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User:R8R/Indium

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Not to be confused with Iridium.
Indium, 49In
Indium
Pronunciation/ˈɪndiəm/ ​(IN-dee-əm)
Appearancesilvery lustrous gray
Standard atomic weight Ar°(In)
Indium 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
Ga
↑
In
↓
Tl
cadmium ← indium → tin
Atomic number (Z)49
Groupgroup 13 (boron group)
Periodperiod 5
Block  p-block
Electron configuration[Kr] 4d10 5s2 5p1
Electrons per shell2, 8, 18, 18, 3
Physical properties
Phase at STPsolid
Melting point429.7485 K ​(156.5985 °C, ​313.8773 °F)
Boiling point2345 K ​(2072 °C, ​3762 °F)
Density (at 20° C)7.290 g/cm3[3]
when liquid (at m.p.)7.02 g/cm3
Triple point429.7445 K, ​~1 kPa[4]
Heat of fusion3.281 kJ/mol
Heat of vaporization231.8 kJ/mol
Molar heat capacity26.74 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 1196 1325 1485 1690 1962 2340
Atomic properties
Oxidation statescommon: 3
−5,[5] −2,[6] −1,[7] 0,[8] 1,[9] 2[9]
ElectronegativityPauling scale: 1.78
Ionization energies
  • 1st: 558.3 kJ/mol
  • 2nd: 1820.7 kJ/mol
  • 3rd: 2704 kJ/mol
Atomic radiusempirical: 167 pm
Covalent radius142±5 pm
Van der Waals radius193 pm
Color lines in a spectral range
Spectral lines of indium
Other properties
Natural occurrenceprimordial
Crystal structure ​body-centered tetragonal (tI2)
Lattice constants
Body-centered-tetragonal crystal structure for indium
a = 325.16 pm
c = 494.71 pm (at 20 °C)[3]
Thermal expansion32.2×10−6/K (at 20 °C)[a]
Thermal conductivity81.8 W/(m⋅K)
Electrical resistivity83.7 nΩ⋅m (at 20 °C)
Magnetic orderingdiamagnetic[10]
Molar magnetic susceptibility−64.0×10−6 cm3/mol (298 K)[11]
Young's modulus11 GPa
Speed of sound thin rod1215 m/s (at 20 °C)
Mohs hardness1.2
Brinell hardness8.8–10.0 MPa
CAS Number7440-74-6
History
DiscoveryFerdinand Reich and Hieronymous Theodor Richter (1863)
First isolationHieronymous Theodor Richter (1864)
Isotopes of indium
Main isotopes[12] Decay
abun­dance half-life (t1/2) mode pro­duct
111In synth 2.8 d ε 111Cd
113In 4.28% stable
115In 95.7% 4.41×1014 y β− 115Sn
 Category: Indium
| references

Indium (/ˈɪndiəm/ IN-dee-əm) is a chemical element with chemical symbol In and atomic number 49. This rare, very soft, malleable and easily fusible post-transition metal is chemically similar to gallium and thallium, and shows the intermediate properties between these two. Indium was discovered in 1863 and named for the indigo blue line in its spectrum that was the first indication of its existence in zinc ores, as a new and unknown element. The metal was first isolated in the following year. Zinc ores continue to be the primary source of indium, where it is found in compound form. Very rarely the element can be found as grains of native (free) metal, but these are not of commercial importance.

Indium's current primary application is to form transparent electrodes from indium tin oxide in liquid crystal displays and touchscreens, and this use largely determines its global mining production. It is widely used in thin-films to form lubricated layers (during World War II it was widely used to coat bearings in high-performance aircraft). It is also used for making particularly low melting point alloys, and is a component in some lead-free solders.

Indium is not known to be used by any organism. In a similar way to aluminum salts, indium(III) ions can be toxic to the kidney when given by injection, but oral indium compounds do not have the chronic toxicity of salts of heavy metals, probably due to poor absorption in basic conditions. Radioactive indium-111 (in very small amounts on a chemical basis) is used in nuclear medicine tests, as a radiotracer to follow the movement of labeled proteins and white blood cells in the body.

