Indium (In)
post-transition-metalSolid
Standard Atomic Weight
114.818 uElectron configuration
[Kr] 5s2 4d10 5p1Melting point
156.6 °CBoiling point
2071.85 °CDensity
7310 kg/m³Oxidation states
−5, −2, −1, 0, +1, +2, +3Electronegativity (Pauling)
1.78Ionization energy (1st)
5.786356 eVDiscovery year
1863Atomic radius
155 pmDetails
Indium is a soft, silvery post-transition metal in group 13. It is chemically related to gallium and thallium, but its stable chemistry is dominated by the +3 oxidation state, with +1 compounds also known. The element is rare in Earth's crust and is obtained chiefly as a by-product of zinc refining. Its technological importance is disproportionate to its abundance, especially because transparent conducting indium tin oxide is central to flat-panel displays, touch screens, and other optoelectronic devices.
Indium is available in ultra pure form. Indium is a very soft, silvery-white metal with a brilliant luster. The pure metal gives a high-pitched "cry" when bent. It wets glass, as does gallium.
The name derives from the term "indigo" for the indigo-blue line in the element's spark spectrum. It was discovered in 1863 by the German physicist Ferdinand Reich and the German metallurgist Hieronymus Theodor Richter, while examining zinc blende. They isolated indium in 1867.
Indium was discovered by the German chemists Ferdinand Reich and Hieronymus Theodor Richter in 1863. Reich and Richter had been looking for traces of the element thallium in samples of zinc ores. A brilliant indigo line in the sample's spectrum revealed the existence of indium. Indium is about as abundant as silver but is much easier to recover since it typically occurs along with zinc, iron, lead and copper ores.
From the brilliant indigo line in its spectrum. Discovered by Reich and Richter, who later isolated the metal. Until 1924, a gram or so constituted the world's supply of this element in isolated form. It is probably about as abundant as silver. About 4 million troy ounces of indium are now produced annually in the Free World. Canada is presently producing more than 1,000,000 troy ounces annually.
Pure indium is a very soft, lustrous, silvery-white metal at ordinary conditions. It can be cut with a knife, leaves a mark on paper, and emits a characteristic high-pitched “cry” when bent as its crystals deform. It melts at a relatively low temperature for a metal, about 157 °C.
The largest use of indium is in indium tin oxide, a transparent and electrically conducting oxide coating used on displays, touch panels, solar cells, and low-emissivity glass. Indium metal and indium-rich alloys are used in low-melting solders, fusible alloys, thermal interface materials, and seals that wet glass or ceramics. Indium is also used in compound semiconductors such as indium phosphide and indium gallium arsenide for high-speed electronics, lasers, photodetectors, and some photovoltaic cells.
Indium is used to coat the bearings of high speed motors since it allows for the even distribution of lubricating oil. Indium is used to dope germanium to make transistors. It is also used to make other electrical components such as rectifiers, thermistors and photoconductors. Indium can be used to make mirrors that are as reflective as silver mirrors but do not tarnish as quickly. Indium is also used to make low melting alloys. An alloy of 24% indium and 76% gallium is a liquid at room temperature.
It has found application in making low-melting allows; an allow of 24% indium - 76% gallium is liquid at room temperature. It is used in making bearing alloys, germanium transistors, rectifiers, thermistors, and photoconductors. It can be plated onto metal and evaporated onto glass, forming a mirror as good as that made with silver but with more resistance to atmospheric corrosion.
Isotopes in Medicine
111In (with a half-life of 2.8 days) is used in indium leukocyte imaging (Fig. IUPAC.49.1), in which white blood cells that are abundant at sites of infection are labeled with 111In to help locate the source of the infection [361] M. T. Syrjälä, V. Valtonen, K. Liewendahl, G. Myllylä. J. Nucl. Med.28, 155 (1987)., [362] M. D. Cerqueira, A. F. Jacobson. J. Nucl. Med.30, 703 (1989)., [363] C. Love, C. J. Palestro. J. Nucl. Med.Technol.32, 47 (2004)..
