Difference between revisions of "Indium" - New World Encyclopedia

Vapor pressure
49	cadmium ← indium → tin
	periodic table
General
Name, Symbol, Number	indium, In, 49
Chemical series	poor metals
Group, Period, Block	13, 5, p
Appearance	silvery lustrous gray ;
Atomic mass	114.818(3) g/mol
Electron configuration	[Kr] 4d10 5s2 5p1
Electrons per shell	2, 8, 18, 18, 3
Physical properties
Phase	solid
Density (near r.t.)	7.31 g/cm³
Liquid density at m.p.	7.02 g/cm³
Melting point	429.75 K; (156.60 °C, 313.88 °F)
Boiling point	2345 K; (2072 °C, 3762 °F)
Heat of fusion	3.281 kJ/mol
Heat of vaporization	231.8 kJ/mol
Heat capacity	(25 °C) 26.74 J/(mol·K)
Atomic properties
Crystal structure	tetragonal
Oxidation states	3; (amphoteric oxide)
Electronegativity	1.78 (Pauling scale)
Ionization energies; (more)	1st: 558.3 kJ/mol
	2nd: 1820.7 kJ/mol
	3rd: 2704 kJ/mol
Atomic radius	155 pm
Atomic radius (calc.)	156 pm
Covalent radius	144 pm
Van der Waals radius	193 pm
Miscellaneous
Magnetic ordering	no data
Electrical resistivity	(20 °C) 83.7 nΩ·m
Thermal conductivity	(300 K) 81.8 W/(m·K)
Thermal expansion	(25 °C) 32.1 µm/(m·K)
Speed of sound (thin rod)	(20 °C) 1215 m/s
Speed of sound (thin rod)	(r.t.) 11 m/s
Mohs hardness	1.2
Brinell hardness	8.83 MPa
CAS registry number	7440-74-6
Notable isotopes

Latest revision as of 16:59, 2 March 2018

Indium (chemical symbol In, atomic number 49) is a rare, soft, malleable and easily fusible metal. It is chemically similar to aluminum and gallium, but it looks more like zinc. Zinc ores are also the primary source of this metal.

The primary application of indium is to make thin, transparent electrodes from indium tin oxide for liquid crystal displays (LCDs). It is also used as a semiconductor dopant, as a plating on metals and glass (for mirrors), as a light filter in sodium vapor lamps, and as a component in low-melting-temperature alloys. Several indium compounds are useful as semiconductors, and the oxide is good for making electroluminescent panels. In addition, indium, antimonide, and arsenide are used in infrared detectors.

Occurrence

Ductile Indium wire

Indium is produced mainly from residues generated during zinc ore processing, but it is also found in iron, lead, and copper ores. The amount of indium consumed is largely a function of worldwide LCD production. 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.

Up until 1924, there was only about one gram of isolated indium on the planet. The Earth is estimated to contain about 0.1 parts per million (ppm) of indium. This means it is about as abundant as silver, but indium is nearly three times more expensive by weight. Canada is a leading producer of indium. Worldwide production is typically over 300 metric tons per year, but demand has risen rapidly with the increased popularity of LCD computer monitors and television sets.

History

Indium was discovered by Ferdinand Reich and Hieronymous Theodor Richter in 1863, when they were testing zinc ores with a spectrograph in search of thallium. The element was named after the indigo line in its atomic spectrum. It is interesting to note that most elements were discovered while searching for other elements. Richter went on to isolate the metal in 1867.

Notable characteristics

In the periodic table, indium lies in group 13 (former group 3A), between gallium and thallium, and in the same group as aluminum. Consequently, its properties resemble those of these three elements. In addition, it is situated in period 5, between cadmium and tin. It is also said to be one of the "poor metals"—elements located between the transition metals and metalloids in the periodic table.

Indium is a very soft, silvery white metal, with a bright luster. As a pure metal, it emits a high-pitched "cry" when bent. This element and gallium are able to “wet” (coat) glass.

Isotopes

One unusual property of indium is that its most common isotope, ¹¹⁵In, is slightly radioactive—it decays very slowly by beta emission to tin. The estimated abundance of ¹¹⁵In is about 95.7%, while that of the stable isotope, ¹¹³In, is 4.3%.

The radioactivity of ¹¹⁵In is not considered hazardous, mainly because its decay rate is nearly 50,000 times slower than that of natural thorium, with a half-life of 4×10¹⁴ years. Also, indium is not a notorious cumulative poison, like its neighbor cadmium, and is relatively rare.

