What are the physical and chemical properties uses and electronic configuration of indium
Properties, History and Uses of Indium
Indium can be as a lustrous and silvery metal. This post-transition and ductile material is so malleable and soft that it can easily be scratched with fingernails and even bent into almost any shape. This silver-coloured metal has a tetragonal structure and is available in liquid form at varying temperatures. This makes it quite similar to gallium which belongs to the same group of metals. Both Gallium and Indium have the wet glass ability or the potential of sticking to the surface of the glass they are in contact with. Indium remains stable when it reacts with water and air but dissolves in acids. It transforms into a violet-coloured flame when heated over its basic melting point.
Indium is not found abundantly in nature, and it is worth noting that cultivated areas possess more of this metal than the non-cultivated regions. In nature, this is a rare metal found in the form of trace elements in various other minerals, specifically, lead and zinc. It is through these metals that Indium is obtained typically in the form of a by-product. The estimated availability of Indium in the Earth’s crust is approximately 0.1 ppm or parts per million. It is more abundant than mercury or silver as per reports by the Royal Society of Chemistry. Indium melting point is 156.6°C, which is low for any metal. If heated above this melting point, Indium transforms into an indigo or violet flame. The name of this metal comes from the bright light in indigo colour that it displays in the spectroscope.
Chemical and Physical Properties of Indium
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This image depicts the symbol of Indium.
The chemical and physical properties of Indium are as follows:
Indium melting and boiling point: 156.6°C and 2027°C, respectively.
Indium electron configuration: (Kr) 4d105s26p1
Indium atomic number: 49
Group: 13
Period: 5
Density: 7.31 g cm-3
Relative atomic weight: 114.818
Solid key isotopes: 115In
State at room temperature: Solid
Element categorization: Metal
An atomic symbol used in the periodic table of elements: In
Count of isotopes or atoms of the same element with a varied count of neutrons: 35 with half-lives, 2 occurring naturally and 1 stable.
Most common Indium isotope: In-115
Indium boiling point is 3681°for 2300K. This will probably offer you a clearer understanding of the boiling point of the Indium element.
The History of the Discovery of Indium
The well-known chemists from Germany, namely Hieronymus Theodor Richter and Ferdinand Reich discovered Indium in the year 1863. Both Richter and Reich had long been in the lookout of traces of thallium elements in samples of different zinc deposits and ores. It was only when a bright and brilliant indigo line appeared in the spectrum of a sample that the chemists came to know about the existence and the availability of Indium. The metal has the same natural abundance as silver; however, it can be recovered more conveniently and easily than silver because it typically appears along with iron, copper, zinc and lead ores.
Indium Uses
One of the most prominent uses of this metal is as casting for the bearings in high-speed motors. This is because Indium makes way for the even distribution of the lubricating oils used in these motors. The metal is also ideal for doping germanium in the manufacturing procedure of transistors. Indium is even used for making various other electronic elements like thermistors, photoconductors and rectifiers. You can use it for making mirrors that seem to be more reflective in comparison to silver mirrors but have a long shelf life and do not get tarnished very quickly. Indium works out to be the best metal when used for making low melting alloys. At room temperature, an alloy made with 76% gallium, and 24% indium stays in a liquid state.
Other Uses of Indium are as Follows:
Used in semiconductor firms for the manufacture of diodes.
Used for manufacturing bearings that are moisture-resistant and the ones that improve anti-seizure characteristics.
Utilized in different plating applications.
Indium Uses in Everyday Life
In these present times, Indium seems to be one of the essential elements for the economies of the world. ITO or Indium Tin Oxide is widely used in different manufacturing procedures practised at varied industries and even in the everyday life of individuals. This is one form of the element Indium that serves to be one of the best materials for filling the growing requirements of LCDs or liquid crystal displays along with solar panels, TVs, flat screens and touch screens.
Different properties of this element make it ideal for flat panel displays and LCDs. These include transparency, adhering very strongly to glass, conducting electricity, mechanical and chemical corrosion resistance.
FAQs on Indium Element in Chemistry Properties and Applications
1. What is indium in chemistry?
Indium is a chemical element with the symbol In and atomic number 49. It is a soft, silvery-white post-transition metal located in Group 13 of the periodic table. Key chemical properties include:
- Electronic configuration: [Kr] 4d10 5s2 5p1
- Common oxidation state: +3
- Relatively low melting point: about 156.6 °C
2. What is the atomic number and electronic configuration of indium?
The atomic number of indium is 49, and its electronic configuration is [Kr] 4d10 5s2 5p1. This means:
- It has 49 protons and 49 electrons in a neutral atom.
- The outermost (valence) electrons are in the 5s and 5p orbitals.
- It has three valence electrons, which explains its common +3 oxidation state.
3. What group and period does indium belong to?
Indium belongs to Group 13 and Period 5 of the periodic table. Specifically:
- Group 13 elements are known as the boron group (B, Al, Ga, In, Tl).
- Period 5 means indium has five occupied electron shells.
- It is classified as a p-block element.
4. What are the common oxidation states of indium?
The most common oxidation state of indium is +3, although +1 can also occur in some compounds. In detail:
- +3 oxidation state: Found in compounds like InCl3 and In2O3.
- +1 oxidation state: Found in compounds such as InCl, but it is less stable.
5. What is the chemical formula of indium oxide?
The chemical formula of indium(III) oxide is In2O3. In this compound:
- Indium has an oxidation state of +3.
- Oxygen has an oxidation state of −2.
6. How does indium react with oxygen?
Indium reacts with oxygen on heating to form indium(III) oxide, In2O3. The balanced chemical equation is:
- 4In(s) + 3O2(g) → 2In2O3(s)
7. What is indium tin oxide (ITO)?
Indium tin oxide (ITO) is a transparent conductive material made mainly of In2O3 doped with SnO2. Chemically:
- Indium is primarily in the +3 oxidation state.
- Partial substitution of In3+ with Sn4+ increases electrical conductivity.
- It retains optical transparency while conducting electricity.
8. Is indium a metal, nonmetal, or metalloid?
Indium is a metal, specifically classified as a post-transition metal. Its metallic properties include:
- Good electrical conductivity.
- Malleability and softness.
- Ability to form positive ions such as In3+.
9. How is indium extracted from its ores?
Indium is mainly extracted as a byproduct during the processing of zinc ores, especially sphalerite (ZnS). The general steps include:
- Roasting of zinc sulfide: 2ZnS(s) + 3O2(g) → 2ZnO(s) + 2SO2(g)
- Leaching and purification, where indium impurities are separated.
- Reduction of indium compounds to metallic indium.
10. What are the main uses of indium in chemistry and industry?
The main uses of indium are in semiconductors, alloys, and transparent conductive coatings. Important applications include:
- Production of indium tin oxide (ITO) for touchscreens and displays.
- Manufacture of semiconductor compounds such as InP (indium phosphide) and InAs (indium arsenide).
- Low-melting alloys and solders due to its low melting point.