Isotopes Used as a Source of Radioactive Isotope(s)
113In is used to produce 113Sn (with a half-life of 115 days) via the reaction 113In (p, n) 113Sn, and 113In is used to produce the radioisotope 110In (with a half-life of 1.15 h) [364] F. E. Fakhari. Separation and Purification of 111In from Irradiated Cadmium Targets by Solid Phase Extraction (SPE) Method for Medical Applications, Deutsche National Bibliothek (2014), Feb. 26; http://archiv.ub.uni-marburg.de/diss/z2006/0132/view.html., [365] M. Mostafa, A. A. El Sadek, H. El Said, M. A. El Amir. J. Nucl. Radiochem. Sci.10, 1 (2009)..
Indium most often forms In³⁺ compounds, although In⁺ chemistry is significant and can be stabilized in some solids and salts. Indium(III) oxide, In₂O₃, is a wide-band-gap oxide and the main component of indium tin oxide. Indium(III) chloride, InCl₃, is a common Lewis-acidic reagent and precursor. Indium phosphide, InP, and indium arsenide, InAs, are important III-V semiconductors. Indium forms many alloys and intermetallic compounds, and its organometallic chemistry includes precursors used in vapor deposition.
See more information at the Indium compound page.
Bulk indium metal has low acute toxicity, but fine dusts, fumes, and soluble indium compounds require control in industrial settings. Inhalation exposure to indium tin oxide and some indium compounds has been associated with serious lung disease in workers. Many semiconductor compounds containing indium also contain toxic partners such as arsenic or phosphide-forming materials, so hazards are not due to indium alone. Natural indium has no significant radiological hazard.
There is evidence that indium has a low order of toxicity; however, care should be taken until further information is available.
Indium occurs mainly as a trace constituent in sulfide ores, especially zinc ores such as sphalerite, rather than as abundant indium minerals. During weathering and processing it tends to follow chalcophile pathways and can be retained in sulfide-rich residues or industrial wastes. Environmental concentrations are usually very low, and indium has no known biological role. Releases are most relevant near mining, smelting, refining, and electronic-material manufacturing sites.
Indium is not mined as a primary metal in most operations. It is recovered chiefly from residues and intermediate streams produced during zinc smelting and refining, with smaller contributions from other base-metal processing. Supply therefore depends strongly on ore composition, recovery technology, and the economics of host metals. Demand is led by transparent conducting oxides and specialized semiconductors, while solders and alloys account for smaller but useful markets. Recycling occurs from manufacturing scrap and some end-of-life products, but dispersed thin-film uses make complete recovery difficult. Substitution is possible in some applications, yet often involves trade-offs in conductivity, transparency, processing, or reliability.
Indium is most frequently associated with zinc materials, and it is from these that most commercial indium is now obtained; however, it is also found in iron, lead, and copper ores.
Indium is a relatively scarce element in the cosmos. Its stable isotopes are produced by neutron-capture processes in earlier generations of stars, with contributions from both slow and rapid neutron-capture nucleosynthesis. In planetary materials it is strongly chalcophile and is concentrated more readily in sulfide phases than in silicates, helping explain its association with zinc, lead, and tin ores on Earth.
- Natural indium is dominated by ¹¹⁵In, which is very weakly radioactive but has an extremely long half-life.
- Indium metal can form cold-welded seals because it remains soft and malleable at low temperatures.
- The element was named from the indigo-blue spectral line used in its discovery.
- Indium tin oxide is useful because it combines optical transparency with electrical conductivity.
- Indium wets glass better than many common metals, making it useful in special seals.
