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{{chembox
{{chembox
| Verifiedfields = changed
|Verifiedfields = changed
| Watchedfields = changed
|Watchedfields = changed
| verifiedrevid = 441020860
|verifiedrevid = 441020860
| ImageFileL1 = Antimony-pentafluoride-2D.png
|ImageFileL1 = Antimony-pentafluoride-2D.png
| ImageNameL1 = Antimony pentafluoride
|ImageNameL1 = Antimony pentafluoride
| ImageFileR1 = Antimony-pentafluoride-monomer-3D-balls.png
|ImageFileR1 = Antimony-pentafluoride-monomer-3D-balls.png
| ImageNameR1 = Antimony pentafluoride
|ImageNameR1 = Antimony pentafluoride
| IUPACName = antimony(V) fluoride
|IUPACName = Antimony pentafluoride
| OtherNames = antimony pentafluoride<br>pentafluoridoantimony
|OtherNames = Antimony(V) fluoride<br>pentafluoridoantimony
|SystematicName = Pentafluoro-λ<sup>5</sup>-stibane
|Section1={{Chembox Identifiers
|Section1 = {{Chembox Identifiers
| SMILES = F[Sb](F)(F)(F)F
| InChI = 1/5FH.Sb/h5*1H;/q;;;;;+5/p-5/rF5Sb/c1-6(2,3,4)5
|SMILES = F[Sb](F)(F)(F)F
|InChI = 1/5FH.Sb/h5*1H;/q;;;;;+5/p-5/rF5Sb/c1-6(2,3,4)5
| InChIKey = VBVBHWZYQGJZLR-NMXCDXEPAW
|InChIKey = VBVBHWZYQGJZLR-NMXCDXEPAW
| StdInChI = 1S/5FH.Sb/h5*1H;/q;;;;;+5/p-5
|StdInChI = 1S/5FH.Sb/h5*1H;/q;;;;;+5/p-5
| StdInChIKey = VBVBHWZYQGJZLR-UHFFFAOYSA-I
|StdInChIKey = VBVBHWZYQGJZLR-UHFFFAOYSA-I
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
|StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
|StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| CASNo = 7783-70-2
|CASNo = 7783-70-2
| CASNo_Ref = {{cascite|correct|CAS}}
|CASNo_Ref = {{cascite|correct|CAS}}
| UNII_Ref = {{fdacite|correct|FDA}}
|UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 6C93R71VRF
|UNII = 6C93R71VRF
| PubChem = 24557
|PubChem = 24557
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
|ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| ChemSpiderID = 22963
|ChemSpiderID = 22963
| RTECS = CC5800000
|RTECS = CC5800000
| UNNumber = 1732
|UNNumber = 1732
| EC_number = 232-021-8
|EC_number = 232-021-8
| DTXSID = DTXSID00893075
|DTXSID = DTXSID00893075
⚫
}}
⚫
|Section2={{Chembox Properties
⚫
| Formula = SbF<sub>5</sub>
⚫
| MolarMass = 216.74 g/mol
⚫
| Appearance = colorless oily liquid <br> [[hygroscopic]]
⚫
| Odor = pungent
⚫
| Density = 2.99 g/cm<sup>3</sup> <ref>{{RubberBible87th}}</ref>
⚫
| MeltingPtC = 8.3
⚫
| BoilingPtC = 149.5
⚫
| Solubility = Reacts
⚫
| SolubleOther = soluble in [[potassium fluoride|KF]], liquid [[sulfur dioxide|SO<sub>2</sub>]]
⚫
}}
⚫
|Section7={{Chembox Hazards
⚫
| MainHazards = Releases hydrofluoric acid upon contact with water or biological tissues, oxidizer, corrosive
⚫
| ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics0220.htm ICSC 0220]
⚫
| NFPA_ref = <ref>[https://www.worldofchemicals.com/chemicals/chemical-properties/antimony-pentafluoride%20.html World of Chemicals SDS]</ref>
⚫
| NFPA-H = 4
⚫
| NFPA-F = 0
⚫
| NFPA-R = 2
⚫
| NFPA-S = WOX
⚫
| GHSPictograms = {{GHS05}}{{GHS07}}{{GHS09}}{{GHS03}}
⚫
| GHSSignalWord = Danger
⚫
| HPhrases = {{H-phrases|302|314|332|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 =
⚫
| 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/>
⚫
}}
⚫
|Section8={{Chembox Related
⚫
| OtherCompounds = [[Antimony trifluoride]]
⚫
| OtherAnions = [[Antimony pentachloride]]
⚫
| OtherCations = [[Phosphorus pentafluoride]]<br/>[[Arsenic pentafluoride]]<br/>[[Bismuth pentafluoride]]
⚫
}}
}}
}}
⚫
|Section2 = {{Chembox Properties
⚫
'''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]], formed when mixing liquid HF with liquid SbF<sub>5</sub> in a 2:1 ratio. 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|10.1002/047084289X}}.</ref>
⚫
|Formula = SbF<sub>5</sub>
⚫
|MolarMass = 216.74 g/mol
⚫
|Appearance = colorless oily, viscous liquid <br> [[hygroscopic]]
⚫
|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 [[potassium fluoride|KF]], liquid [[sulfur dioxide|SO<sub>2</sub>]]
⚫
}}
⚫
|Section3 = {{Chembox Hazards
⚫
|MainHazards = Extremely toxic, corrosive, hazardous to health. Releases [[hydrofluoric acid]] upon contact with [[water]] and biological tissues. Strong [[oxidizing agent]].
⚫
|ExternalSDS = [http://www.inchem.org/documents/icsc/icsc/eics0220.htm ICSC 0220]
⚫
|NFPA_ref = <ref>[https://www.worldofchemicals.com/chemicals/chemical-properties/antimony-pentafluoride%20.html World of Chemicals SDS]</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 = [[Antimony trifluoride]]
⚫
|OtherAnions = [[Antimony pentachloride]]
⚫
|OtherCations = [[Phosphorus pentafluoride]]<br/>[[Arsenic pentafluoride]]<br/>[[Bismuth pentafluoride]]
⚫
}}
⚫
}}
⚫
'''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>


