Antimony pentafluoride: Difference between revisions
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| verifiedrevid = 401805456 |
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|verifiedrevid = 441020860 |
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| ImageFileL1 = Antimony-pentafluoride-2D.png |
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|ImageFileL1 = Antimony-pentafluoride-2D.png |
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| ImageSizeL1 = 120px |
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|ImageNameL1 = Antimony pentafluoride |
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|ImageFileR1 = Antimony-pentafluoride-monomer-3D-balls.png |
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|ImageNameR1 = Antimony pentafluoride |
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| ImageSizeR1 = 120px |
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|IUPACName = Antimony pentafluoride |
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|OtherNames = Antimony(V) fluoride<br>pentafluoridoantimony |
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|SystematicName = Pentafluoro-λ<sup>5</sup>-stibane |
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| OtherNames = antimony pentafluoride<br>pentafluoridoantimony |
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|Section1 = {{Chembox Identifiers |
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|SMILES = F[Sb](F)(F)(F)F |
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| InChI = 1/5FH.Sb.3H/h5*1H;;;;/q;;;;;+3;;;/p-5/r5FH.H3Sb/h5*1H;1H3/q;;;;;+3/p-5 |
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|InChI = 1/5FH.Sb/h5*1H;/q;;;;;+5/p-5/rF5Sb/c1-6(2,3,4)5 |
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| SMILES = [F-].[F-].[F-].[F-].[F-].[SbH3+3] |
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|InChIKey = VBVBHWZYQGJZLR-NMXCDXEPAW |
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|StdInChI = 1S/5FH.Sb/h5*1H;/q;;;;;+5/p-5 |
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|StdInChIKey = VBVBHWZYQGJZLR-UHFFFAOYSA-I |
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| InChIKey1 = QURIHDPNDNCSEV-AACRGIKGAU |
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|StdInChI_Ref = {{stdinchicite|changed|chemspider}} |
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| SMILES1 = [SbH3+3].[F-].[F-].[F-].[F-].[F-] |
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|StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} |
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|CASNo = 7783-70-2 |
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| StdInChI = 1S/5FH.Sb/h5*1H;/q;;;;;+3/p-5 |
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|CASNo_Ref = {{cascite|correct|CAS}} |
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|UNII_Ref = {{fdacite|correct|FDA}} |
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| StdInChIKey = QURIHDPNDNCSEV-UHFFFAOYSA-I |
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|UNII = 6C93R71VRF |
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| CASNo = 7783-70-2 |
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|PubChem = 24557 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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|ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} |
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| PubChem = |
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|ChemSpiderID = 22963 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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|RTECS = CC5800000 |
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| ChemSpiderID = 10617727 |
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|UNNumber = 1732 |
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| RTECS = CC5800000 |
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|EC_number = 232-021-8 |
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| UNNumber = 1732 |
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|DTXSID = DTXSID00893075 |
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}} |
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| Section2 = {{Chembox Properties |
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| Formula = SbF<sub>5</sub> |
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| MolarMass = 216.74 g/mol |
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| Appearance = colorless oily liquid <br> [[hygroscopic]] |
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| Odor = pungent |
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| Density = 2.99 g/cm<sup>3</sup> <ref>{{RubberBible87th}}</ref> |
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| MeltingPtC = 8.3 |
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| BoilingPtC = 149.5 |
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| Solubility = Reacts |
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| SolubleOther = soluble in [[potassium fluoride|KF]], liquid [[sulfur dioxide|SO<sub>2</sub>]] |
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}} |
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| Section7 = {{Chembox Hazards |
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| ExternalMSDS = [http://www.inchem.org/documents/icsc/icsc/eics0220.htm ICSC 0220] |
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| EUClass = Harmful ('''Xn''')<br/>Dangerous for the environment ('''N''') |
