GaCl can also be produced by reacting Ga with HCl at 950°C; the product can be condensed as a red solid. [29] :1036

a b c Shiller, A. M.; Bairamadgi, G. R. (August 2006). "Dissolved Gallium in the northwest Pacific and the south and central Atlantic Oceans: Implications for aeolian Fe input and reconsideration of Profiles". Geochemistry, Geophysics, Geosystems. 7 (8): n/a. Bibcode: 2006GGG.....7.8M09S. doi: 10.1029/2005GC001118. S2CID 129738391. a b Kramer, Deborah A. "Mineral Commodity Summary 2006: Gallium" (PDF). United States Geological Survey. Archived (PDF) from the original on 2008-05-14 . Retrieved 2008-11-20. a new phosphor". Physica. 31 (1): 113–121. Bibcode: 1965Phy....31..113K. doi: 10.1016/0031-8914(65)90110-2. The melting point of gallium is used as a temperature reference point. Gallium alloys are used in thermometers as a non-toxic and environmentally friendly alternative to mercury, and can withstand higher temperatures than mercury. An even lower melting point of −19°C (−2°F), well below the freezing point of water, is claimed for the alloy galinstan (62–⁠95% gallium, 5–⁠22% indium, and 0–⁠16% tin by weight), but that may be the freezing point with the effect of supercooling.

First Ionization Energy of Gallium

They also produce less noise than silicon devices, especially at high operating frequencies, making them useful in radars and radio communication devices, satellites and LEDs, Wafer World says. SUBSTITUTES? a b c Shiller, A. M. (June 1998). "Dissolved Gallium in the Atlantic Ocean". Marine Chemistry. 61 (1): 87–99. Bibcode: 1998MarCh..61...87S. doi: 10.1016/S0304-4203(98)00009-7.

has 3 possible crystal modifications. [34] :104 It can be made by the reaction of gallium with hydrogen sulfide ( H Greber, J. F. (2012) "Gallium and Gallium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, doi: 10.1002/14356007.a12_163. Font, O; Querol, Xavier; Juan, Roberto; Casado, Raquel; Ruiz, Carmen R.; López-Soler, Ángel; Coca, Pilar; Peña, Francisco García (2007). "Recovery of gallium and vanadium from gasification fly ash". Journal of Hazardous Materials. 139 (3): 413–23. doi: 10.1016/j.jhazmat.2006.02.041. PMID 16600480.Gallium is found primarily in the +3 oxidation state. The +1 oxidation state is also found in some compounds, although it is less common than it is for gallium's heavier congeners indium and thallium. For example, the very stable GaCl 2 contains both gallium(I) and gallium(III) and can be formulated as Ga IGa IIICl 4; in contrast, the monochloride is unstable above 0°C, disproportionating into elemental gallium and gallium(III) chloride. Compounds containing Ga–Ga bonds are true gallium(II) compounds, such as GaS (which can be formulated as Ga 2 4+(S 2−) 2) and the dioxan complex Ga 2Cl 4(C 4H 8O 2) 2. [28] Aqueous chemistry [ edit ] Gallium resembles silver or aluminium. The element is also a very unique metal. Although solid at room temperature, the metal is soft enough to cut apart. Its melting point is so low that it often melts in a person's hand. Once it turns into liquid metal, gallium's colour is silvery white. Its boiling point is very high at 2,204 C (3,999 F). At very low temperatures, gallium shatters like glass.

Gallium is a chemical element; it has symbol Ga and atomic number 31. Discovered by the French chemist Paul-Émile Lecoq de Boisbaudran in 1875, [7] gallium is in group 13 of the periodic table and is similar to the other metals of the group ( aluminium, indium, and thallium). Germanium is key to fibre optic cables and also used in high-speed computer chips and plastics as well as infrared radiation. He named the element "gallia", from Latin Gallia meaning Gaul, after his native land of France. It was later claimed that, in a multilingual pun of a kind favoured by men of science in the 19th century, he had also named gallium after himself: Le coq is French for "the rooster", and the Latin word for "rooster" is gallus. In an 1877 article, Lecoq denied this conjecture. [46]

a b c d e f g h Downs, Anthony John (1993). Chemistry of aluminium, gallium, indium, and thallium. Springer. ISBN 978-0-7514-0103-5. Arora, Amit (2005). Text Book Of Inorganic Chemistry. Discovery Publishing House. pp.389–399. ISBN 978-81-8356-013-9. Besides its applications in the medical field, gallium is mostly used in electronics. Roughly 95% is used to create gallium arsenide (GaAs). The latter is an essential component in circuits, semiconductors and LEDs. Gallium is also used to make alloys with low melting points. Due to its liquid properties, it is also a safer choice than liquid mercury to be used inside thermometers and barometers. Production