Silicon tetrachloride or tetrachlorosilane is the inorganic compound with the formula SiCl4. It is a colorless volatileliquid that fumes in air. It is used to produce high purity silicon and silica for commercial applications. It is a part of the chlorosilane family.
Preparation
Silicon tetrachloride is prepared by the chlorination of various silicon compounds such as ferrosilicon, silicon carbide, or mixtures of silicon dioxide and carbon. The ferrosilicon route is most common.[3]
In the laboratory, SiCl4 can be prepared by treating silicon with chlorine at 600 °C (1,112 °F):[1]
Brine can be contaminated with silica when the production of chlorine is a byproduct of a metal refining process from metal chloride ore. In rare occurrences, the silicon dioxide in silica is converted to silicon tetrachloride when the contaminated brine is electrolyzed.[5]
Reactions
Hydrolysis and related reactions
Like other chlorosilanes or silanes, silicon tetrachloride reacts readily with water:
SiCl4 + 2 H2O → SiO2 + 4 HCl
The reaction can be noticed on exposure of the liquid to air, as SiCl4 vapour produces fumes as it reacts with moisture to give a cloud-like aerosol of silica and hydrochloric acid.[6] In contrast, carbon tetrachloride is not readily hydrolyzed.
At higher temperatures homologues of silicon tetrachloride can be prepared by the reaction:
Si + 2 SiCl4 → Si3Cl8
In fact, the chlorination of silicon is accompanied by the formation of hexachlorodisilane Si2Cl6. A series of compounds containing up to six silicon atoms in the chain can be separated from the mixture using fractional distillation.[1]
Silicon tetrachloride is used as an intermediate in the manufacture of polysilicon, a hyper-pure form of silicon,[3] since it has a boiling point convenient for purification by repeated fractional distillation. It is reduced to trichlorosilane (HSiCl3) by hydrogen gas in a hydrogenation reactor, and either directly used in the Siemens process or further reduced to silane (SiH4) and injected into a fluidized bed reactor. Silicon tetrachloride reappears in both these two processes as a by-product and is recycled in the hydrogenation reactor. Vapor phase epitaxy of reducing silicon tetrachloride with hydrogen at approximately 1250 °C was done:
SiCl 4(g) + 2 H 2(g) → Si(s) + 4 HCl(g) at 1250°C[11]
The produced polysilicon is used as wafers in large amounts by the photovoltaic industry for conventional solar cells made of crystalline silicon and also by the semiconductor industry.
Silicon tetrachloride can also be hydrolysed to fumed silica. High purity silicon tetrachloride is used in the manufacture of optical fibres. This grade should be free of hydrogen containing impurities like trichlorosilane. Optical fibres are made using processes like MCVD and OFD where silicon tetrachloride is oxidized to pure silica in the presence of oxygen.
Pollution from the production of silicon tetrachloride has been reported in China associated with the increased demand for photovoltaic cells that has been stimulated by subsidy programs.[12]
^Berzelius, Jac. (1824). "Undersökning af flusspatssyran och dess märkvärdigaste föreningar" [Examination of hydrofluoric acid and its most significant compounds]. Kongliga Vetenskapsakademiens Nya Handlingar [New Proceedings of the Royal Academy of Sciences]. 3rd series (in Swedish). 12: 46–98. From pp. 57-58: "Då silicium upphettas i en ström ab chlor, tänder det sig och brinner, samt om gasen innehöll atm. luft, lemnar det kiseljord i form af ett ullikt skelett. […] Silicium glödgadt i en ström af iodgas, har icke kunnat fås att dermed förbinda sig." (When silicon is heated in a stream of chlorine, it ignites and burns, as well as if the gas contained atmospheric air, it leaves silica in the form of an odd "skeleton". If the silicon was previously oxidized to some extent, then the siliceous earth also remains. Silicon burns in chlorine with equal slowness, whether it has lost its flammability in air or not. The product of the combustion is condensed and forms a liquid, which, when freed from it, should be colorless. This liquid is quite volatile and easy-flowing; it evaporates in the open air, almost instantly, with the emission of a white smoke and with a residue of siliceous earth. It has a pungent smell, somewhat like cyanide; precipitated in water, it quickly floats up, dissolves for the most part, but leaves a little siliceous earth undissolved; if the quantity of water is small, e.g., a drop of each, then the chlorosilicon floats around and the silica becomes undissolved in an exfoliated, semi-transparent state. This liquid is analogous to the compound of other electronegative substances with chlorine. Reacts like acid with litmus paper, so that, by its volatility, the paper reddens quite a distance from the point of contact. It is the second known example of a compound in which silicon is volatile. At the ordinary temperature of the air, potassium does not act on it; but if it is heated in the gas of chlorosilicon, it ignites and burns, with a residue of silicon-bound potassium. Silicon heated in a stream of iodine gas, could not be made to bond with it.)
^White, George Clifford (1986). The handbook of chlorination (2nd ed.). New York: Van Nostrand Reinhold. pp. 33–34. ISBN0-442-29285-6.
^Clugston, M.; Flemming, R. (2000). Advanced Chemistry. Oxford University Press. p. 342. ISBN978-0199146338.
^Ebsworth, E. A. V. In Volatile Silicon Compounds; Taube, H.; Maddock, A. G.; Inorganic Chemistry; Pergamon Press Book: New York, NY, 1963; Vol. 4.
^Morgan, D. V.; Board, K. (1991). An Introduction To Semiconductor Microtechnology (2nd ed.). Chichester, West Sussex, England: John Wiley & Sons. p. 23. ISBN0471924784.