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| EUIndex = 051-003-00-9 |
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| NFPA-H = 4 |
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| NFPA-F = 0 |
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| NFPA-R = 1 |
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| NFPA-O = W |
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| RPhrases = {{R20/22}}, {{R51/53}} |
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| SPhrases = {{S2}}, {{S61}} |
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| FlashPt = |
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| PEL = |
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}} |
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| Section8 = {{Chembox Related |
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| OtherCpds = [[Antimony trifluoride]] |
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| OtherAnions = [[Antimony pentachloride]] |
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| OtherCations = [[Phosphorus pentafluoride]]<br/>[[Arsenic pentafluoride]]<br/>[[Bismuth pentafluoride]] |
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}} |
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}} |
}} |
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|Section2 = {{Chembox Properties |
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'''Antimony pentafluoride''' is the [[inorganic compound]] with the formula [[Antimony|Sb]][[Fluorine|F]]<sub>5</sub>. This colourless, viscous liquid is a valuable [[Lewis acid]] and a component of the [[superacid]] [[fluoroantimonic acid]], the strongest known acid. It is notable for its [[Lewis acid]]ity and its ability to react with almost all known compounds.<ref>Olah, G. A.; Prakash, G. K. S.; Wang, Q.; Li, X.-y."Antimony(V) Fluoride" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. DOI: 10.1002/047084289.</ref> |
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|Formula = SbF<sub>5</sub> |
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|MolarMass = 216.74 g/mol |
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|Appearance = colorless oily, viscous liquid <br> [[hygroscopic]] |
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|Odor = pungent, sharp |
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|Density = 2.99 g/cm<sup>3</sup> <ref>{{RubberBible87th}}</ref> |
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|MeltingPtC = 8.3 |
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|BoilingPtC = 149.5 |
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|Solubility = Reacts |
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|SolubleOther = soluble in [[potassium fluoride|KF]], liquid [[sulfur dioxide|SO<sub>2</sub>]] |
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}} |
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|Section3 = {{Chembox Hazards |
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|MainHazards = Extremely toxic, corrosive, hazardous to health. Releases [[hydrofluoric acid]] upon contact with [[water]] and biological tissues. Strong [[oxidizing agent]]. |
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|ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics0220.htm ICSC 0220] |
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|NFPA_ref = <ref>[https://www.worldofchemicals.com/chemicals/chemical-properties/antimony-pentafluoride%20.html World of Chemicals SDS]</ref> |
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|NFPA-H = 4 |
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|NFPA-F = 0 |
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|NFPA-R = 3 |
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|NFPA-S = W+OX |
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|GHSPictograms = {{GHS06}}{{GHS05}}{{GHS07}}{{GHS09}}{{GHS03}}{{GHS08}} |
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|GHSSignalWord = Danger |
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|HPhrases = {{H-phrases|300+310+330|314|411|412}} |
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|PPhrases = {{P-phrases|260|261|264|270|271|273|280|301+312|301+330+331|303+361+353|304+312|304+340|305+351+338|310|312|321|330|363|391|405|501}} |
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|FlashPt = noncombustible |
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|LC50 = 270 mg/m<sup>3</sup> (mouse, inhalation) |
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|LCLo = 15 mg/m<sup>3</sup> (rat, |
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inhalation, 2 hours) |
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|LD50 = 270 mg/kg (mouse, subcutaneous) |
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|REL = TWA 0.5 mg/m<sup>3</sup> (as Sb)<ref name=PGCH>{{PGCH|0036}}</ref> |
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|PEL = TWA 0.5 mg/m<sup>3</sup> (as Sb)<ref name=PGCH/> |
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|IDLH = 50 mg/m<sup>3</sup> |
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}} |
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|Section4 = {{Chembox Related |
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|OtherCompounds = [[Antimony trifluoride]] |
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|OtherAnions = [[Antimony pentachloride]] |
