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T h i s i s a n o l d r e v i s i o n o f t h i s p a g e , a s e d i t e d b y V 1 a d i s 1 a v ( t a l k | c o n t r i b s ) at 2 1 : 3 1 , 1 5 J u l y 2 0 2 3 . T h e p r e s e n t a d d r e s s ( U R L ) i s a p e r m a n e n t l i n k t o t h i s r e v i s i o n , w h i c h m a y d i f f e r s i g n i f i c a n t l y f r o m t h e c u r r e n t r e v i s i o n .
( d i f f ) ← P r e v i o u s r e v i s i o n | L a t e s t r e v i s i o n ( d i f f ) | N e w e r r e v i s i o n → ( d i f f )
Silicon tetrafluoride or tetrafluorosilane is a chemical compound with the formula Si F 4 . This colorless gas is notable for having a narrow liquid range: its boiling point is only 4 °C above its melting point. It was first prepared in 1771 by Carl Wilhelm Scheele by dissolving silica in hydrofluoric acid ., later synthesized by John Davy in 1812.[5] It is a tetrahedral molecule and is corrosive.[6]
Preparation
SiF4 is a by-product of the production of phosphate fertilizers wet process production , resulting from the attack of HF (derived from fluorapatite protonolysis) on silicates , which are present as impurities in the phosphate rocks .[7] The hydrofluoric acid and silicon dioxide (SiO2 ) react to produce hexafluorosilicic acid :[7]
6 HF + SiO2 → H2 SiF6 + 2 H2 O
In the laboratory, the compound is prepared by heating barium hexafluorosilicate (Ba[SiF6 ]) above 300 °C (572 °F) whereupon the solid releases volatile SiF4 , leaving a residue of BaF2 .
Ba[SiF6 ] + 400°C → BaF2 + SiF4
Alternatively, sodium hexafluorosilicate (Na 2 [SiF6 ] ) may also be thermally decomposed at 400 °C (752 °F)—600 °C (1,112 °F) (optionally in inert nitrogen gas atmosphere) [8] : 8
Na 2 [SiF6 ] + 400°C → 2NaF + SiF4
Uses
This volatile compound finds limited use in microelectronics and organic synthesis .[9]
It's also used in production of fluorosilicic acid (see above).[6]
Staying in the 1980s, as part of the Low-Cost Solar Array Project by Jet Propulsion Laboratory ,[10] it was investigated as a potentially cheap feedstock for polycrystalline silicon production in fluidized bed reactors .[11] Few methods using it for the said production process were patented.[8] [12]
The Ethyl Corporation process
In 80s the Ethyl Corporation came up with a process that uses hexafluorosilicic acid and sodium aluminium hydride (NaAlH4 ) (or other alkali metal hydride) to produce silane (SiH4 ).[13]
Occurrence
Volcanic plumes contain significant amounts of silicon tetrafluoride. Production can reach several tonnes per day.[14] Some amounts are also emitted from spontaneous coal fires.[15] The silicon tetrafluoride is partly hydrolysed and forms hexafluorosilicic acid .
Safety
In 2001 it was listed by New Jersey authorities as a hazardous substance that is corrosive and may severely irritate or even burn skin and eyes.[6] It is fatal if inhaled.[2]
See also
References
^ "Fluorides (as F)" . Immediately Dangerous to Life or Health Concentrations (IDLH) . National Institute for Occupational Safety and Health (NIOSH).
^ 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 .
^ a b c "Hazardous Substance Fact Sheet" (PDF) . New Jersey Department of Health and Senior services. November 2001.
^ a b Hoffman, C. J.; Gutowsky, H. S. (1953). Silicon Tetrafluoride . Inorganic Syntheses. Vol. 4. pp. 147–8. doi :10.1002/9780470132357.ch48 .
^ a b Us Granted A345458 , Keith, C. Hansen & L. Yaws, Carl, "Patent Silicon tetrafluoride generation", published January 3, 1982, issued 1982
^ Shimizu, M. "Silicon(IV ) Fluoride" Encyclopedia of Reagents for Organic Synthesis, 2001 John Wiley & Sons. doi :10.1002/047084289X.rs011
^ Callaghan, William T. (1981). Palz, W. (ed.). "Low-Cost Solar Array Project Progress and Plans" . Photovoltaic Solar Energy Conference . Dordrecht: Springer Netherlands: 279–286. doi :10.1007/978-94-009-8423-3_40 . ISBN 978-94-009-8423-3 .
^ Acharya, H. N.; Datta, S. K.; Banerjee, H. D.; Basu, S. (1982-09-01). "Low-temperature preparation of polycrystalline silicon from silicon tetrachloride" . Materials Letters . 1 (2 ): 64–66. doi :10.1016/0167-577X(82 )90008-8 . ISSN 0167-577X .
^ CA 2741023A1 , Anatoli, V. Pushko & Tozzoli, Silvio, "Method for the production of polycrystalline silicon", issued 2008
^ "The Ethyl Corporation Process: Silane and Fluidised Bed Reactor" . August 11, 2015.
^ 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" (PDF) . Earth Planets Space . 54 (3 ): 249–256. Bibcode :2002EP&S...54..249M . doi :10.1186/BF03353024 . S2CID 55173591 .
^ Kruszewski, Ł., Fabiańska, M.J., Ciesielczuk, J., Segit, T., Orłowski, R., Motyliński, R., Moszumańska, I., Kusy, D. 2018 – First multi-tool exploration of a gas-condensate-pyrolysate system from the environment of burning coal mine heaps: An in situ FTIR and laboratory GC and PXRD study based on Upper Silesian materials. Science of the Total Environment, 640-641, 1044-1071; DOI: 10.1016/j.scitotenv.2018.05.319
t
e
Si(II )
Si(III)
Si(IV )
t
e
PF 6 − , AsF6 − , SbF6 − compounds
AlF6 − compounds
chlorides, bromides, iodides and pseudohalogenides
SiF6 2- , GeF6 2- compounds
Oxyfluorides
Organofluorides
with transition metal, lanthanide, actinide, ammonium
nitric acids
bifluorides
thionyl, phosphoryl, and iodosyl
Chemical formulas
R e t r i e v e d f r o m " https://en.wikipedia.org/w/index.php?title=Silicon_tetrafluoride&oldid=1165545840 "
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● T h i s p a g e w a s l a s t e d i t e d o n 1 5 J u l y 2 0 2 3 , a t 2 1 : 3 1 ( U T C ) .
● T h i s v e r s i o n o f t h e p a g e h a s b e e n r e v i s e d . B e s i d e s n o r m a l e d i t i n g , t h e r e a s o n f o r r e v i s i o n m a y h a v e b e e n t h a t t h i s v e r s i o n c o n t a i n s f a c t u a l i n a c c u r a c i e s , v a n d a l i s m , o r m a t e r i a l n o t c o m p a t i b l e w i t h t h e C r e a t i v e C o m m o n s A t t r i b u t i o n - S h a r e A l i k e L i c e n s e .
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