Silicon tetrafluoride
| Silicon tetrafluoride | |
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Tetrafluorosilane |
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Other names
Silicon fluoride |
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| Identifiers | |
| CAS number | 7783-61-1  |
| PubChem | 24556 |
| UN number | 1859 |
| RTECS number | VW2327000 |
| Jmol-3D images | Image 1 |
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| Properties | |
| Molecular formula | SiF4 |
| Molar mass | 104.0791 g/mol |
| Appearance | colourless gas, fumes in moist air |
| Density | 1.66 g/cm3, solid (−95 °C) 4.69 g/L (gas) |
| Melting point |
−90 °C |
| Boiling point |
−86 °C |
| Solubility in water | decomposes |
| Structure | |
| Molecular shape | tetrahedral |
| Dipole moment | 0 D |
| Hazards | |
| MSDS | ICSC 0576 |
| EU Index | Not listed |
| Main hazards | toxic, corrosive |
| NFPA 704 |
 0
3
2
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| Related compounds | |
| Other anions | Silicon tetrachloride Silicon tetrabromide Silicon tetraiodide |
| Other cations | Carbon tetrafluoride Germanium tetrafluoride Tin tetrafluoride Lead tetrafluoride |
| Related compounds | Hexafluorosilicic acid |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
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| Infobox references | |
Silicon tetrafluoride or Tetrafluorosilane is the chemical compound with the formula SiF4. This tetrahedral molecule is notable for having a remarkably narrow liquid range (its boiling point is only 4 °C above its melting point). It was first synthesized by John Davy in 1812.[1]
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[edit] Preparation
SiF4 is a by-product of the production of phosphate fertilizers, resulting from the attack of HF (derived from fluorapatite protonolysis) on silicates. In the laboratory, the compound is prepared by heating BaSiF6 >300 °C, whereupon the solid releases volatile SiF4, leaving a residue of BaF2. The required BaSiF6 is prepared by treating aqueous hexafluorosilicic acid with barium chloride.[2] The corresponding GeF4 is prepared analogously, except that the thermal "cracking" requires 700 °C.[3]
[edit] Uses
This volatile compound finds limited use in microelectronics and organic synthesis.[4]
[edit] Occurrence
Volcanic plumes contain significant amounts of silicon tetrafluoride, the daily production can reach several tonnes per day.[5] The silicon tetrafluoride is partly hydrolysed and forms hexafluorosilicic acid.
[edit] References
- ^ John Davy (1812). "An Account of Some Experiments on Different Combinations of Fluoric Acid". Philosophical Transactions of the Royal Society of London 102: 352–369. doi:10.1098/rstl.1812.0020. ISSN 0261-0523. JSTOR 107324.
- ^ Hoffman, C. J.; Gutowsky, H. S. “Silicon Tetrafluoride” Inorganic Syntheses McGraw-Hill: New York, Volume 4, pages 145-6, 1953.
- ^ Hoffman, C. J.; Gutowsky, H. S. "Germanium Tetrafluoride” Inorganic Syntheses McGraw-Hill: New York, Volume 4, pages 147-8, 1953.
- ^ Shimizu, M. "Silicon(IV) Fluoride" Encyclopedia of Reagents for Organic Synthesis, 2001 John Wiley & Sons. DOI: 10.1002/047084289X.rs011
- ^ T. Mori, M. Sato, Y. Shimoike, K. Notsu (2002). "High SiF4/HF ratio detected in Satsuma-Iwojima volcano's plume by remote FT-IR observation". Earth Planets Space 54: 249–256. http://www.terrapub.co.jp/journals/EPS/pdf/2002/5403/54030249.pdf.
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