Images
Properties
Physical
- Atomic radius (empirical)
- 155 pm Compare Atomic radius (empirical) of all elements →
- Covalent radius
- 142 pm Compare Covalent radius of all elements →
- Van der Waals radius
- 193 pm Compare Van der Waals radius of all elements →
- Metallic radius
- 142 pm Compare Metallic radius of all elements →
- Density
- 7310 kg/m³ Compare Density of all elements →
- Molar volume
- 0.0157 L/mol
- Phase at STP
- Solid Compare Phase at STP of all elements →
- Melting point
- 156.6 °C Compare Melting point of all elements →
- Boiling point
- 2071.85 °C Compare Boiling point of all elements →
- Thermal conductivity
- 81.8 W/(m·K) Compare Thermal conductivity of all elements →
- Specific heat capacity
- 0.233 J/(g·K) Compare Specific heat capacity of all elements →
- Molar heat capacity
- 26.74 J/(mol·K) Compare Molar heat capacity of all elements →
- Crystal structure
- Tetragonal Compare Crystal structure of all elements →
Chemical
- Electronegativity (Pauling)
- 1.78 Compare Electronegativity (Pauling) of all elements →
- Electronegativity (Allen)
- 1.656
- Electron affinity
- 0.3 eV
- Ionization energy (1st)
- 5.786356 eV Compare Ionization energy (1st) of all elements →
- Ionization energy (2nd)
- 18.870475 eV Compare Ionization energy (2nd) of all elements →
- Ionization energy (3rd)
- 28.044247 eV Compare Ionization energy (3rd) of all elements →
- Ionization energy (4th)
- 55.450191 eV Compare Ionization energy (4th) of all elements →
- Ionization energy (5th)
- 69.300239 eV Compare Ionization energy (5th) of all elements →
- Oxidation states
- −5, −2, −1, 0, +1, +2, +3 Compare Oxidation states of all elements →
- Valence electrons
- 3 Compare Valence electrons of all elements →
- Electron configuration
- [Kr] 5s2 4d10 5p1
Thermodynamic
- Triple point (temperature)
- 156.5936 °C
- Heat of fusion
- 0.03378764 eV Compare Heat of fusion of all elements →
- Heat of vaporization
- 2.402446 eV Compare Heat of vaporization of all elements →
- Heat of sublimation
- 2.518526 eV
- Heat of atomization
- 2.518526 eV
- Atomization enthalpy
- 2.518526 eV
Nuclear
- Protons
- 49 Compare Protons of all elements →
- Neutrons
- 64 Compare Neutrons of all elements →
- Known isotopes
- 42 Compare Known isotopes of all elements →
- Stable isotopes
- 1 Compare Stable isotopes of all elements →
- Most stable isotope
- In-113
- Discovery year
- 1863
Abundance
- Abundance (Earth's crust)
- 0.25 mg/kg Compare Abundance (Earth's crust) of all elements →
- Abundance (ocean)
- 0.02 mg/L Compare Abundance (ocean) of all elements →
Crystal Structure
- Lattice constant a
- 459 pm
Electronic Structure
- Electrons per shell
- 2, 8, 18, 18, 3 Compare Electrons per shell of all elements →
Identifiers
- CAS number
- 7440-74-6 Compare CAS number of all elements →
- Term symbol
- 2P°1/2
- InChI
- InChI=1S/In
- InChI Key
- APFVFJFRJDLVQX-UHFFFAOYSA-N
Electron Configuration Measured
In: 4d¹⁰ 5s² 5p¹[Kr] 4d¹⁰ 5s² 5p¹1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p¹Atomic model
Isotopes change neutron count, mass, and stability — not the electron configuration of a neutral atom.
Schematic atomic model, not to scale.
Atomic Fingerprint
Emission / Absorption Spectrum
Isotope Distribution
| Mass number | Atomic mass (u) | Natural abundance | Half-life |
|---|---|---|---|
| 113 Stable | 112.90406184 ± 0.00000091 | 4.2900% | Stable |
Phase / State
Reason: 131.6 °C below melting point (156.6 °C)
Schematic, not to scale
Phase transition points
Transition energies
Energy required to melt 1 mol at melting point
Energy required to vaporize 1 mol at boiling point
Energy required to sublime 1 mol at sublimation point
Density
At standard conditions
At standard conditions
Advanced
Atomic Spectra
Showing 10 of 49. Sorted by ion charge (ascending).
Lines Holdings ?
| Ion | Charge | Total lines | Transition probabilities | Level designations |
|---|---|---|---|---|
| In I | 0 | 92 | 27 | 91 |
| In II | +1 | 899 | 528 | 899 |
| In III | +2 | 55 | 0 | 0 |
| In IV | +3 | 42 | 0 | 0 |
| In V | +4 | 38 | 0 | 0 |
Levels Holdings ?
