Gallium: the essentials
Gallium is the only metal, except for mercury, caesium, and rubidium, which can be liquid near room temperatures; this makes possible its use in high-temperature thermometers. It has one of the longest liquid ranges of any metal and has a low vapour pressure even at high temperatures.
Ultra-pure gallium has a beautiful, silvery appearance, and the solid metal exhibits a conchoidal fracture similar to glass. The metal expands on solidifying; therefore, it should not be stored in glass or metal containers, as they may break as the metal solidifies.
High-purity gallium is attacked only slowly by mineral acids. Gallium arsenide is capable of converting electricity directly into coherent light and gallium arsenide is a key component of LEDs (light emitting diodes). In the 1990s gallium nitride (GaN) was discovered to emit blue light in light-emitting diodes (LEDs). As red and green LEDs were already known, this meant that red green, and blue LEDS could be used in full-colour LED displays while white LEDs and blue laser devices became possible as well.
Image adapted with permission from Prof James Marshall's (U. North Texas, USA) Walking Tour of the elements CD.
Gallium: historical information
Gallium was an element whose existence was predicted by Mendeleev in 1871. He predicted that the then unknown element gallium should resemble aluminium in its properties. He suggested therefore the name ekaaluminium (symbol Ea). His predictions for the properties of gallium are remarkably close to the reality. Gallium was discovered spectroscopically by Paul-Emile Lecoq de Boisbaudran in 1875, who in the same year obtained the free metal by electrolysis of a solution of the hydroxide Ga(OH)3 in KOH.
Gallium around us Read more »
Gallium apparently has no biological role but is said to stimulate the metabolism. Gallium compounds appear not to be particularly toxic.
Gallium is not found as the free element in nature. Gallium ores are rare but gallium contaminates some other ores. It is contained in coal and some flue dusts from coal burning contain up to 1.5% gallium.
|Location||ppb by weight||ppb by atoms||Links|
|Human||(no data) ppb by weight||(no data) atoms relative to C = 1000000|
Physical properties Read more »
Heat properties Read more »
- Melting point: 302.91 [29.76 °C (85.57 °F)] K
- Boiling point: 2477 [2204 °C (3999 °F)] K
- Enthalpy of fusion: |203| kJ mol-1
Crystal structure Read more »
The solid state structure of gallium is: orthorhombic.
Gallium: orbital properties Read more »
Gallium atoms have 31 electrons and the shell structure is 188.8.131.52. The ground state electronic configuration of neutral Gallium is [Ar].3d10.4s2.4p1 and the term symbol of Gallium is 2P1/2.
- Pauling electronegativity: 1.81 (Pauling units)
- First ionisation energy: 578.8 kJ mol‑1
- Second ionisation energy: 1979.3 kJ mol‑1
Isolation: gallium is normally a byproduct of the manufacture of aluminium. The purification of bauxite by the Bayer process results in concentration of gallium in the alkaline solutions from an aluminium:gallum ratio from 5000 to 300. Electrolysis using a mercury electrode gives a further concentration and further electrolysis using a stainless steel cathode of the resulting sodium gallate affords liquid gallium metal.
Very pure gallium requires a number of further processes ending with zone refining to make very pure gallium metal.
Gallium isotopes Read more »
Gallium has two stable isotopes and both are used in nuclear medicine and physics. Ga-69 is used for production of the radioisotope Ge-68. This isotope is used for so-called Ge-68/Ga-68 generators. The Ga-68 that is created from the decay of Ge-68 is used as a PET isotope. Ga-71 has been used to study the behavior of solar neutrinos and it is also used in NMR studies.
|69Ga||68.925580 (3)||60.108 (9)||3/2||2.01659|
|71Ga||70.9247005 (25)||39.892 (9)||3/2||2.56227|