==Preparation==
==Preparation==
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>
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>
: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 [[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>


==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> [[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>
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>


In the same way that SbF<sub>5</sub> enhances the [[Brønsted-Lowry acid|Brønsted acidity]] of HF, it augments 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>
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>
: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>
: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>
Antimony pentafluoride has also been used in the first discovered chemical reaction that produces [[fluorine]] gas from fluoride compounds:
Antimony pentafluoride by itself, is also a very strong [[oxidizing agent]]. [[Phosphorus]] burns on contact with it.
:4 {{chem|SbF|5}} + 2 {{chem|K|2|MnF|6}} → 4 {{chem|KSbF|6}} + 2 {{chem|MnF|3}} + {{chem|F|2}}


SbF<sub>5</sub> has also been used in the first discovered chemical reaction that produces [[fluorine]] gas from fluoride compounds:
⚫
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.
:{{chem2|4 SbF5 + 2 K2MnF6 → 4 KSbF6 + 2 MnF3 + F2}}

⚫
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.


===Hexafluoroantimonate===
===Hexafluoroantimonate===
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> is a [[weakly coordinating anion]] akin to [[hexafluorophosphate|PF<sub>6</sub><sup>−</sup>]].
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]]:

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]]:
:SbF<sub>5</sub> + [SbF<sub>6</sub>]<sup>−</sup> → [Sb<sub>2</sub>F<sub>11</sub>]<sup>−</sup>
:SbF<sub>5</sub> + [SbF<sub>6</sub>]<sup>−</sup> → [Sb<sub>2</sub>F<sub>11</sub>]<sup>−</sup>

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.


==Safety==
==Safety==
SbF<sub>5</sub> reacts violently with many compounds, often releasing dangerous [[hydrogen fluoride]]. 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 | 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>
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>


==References==
==References==
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{{Antimony compounds}}
{{Antimony compounds}}
{{fluorides}}
{{fluorine compounds}}

{{DEFAULTSORT:Antimony Pentafluoride}}
[[Category:Superacids]]
[[Category:Superacids]]
[[Category:Antimony(V) compounds]]
[[Category:Antimony(V) compounds]]

Latest revision as of 05:43, 18 February 2024

Antimony pentafluoride
Antimony pentafluoride
Antimony pentafluoride
Antimony pentafluoride
Antimony pentafluoride
Names
IUPAC name
Antimony pentafluoride
Systematic IUPAC name
Pentafluoro-λ5-stibane
Other names
Antimony(V) fluoride
pentafluoridoantimony
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.110 Edit this at Wikidata
EC Number
  • 232-021-8
RTECS number
  • CC5800000
UNII
UN number 1732
  • InChI=1S/5FH.Sb/h5*1H;/q;;;;;+5/p-5 ☒N
    Key: VBVBHWZYQGJZLR-UHFFFAOYSA-I ☒N
  • InChI=1/5FH.Sb/h5*1H;/q;;;;;+5/p-5/rF5Sb/c1-6(2,3,4)5
    Key: VBVBHWZYQGJZLR-NMXCDXEPAW
  • F[Sb](F)(F)(F)F
Properties
SbF5
Molar mass 216.74 g/mol
Appearance colorless oily, viscous liquid
hygroscopic
Odor pungent, sharp
Density 2.99 g/cm3 [1]
Melting point 8.3 °C (46.9 °F; 281.4 K)
Boiling point 149.5 °C (301.1 °F; 422.6 K)
Reacts
Solubility soluble in KF, liquid SO2
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Extremely toxic, corrosive, hazardous to health. Releases hydrofluoric acid upon contact with water and biological tissues. Strong oxidizing agent.
GHS labelling:
GHS06: ToxicGHS05: CorrosiveGHS07: Exclamation markGHS09: Environmental hazardGHS03: OxidizingGHS08: Health hazard
Danger
H300+H310+H330, H314, H411, H412
P260, P261, P264, P270, P271, P273, P280, P301+P312, P301+P330+P331, P303+P361+P353, P304+P312, P304+P340, P305+P351+P338, P310, P312, P321, P330, P363, P391, P405, P501
NFPA 704 (fire diamond)
[3]
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 0: Will not burn. E.g. waterInstability 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g. hydrogen peroxideSpecial hazard W+OX: Reacts with water in an unusual or dangerous manner AND is oxidizer
4
0
3
W
OX
Flash point noncombustible
Lethal dose or concentration (LD, LC):
270 mg/kg (mouse, subcutaneous)
270 mg/m3 (mouse, inhalation)
15 mg/m3 (rat,