Numerous other radioactive isotopes of indium are known, but most of them are extremely short-lived.

Compounds

Indium antimonide (InSb): This crystalline compound is a narrow-gap semiconductor material. It is used in infrared detectors, including thermal-imaging cameras, infrared homing missile guidance systems, and instruments for infrared astronomy.

Indium arsenide or indium monoarsenide (InAs): It is a semiconductor composed of indium and arsenic. It has the appearance of gray cubic crystals, with a melting point 942 °C. It is used for the construction of infrared detectors (wavelength range of 1-3.8 µm) and diode lasers. Alloyed with gallium arsenide, it forms indium gallium arsenide, which is also used in the semiconductor industry.

Indium nitride (InN): This is a small bandgap semiconductor material that has potential applications in solar cells and high speed electronics. Currently there is research into developing solar cells using nitride-based semiconductors.

Indium phosphide (InP): It is a binary semiconductor, composed of indium and phosphorus. It is used in high-power and high-frequency electronics because of its superior electron velocity, compared with the more common semiconductors silicon and gallium arsenide. It has a direct bandgap, making it useful for optoelectronics devices such as laser diodes.

Applications

The first large-scale application for indium was as a coating for bearings in high-performance aircraft engines during World War II. Later, production gradually increased as new uses were found in fusible alloys, solders, and electronics. In the middle and late 1980s, the development of indium phosphide semiconductors and indium-tin oxide thin films for liquid crystal displays (LCDs) aroused much interest. By 1992, the thin-film application had become the largest end use.

Other uses are as follows:

Indium is used in the manufacture of low-melting-temperature alloys. An alloy consisting of 24 percet indium and 76 percent gallium is liquid at room temperature.
It is also used as a semiconductor dopant.
It can be plated onto metals and evaporated onto glass to form a mirror that is as good as those made with silver, but with higher corrosion resistance.
Several indium compounds—such as indium antimonide, indium arsenide, indium phosphide, and indium nitride—are semiconductors with useful properties.
Indium antimonide and arsenide are used in infrared detectors.
Its oxide is used in making electroluminescent panels.
It is used as a light filter in low-pressure sodium vapor lamps.
Its freezing point of 429.7485 K (156.5985 °C) is a defining fixed point on the international temperature scale.
It is occasionally used as a component of nuclear reactor control rods.
Very small amounts of indium are used in aluminum alloy sacrificial anodes (for salt water applications), to prevent passivation of the aluminum.

Precautions

Pure indium in metallic form is considered nontoxic by most sources. In the welding and semiconductor industries, where exposure to indium and its compounds is relatively high, there have been no reports of any toxic side-effects. Yet, some sources maintain that indium has a low level of toxicity, and its compounds are highly toxic.^[1]

Footnotes

↑ WebElements states that "All indium compounds should be regarded as highly toxic. Indium compounds damage the heart, kidney, and liver, and may be teratogenic." For example, indium trichloride anhydrous (InCl3) is quite toxic, while indium phosphide (InP) is both toxic and a suspected carcinogen.

References
ISBN links support NWE through referral fees

Cotton, F. Albert; and Geoffrey Wilkinson. 1980. Advanced Inorganic Chemistry 4th ed. New York: Wiley. ISBN 0471027758.
Chang, Raymond. 2006. Chemistry 9th ed. New York: McGraw-Hill Science/Engineering/Math. ISBN 0073221031.
Greenwood, N.N. and A. Earnshaw. 1998. Chemistry of the Elements 2nd ed. Oxford, U.K.; Burlington, Massachusetts: Butterworth-Heinemann, Elsevier Science. ISBN 0750633654. Online version available at [1]. Retrieved on October 29, 2006.
Indium Los Alamos National Laboratory. Accessed on October 29, 2006.

External links

All links retrieved March 2, 2018.

Credits

New World Encyclopedia writers and editors rewrote and completed the Wikipedia article in accordance with New World Encyclopedia standards. This article abides by terms of the Creative Commons CC-by-sa 3.0 License (CC-by-sa), which may be used and disseminated with proper attribution. Credit is due under the terms of this license that can reference both the New World Encyclopedia contributors and the selfless volunteer contributors of the Wikimedia Foundation. To cite this article click here for a list of acceptable citing formats.The history of earlier contributions by wikipedians is accessible to researchers here:

The history of this article since it was imported to New World Encyclopedia:

History of "Indium"

Note: Some restrictions may apply to use of individual images which are separately licensed.