Characteristics

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Physical

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Indium wetting the glass surface of a test tube

Indium is a very soft, silvery-white, relatively rare true metal with a bright luster. When it is bent, indium emits a high-pitched "cry".[13] Like gallium, indium is able to wet glass. Indium has a low melting point, compared to those of most other metals, 156.60 °C (313.88 °F); it is higher than that of its lighter homologue, gallium, but lower than that of the heavier homologue, thallium.[14] Its bolling point is, however, moderate, being 2072 °C (3762 °F), which is higher than that of thallium, but lower than that of gallium, showing opposition to melting points trend. The density of indium, 7.31 g·cm−3, is also higher than that of gallium, but lower than that of thallium.[14]

Indium atom has 49 electrons, having electronic configuration [Kr]4d105s25p1. In its compounds, indium most often loses its three outermost electrons, becoming indium(III) ions, In3 , but in some cases the pair of 5s-electrons can stay within the atom, indium thus oxidized only to indium(I), In . This happens due to inert pair effect, which occurs because of stabilization of 5s-orbital due to relativistic effects, which are stronger closer to the bottom of the periodic table. Its heavier homologue, thallium, shows an even stronger effect, making oxidation to thallium(I) more likely than to thallium(III), making 1 the more likely oxidation state.[15]

A number of standard electrode potentials, depending on the reaction under study,[16] is reported for indium:

-0.40In2 e− ↔ In
-0.49In3 e− ↔ In2
-0.443In3 2 e− ↔ In
-0.3382In3 3 e− ↔ In
-0.14In e− ↔ In

Chemical

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Indium is a post-transition metal and chemically, is the intermediate element between its group 13 neighbors gallium and thallium. It shows two main oxidation states, which are 1 and 3, with latter being more stable, where as the only common oxidation state of gallium is 3 and thallium shows 1 more likely than 3, with thallium(III) being a moderately strong oxidizing agent, while indium(III) is stable and indium(I) is a powerful reducing agent.[17]

Indium does not react with water, but it is oxidized by stronger oxidizing agents, such as halogens or oxalic acid, to give indium(III) compounds. It does not react with boron, silicon or carbon, and the corresponding boride, silicide or carbide are not known. Similarly, reaction between indium and hydrogen has not been observed, but both indium(I) and indium(III) hydrides are known.[18]

Indium(III) oxide is formed at hot temperatures during reaction between indium and oxygen, with blue flame. It is amphoteric, i. e. it can react with both alkalies and bases. Its reaction with water results in insoluble indium(III) hydroxide, which is also amphoteric, reacting with alkalies to give indates(III) and with acids to give indium(III) salts:

In(OH)3 2 NaOH → 2 Na[InO2] H2O
In(OH)3 3 HCl → InCl3 3 H2O

The hydrolysis of sodium indate(III) gives weak indic acid, HInO2. Out of common indium(III) salts, chloride, sulfate and nitrate are soluble. In water solutions, In3 and [InO2]- ions are hydrolyzed to give InOH2 and HInO2 due to generally amphoteric character of indium(III) ions. Indium(III) compounds are not well-soluble, similarly to thallium(III) compounds; however, indium(III) salts of strong acids, such as chloride, sulfate and nitrate are soluble, hydrolyzing in water solutions. The In3 ion is colorless in solution because of the absence of unpaired electrons in the d- and f-electron shells.[17]

Indium(I) compounds are not as common as indium(III) ones; only chloride, bromide, iodide, sulfide and cyclopentadienyl are well-characterized. Indium(I) sulfide is the product of reaction between indium and sulfur or indium and hydrogen sulfide, and can be received at 700—1000 °C. Indium(I) oxide black powder is received at 850 °C during reaction between indium and carbon dioxide or during decomposition of indium(III) oxide at 1200 °C. Cyclopentadienylindium(I), which was the first organoindium(I) compound reported,[19] is polymer consisting of zigzag chains of alternating indium atoms and cyclopentadienyl complexes.