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|OtherCations = [[Phosphorus pentafluoride]]<br/>[[Arsenic pentafluoride]]<br/>[[Bismuth pentafluoride]] |
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}} |
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}} |
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'''Antimony pentafluoride''' is the [[inorganic compound]] with the formula [[Antimony|Sb]][[Fluoride|F]]<sub>5</sub>. This colourless, viscous liquid is a strong [[Lewis acid]] and a component of the [[superacid]] [[fluoroantimonic acid]], formed upon mixing liquid [[hydrogen fluoride|HF]] with liquid SbF<sub>5</sub> in 1:1 ratio. It is notable for its strong Lewis acidity and the ability to react with almost all known compounds.<ref>Olah, G. A.; Prakash, G. K. S.; Wang, Q.; Li, X.-y."Antimony(V) Fluoride" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. {{doi|10.1002/047084289X}}.</ref> |
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==Preparation== |
==Preparation== |
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Antimony pentafluoride is prepared by the reaction of [[antimony pentachloride]] with anhydrous [[hydrogen fluoride]]:<ref name=Ullmann>Sabina C. Grund, Kunibert Hanusch, Hans J. Breunig, Hans Uwe Wolf |
Antimony pentafluoride is prepared by the reaction of [[antimony pentachloride]] with anhydrous [[hydrogen fluoride]]:<ref name=Ullmann>Sabina C. Grund, Kunibert Hanusch, Hans J. Breunig, Hans Uwe Wolf "Antimony and Antimony Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2006, Wiley-VCH, Weinheim {{doi| 10.1002/14356007.a03_055.pub2}}</ref> |
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:SbCl<sub>5</sub> + 5 HF → SbF<sub>5</sub> + 5 HCl |
:SbCl<sub>5</sub> + 5 HF → SbF<sub>5</sub> + 5 HCl |
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It can also be prepared from antimony trifluoride and fluorine.<ref>Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.</ref> |
It can also be prepared from [[antimony trifluoride]] and [[fluorine]].<ref>Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.</ref> |
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==Structure and chemical reactions== |
==Structure and chemical reactions== |
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In the gas phase, SbF<sub>5</sub> adopts a trigonal bipyramidal structure of D<sub>3h</sub> [[symmetry group|point group symmetry]] (see picture). |
In the gas phase, SbF<sub>5</sub> adopts a trigonal bipyramidal structure of D<sub>3h</sub> [[symmetry group|point group symmetry]] (see picture). The material adopts a more complicated structure in the liquid and solid states. The liquid contains polymers wherein each Sb is octahedral, the structure being described with the formula [SbF<sub>4</sub>(μ-F)<sub>2</sub>]<sub>''n''</sub> ((μ-F) denotes the fact that fluoride centres [[bridging ligand|bridge]] two Sb centres). The crystalline material is a tetramer, meaning that it has the formula [SbF<sub>4</sub>(μ-F)]<sub>4</sub>. The Sb-F bonds are 2.02 Å within the eight-membered Sb<sub>4</sub>F<sub>4</sub> ring; the remaining fluoride ligands radiating from the four Sb centers are shorter at 1.82 Å.<ref>Edwards, A. J.; Taylor, P. "Crystal structure of Antimony Pentafluoride" Journal of the Chemical Society, Chemical Communications 1971, pp. 1376-7.{{doi|10.1039/C29710001376}}</ref> The related species [[Phosphorus pentafluoride|PF<sub>5</sub>]] and [[Arsenic pentafluoride|AsF<sub>5</sub>]] are [[monomer]]ic in the solid and liquid states, probably due to the smaller sizes of the central atom, which limits their coordination number. [[Bismuth pentafluoride|BiF<sub>5</sub>]] is a polymer.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref> |
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SbF<sub>5</sub> oxidizes [[oxygen]] in the presence of fluorine:<ref>Shamir, J.; Binenboym, J. "Dioxygenyl Salts" ''Inorganic Syntheses'' 1973, XIV, 109-122. {{ISSN|0073-8077}}</ref> |
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SbF<sub>5</sub> is a strong Lewis acid, exceptionally so toward sources of F<sup>−</sup> to give the very stable anion [SbF<sub>6</sub>]<sup>−</sup>, called hexafluoroantimonate. [SbF<sub>6</sub>]<sup>−</sup> reacts with additional SbF<sub>5</sub> to give [Sb<sub>2</sub>F<sub>11</sub>]<sup>−</sup>: |
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:SbF<sub>5</sub> |
:2 SbF<sub>5</sub> + F<sub>2</sub> + 2 O<sub>2</sub> → 2 [[Dioxygenyl|[O<sub>2</sub>]<sup>+</sup>]][SbF<sub>6</sub>]<sup>−</sup> |
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Antimony pentafluoride by itself, is also a very strong [[oxidizing agent]]. [[Phosphorus]] burns on contact with it. |
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SbF<sub>5</sub> has also been used in the first discovered chemical reaction that produces [[fluorine]] gas from fluoride compounds: |
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In the same way that SbF<sub>5</sub> enhances the [[Brønsted-Lowry acid|Brønsted acidity]] of HF, it enhances the [[oxidation|oxidizing]] power of F<sub>2</sub>. This effect is illustrated by the oxidation of [[oxygen]]:<ref>Shamir, J.; Binenboym, J. "Dioxygenyl Salts" Inorganic Syntheses, 1973, XIV, 109-122. {{ISSN|0073-8077}}</ref> |
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:{{chem2|4 SbF5 + 2 K2MnF6 → 4 KSbF6 + 2 MnF3 + F2}} |
