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491.780
114.818 u+1, +3
[Kr] 4d10 5s2 5p1InIndium

Indium

Indium is a chemical element with symbol In and atomic number 49. It is a post-transition metallic element that is rare in Earth's crust. The metal is very soft, malleable and easily fusible, with a melting point higher than sodium, but lower than lithium or tin.

Identity

Atomic mass
114.818 u
Category
Post-transition metals
Group
13
Period
5
Block
p
Oxidation States
+1, +3
Phase (25 °C)
Solid
Appearance
silvery lustrous gray

Electronic Structure

Electron configuration
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p1
Short configuration
[Kr] 4d10 5s2 5p1
Electrons per shell
2, 8, 18, 18, 3
Electronegativity (Pauling)
1.78
Electron affinity
37.0 kJ/mol
1st ionization energy
558 kJ/mol
Ionization energies
558 · 1821 · 2704 · 5210 kJ/mol

Physical properties

Melting point
156.6 °C (430 K)
Boiling point
2071.8 °C (2345 K)
Density
7.31 g/cm³
Molar heat capacity
26.7 J/(mol·K)

Chemical behavior of indium

Indium is a metal of group 13 (boron family) that presents the oxidation states +1 and +3, +3 being the most stable and most frequent in its chemistry. Its electronegativity of 1.78 (Pauling scale) confers characteristic metallic properties. Its predominant bond is metallic, with a tendency to form salts with covalent character in compounds of oxidation state +1 or +3. Exceptions: metallic indium produces a characteristic sound when bent (the tin cry effect), and it can maintain ductility at very low temperatures, which makes it useful in cryogenic applications.

Reactivity

  • 4 In + 3 O2 -> 2 In2O3

    Indium reacts with oxygen at high temperatures forming indium(III) oxides, a stable compound used in a variety of industrial applications.

  • 2 In + 3 H2SO4 -> 2 In2(SO4)3 + 3 H2

    Indium reacts with hot concentrated sulfuric acid forming indium sulfate, a water-soluble compound.

Notable compounds

CompoundFormulaUse or importance
Indium tin oxideITOCrucial material for transparent touchscreens; conducts electricity and allows visible light
Indium phosphideInPSemiconductor used in optical communication and high-speed electronics
Indium arsenideInAsHigh-frequency semiconductor; application in photon detectors and communication systems
Indium nitrideInNUltrabroad-bandgap semiconductor; candidate for high-power and optoelectronic applications

Electron shell distribution

Electron shell distribution diagram of Indium.Bohr-style diagram: the nucleus sits at the center and the electrons are arranged on concentric circular orbits, one per energy level.InView in the atom builder

Isotopes

Natural indium is composed of two stable isotopes: indium-113 (¹¹³In, 4.29%) and indium-115 (¹¹⁵In, 95.71%). The isotope 115In is the most abundant. 115In is slightly radioactive with a half-life of approximately 4.41 × 10¹⁴ years (much greater than the age of the universe). Both are considered stable for practical applications. The proportion of these two isotopes is the basis for the identification of indium by mass spectrometry.

Occurrence and production

Indium is a trace element in the Earth's crust, with a concentration of about 0.0005-0.005 ppm. It occurs mainly in zinc minerals, where it is found in minor traces. It is almost always obtained as a byproduct of zinc refining and, to a lesser extent, of lead, tin and copper. The main reserves are in Canada, Australia, China, South Korea and Peru. Indium never appears free in nature: it is always combined with other elements in minerals.

History and origin of the name

Indium was discovered in 1863 by German chemists Ferdinand Reich and Hieronymus Theodor Richter. While they were analysing zinc mineral (sphalerite) in a Hildesheim, Germany mine, they discovered a new element in the spectral fraction: it emitted a vibrant magenta colour, which corresponded to no known element. They baptised it 'indigo', in reference to the colour of its spectrum. It was isolated as pure metal in 1864 by Hieronymus Theodor Richter. Its name derives from the Latin 'indigo', the characteristic colour of the spectrum.

Applications and relevance of indium

Uses of the element

Metallic indium is used mainly in specialised applications: thermal joints and seals for electronic components, electrical contacts at high amplitude, welding for cryogenic applications, and intervention materials for cooling systems. Its softness and ability to adapt to surfaces make it a valuable interface material.