Less frequently, indium shows intermediate oxidation state 2, which lies between the common ones, most notably in halides, In2X4 and [In2X6]2-.[20] Several other compounds are known to combine indium(I) and indium(III), such as InI6(InIIICl6)Cl3,[21] InI5(InIIIBr4)2(InIIIBr6),[22] InIInIIIBr4.[23]

Isotopes

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Main article: Isotopes of indium

Indium occurs naturally on Earth only in two primordial nuclides, indium-113 and indium-115. Out of this two, indium-115 makes up 95.7% of all indium but it is radioactive, decaying to tin-115 via beta decay with half-life of 4.41×1014 years, four orders of magnitude larger than the age of the universe and nearly 50,000 times longer than that of natural thorium.[24] This effect is uncommon between chemical elements; only indium and rhenium have been shown that their most abundant isotopes are radioactive. The less common natural isotope of indium, indium-113, is however stable.

Indium has 39 known isotopes, ranging in mass between 97 and 135. Only one of them is stable and one has half-life exceeding 1014 years; the most stable other indium isotope is indium-111, which has half-life of approximately 2.8 days. All other isotopes have half-lives shorter than 5 hours. Indium also has 46 meta states, out of which indium-114m1 is the most stable, being more stable than ground state of any indium isotope, except for the primordial ones.

Creation and occurrence

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The s-process acting in the range from silver to antimony.

Indium is created via the long-lasting, up to thousands years, s-process in low-medium mass stars (which range in mass between 0.6 and 10 masses of Sun). When a silver-109 atom, which make approximately half of all silver existing, catches a neutron, it undergoes a beta decay to become cadmium-110 atom. Capturing further neutrons, it becomes cadmium-115 atom, which decay to indium-115 via another beta decay, which explains, why the radioactive isotope predominates in abundance compared to the stable one.[25]

Indium is 61st most abundant element in the Earth's crust at approximately 49 ppb, making indium approximately as abundant as mercury.[26] Fewer than 10 indium minerals are known, such as dzhalindite (In(OH)3) and indite (FeIn2S4),[27] but none of these occurs in significant deposits.

Resources

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Based on content of indium in zinc ore stocks, there is a worldwide reserve base of approximately 6,000 tonnes of economically viable indium.[28] This figure has led to estimates suggesting that, at current consumption rates, there is only 13 years' supply of indium left.[29] However, the Indium Corporation, the largest processor of indium, claims that, on the basis of increasing recovery yields during extraction, recovery from a wider range of base metals (including tin, copper and other polymetallic deposits) and new mining investments, the long-term supply of indium is sustainable, reliable and sufficient to meet increasing future demands.[30]

This conclusion also seems reasonable in light of the fact that silver, one-third as abundant as indium in the earths crust,[31] is currently mined at approximately 18,300 tonnes per annum,[32] which is 40 times greater than current indium mining rates.

Discovery

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In 1863, the German chemists Ferdinand Reich and Hieronymous Theodor Richter were testing ores from the mines around Freiberg, Saxony. They dissolved the minerals pyrite, arsenopyrite, galena and sphalerite in hydrochloric acid and distilled the raw zinc chloride. As it was known that ores from that region sometimes contain thallium they searched for the green emission lines with spectroscopic methods. The green lines were absent but a blue line was present in the spectrum. As no element was known with a bright blue emission they concluded that a new element was present in the minerals. They named the element with the blue spectral line indium, from the indigo color seen in its spectrum.[33][34] Richter went on to isolate the metal in 1864.[35] At the World Fair 1867 an ingot of 0.5 kg (1.1 lb) was presented.[36]

Production

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The lack of indium mineral deposits and the fact that indium is enriched in sulfidic lead, tin, copper, iron and predominately in zinc deposits, makes zinc production the main source for indium. The indium is leached from slag and dust of zinc production. Further purification is done by electrolysis.[36]

Indium is produced mainly from residues generated during zinc ore processing but is also found in iron, lead, and copper ores.[13] Canada is a leading producer of indium. The Teck Cominco refinery in Trail, British Columbia, is the largest single source indium producer, with production of 32,500 kg in 2005, 41,800 kg in 2004 and 36,100 kg in 2003. South American Silver's Malku Khota property in Bolivia is the largest resource of indium with an indicated resource of 845,000 kg and inferred resource of 968,000 kg.Adex Mining Inc.’s Mount Pleasant Mine in New Brunswick, Canada, holds about 15 to 20% of the world’s total known indium resources.[37]