inhalation, 2 hours)

NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 0.5 mg/m3 (as Sb)[2]
REL (Recommended)
 TWA 0.5 mg/m3 (as Sb)[2]
IDLH (Immediate danger)
 50 mg/m3
Safety data sheet (SDS) ICSC 0220
Related compounds
Other anions
 Antimony pentachloride
Other cations
 Phosphorus pentafluoride
Arsenic pentafluoride
Bismuth pentafluoride
Related compounds
 Antimony trifluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Antimony pentafluoride is the inorganic compound with the formula SbF5. This colourless, viscous liquid is a strong Lewis acid and a component of the superacid fluoroantimonic acid, formed upon mixing liquid HF with liquid SbF5 in 1:1 ratio. It is notable for its strong Lewis acidity and the ability to react with almost all known compounds.[4]

Preparation

[edit]

Antimony pentafluoride is prepared by the reaction of antimony pentachloride with anhydrous hydrogen fluoride:[5]

SbCl5 + 5 HF → SbF5 + 5 HCl

It can also be prepared from antimony trifluoride and fluorine.[6]

Structure and chemical reactions

[edit]

In the gas phase, SbF5 adopts a trigonal bipyramidal structure of D3h 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 [SbF4(μ-F)2]n ((μ-F) denotes the fact that fluoride centres bridge two Sb centres). The crystalline material is a tetramer, meaning that it has the formula [SbF4(μ-F)]4. The Sb-F bonds are 2.02 Å within the eight-membered Sb4F4 ring; the remaining fluoride ligands radiating from the four Sb centers are shorter at 1.82 Å.[7] The related species PF5 and AsF5 are monomeric in the solid and liquid states, probably due to the smaller sizes of the central atom, which limits their coordination number. BiF5 is a polymer.[8]

SbF5 oxidizes oxygen in the presence of fluorine:[9]

2 SbF5 + F2 + 2 O2 → 2 [O2]+[SbF6]−

Antimony pentafluoride by itself, is also a very strong oxidizing agent. Phosphorus burns on contact with it.

SbF5 has also been used in the first discovered chemical reaction that produces fluorine gas from fluoride compounds:

4 SbF5 + 2 K2MnF6 → 4 KSbF6 + 2 MnF3 + F2

The driving force for this reaction is the high affinity of SbF5 for F−, which is the same property that recommends the use of SbF5 to generate superacids.

Hexafluoroantimonate

[edit]

SbF5 is a strong Lewis acid, exceptionally so toward sources of F− to give the very stable anion [SbF6]−, called hexafluoroantimonate. It is the conjugate base of the superacid fluoroantimonic acid. [SbF6]− is a weakly coordinating anion akin to PF6−. Although it is only weakly basic, [SbF6]− does react with additional SbF5 to give a centrosymmetric adduct:

SbF5 + [SbF6]− → [Sb2F11]−

The [Sb2F11]− anion is one of the ions found in HF/SbF5 Mixture.

Safety

[edit]

SbF5 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.[10][11]

References

[edit]
  1. ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
  2. ^ a b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  3. ^ World of Chemicals SDS
  4. ^ 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.
  5. ^ 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
  6. ^ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 200.
  7. ^ 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
  8. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  9. ^ Shamir, J.; Binenboym, J. "Dioxygenyl Salts" Inorganic Syntheses 1973, XIV, 109-122. ISSN 0073-8077
  10. ^ International Programme on Chemical Safety (2005). "Antimony pentafluoride". Commission of the European Communities (CEC). Retrieved 2010-05-10.
  11. ^ Barbalace, Kenneth (2006). "Chemical Database - Antimony Pentafluoride". Environmental Chemistry. Retrieved 2010-05-10.
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