[1] WebElements states that "All indium compounds should be regarded as highly toxic. Indium compounds damage the heart, kidney, and liver, and may be teratogenic." For example, indium trichloride anhydrous (InCl3) is quite toxic, while indium phosphide (InP) is both toxic and a suspected carcinogen.

[1]

@@ Line 1: / Line 1: @@
+{{Paid}}{{Images OK}}{{Submitted}}{{Approved}}{{Copyedited}}
 {{Elementbox_header | number=49 | symbol=In | name=indium | left=[[cadmium]] | right=[[tin]] | above=[[gallium|Ga]] | below=[[thallium|Tl]] | color1=#cccccc | color2=black }}
 {{Elementbox_series | [[poor metal]]s }}
@@ Line 43: / Line 44: @@
 {{Elementbox_footer | color1=#cccccc | color2=black }}
-'''Indium''' ([[International Phonetic Alphabet|IPA]]: {{IPA|/ˈɪndiəm/}}) is a [[chemical element]] in the [[periodic table]] that has the symbol '''In''' and [[atomic number]] 49. This rare, soft, malleable and easily fusible [[poor metal]], is chemically similar to [[aluminium]] or [[gallium]] but looks more like [[zinc]] (zinc ores are also the primary source of this metal). Its current primary application is to form transparent electrodes from [[Indium tin oxide]] in [[liquid crystal displays]].  It is also widely used in thin-films to form lubricated layers (during [[World War II]] it was widely used to coat bearings in high-performance [[aircraft]]).
+'''Indium''' (chemical symbol '''In''', [[atomic number]] 49) is a rare, soft, malleable and easily fusible [[metal]]. It is chemically similar to [[aluminum]] and [[gallium]], but it looks more like [[zinc]]. Zinc [[ore]]s are also the primary source of this metal.
+{{toc}}
+The primary application of indium is to make thin, transparent [[electrode]]s from [[indium tin oxide]] for [[liquid crystal display]]s (LCDs). It is also used as a [[semiconductor]] [[dopant]], as a plating on [[metal]]s and [[glass]] (for [[mirror]]s), as a light filter in sodium vapor lamps, and as a component in low-melting-temperature [[alloy]]s. Several indium compounds are useful as semiconductors, and the [[oxide]] is good for making [[electroluminescent]] panels. In addition, indium, antimonide, and arsenide are used in [[infrared]] detectors.
+== Occurrence ==
+[[Image:Indium wire.jpg|thumb|left|Ductile Indium wire]]
+Indium is produced mainly from residues generated during [[zinc]] [[ore]] processing, but it is also found in [[iron]], [[lead]], and [[copper]] ores. The amount of indium consumed is largely a function of worldwide [[liquid crystal display|LCD]] production. Increased manufacturing efficiency and recycling (especially in [[Japan]]) maintain a balance between demand and supply. Demand increased as the metal is used in [[LCD]]s and televisions, and supply decreased when a number of [[China|Chinese]] [[mining]] concerns stopped extracting indium from their zinc tailings.
+Up until 1924, there was only about one [[gram]] of isolated indium on the planet. The Earth is estimated to contain about 0.1 parts per million (ppm) of indium. This means it is about as abundant as [[silver]], but indium is nearly three times more expensive by weight. [[Canada]] is a leading producer of indium. Worldwide production is typically over 300 metric tons per year, but demand has risen rapidly with the increased popularity of LCD [[computer]] monitors and [[television]] sets.
+== History ==
+Indium was discovered by [[Ferdinand Reich]] and [[Hieronymous Theodor Richter]] in 1863, when they were testing [[zinc]] [[ore]]s with a [[spectrograph]] in search of [[thallium]]. The element was named after the [[indigo]] line in its [[atomic spectrum]]. It is interesting to note that most elements were discovered while searching for other elements. Richter went on to isolate the metal in 1867.
 == Notable characteristics ==
-Indium is a very soft, silvery-[[white]] true [[metal]] that has a bright [[Lustre (mineralogy)|luster]]. As a pure metal indium emits a high-pitched "cry" when it is bent. Both [[gallium]] and indium are able to wet [[glass]].
