings of the Royal Society of London. Series A, Mathematical and Physical Sciences. 314 (1516): 1–25. Bibcode:1969RSPSA.314....1P. doi:10.1098/rspa.1969.0212. JSTOR 2416528. S2CID 109981215.
  107. ^ Lucas, Ivan T.; Syzdek, Jarosław; Kostecki, Robert (2011). "Interfacial processes at single-crystal β-Sn electrodes in organic carbonate electrolytes". Electrochemistry Communications. 13 (11): 1271–1275. doi:10.1016/j.elecom.2011.08.026.
  108. ^ "Colgate Gel-Kam". Archived from the original on 2009-04-27. Retrieved 2009-05-05.
  109. ^ Hattab, F. (April 1989). "The State of Fluorides in Toothpastes". Journal of Dentistry. 17 (2): 47–54. doi:10.1016/0300-5712(89)90129-2. PMID 2732364.
  110. ^ Perlich, M. A.; Bacca, L. A.; Bollmer, B. W.; Lanzalaco, A. C.; McClanahan, S. F.; Sewak, L. K.; Beiswanger, B. B.; Eichold, W. A.; Hull, J. R.; et al. (1995). "The clinical effect of a stabilized stannous fluoride dentifrice on plaque formation, gingivitis and gingival bleeding: a six-month study". The Journal of Clinical Dentistry. 6 (Special Issue): 54–58. PMID 8593194.
  111. ^ Versolato, Oscar O. (2019). "Physics of laser-driven tin plasma sources of EUV radiation for nanolithography". Plasma Sources Science and Technology. 28 (8). doi:10.1088/1361-6595/ab3302.
  112. ^ Ebdon, L.; Britain), Royal Society of Chemistry (Great (2001). "Organotin in Industrial and Domestic Products". Trace element speciation for environment, food and health. Royal Society of Chemistry. p. 144. ISBN 978-0-85404-459-7. Archived from the original on 2016-05-21.
  113. ^ a b c d Atkins, Peter; Shriver, Duward F.; Overton, Tina & Rourke, Jonathan (2006). Inorganic chemistry (4th ed.). W.H. Freeman. pp. 343, 345. ISBN 978-0-7167-4878-6.
  114. ^ Wilkes, Charles E.; Summers, James W.; Daniels, Charles Anthony; Berard, Mark T. (August 2005). PVC handbook. Hanser. p. 108. ISBN 978-1-56990-379-7. Archived from the original on 2016-05-09.
  115. ^ David N.-S. Hon; Nobuo Shiraishi, eds. (2001). "Preservation of Wood". Wood and cellulosic chemistry. New York, NY: Dekker. p. 799. ISBN 978-0-8247-0024-9.
  116. ^ Antizar-Ladislao, Blanca (1 February 2008). "Environmental levels, toxicity and human exposure to tributyltin (TBT)-contaminated marine environment. A review". Environment International. 34 (2): 292–308. Bibcode:2008EnInt..34..292A. doi:10.1016/j.envint.2007.09.005. PMID 17959247.
  117. ^ Eisler, Ronald. "Tin Hazards To Fish, Wildlife, and Invertebrates: A Synoptic Review" (PDF). U.S. Fish and Wildlife Service Patuxent Wildlife Research Center. Archived (PDF) from the original on 2012-01-18.
  118. ^ "Regulation (EC) No 782/2003 of the European Parliament and of the Council of 14 April 2003 on the prohibition of organotin compounds on ships". europa.eu. Retrieved 2009-05-05.
  119. ^ Dürr, Simone; Thomason, Jeremy, eds. (2008). "Fouling on Shipping". Biofouling. Oxford: Blackwell. p. 227. ISBN 978-1-4051-6926-4.
  120. ^ a b Maguire, R. James (1987). "Environmental aspects of tributyltin". Applied Organometallic Chemistry. 1 (6): 475–498. doi:10.1002/aoc.590010602.
  121. ^ de Mora, S. J.; Stewart, C.; Phillips, D. (1 January 1995). "Sources and rate of degradation of tri(n-butyl)tin in marine sediments near Auckland, New Zealand". Marine Pollution Bulletin. 30 (1): 50–57. Bibcode:1995MarPB..30...50D. doi:10.1016/0025-326X(94)00178-C.
  122. ^ a b Axiak, Victor; Micallef, Diane; Muscat, Joanne; Vella, Alfred; Mintoff, Bernardette (1 March 2003). "Imposex as a biomonitoring tool for marine pollution by tributyltin: some further observations". Environment International. Secotox S.I. 28 (8): 743–749. Bibcode:2003EnInt..28..743A. doi:10.1016/S0160-4120(02)00119-8. PMID 12605923.
  123. ^ a b c "The Effects of Tributyltin on the Marine Environment". ScienceBuzz. 17 November 2018. Archived from the original on 2021-01-25. Retrieved 2020-11-17.
  124. ^ Farina, Vittorio; Krishnamurthy, Venkat; Scott, William J. (1997). "The Stille Reaction". Organic Reactions. pp. 1–652. doi:10.1002/0471264180.or050.01. ISBN 0-471-26418-0.
  125. ^ Mou, Haoyi; Xiao, Wei; Miao, Chang; Li, Rui; Yu, Liming (2020). "Tin and Tin Compound Materials as Anodes in Lithium-Ion and Sodium-Ion Batteries: A Review". Frontiers in Chemistry. 8: 141. Bibcode:2020FrCh....8..141M. doi:10.3389/fchem.2020.00141. PMC 7096543. PMID 32266205.
  126. ^ Lucas, Ivan; Syzdek, Jaroslaw (2011). "Interfacial processes at single-crystal β-Sn electrodes in organic carbonate electrolytes". Electrochemistry Communications. 13 (11): 1271. doi:10.1016/j.elecom.2011.08.026.
  127. ^ "NIOSH Pocket Guide to Chemical Hazards – Tin". CDC. Archived from the original on 2015-11-25. Retrieved 2015-11-24.

Bibliography

[edit]
[edit]
Retrieved from "https://en.wikipedia.org/w/index.php?title=Tin&oldid=1241575109#Physical"