| Ion | Charge | Levels |
|---|---|---|
| In I | 0 | 114 |
| In II | +1 | 195 |
| In III | +2 | 28 |
| In IV | +3 | 18 |
| In V | +4 | 42 |
| In VI | +5 | 2 |
| In VII | +6 | 2 |
| In VIII | +7 | 2 |
| In IX | +8 | 2 |
| In X | +9 | 2 |
Crystal structure data not available
Crystal structure: tetragonal
Ionic Radii
| Charge | Coordination | Spin | Radius |
|---|---|---|---|
| +3 | 4 | N/A | 62 pm |
| +3 | 6 | N/A | 80 pm |
| +3 | 8 | N/A | 92 pm |
Compounds
Isotopes (1)
| Mass number | Atomic mass (u) | Natural abundance | Half-life | Decay mode | |
|---|---|---|---|---|---|
| 113 Stable | 112.90406184 ± 0.00000091 | 4.2900% ± 0.0500% | Stable | stable |
Spectral Lines
Showing 50 of 277. Only spectral lines with measured intensity are shown by default.
| Wavelength (nm) | Intensity | Ion stage | Type | Transition | Accuracy | Source | |
|---|---|---|---|---|---|---|---|
| 383.46308 nm | 32000 | In II | emission | 5s.5d 1D → 5s.4f 1F* | Measured | NIST | |
| 451.12972 nm | 18000 | In I | emission | 5s2.5p 2P* → 5s2.6s 2S | Measured | NIST | |
| 410.17504 nm | 17000 | In I | emission | 5s2.5p 2P* → 5s2.6s 2S | Measured | NIST | |
| 468.1115 nm | 16000 | In II | emission | 5s.5d 3D → 5s.4f 3F* | Measured | NIST | |
| 590.33916 nm | 9000 | In II | emission | 5s.6p 3P* → 5s.6d 3D | Measured | NIST | |
| 463.8162 nm | 8800 | In II | emission | 5s.5d 3D → 5s.4f 3F* | Measured | NIST | |
| 465.562 nm | 7800 | In II | emission | 5s.5d 3D → 5s.4f 3F* | Measured | NIST | |
| 464.4572 nm | 5900 | In II | emission | 5s.5d 3D → 5s.4f 1F* | Measured | NIST | |
| 718.29048 nm | 5800 | In II | emission | 5s.6s 3S → 5s.6p 3P* | Measured | NIST | |
| 384.2918 nm | 5600 | In II | emission | 5s.5d 1D → 5s.4f 3F* | Measured | NIST | |
| 591.87693 nm | 5100 | In II | emission | 5s.6p 1P* → 5s.6d 1D | Measured | NIST | |
| 616.254 nm | 4100 | In II | emission | 5s.4f 1F* → 5s<1/2,F=4>.6g | Measured | NIST | |
| 689.15826 nm | 3900 | In II | emission | 5s.6s 3S → 5s.6p 3P* | Measured | NIST | |
| 585.31709 nm | 3400 | In II | emission | 5s.6p 3P* → 5s.6d 3D | Measured | NIST | |
| 609.59333 nm | 3300 | In II | emission | 5s.6p 3P* → 5s.6d 3D | Measured | NIST | |
| 468.4791 nm | 2500 | In II | emission | 5s.5d 3D → 5s.4f 3F* | Measured | NIST | |
| 727.66388 nm | 2400 | In II | emission | 5s.6s 3S → 5s.6p 3P* | Measured | NIST | |
| 614.953 nm | 2200 | In II | emission | 5s.4f 3F* → 5s<1/2,F=4>.6g | Measured | NIST | |
| 613.986 nm | 2100 | In II | emission | 5s.4f 3F* → 5s<1/2,F=5>.6g | Measured | NIST | |
| 614.32 nm | 2100 | In II | emission | 5s.4f 3F* → 5s<1/2,F=4>.6g | Measured | NIST | |
| 614.813 nm | 2100 | In II | emission | 5s.4f 3F* → 5s<1/2,F=5>.6g | Measured | NIST | |
| 616.113 nm | 2000 | In II | emission | 5s.4f 1F* → 5s<1/2,F=5>.6g | Measured | NIST | |
| 465.6736 nm | 1700 | In II | emission | 5s.5d 3D → 5s.4f 3F* | Measured | NIST | |