-One unusual property of indium is that its most common [[isotope]] is very slightly radioactive; it very slowly decays by [[beta emission]] to [[tin]] over time. This radioactivity is not considered hazardous, mainly because its decay rate is nearly 50,000 times slower than that of natural [[thorium]], with a half-life of 4{{e|14}} years. Also, indium is not a notorious [[cumulative poison]], like its neighbor [[cadmium]], and is relatively rare.
+In the [[periodic table]], indium lies in group 13 (former group 3A), between [[gallium]] and [[thallium]], and in the same group as [[aluminum]]. Consequently, its properties resemble those of these three elements. In addition, it is situated in period 5, between [[cadmium]] and [[tin]]. It is also said to be one of the "poor metals"&mdash;elements located between the [[transition metal]]s and [[metalloid]]s in the periodic table.
+Indium is a very soft, silvery [[white]] [[metal]], with a bright [[Luster (mineralogy)|luster]]. As a pure metal, it emits a high-pitched "cry" when bent. This element and [[gallium]] are able to “wet” (coat) [[glass]].
+=== Isotopes ===
+One unusual property of indium is that its most common [[isotope]], <sup>115</sup>In, is slightly radioactive&mdash;it decays very slowly by [[beta emission]] to [[tin]]. The estimated abundance of <sup>115</sup>In is about 95.7%, while that of the stable isotope, <sup>113</sup>In, is 4.3%.
+The radioactivity of <sup>115</sup>In is not considered hazardous, mainly because its decay rate is nearly 50,000 times slower than that of natural [[thorium]], with a half-life of 4{{e|14}} years. Also, indium is not a notorious [[cumulative poison]], like its neighbor [[cadmium]], and is relatively rare.
+Numerous other radioactive [[isotope]]s of indium are known, but most of them are extremely short-lived.
+== Compounds ==
+* '''[[Indium antimonide]]''' (InSb): This [[cyrstal|crystalline]] compound is a [[narrow-gap]] [[semiconductor]] material. It is used in [[infrared]] detectors, including [[thermal-imaging]] cameras, [[infrared homing]] [[missile guidance]] systems, and instruments for [[infrared astronomy]].
+* '''Indium arsenide''' or '''indium monoarsenide''' (InAs): It is a [[semiconductor]] composed of indium and [[arsenic]]. It has the appearance of gray cubic [[crystal]]s, with a melting point 942&nbsp;°C. It is used for the construction of [[infrared]] detectors ([[wave|wavelength]] range of 1-3.8&nbsp;µm) and [[diode laser]]s. Alloyed with [[gallium arsenide]], it forms [[indium gallium arsenide]], which is also used in the semiconductor industry.
+* '''Indium nitride''' (InN): This is a [[narrow gap|small bandgap semiconductor]] material that has potential applications in [[solar cell]]s and high speed electronics. Currently there is research into developing solar cells using [[nitride]]-based semiconductors.
+* '''Indium phosphide''' (InP): It is a binary [[semiconductor]], composed of [[indium]] and [[phosphorus]]. It is used in high-power and high-frequency electronics because of its superior [[electron velocity]], compared with the more common semiconductors [[silicon]] and [[gallium arsenide]]. It has a [[direct bandgap]], making it useful for [[optoelectronics]] devices such as [[laser diode]]s.
 == Applications ==
-The first large-scale application for indium was as a coating for [[bearing (mechanical)|bearing]]s in high-performance [[aircraft]] engines during [[World War II]].  Afterwards, production gradually increased as new uses were found in fusible [[alloy]]s, [[solder]]s, and [[electronics]].  In the middle and late [[1980s]], the development of indium phosphide [[semiconductor]]s and indium-[[tin]]-[[oxide]] thin films for [[liquid crystal display]]s (LCD) aroused much interest.  By 1992, the thin-film application had become the largest end use. Other uses;
-*Used in the manufacture of low-melting-temperature [[alloy]]s. An alloy consisting of 24% indium and 76% gallium is [[liquid]] at room temperature.
-*Some indium compounds such as [[indium antimonide]], [[indium phosphide]], and [[indium nitride]] are [[semiconductors]] with useful properties