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:2 SbF<sub>5</sub> + F<sub>2</sub> + 2 O<sub>2</sub> → 2 {{chem|[O|2|]|+|[SbF|6|]|-}} |
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The driving force for this reaction is the high affinity of SbF<sub>5</sub> for {{chem2|F-}}, which is the same property that recommends the use of SbF<sub>5</sub> to generate superacids. |
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Antimony pentafluoride has also been used in the first discovered chemical reaction that produces [[fluorine]] gas from fluoride compounds: |
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:4 {{chem|SbF|5}} + 2 {{chem|K|2|MnF|6}} → 4 {{chem|KSbF|6}} + 2 {{chem|MnF|3}} + {{chem|F|2}} |
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===Hexafluoroantimonate=== |
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The driving force for this reaction is the high affinity of SbF<sub>5</sub> for {{chem|F|-}}, which is the same property that recommends the use of SbF<sub>5</sub> to generate superacids. |
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SbF<sub>5</sub> is a strong Lewis acid, exceptionally so toward sources of F<sup>−</sup> to give the very stable anion [SbF<sub>6</sub>]<sup>−</sup>, called hexafluoroantimonate. It is the [[conjugate base]] of the superacid [[fluoroantimonic acid]]. [SbF<sub>6</sub>]<sup>−</sup> is a [[weakly coordinating anion]] akin to [[hexafluorophosphate|PF<sub>6</sub><sup>−</sup>]]. Although it is only weakly basic, [SbF<sub>6</sub>]<sup>−</sup> does react with additional SbF<sub>5</sub> to give a centrosymmetric [[adduct]]: |
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:SbF<sub>5</sub> + [SbF<sub>6</sub>]<sup>−</sup> → [Sb<sub>2</sub>F<sub>11</sub>]<sup>−</sup> |
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The [Sb<sub>2</sub>F<sub>11</sub>]<sup>−</sup> anion is one of the ions found in HF/SbF<sub>5</sub> Mixture. |
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==Safety== |
==Safety== |
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SbF<sub>5</sub> reacts violently with many compounds, often releasing dangerous [[hydrogen fluoride]]. |
SbF<sub>5</sub> reacts violently with water. It reacts with many compounds, often releasing dangerous [[hydrogen fluoride]]. It is highly toxic and corrosive to the skin and eyes. It is a strong oxidizer.<ref name="ipcs">{{cite web | publisher = Commission of the European Communities (CEC) | author = International Programme on Chemical Safety | title = Antimony pentafluoride | access-date = 2010-05-10 | year = 2005 | url = http://www.inchem.org/documents/icsc/icsc/eics0220.htm }}</ref><ref name="ec">{{cite web | url = http://environmentalchemistry.com/yogi/chemicals/cn/Antimony%A0Pentafluoride.html | title = Chemical Database - Antimony Pentafluoride | access-date = 2010-05-10 | author = Barbalace, Kenneth | year = 2006 | publisher = Environmental Chemistry }}</ref> |
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==References== |
==References== |
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==External links== |
==External links== |
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* [http://webbook.nist.gov/cgi/cbook.cgi?ID=C7783702 WebBook page for SbF5] |
* [http://webbook.nist.gov/cgi/cbook.cgi?ID=C7783702 WebBook page for SbF5] |
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*[http://www.npi.gov.au/ |
*[http://www.npi.gov.au/resource/antimony-and-compounds National Pollutant Inventory - Antimony and compounds fact sheet] |
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*[http://www.npi.gov.au/ |
*[http://www.npi.gov.au/resource/fluoride-compounds-sources-emissions National Pollutant Inventory - Fluoride compounds fact sheet] |
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{{Antimony compounds}} |
{{Antimony compounds}} |
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{{fluorides}} |
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{{DEFAULTSORT:Antimony Pentafluoride}} |
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[[Category:Superacids]] |
[[Category:Superacids]] |
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[[Category:Antimony compounds]] |
[[Category:Antimony(V) compounds]] |
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[[Category:Fluorides]] |
[[Category:Fluorides]] |
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[[Category:Metal halides]] |
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[[ar:فلوريد أنتيموان خماسي]] |
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[[cs:Fluorid antimoničný]] |
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[[de:Antimon(V)-fluorid]] |
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[[fr:Pentafluorure d'antimoine]] |
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[[ko:오플루오르안티몬산]] |
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[[it:Pentafluoruro di antimonio]] |
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[[hu:Antimon-pentafluorid]] |
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[[nl:Antimoon(V)fluoride]] |
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[[ja:五フッ化アンチモン]] |
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[[pl:Pentafluorek antymonu]] |
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[[pt:Pentafluoreto de antimônio]] |
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[[fi:Antimonipentafluoridi]] |
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[[zh:五氟化锑]] |