Uses of its compounds

Indium compounds are fundamental in modern technology: indium tin oxide (ITO) is essential for touch screens, flat screens and transparent electrodes; indium phosphide (InP) is used in optical communication and high-speed electronics; indium arsenide (InAs) is key in photon detectors and high-frequency communication systems; and indium nitride (InN) is promising for high-power and optoelectronic applications.

Health, safety and environment

Biological role

Indium is not essential for living things, although the body does not need it. Indium is absorbed through skin, lungs and gastrointestinal system. Its compounds can be irritating and toxic in high doses. Indium can accumulate in tissues and affect metabolism of other trace elements. The toxicity of indium compounds is relatively low compared with other heavy metals, but requires control. Metallic indium is stable and does not easily dissolve in natural biological environment.

Safety

Metallic indium is relatively stable, but inorganic indium compounds are toxic. Exposure to indium dust can cause skin, eye and respiratory irritation. Indium can accumulate in tissues and affect liver and kidney function at high doses. Indium can damage some metals by penetrating their structure, especially aluminium. It should be handled with adequate ventilation, respiratory protection and gloves. Industrial waste must be treated in safety facilities.

Environment

Indium does not degrade in the environment and its accumulation can affect soils and surface waters. Industrial discharges of indium compounds can be dangerous for aquatic life, especially if they accumulate in sediments. Indium in nature is mainly in zinc minerals, and extraction and refining of this rock can release indium compounds into nature. Proper management of mining waste and electronic panel manufacturing is essential to prevent environmental contamination by indium.

Frequently asked questions about Indium

Why is indium still important in the manufacture of screens?

Indium continues to be relevant because it allows the manufacture of conductive transparent coatings used in numerous screens and optoelectronic devices. ITO combines good light transmission with adequate conductivity, which allows integrating electrodes without obscuring the image. Although there are alternatives that seek to reduce indium consumption, replacing it requires maintaining comparable optical, electrical and mechanical properties, in addition to guaranteeing viable large-scale manufacturing. Therefore, it remains an important material in certain display technologies.

What is the difference between indium and indium tin oxide?

Indium is a metallic element, while indium tin oxide is a material composed of oxides of both metals. ITO has a combination of properties that do not correspond to pure indium: it can conduct electricity and, at the same time, be transparent when deposited in appropriate layers. This combination explains its use in screens and optical electrodes. Its final behaviour depends on the proportion of components, coating structure and manufacturing conditions.

Which properties make indium useful in semiconductors?

Indium forms numerous semiconductor compounds, such as indium phosphide (InP), indium arsenide (InAs) and indium nitride (InN). These materials present different electronic and optical properties, which allow selecting the most suitable for each device. Indium phosphide, for example, is important in optical communication components and high-speed electronics. The composition of the semiconductor determines aspects such as carrier mobility, response to light and operating frequencies.

Why does indium emit a sound when bent?

Metallic indium can produce a characteristic sound when it is bent or deformed. This phenomenon is related to the changes it undergoes in its crystalline structure during deformation, when atomic planes move relative to each other. There is a similar effect in tin, although the intensity and the conditions in which it is perceived can vary. The sound is not a sign that the metal is reacting chemically, but a consequence of its mechanical behaviour.

Why is indium used in some electronic cooling systems?

Indium can be used as a thermal interface material between electronic components and heat sinks. Due to its softness, it can adapt to small surface irregularities and reduce air gaps that hinder heat transfer. This favours the passage of heat from the component to the cooling system. Its use is especially interesting in specialised equipment, although the selection depends on operating temperature, contact pressure, material compatibility and reliability requirements.

Why is indium useful for making special joints and seals?

Indium is a soft, malleable metal that can adapt to small surface irregularities with which it comes into contact. This characteristic allows its use in specialised joints and seals, especially when it is necessary to maintain close contact or reduce leaks in certain systems. It can also maintain ductility at very low temperatures, which is useful in some cryogenic applications. The design of these joints depends on pressure, temperature and indium compatibility with adjacent materials.

How does indium tin oxide make transparent touch screens?

Indium tin oxide, known as ITO, combines two especially useful properties: it conducts electricity and allows most visible light to pass through. Applied in very thin layers over glass or plastic, it can act as a transparent electrode in touch screens, flat screens and other electronic devices. Thus, the surface can detect contacts or control pixels without blocking the image. Its composition and thickness must be adjusted to balance optical transparency and electrical conductivity.

Main sources consulted: PubChem, Royal Society of Chemistry, NIST, IUPAC. Last revision: November 2026.