The amount of indium consumed is largely a function of worldwide LCD production. Worldwide production is currently 476 tonnes per year from mining and a further 650 tonnes per year from recycling.[30] Demand has risen rapidly in recent years with the popularity of LCD computer monitors and television sets, which now account for 50% of indium consumption.[38] Increased manufacturing efficiency and recycling (especially in Japan) maintain a balance between demand and supply. Demand increased as the metal is used in LCDs and televisions, and supply decreased when a number of Chinese mining concerns stopped extracting indium from their zinc tailings. In 2002, the price was US$94 per kilogram. The recent changes in demand and supply have resulted in high and fluctuating prices of indium, which from 2005 to 2007 ranged from US$700/kg to US$1,000/kg.[28] Demand for indium may increase with large-scale manufacture of CIGS-based thin film solar technology starting by several companies in 2008, including Nanosolar and Miasole.

Applications

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A magnified image of an LCD screen showing RGB pixels. Individual transistors are seen as white dots in the bottom part.

The first large-scale application for indium was as a coating for bearings in high-performance aircraft engines during World War II. Afterward, production gradually increased as new uses were found in fusible alloys, solders, and electronics. In the 1950s, tiny beads of it were used for the emitters and collectors of PNP alloy junction transistors. In the middle and late 1980s, the development of indium phosphide semiconductors and indium tin oxide thin films for liquid crystal displays (LCD) aroused much interest. By 1992, the thin-film application had become the largest end use.[39][40]

Electronics

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Metal and alloys

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Ductile indium wire
  • Very small amounts used in aluminium alloy sacrificial anodes (for salt water applications) to prevent passivation of the aluminium.
  • To bond gold electrical test leads to superconductors, indium is used as a conducting adhesive and applied under a microscope with precision tweezers.
  • In the form of a wire it is used as a vacuum seal and a thermal conductor in cryogenics and ultra-high vacuum applications. For example, in manufacturing gaskets which deform to fill gaps.[45]
  • Used as a calibration material for Differential scanning calorimetry.
  • It is an ingredient in the gallium-indium-tin alloy Galinstan, which is liquid at room temperature while not being toxic like mercury.

Other uses

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  • Indium tin oxide is used as a light filter in low pressure sodium vapor lamps. The infrared radiation is reflected back into the lamp, which increases the temperature within the tube and therefore improves the performance of the lamp.[40]
  • Indium's melting point of 429.7485 K (156.5985 °C) is a defining fixed point on the international temperature scale ITS-90.
  • Indium's high neutron capture cross section for thermal neutrons makes it suitable for use in control rods for nuclear reactors, typically in an alloy containing 80% silver, 15% indium, and 5% cadmium.
  • In nuclear engineering, the (n,n') reactions of 113In and 115In are used to determine magnitudes of neutron fluxes.
  • Indium is also used as a thermal interface material by personal computer enthusiasts in the form of pre-shaped foil sheets fitted between the heat-transfer surface of a microprocessor and its heat sink. The application of heat partially melts the foil and allows the indium metal to fill in any microscopic gaps and pits between the two surfaces, removing any insulating air pockets that would otherwise compromise heat transfer efficiency.
  • 111In emits gamma radiation and is used in indium leukocyte imaging, or indium scintigraphy, a technique of medical imaging. Indium leukocyte scintigraphy has many applications, including early phase drug development, and the monitoring of activity of white blood cells. For the test, blood is taken from the patient, white cells removed, labeled with the radioactive 111In, then re-injected back into the patient. Gamma imaging will then reveal any areas of on-going white cell localization such as new and developing areas of infection.

