[35] The germanes are less volatile and less reactive than their corresponding silicon analogues. Many germanium reactive intermediates are known: germyl free radicals, germylenes (similar to carbenes), and germynes (similar to carbynes). Regulatory process names 2 IUPAC names 5 Other identifiers 1 . Germanium did not become economically significant until after 1945, when its properties as a semiconductor were recognized as being of value in electronics. [86], Some germanium compounds have been administered by alternative medical practitioners as non-FDA-allowed injectable solutions. [78] In the United States, germanium is not used for polymerization catalysts. [9] Argyrodite proved empirically to be Ag8GeS6. [50] Germanium has been detected in some of the most distant stars[51] and in the atmosphere of Jupiter. Encyclopaedia Britannica's editors oversee subject areas in which they have extensive knowledge, whether from years of experience gained by working on that content or via study for an advanced degree.... 36 Questions from Britannica’s Most Popular Science Quizzes. The pure element was commonly doped with arsenic, gallium or other elements and used as a transistor in thousands of electronic applications. Like silicon, germanium naturally reacts and forms complexes with oxygen in nature. Germanium dioxide, also called germanium oxide, germania, and salt of germanium, is an inorganic compound with the chemical formula GeO2. I'm Germanium 4 I know Germanium 2. 1. Both zinc-process concentrates and ash and flue dusts from coal-burning installations provide commercial sources of germanium. [75], Germanium-on-insulator (GeOI) substrates are seen as a potential replacement for silicon on miniaturized chips. Some complex organic germanium compounds are being investigated as possible pharmaceuticals, though none have yet proven successful. Get exclusive access to content from our 1768 First Edition with your subscription. Although aqueous caustic solutions produce little effect on it, germanium dissolves rapidly in molten sodium hydroxide or potassium hydroxide, thereby forming the respective germanates. The five stable isotopes of germanium occur in the following relative amounts: germanium-70, 20.5 percent; germanium-72, 27.4 percent; germanium-73, 7.8 percent; germanium-74, 36.5 percent; and germanium-76, 7.8 percent. Trace quantities of germanium are found in certain zinc blendes, in sulfidic ores of copper and arsenic, and in coals, the latter possibly a consequence of the concentration of the element by plants of the Carboniferous Period in geologic history. − The ore concentrates are mostly sulfidic; they are converted to the oxides by heating under air in a process known as roasting: Some of the germanium is left in the dust produced, while the rest is converted to germanates, which are then leached (together with zinc) from the cinder by sulfuric acid. [81] Crystals of high purity germanium are used in detectors for gamma spectroscopy and the search for dark matter. Silicon has superior electrical properties, but it requires much greater purity that could not be commercially achieved in the early years of semiconductor electronics. [8][9][17] He also determined an atomic weight of 72.32 by analyzing pure germanium tetrachloride (GeCl4), while Lecoq de Boisbaudran deduced 72.3 by a comparison of the lines in the spark spectrum of the element. [19] The first silicon-germanium alloys were obtained in 1955. 3. How about quantum mechanics? [62][63] In 2007 35% of the demand was met by recycled germanium. [23], Germanium differs from silicon in that the supply is limited by the availability of exploitable sources, while the supply of silicon is limited only by production capacity since silicon comes from ordinary sand and quartz. High-brightness LEDs, used for automobile headlights and to backlight LCD screens, are an important application. [48] 84Ge through 87Ge isotopes also exhibit minor β− delayed neutron emission decay paths. Germanium hydride and germanium tetrahydride are very flammable and even explosive when mixed with air. [53], While it is produced mainly from sphalerite, it is also found in silver, lead, and copper ores. [26] While in crystal form, germanium has a displacement threshold energy of [30] The dioxide, GeO2 can be obtained by roasting germanium disulfide (GeS2), and is a white powder that is only slightly soluble in water but reacts with alkalis to form germanates. Its chemical symbol is Ge.   Atomic number 32, Bis-Carboxyethyl Germanium Sesquioxide, Carboxyethylgermanium Sesquioxide, Ge, Ge-132, Ge- Oxy 132, Germanio, Germanium-132, Germanium Inorganique, Germanium Lactate Citrate, Germanium Sesquioxide, Inorganic Germanium, Numéro Atomique 32, Organic Germanium, Sesquioxyde de Germanium, Spirogermanium. Fun Facts about the name Germanium. + Polygermanes—compounds that are similar to alkanes—with formula GenH2n+2 containing up to five germanium atoms are known. Germanium forms many organometallic compounds. OXY-Germanium 10 g (10,000 mg) [30] Upon melting with alkaline carbonates and sulfur, germanium compounds form salts known as thiogermanates. It is the main commercial source of germanium. [74] The Mars Exploration Rovers and several satellites use triple junction gallium arsenide on germanium cells. 2. Because this new element showed some similarities with the elements arsenic and antimony, its proper place in the periodic table was under consideration, but its similarities with Dmitri Mendeleev's predicted element "ekasilicon" confirmed that place on the periodic table. Germanium selenide is a chemical compound with the formula GeSe. Two oxides of germanium are known: germanium dioxide (GeO2, germania) and germanium monoxide, (GeO). Other metalloids on the periodic table are boron, silicon, arsenic, antimony, tellurium, and polonium, according to the Los Alamos National Laboratory. Germanium is not thought to be an essential element for any living organism. Germanium disulfide refers to the chemical compound with the formula Ge S 2.It is a colourless white crystalline material, which melts at roughly 800 °C. Similar to silicon and aluminium, naturally-occurring germanium compounds tend to be insoluble in water and thus have little oral toxicity. For use in electronic devices, germanium ingots or billets require further purification, which usually is effected by the technique of zone refining. [68] It has a very high refractive index (4.0) and must be coated with anti-reflection agents. This germaniu… [26] The remaining 5% went into such uses as phosphors, metallurgy, and chemotherapy. Au moins 27 radioisotopes ont été synthétisés. [77], Germanium dioxide is also used in catalysts for polymerization in the production of polyethylene terephthalate (PET). [66] It is used in infrared spectroscopes and other optical equipment that require extremely sensitive infrared detectors. 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