| 551.3006 nm | 1500 | In II | emission | 5p2 3P → 5s.4f 1F* | Measured | NIST | |
| 614.126 nm | 1500 | In II | emission | 5s.4f 3F* → 5s<1/2,F=4>.6g | Measured | NIST | |
| 405.69377 nm | 1300 | In II | emission | 5s.6p 3P* → 5s.8s 3S | Measured | NIST | |
| 591.52626 nm | 1300 | In II | emission | 5s.6p 3P* → 5s.6d 3D | Measured | NIST | |
| 557.6866 nm | 1200 | In II | emission | 5s.7p 1P* → 5s.10d 1D | Measured | NIST | |
| 551.935 nm | 1100 | In II | emission | 5s.6d 3D → 5s.7f 3F* | Measured | NIST | |
| 549.7486 nm | 1000 | In II | emission | 5s.6d 3D → 5s.7f 3F* | Measured | NIST | |
| 550.7048 nm | 1000 | In II | emission | 5s.6d 3D → 5s.7f 3F* | Measured | NIST | |
| 551.0883 nm | 1000 | In II | emission | 5s.7p 3P* → 5s.10d 3D | Measured | NIST | |
| 512.0847 nm | 960 | In II | emission | 5s.4f 3F* → 5s<1/2,F=5>.7g | Measured | NIST | |
| 390.20794 nm | 910 | In II | emission | 5s.6p 1P* → 5s.7d 1D | Measured | NIST | |
| 384.2158 nm | 900 | In II | emission | 5s.5d 1D → 5s.4f 3F* | Measured | NIST | |
| 512.1781 nm | 880 | In II | emission | 5s.4f 3F* → 5s<1/2,F=4>.7g | Measured | NIST | |
| 611.58707 nm | 830 | In II | emission | 5s.6p 3P* → 5s.6d 3D | Measured | NIST | |
| 511.7388 nm | 810 | In II | emission | 5s.4f 3F* → 5s<1/2,F=4>.7g | Measured | NIST | |
| 511.5109 nm | 800 | In II | emission | 5s.4f 3F* → 5s<1/2,F=5>.7g | Measured | NIST | |
| 512.9865 nm | 710 | In II | emission | 5s.4f 1F* → 5s<1/2,F=5>.7g | Measured | NIST | |
| 463.7055 nm | 610 | In II | emission | 5s.5d 3D → 5s.4f 3F* | Measured | NIST | |
| 511.6041 nm | 590 | In II | emission | 5s.4f 3F* → 5s<1/2,F=4>.7g | Measured | NIST | |
| 550.7779 nm | 570 | In II | emission | 5s.6d 3D → 5s.7f 3F* | Measured | NIST | |
| 414.9635 nm | 550 | In II | emission | 5s.4f 1F* → 5s<1/2,F=5>.10g | Measured | NIST | |
| 530.94926 nm | 550 | In II | emission | 5s.6p 3P* → 5s.6d 1D | Measured | NIST | |
| 454.8998 nm | 540 | In II | emission | 5p2 1D → 5s.8p 3P* | Measured | NIST | |
| 461.6069 nm | 540 | In II | emission | 5s.4f 3F* → 5s<1/2,F=4>.8g | Measured | NIST | |
| 457.0881 nm | 520 | In II | emission | 5s.6d 3D → 5s.9f 3F* | Measured | NIST | |
| 458.701 nm | 520 | In II | emission | 5s.6d 3D → 5s.9f 3F* | Measured | NIST | |
| 457.1286 nm | 510 | In II | emission | 5s.6d 3D → 5s.9f 3F* | Measured | NIST |
Extended Properties
Covalent Radii (Extended)
- Covalent radius (Pyykkö)
- 142 pm
- Covalent radius (Pyykkö, double)
- 136 pm
- Covalent radius (Pyykkö, triple)
- 146 pm
Van der Waals Radii
- Bondi
- 193 pm
- Batsanov
- 220 pm
- Alvarez
- 243 pm
- UFF
- 446.3 pm
- MM3
- 264 pm
- Dreiding
- 459 pm
Atomic & Metallic Radii
- Atomic radius (Rahm)
- 246 pm
- Metallic radius (C12)
- 158 pm
Numbering Scales
- Mendeleev
- 84
- Pettifor
- 79
- Glawe
- 80
Electronegativity Scales
- Ghosh
- 0
- Miedema
- 4
- Gunnarsson–Lundqvist
- 3
- Robles–Bartolotti
- 2
Polarizability & Dispersion
- Dipole polarizability
- 65 a.u.
