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{{chembox {{chembox
| Watchedfields = changed |Verifiedfields = changed
|Watchedfields = changed
| verifiedrevid = 401805456
|verifiedrevid = 441020860
| ImageFileL1 = Antimony-pentafluoride-2D.png
|ImageFileL1 = Antimony-pentafluoride-2D.png
| ImageSizeL1 = 120px
| ImageNameL1 = Antimony pentafluoride |ImageNameL1 = Antimony pentafluoride
| ImageFileR1 = Antimony-pentafluoride-monomer-3D-balls.png |ImageFileR1 = Antimony-pentafluoride-monomer-3D-balls.png
|ImageNameR1 = Antimony pentafluoride
| ImageSizeR1 = 120px
| ImageNameR1 = Antimony pentafluoride |IUPACName = Antimony pentafluoride
| IUPACName = antimony(V) fluoride |OtherNames = Antimony(V) fluoride<br>pentafluoridoantimony
|SystematicName = Pentafluoro-λ<sup>5</sup>-stibane
| OtherNames = antimony pentafluoride<br>pentafluoridoantimony
| Section1 = {{Chembox Identifiers |Section1 = {{Chembox Identifiers
|SMILES = F(F)(F)(F)F
| InChI = 1/5FH.Sb.3H/h5*1H;;;;/q;;;;;+3;;;/p-5/r5FH.H3Sb/h5*1H;1H3/q;;;;;+3/p-5
|InChI = 1/5FH.Sb/h5*1H;/q;;;;;+5/p-5/rF5Sb/c1-6(2,3,4)5
| SMILES = .....
| InChIKey = CCIMPPQYTRNALI-RNQIAQHSAI |InChIKey = VBVBHWZYQGJZLR-NMXCDXEPAW
| InChI1 = 1/5FH.Sb/h5*1H;/q;;;;;+3/p-5 |StdInChI = 1S/5FH.Sb/h5*1H;/q;;;;;+5/p-5
|StdInChIKey = VBVBHWZYQGJZLR-UHFFFAOYSA-I
| InChIKey1 = QURIHDPNDNCSEV-AACRGIKGAU
|StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| SMILES1 = .....
| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
|CASNo = 7783-70-2
| StdInChI = 1S/5FH.Sb/h5*1H;/q;;;;;+3/p-5
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |CASNo_Ref = {{cascite|correct|CAS}}
|UNII_Ref = {{fdacite|correct|FDA}}
| StdInChIKey = QURIHDPNDNCSEV-UHFFFAOYSA-I
|UNII = 6C93R71VRF
| CASNo = 7783-70-2
|PubChem = 24557
| CASNo_Ref = {{cascite|correct|CAS}}
|ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| PubChem =
|ChemSpiderID = 22963
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
|RTECS = CC5800000
| ChemSpiderID = 10617727
|UNNumber = 1732
| RTECS = CC5800000
|EC_number = 232-021-8
| UNNumber = 1732
|DTXSID = DTXSID00893075
}}
| Section2 = {{Chembox Properties
| Formula = SbF<sub>5</sub>
| MolarMass = 216.74 g/mol
| Appearance = colorless oily liquid <br> ]
| Odor = pungent
| Density = 2.99 g/cm<sup>3</sup> <ref>{{RubberBible87th}}</ref>
| MeltingPtC = 8.3
| BoilingPtC = 149.5
| Solubility = Reacts
| SolubleOther = soluble in ], liquid ]
}}
| Section7 = {{Chembox Hazards
| ExternalMSDS =
| EUClass = Harmful ('''Xn''')<br/>Dangerous for the environment ('''N''')
| EUIndex = 051-003-00-9
| NFPA-H = 4
| NFPA-F = 0
| NFPA-R = 1
| NFPA-O = W
| RPhrases = {{R20/22}}, {{R51/53}}
| SPhrases = {{S2}}, {{S61}}
| FlashPt =
| PEL =
}}
| Section8 = {{Chembox Related
| OtherCpds = ]
| OtherAnions = ]
| OtherCations = ]<br/>]<br/>]
}}
}} }}
|Section2 = {{Chembox Properties
'''Antimony pentafluoride''' is the ] with the formula ]]<sub>5</sub>. This colourless, viscous liquid is a valuable ] and a component of the ] ], the strongest known acid. It is notable for its ]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>
|Formula = SbF<sub>5</sub>
|MolarMass = 216.74 g/mol
|Appearance = colorless oily, viscous liquid <br> ]
|Odor = pungent, sharp
|Density = 2.99 g/cm<sup>3</sup> <ref>{{RubberBible87th}}</ref>
|MeltingPtC = 8.3
|BoilingPtC = 149.5
|Solubility = Reacts
|SolubleOther = soluble in ], liquid ]
}}
|Section3 = {{Chembox Hazards
|MainHazards = Extremely toxic, corrosive, hazardous to health. Releases ] upon contact with ] and biological tissues. Strong ].
|ExternalSDS =
|NFPA_ref = <ref></ref>
|NFPA-H = 4
|NFPA-F = 0
|NFPA-R = 3
|NFPA-S = W+OX
|GHSPictograms = {{GHS06}}{{GHS05}}{{GHS07}}{{GHS09}}{{GHS03}}{{GHS08}}
|GHSSignalWord = Danger
|HPhrases = {{H-phrases|300+310+330|314|411|412}}
|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}}
|FlashPt = noncombustible
|LC50 = 270 mg/m<sup>3</sup> (mouse, inhalation)
|LCLo = 15 mg/m<sup>3</sup> (rat,
inhalation, 2 hours)
|LD50 = 270 mg/kg (mouse, subcutaneous)
|REL = TWA 0.5 mg/m<sup>3</sup> (as Sb)<ref name=PGCH>{{PGCH|0036}}</ref>
|PEL = TWA 0.5 mg/m<sup>3</sup> (as Sb)<ref name=PGCH/>
|IDLH = 50 mg/m<sup>3</sup>
}}
|Section4 = {{Chembox Related
|OtherCompounds = ]
|OtherAnions = ]
|OtherCations = ]<br/>]<br/>]
}}
}}
'''Antimony pentafluoride''' is the ] with the formula ]]<sub>5</sub>. This colourless, viscous liquid is a strong ] and a component of the ] ], formed upon mixing liquid ] 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>