Precautions and health issues

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Pure indium in metal form is considered non-toxic by most sources. In the welding and semiconductor industries, where indium exposure is relatively high, there have been no reports of any toxic side-effects. Indium compounds, like aluminum compounds, complex with hydroxyls to form insoluble salts in basic conditions, and are thus not well-absorbed from food, giving them fairly low oral toxicty. Soluble indium(III) is toxic when delivered parenterally, however, causing damage primarily to the kidney (both inner and outer parts), but additionally to heart and liver, and may be teratogenic.[46] Other indium compounds are toxic when administered outside the gastrointestinal tract: for example, anhydrous indium trichloride (InCl3) and indium phosphide (InP) are quite toxic when delivered into the lungs (the latter is a suspected carcinogen).[47][48]

See also

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References

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  1. ^ "Standard Atomic Weights: Indium". CIAAW. 2011.
  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. (2022-05-04). "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 Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. ISBN 978-1-62708-155-9.
  4. ^ Mangum, B. W. (1989). "Determination of the Indium Freezing-point and Triple-point Temperatures". Metrologia. 26 (4): 211. Bibcode:1989Metro..26..211M. doi:10.1088/0026-1394/26/4/001.
  5. ^ Guloy, A. M.; Corbett, J. D. (1996). "Synthesis, Structure, and Bonding of Two Lanthanum Indium Germanides with Novel Structures and Properties". Inorganic Chemistry. 35 (9): 2616–22. doi:10.1021/ic951378e. PMID 11666477.
  6. ^ In(−2) has been observed in Na2In, see [1], p. 69.
  7. ^ In(−1) has been observed in NaIn; see Holleman, Arnold F.; Wiberg, Egon; Wiberg, Nils (2008). Lehrbuch der Anorganischen Chemie (in German) (102 ed.). Walter de Gruyter. p. 1185. ISBN 9783110206845.
  8. ^ Unstable In(0) carbonyls and clusters have been detected, see [2], p. 6.
  9. ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 28. ISBN 978-0-08-037941-8.
  10. ^ 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.
  11. ^ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
  12. ^ 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.
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  14. ^ a b Dean, John A. (1999). Lange's handbook of chemistry (Fifteenth edition). McGraw-Hill, Inc. p. 523. ISBN 0070161909. {{cite book}}: |access-date= requires |url= (help)
  15. ^ (in German)Holleman, Arnold F. (1985). "Thallium". Lehrbuch der Anorganischen Chemie (91–100 ed.). Walter de Gruyter. pp. 892–893. ISBN 3110075113. {{cite book}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  16. ^ Handbook of Chemistry and Physics 91st edition, pg 8-20
  17. ^ a b (in Russian)Bleshinsky, S. V.; Abramova, V. F. (1958). Химия индия. Frunze. p. 252. {{cite book}}: |access-date= requires |url= (help)CS1 maint: multiple names: authors list (link) Cite error: The named reference "In" was defined multiple times with different content (see the help page).
  18. ^ (in Russian)Bleshinsky, S. V.; Abramova, V. F. (1958). Химия индия. Frunze. p. 301. {{cite book}}: |access-date= requires |url= (help)CS1 maint: multiple names: authors list (link)
  19. ^ (in French)Fischer, E.O.; Hofmann, H.P. (1957). "Metall-cyclopentadienyle des Indiums". Angew. Chemie. 69: 639. doi:10.1002/ange.19570692008.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  20. ^ Sinclair I., Worrall I.J. Can. J. Chem./Rev. can. chim. 60(6): 695-698 (1982)
  21. ^ H.P. Beck D. Wilhelm Angew. Chem., Int. Ed. Engl., 30 (7) (1991) 824-25
  22. ^ R.Dronskowski, Angew. Chem. Int. Ed. Engl. 34 (1995) 1126.
  23. ^ Sinclair I., Worrall I.J Can. J. Chem./Rev. can. chim. 60(6): 695-698 (1982)
  24. ^ Audi, Georges (2003). "The NUBASE Evaluation of Nuclear and Decay Properties". Nuclear Physics A. 729. Atomic Mass Data Center: 3–128. doi:10.1016/j.nuclphysa.2003.11.001.