- Dipole polarizability (unc.)
- 4 a.u.
- C₆
- 779 Ha·Bohr6
- C₆ (Gould–Bučko)
- 643 Ha·Bohr6
Miedema Parameters
- Miedema molar volume
- 15.75 cm3/mol
- Miedema electron density
- 2
Supply Risk & Economics
- Production concentration
- 53
- Relative supply risk
- 8
- Political stability (top producer)
- 24
Phase Transitions & Allotropes
| Melting point | 429.75 K |
| Boiling point | 2300.15 K |
| Triple point (temperature) | 429.74 K |
Oxidation State Categories
Advanced Reference Data
Screening Constants (11)
| n | Orbital | σ |
|---|---|---|
| 1 | s | 0.9903 |
| 2 | p | 4.102 |
| 2 | s | 12.8764 |
| 3 | d | 14.3218 |
| 3 | p | 17.4793 |
| 3 | s | 17.3692 |
| 4 | d | 32.0584 |
| 4 | p | 28.6312 |
| 4 | s | 27.2388 |
| 5 | p | 40.53 |
Crystal Radii Detail (3)
| Charge | CN | Spin | rcrystal (pm) | Origin |
|---|---|---|---|---|
| 3 | IV | 76 | ||
| 3 | VI | 94 | from r^3 vs V plots, | |
| 3 | VIII | 106 | from r^3 vs V plots, calculated, |
Isotope Decay Modes (69)
| Isotope | Mode | Intensity |
|---|---|---|
| 96 | B+ | — |
| 96 | p | — |
| 97 | B+ | 100% |
| 97 | B+p | 2.3% |
| 97 | p | — |
| 98 | B+ | 100% |
| 98 | B+p | 0.1% |
| 99 | B+ | 100% |
| 99 | B+p | 0.3% |
| 100 | B+ | 100% |
X‑ray Scattering Factors (510)
| Energy (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 2.16244 |
| 10.1617 | — | 2.07002 |
| 10.3261 | — | 1.98155 |
| 10.4931 | — | 1.89686 |
| 10.6628 | — | 1.81579 |
| 10.8353 | — | 1.72844 |
| 11.0106 | — | 1.54985 |
| 11.1886 | — | 1.35731 |
| 11.3696 | — | 0.99325 |
| 11.5535 | — | 0.74202 |
Additional Data
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
2.5×10-1 milligrams per kilogram
References (1)
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
2×10-2 milligrams per liter
References (1)
Sources
Sources of this element.
Indium is most frequently associated with zinc materials, and it is from these that most commercial indium is now obtained; however, it is also found in iron, lead, and copper ores.
References (1)
- [6] Indium https://periodic.lanl.gov/49.shtml
References
(9)
Data deposited in or computed by PubChem
The half-life and atomic mass data was provided by the Atomic Mass Data Center at the International Atomic Energy Agency.
Element data are cited from the Atomic weights of the elements (an IUPAC Technical Report). The IUPAC periodic table of elements can be found at https://iupac.org/what-we-do/periodic-table-of-elements/. Additional information can be found within IUPAC publication doi:10.1515/pac-2015-0703 Copyright © 2020 International Union of Pure and Applied Chemistry.
The information are cited from Pure Appl. Chem. 2018; 90(12): 1833-2092, https://doi.org/10.1515/pac-2015-0703.
Thomas Jefferson National Accelerator Facility (Jefferson Lab) is one of 17 national laboratories funded by the U.S. Department of Energy. The lab's primary mission is to conduct basic research of the atom's nucleus using the lab's unique particle accelerator, known as the Continuous Electron Beam Accelerator Facility (CEBAF). For more information visit https://www.jlab.org/
The periodic table at the LANL (Los Alamos National Laboratory) contains basic element information together with the history, source, properties, use, handling and more. The provenance data may be found from the link under the source name.
The periodic table contains NIST's critically-evaluated data on atomic properties of the elements. The provenance data that include data for atomic spectroscopy, X-ray and gamma ray, radiation dosimetry, nuclear physics, and condensed matter physics may be found from the link under the source name. Ref: https://www.nist.gov/pml/atomic-spectra-database
This section provides all form of data related to element Indium.
The element property data was retrieved from publications.