Chemistry:Silicon tetrachloride
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| Names | |||
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| IUPAC name
Tetrachlorosilane
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| Other names
Silicon tetrachloride
Tetrachlorosilane | |||
| Identifiers | |||
3D model (JSmol)
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PubChem CID
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| UNII | |||
| UN number | 1818 | ||
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| Properties | |||
| SiCl4 | |||
| Molar mass | 169.90 g/mol | ||
| Appearance | Colourless liquid | ||
| Density | 1.483 g/cm3 | ||
| Melting point | −68.74 °C (−91.73 °F; 204.41 K) | ||
| Boiling point | 57.65 °C (135.77 °F; 330.80 K) | ||
| Reacts to form silica | |||
| Solubility | soluble in benzene, toluene, chloroform, ether[1] | ||
| Vapor pressure | 25.9 kPa at 20 °C | ||
| −88.3·10−6 cm3/mol | |||
| Structure | |||
| Tetrahedral | |||
| 4 | |||
| Thermochemistry | |||
Std molar
entropy (S |
240 J·mol−1·K−1[2] | ||
Std enthalpy of
formation (ΔfH⦵298) |
−687 kJ·mol−1[2] | ||
| Hazards | |||
| Safety data sheet | ICSC 0574 MSDS | ||
| GHS pictograms | 
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| GHS Signal word | Warning | ||
| H315, H319, H335 | |||
| P261, P264, P271, P280, P302+352, P304+340, P305+351+338, P312, P321, P332+313, P337+313, P362, P403+233, P405, P501 | |||
| NFPA 704 (fire diamond) | |||
| Related compounds | |||
Other anions
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Silicon tetrafluoride Silicon tetrabromide Silicon tetraiodide | ||
Other cations
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Carbon tetrachloride Germanium tetrachloride Tin(IV) chloride Titanium tetrachloride | ||
Related chlorosilanes
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Chlorosilane Dichlorosilane Trichlorosilane | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |||
 verify (what is   ?)
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| Infobox references | |||
Silicon tetrachloride or tetrachlorosilane is the inorganic compound with the formula SiCl4. It is a colorless volatile liquid 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, SiCl
4 can be prepared by treating silicon with chlorine at 600 °C (1,112 °F):[1]
- Si + 2 Cl
2 → SiCl
4
It was first prepared by Jöns Jakob Berzelius in 1823.[4]
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
Like other chlorosilanes or silanes, silicon tetrachloride reacts readily with water:
- SiCl4 + 2 H2O → SiO2 + 4 HCl
In contrast, carbon tetrachloride does not hydrolyze readily. The reaction can be noticed on exposure of the liquid to air, the vapour produces fumes as it reacts with moisture to give a cloud-like aerosol of hydrochloric acid.[6]
With alcohols it reacts to give orthosilicate esters:
- SiCl4 + 4 ROH → Si(OR)4 + 4 HCl
Polysilicon chlorides
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]
Reactions with other nucleophiles
Silicon tetrachloride is a classic electrophile in its reactivity.[7] It forms a variety of organosilicon compounds upon treatment with Grignard reagents and organolithium compounds:
- 4 RLi + SiCl4 → R4Si + 4 LiCl
Reduction with hydride reagents afford silane.
Comparison with other SiX4 compounds
| SiH4 | SiF4 | SiCl4 | SiBr4 | SiI4 | |
|---|---|---|---|---|---|
| b.p. (˚C)[8] | -111.9 | -90.3 | 56.8 | 155.0 | 290.0 |
| m.p. (˚C)[8] | -185 | -95.0 | -68.8 | 5.0 | 155.0 |
| Si-X bond length (Å) | >0.74 [9] | 1.55 | 2.02 | 2.20 | 2.43 |
| Si-X bond energy (kJ/mol)[10] | 384 | 582 | 391 | 310 | 234 |
Uses
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:
- SiCl4(g) + 2 H2(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.
As a feedstock in production of fused silica.
Safety and environmental issues
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] The MSDS notes that one should "avoid all contact! In all cases consult a doctor! ... inhalation causes sore throat and Burning sensation".[13]
See also
- Silicon tetrachloride (data page)
References
- ↑ 1.0 1.1 1.2 P. W. Schenk (1963). "Phosphorus(V) fluoride". in G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed.. 1. NY, NY: Academic Press. pp. 282–683.
- ↑ 2.0 2.1 Zumdahl, S. S. (2009). Chemical Principles (6th ed.). Houghton Mifflin. p. A22. ISBN 978-0-618-94690-7.
- ↑ 3.0 3.1 Simmler, W.. "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a24_001.
- ↑ Berzelius, Jac. (1824). "Undersökning af flusspatssyran och dess märkvärdigaste föreningar" (in Swedish). Kongliga Vetenskapsakademiens Nya Handlingar [New Proceedings of the Royal Academy of Sciences]. 3rd series 12: 46–98. https://www.biodiversitylibrary.org/item/107454#page/54/mode/1up. 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. ISBN 0-442-29285-6.
- ↑ Clugston, M.; Flemming, R. (2000). Advanced Chemistry. Oxford University Press. p. 342. ISBN 978-0199146338.
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ↑ 8.0 8.1 Silicon Compounds, Silicon Halides. Collins, W.: Kirk-Othmer Encyclopedia of Chemical Technology; John Wiley & Sons, Inc, 2001.
- ↑ "What is the bond length of the H-H bond?". https://www.answers.com/Q/What_is_the_bond_length_of_the_H-H_bond.
- ↑ 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. ISBN 0471924784.
- ↑ "Solar Energy Firms Leave Waste Behind in China". The Washington Post. 9 March 2008. https://www.washingtonpost.com/wp-dyn/content/article/2008/03/08/AR2008030802595.html.
- ↑ "International Chemical Safety Cards Tetrachlorosilane". https://www.inchem.org/documents/icsc/icsc/eics0574.htm.
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