  25. ^ A. I. Boothroyd (2006). "Heavy elements in stars". Science. 314 (5806): 1690–1691. doi:10.1126/science.1136842. PMID 17170281.
  26. ^ "Elements, Terrestrial Abundance". www.daviddarling.info. Retrieved 2007-04-14.
  27. ^ Sutherland, J. K. (1971). "A second occurrence of dzhalindite". The Canadian Mineralogist. 10 (5): 781–786.
  28. ^ a b "Mineral Commodities Summary 2007: Indium" (pdf). United States Geological Survey. Retrieved 2007-12-26.
  29. ^ "How Long Will it Last?". New Scientist. 194 (2605): 38–39. May 26, 2007. ISSN 0262-4079.
  30. ^ a b "Indium and Gallium Supply Sustainability September 2007 Update" (pdf). 22nd EU PV Conference, Milan, Italy. Retrieved 2007-12-26.
  31. ^ "Indium Price Supported by LCD Demand and New Uses for the Metal". September 6, 2009.
  32. ^ "Top World Silver Producers" (pdf). World Silver Survey 2007.
  33. ^ Reich, F. (1863). "Ueber das Indium". Journal für Praktische Chemie (in German). 90 (1): 172–176. doi:10.1002/prac.18630900122. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  34. ^ Venetskii, S. (1971). "Indium". Metallurgist. 15 (2): 148–150. doi:10.1007/BF01088126.
  35. ^ Reich, F. (1864). "Ueber das Indium". Journal für Praktische Chemie (in German). 92 (1): 480–485. doi:10.1002/prac.18640920180. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  36. ^ a b Schwarz-Schampera, Ulrich (2002). Indium: Geology, Mineralogy, and Economics. Springer. ISBN 9783540431350. {{cite book}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  37. ^ Wright, Phillip. “Mineral and Metal Commodity Review: Tin.” Natural Resources Canada, 1996.
  38. ^ "Indium Price Supported by LCD Demand and New Uses for the Metal" (pdf). Geology.com. Retrieved 2007-12-26.
  39. ^ Tolcin, Amy C. "Mineral Yearbook 2007: Indium" (pdf). United States Geological Survey. Retrieved 200-02-03. {{cite web}}: Check date values in: |accessdate= (help)
  40. ^ a b Downs, Anthony John (1993). Chemistry of Aluminium, Gallium, Indium, and Thallium. Springer. pp. 89 and 106. ISBN 9780751401035.
  41. ^ Bachmann, K. J. (1981). "Properties, Preparation, and Device Applications of Indium Phosphide". Annual Review of Materials Science. 11: 441–484. doi:10.1146/annurev.ms.11.080181.002301.
  42. ^ Bhuiyan, Ghani (2003). "Indium nitride (InN): A review on growth, characterization, and properties". Journal of Applied Physics. 94: 2779. doi:10.1063/1.1595135. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  43. ^ Powalla, M. (2000). "Scaling up issues of CIGS solar cells". Thin Solid Films. 361–362: 540–546. doi:10.1016/S0040-6090(99)00849-4. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  44. ^ Shenai, Deodatta V. (2004). "Correlation of film properties and reduced impurity concentrations in sources for III/V-MOVPE using high-purity trimethylindium and tertiarybutylphosphine". Journal of Crystal Growth. 272 (1–4): 603–608. doi:10.1016/j.jcrysgro.2004.09.006. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  45. ^ ed. by G. L. Weissler ... (1990). "Vacuum physics and technology". San Diego: Acad. Press: 296. ISBN 9780124759145. {{cite journal}}: |author= has generic name (help); Cite journal requires |journal= (help)
  46. ^ Lenntech (1998). "Indium". {{cite web}}: Missing or empty |url= (help); Unknown parameter |pubisher= ignored (|publisher= suggested) (help)
  47. ^ Tanaka, A. (2002). "Pulmonary toxicity of indium-tin oxide and indium phosphide after intratracheal instillations into the lung of hamsters". Journal of the Occupational Health. 44: 99–102. doi:10.1539/joh.44.99. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)CS1 maint: extra punctuation (link)
  48. ^ Blazka, M. E. (1994). "Pulmonary toxicity to intratracheally administered indium trichloride in Fischer 344 rats". Fundamental Applied Toxicology. 22: 231–239. doi:10.1006/faat.1994.1027. {{cite journal}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
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