==Preparation== ==Preparation==
Antimony pentafluoride is prepared by the reaction of ] with anhydrous ]:<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> Antimony pentafluoride is prepared by the reaction of ] with anhydrous ]:<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>
:SbCl<sub>5</sub> + 5 HF → SbF<sub>5</sub> + 5 HCl :SbCl<sub>5</sub> + 5 HF → SbF<sub>5</sub> + 5 HCl
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 ] and ].<ref>Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.</ref>


==Structure and chemical reactions== ==Structure and chemical reactions==
In the gas phase, SbF<sub>5</sub> adopts a trigonal bipyramidal structure of D<sub>3h</sub> ] (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 <sub>''n''</sub> ((μ-F) denotes the fact that fluoride centres ] two Sb centres). The crystalline material is a tetramer, meaning that it has the formula <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 PF<sub>5</sub> and AsF<sub>5</sub> are ]ic in the solid and liquid states, probably due to the smaller sizes of the central atom, which limits their coordination number. 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> In the gas phase, SbF<sub>5</sub> adopts a trigonal bipyramidal structure of D<sub>3h</sub> ] (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 <sub>''n''</sub> ((μ-F) denotes the fact that fluoride centres ] two Sb centres). The crystalline material is a tetramer, meaning that it has the formula <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 ] and ] are ]ic in the solid and liquid states, probably due to the smaller sizes of the central atom, which limits their coordination number. ] is a polymer.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref>


SbF<sub>5</sub> oxidizes ] in the presence of fluorine:<ref>Shamir, J.; Binenboym, J. "Dioxygenyl Salts" ''Inorganic Syntheses'' 1973, XIV, 109-122. {{ISSN|0073-8077}}</ref>
SbF<sub>5</sub> is a strong Lewis acid, exceptionally so toward sources of F<sup>−</sup> to give the very stable anion <sup>−</sup>, called hexafluoroantimonate. <sup>−</sup> reacts with additional SbF<sub>5</sub> to give <sup>−</sup>:
:SbF<sub>5</sub> + <sup>−</sup> → <sup>−</sup> :2 SbF<sub>5</sub> + F<sub>2</sub> + 2 O<sub>2</sub> → 2 <sup>+</sup>]]<sup>−</sup>
Antimony pentafluoride by itself is also a very strong ]. ] burns on contact with it.


SbF<sub>5</sub> has also been used in the first discovered chemical reaction that produces ] gas from fluoride compounds:
In the same way that SbF<sub>5</sub> enhances the ] of HF, it enhances the ] power of F<sub>2</sub>. This effect is illustrated by the oxidation of ]:<ref>Shamir, J.; Binenboym, J. "Dioxygenyl Salts" Inorganic Syntheses, 1973, XIV, 109-122. {{ISSN|0073-8077}}</ref>
:{{chem2|4 SbF5 + 2 K2MnF6 → 4 KSbF6 + 2 MnF3 + F2}}
:2 SbF<sub>5</sub> + F<sub>2</sub> + 2 O<sub>2</sub> → 2 {{chem||+||-}}


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.
Antimony pentafluoride has also been used in the first discovered chemical reaction that produces ] gas from fluoride compounds:
:4 {{chem|SbF|5}} + 2 {{chem|K|2|MnF|6}} → 4 {{chem|KSbF|6}} + 2 {{chem|MnF|3}} + {{chem|F|2}}


===Hexafluoroantimonate===
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.
SbF<sub>5</sub> is a strong Lewis acid, exceptionally so toward sources of F<sup>−</sup> to give the very stable anion <sup>−</sup>, called hexafluoroantimonate. It is the ] of the superacid ]. <sup>−</sup> is a ] akin to ]. Although it is only weakly basic, <sup>−</sup> does react with additional SbF<sub>5</sub> to give a centrosymmetric ]:

:SbF<sub>5</sub> + <sup>−</sup> → <sup>−</sup>

The <sup>−</sup> anion is one of the ions found in HF/SbF<sub>5</sub> Mixture.


==Safety== ==Safety==
SbF<sub>5</sub> reacts violently with many compounds, often releasing dangerous ]. It is corrosive to the skin and eyes.<ref name="ipcs">{{cite web | publisher = Commission of the European Communities (CEC) | author = International Programme on Chemical Safety | title = Antimony pentafluoride | accessdate = 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 | accessdate = 2010-05-10 | author = Barbalace, Kenneth | year = 2006 | publisher = Environmental Chemistry }}</ref> SbF<sub>5</sub> reacts violently with water. It reacts with many compounds, often releasing dangerous ]. 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>


==References== ==References==
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==External links== ==External links==
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{{Antimony compounds}} {{Antimony compounds}}
{{fluorides}}


{{DEFAULTSORT:Antimony Pentafluoride}}
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