-*Used as a [[semiconductor]] [[dopant]]
-*Can also be plated onto metals and evaporated onto glass which forms a [[mirror]] which is as good as those made with [[silver]] but has higher [[corrosion]] resistance.
-*Its [[oxide]] is used in the making of [[electroluminescent]] panels.
-*Used as a light filter in [[sodium vapor lamp#Low pressure / LPS / SOX|Low pressure sodium vapor lamp]]s
-*Indium's freezing point of 429.7485 K (156.5985 °C) is a defining fixed point on the international temperature scale [[ITS-90]].
-*Sometimes used as a component of nuclear [[control rod]]s.
-*Very small amounts used in aluminium alloy sacrificial anodes (for salt water applications) to prevent [[passivation]] of the aluminium
-== History ==
+The first large-scale application for indium was as a coating for [[bearing (mechanical)|bearing]]s in high-performance [[aircraft]] engines during [[World War II]]. Later, production gradually increased as new uses were found in fusible [[alloy]]s, [[solder]]s, and [[electronics]]. In the middle and late 1980s, the development of indium phosphide [[semiconductor]]s and indium-[[tin]] [[oxide]] thin films for [[liquid crystal display]]s (LCDs) aroused much interest. By 1992, the thin-film application had become the largest end use.
-Indium (named after the [[indigo]] line in its [[atomic spectrum]]) was discovered by [[Ferdinand Reich]] and [[Hieronymous Theodor Richter]] in [[1863]]  while they were testing [[zinc]] ores with a [[spectrograph]] in search of [[thallium]]. It is interesting to note that most elements were discovered while searching for other elements.  Richter went on to isolate the metal in [[1867]].
-== Occurrence ==
+Other uses are as follows:
-[[Image:Indium wire.jpg|thumb|left|Ductile Indium wire]]
+*Indium is used in the manufacture of low-melting-temperature [[alloy]]s. An alloy consisting of 24 percet indium and 76 percent gallium is [[liquid]] at room temperature.
-Indium is produced mainly from residues generated during [[zinc]] [[ore]] processing but is also found in [[iron]], [[lead]], and [[copper]] ores. The amount of indium consumed is largely a function of worldwide LCD production.  Increased manufacturing efficiency and recycling (especially in [[Japan]]) maintain a balance between demand and supply. The average indium price for 2005 was [[United States dollar|US$]]900 per [[kilogram]].  This is unusually high.  Demand increased as the metal is used in [[LCD]]s and televisions, and supply decreased when a number of [[China|Chinese]] [[mining]] concerns stopped extracting indium from their [[zinc]] tailings.  In 2002, the price was US$94/Kg.
+*It is also used as a [[semiconductor]] [[dopant]].
+*It can be plated onto metals and evaporated onto glass to form a [[mirror]] that is as good as those made with [[silver]], but with higher [[corrosion]] resistance.
+*Several indium compounds&mdash;such as [[indium antimonide]], [[indium arsenide]], [[indium phosphide]], and [[indium nitride]]&mdash;are [[semiconductor]]s with useful properties.
+*Indium antimonide and arsenide are used in [[infrared]] detectors.
+*Its [[oxide]] is used in making [[electroluminescent]] panels.
+*It is used as a light filter in [[sodium vapor lamp#Low pressure / LPS / SOX|low-pressure sodium vapor lamp]]s.
+*Its freezing point of 429.7485 K (156.5985 °C) is a defining fixed point on the international temperature scale.
+*It is occasionally used as a component of nuclear reactor [[control rod]]s.
+*Very small amounts of indium are used in aluminum alloy sacrificial anodes (for salt water applications), to prevent [[passivation]] of the aluminum.
-Up until [[1924]], there was only about a [[gram]] of isolated indium on the planet. The Earth is estimated to contain about 0.1 [[part per million|ppm]] of indium which means it is about as abundant as [[silver]], although indium is in fact nearly three times more expensive by weight. Canada is a leading producer of indium.  The TeckCominco refinery in Trail, BC, is the largest single source, with production of 32,500 kg in 2005, 41,800 kg in 2004 and 36,100 kg in 2003. Worldwide production is typically over 300 tonnes per year, but demand has risen rapidly with the increased popularity of LCD computer monitors and televisions.
