Germanium tetrachloride

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Germanium tetrachloride
Germanium tetrachloride - structural formula
Germanium tetrachloride - space-filling model
Names
IUPAC names
Germanium tetrachloride
Tetrachlorogermane
Tetrachloridogermanium
Other names
Germanium(IV) chloride
Germanium chloride
Identifiers
10038-98-9 YesY
ChemSpider 10606631 YesY
Jmol 3D model Interactive image
PubChem 66226
RTECS number LY5220000
Properties
GeCl4
Molar mass 214.40 g/mol
Appearance Colourless liquid
Density 1.879 g/cm3 (20 °C)
1.844 g/cm3 (30 °C) [1]
Melting point −49.5 °C (−57.1 °F; 223.7 K)
Boiling point 86.5 °C (187.7 °F; 359.6 K)
Decomposes
Solubility Soluble in ether, benzene, chloroform, CCl4
Insoluble in HCl, H2SO4
1.464
Structure
tetrahedral
Hazards
Main hazards Reacts slowly with water to form HCl and GeO2, corrosive, lachrymator
Safety data sheet "External MSDS"
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g., phosphorus Special hazard W: Reacts with water in an unusual or dangerous manner. E.g., cesium, sodiumNFPA 704 four-colored diamond
Flash point Non-flammable
Related compounds
Other anions
Germanium tetrafluoride
Germanium tetrabromide
Germanium tetraiodide
Other cations
Carbon tetrachloride
Silicon tetrachloride
Tin(IV) chloride
Lead(IV) chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Germanium tetrachloride is a colourless, fuming liquid with a peculiar, acidic odour. It is used as an intermediate in the production of purified germanium metal. In recent years, GeCl4 usage has increased substantially due to its use as a reagent for fiber optic production.

Production[edit]

Most commercial production of germanium is from treating flue-dusts of zinc- and copper-ore smelters, although a significant source is also found in the ash from the combustion of certain types of coal called vitrain. Germanium tetrachloride is an intermediate for the purification of germanium metal or its oxide, GeO2.[2]

Germanium tetrachloride can be generated directly from GeO2 (Germanium dioxide) by dissolution of the oxide in concentrated hydrochloric acid. The resulting mixture is fractionally distilled to purify and separate the germanium tetrachloride from other products and impurities.[3] The GeCl4 can be rehydrolyzed with deionized water to produce pure GeO2, which is then reduced under hydrogen to produce germanium metal.[2][3]

Production of GeO2, however, is dependent on the oxidized form of germanium extracted from the ore. Copper-lead-sulfide and zinc-sulfide ores will produce GeS2, which is subsequently oxidized to GeO2 with an oxidizer such as sodium chlorate. Zinc-ores are roasted and sintered and can produce the GeO2 directly. The oxide is then processed as discussed above.[2]

Application[edit]

Germanium tetrachloride is used almost exclusively as an intermediate for several optical processes. GeCl4 can be directly hydrolyzed to GeO2, an oxide glass with several unique properties and applications, described below and in linked articles:

Fiber Optics[edit]

A notable derivative of GeCl4 is Germanium dioxide. In Fibre Optic manufacture, silicon tetrachloride, SiCl4 and germanium tetrachloride, GeCl4 are introduced with oxygen into a hollow glass preform, which is carefully heated to allow for oxidation of the reagents to their respective oxides and formation of a glass mixture. The GeO2 has a high index of refraction, so by varying the flowrate of germanium tetrachloride the overall index of refraction of the optical fiber can be specifically controlled. The GeO2 is about 4% by weight of the glass.[2]

References[edit]

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  2. ^ a b c d "Germanium" Mineral Commodity Profile, U.S. Geological Survey, 2005.
  3. ^ a b "The Elements" C. R. Hammond, David R. Lide, ed. CRC Handbook of Chemistry and Physics, Edition 85 (CRC Press, Boca Raton, FL) (2004)

See also[edit]