+== Precautions ==
-== Precautions ==
+Pure indium in metallic form is considered nontoxic by most sources. In the [[welding]] and [[semiconductor]] industries, where exposure to indium and its compounds is relatively high, there have been no reports of any [[toxin|toxic]] side-effects. Yet, some sources maintain that indium has a low level of toxicity, and its compounds are highly toxic.<ref>[http://www.webelements.com/ WebElements] states that ''"All indium compounds should be regarded as highly toxic. Indium compounds damage the heart, kidney, and liver, and may be [[teratogenic]]."'' For example, [[indium trichloride]] anhydrous (InCl3) is quite toxic, while [[indium phosphide]] (InP) is both toxic and a suspected [[carcinogen]].</ref>
-Pure indium in metal form is considered non-toxic by most sources. This may not be the case with indium compounds: there is some unconfirmed evidence that suggests that indium has a low level of [[toxic]]ity. However, in the [[welding]] and [[semiconductor]] industries, where indium exposure is relatively high, there have been no reports of any toxic side-effects.
-Other sources are more definite about indium compounds' toxicity - for example, the [http://www.webelements.com/ WebElements] website states that ''"All indium compounds should be regarded as highly toxic. Indium compounds damage the heart, kidney, and liver, and may be [[teratogenic]]."'' For example, [[indium trichloride]] anhydrous (InCl3) is quite toxic, while [[indium phosphide]] (InP) is both toxic and a suspected [[carcinogen]].
 ==See also==
-* [[:Category:Indium compounds|Indium compounds]]
+* [[Chemical element]]
+* [[Metal]]
+* [[Periodic table]]
+== Footnotes ==
+<references/>
 ==References==
-*[http://periodic.lanl.gov/elements/49.html Los Alamos National Laboratory &ndash; Indium]
+* Cotton, F. Albert; and Geoffrey Wilkinson. 1980. ''Advanced Inorganic Chemistry'' 4th ed. New York: Wiley. ISBN 0471027758.
+* Chang, Raymond. 2006. ''Chemistry'' 9th ed. New York: McGraw-Hill Science/Engineering/Math. ISBN 0073221031.
+* Greenwood, N.N. and A. Earnshaw. 1998. ''Chemistry of the Elements'' 2nd ed. Oxford, U.K.; Burlington, Massachusetts: Butterworth-Heinemann, Elsevier Science. ISBN 0750633654. Online version available at [http://www.knovel.com/knovel2/Toc.jsp?BookID=402&VerticalID=0]. Retrieved on October 29, 2006.
+* [http://periodic.lanl.gov/elements/49.html Indium] Los Alamos National Laboratory. Accessed on October 29, 2006.
 ==External links==
-{{Commons|Indium}}
+All links retrieved March 2, 2018.
-{{wiktionary|indium}}
 *[http://www.webelements.com/webelements/elements/text/In/index.html WebElements.com &ndash; Indium]
-*[http://www.indium.com The Indium Corporation]
+*[http://www.organic-chemistry.org/chemicals/reductions/indiumlowvalent.shtm Indium low valent]
-*[http://www.organic-chemistry.org/chemicals/reductions/indiumlowvalent.shtm Reducing Agents > Indium low valent]
+[[Category:Physical sciences]]
+[[Category:Chemistry]]
+[[Category:Earth sciences]]
 [[Category:Chemical elements]]
-[[Category:Poor metals]]
-<!-- interwiki —>
-[[ar:إنديوم]]
+{{credit5|Indium|83143316|Indium_arsenide|60695347|Indium_antimonide|75880215|Indium_nitride|60695523|Indium_phosphide|71571922}}
-[[ca:Indi (element)]]
-[[cs:Indium]]
-[[co:Indiu]]
-[[da:Indium]]
-[[de:Indium]]
-[[et:Indium]]
-[[es:Indio (elemento)]]
-[[eo:Indiumo]]
-[[fr:Indium]]
-[[gl:Indio (elemento)]]
-[[ko:인듐]]
-[[hr:Indij]]
-[[io:Indio]]
-[[id:Indium]]
-[[is:Indín]]
-[[it:Indio]]
-[[he:אינדיום]]
-[[ku:Îndiyûm]]
-[[la:Indium]]
-[[lv:Indijs]]
-[[lb:Indium]]
-[[lt:Indis]]
-[[hu:Indium]]
-[[nl:Indium]]
-[[ja:インジウム]]
-[[no:Indium]]
-[[nn:Indium]]
-[[oc:Indi (quimia)]]
-[[ug:ئىندىي]]
-[[pl:Ind]]
-[[pt:Índio (elemento químico)]]
-[[ru:Индий]]
-[[sk:Indium]]
-[[sl:Indij]]
-[[sr:Индијум]]
-[[sh:Indijum]]
-[[fi:Indium]]
-[[sv:Indium]]
-[[th:อินเดียม]]
-[[tr:İndiyum]]
-[[uk:Індій]]
-[[zh:铟]]