Antimony trifluoride#Applications
{{Chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 477163120
| ImageFile = Antimony trifluoride.jpg
| ImageFileL1 = Antimony-trifluoride-2D.png
| ImageClassL1 = skin-invert-image
| ImageNameL1 = Structural formula
| ImageFileR1 = Antimony-trifluoride-molecule-in-xtal-3D-vdW.png
| ImageNameR1 = space-filling model
| ImageClassR1 = bg-transparent
| ImageFileL2 = Antimony-trifluoride-unit-cell-1970-CM-3D-ellipsoids.png
| ImageClassL2 = bg-transparent
| ImageNameL2 = Unit cell
| ImageFileR2 = Antimon(III)-fluorid.png
| ImageClassR2 = bg-transparent
| ImageNameR2 = Unit cell of antimony trifluoride. The distorted-octahedral coordination of the fluorine relative to the antimony is visualized.
| ImageAltR2 = Unit cell of antimony trifluoride. The distorted-octahedral coordination of the fluorine relative to the antimony is visualized.
| PIN = Antimony(III) fluoride
| SystematicName = Trifluorostibane
| OtherNames = Trifluoroantimony
|Section1={{Chembox Identifiers
| InChI1 = 1/3FH.Sb/h3*1H;/q;;;+3/p-3
| InChIKey1 = GUNJVIDCYZYFGV-DFZHHIFOAW
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo = 7783-56-4
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = VWM00O92AM
| PubChem = 24554
| ChemSpiderID = 22960
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| EINECS = 232-009-2
| UNNumber = UN 2923
| RTECS = CC5150000
| InChI = 1S/3FH.Sb/h3*1H;/q;;;+3/p-3
| InChIKey = GUNJVIDCYZYFGV-UHFFFAOYSA-K
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/3FH.Sb/h3*1H;/q;;;+3/p-3
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = GUNJVIDCYZYFGV-UHFFFAOYSA-K
| SMILES = F[Sb](F)F}}
|Section2={{Chembox Properties
| Formula = SbF3
| MolarMass = 178.76 g/mol
| Appearance = light gray to white crystals
| Odor = pungent
| Density = 4.379 g/cm3
| MeltingPtC = 292
| BoilingPtC = 376
| Solubility = 385 g/100 mL (0 °C)
443 g/100 mL (20 °C)
562 g/100 mL (30 °C)
| SolubleOther = soluble in methanol, acetone
insoluble in ammonia
| MagSus = −46.0·10−6 cm3/mol
}}
|Section3={{Chembox Structure
| CrystalStruct = Orthorhombic, oS16
| SpaceGroup = Ama2, No. 40
}}
|Section7={{Chembox Hazards
| MainHazards =
| FlashPt =
| AutoignitionPt =
| NFPA-H = 3
| NFPA-F = 0
| NFPA-R = 0
| LD50 = 100 mg/kg
| REL = TWA 0.5 mg/m3 (as Sb){{PGCH|0036}}
}}
|Section8={{Chembox Related
| OtherCompounds = antimony pentafluoride, antimony trichloride
}}
}}
Antimony trifluoride is the inorganic compound with the formula SbF3. Sometimes called Swarts' reagent, it is one of two principal fluorides of antimony, the other being SbF5. It appears as a white solid. As well as some industrial applications,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}} it is used as a reagent in inorganic and organofluorine chemistry.
Preparation and structure
In solid SbF3, the Sb centres have octahedral molecular geometry and are linked by bridging fluoride ligands. Three Sb–F bonds are short (192 pm) and three are long (261 pm). Because it is a polymer, SbF3 is far less volatile than related compounds AsF3 and SbCl3.{{Greenwood&Earnshaw}}
SbF3 is prepared by treating antimony trioxide with hydrogen fluoride:Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 199.
:Sb2O3 + 6 HF → 2 SbF3 + 3 H2O
The compound is a mild Lewis acid, hydrolyzing slowly in water. With fluorine, it is oxidized to give antimony pentafluoride.
:SbF3 + F2 → SbF5
Applications
It is used as a fluorination reagent in organic chemistry.Tariq Mahmood and Charles B. Lindahl Fluorine Compounds, Inorganic, Antimony in Kirk‑Othmer Encyclopedia of Chemical Technology.{{doi|10.1002/0471238961.0114200913010813.a01}} This application was reported by the Belgian chemist Frédéric Jean Edmond Swarts in 1892,{{cite journal |title=none|last=Swarts|journal=Acad. Roy. Belg|volume=3|issue=24|page=474|year=1892}} who demonstrated its usefulness for converting chloride compounds to fluorides. The method involved treatment with antimony trifluoride with chlorine or with antimony pentachloride to give the active species antimony trifluorodichloride (SbCl2F3). This compound can also be produced in bulk.{{cite patent | country=US |number=4438088}} The Swarts reaction is generally applied to the synthesis of organofluorine compounds, but experiments have been performed using silanes.{{cite journal|doi=10.1021/ja01216a072|last1=Booth|first1=Harold Simmons|last2=Suttle|first2=John Francis|title=IV. The Preparation and Fluorination of Dimethyl and Trimethyl Chlorosilanes|journal=J. Am. Chem. Soc. | year=1946 |volume=68 |issue=12|pages=2658–2660}} It was once used for the industrial production of freon. Other fluorine-containing Lewis acids serve as fluorinating agents in conjunction with hydrogen fluoride.
SbF3 is used in dyeing and in pottery, to make ceramic enamels and glazes.
Safety
The lethal minimum dose (guinea pig, oral) is 100 mg/kg.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}}
References
External links
- [http://webbook.nist.gov/cgi/cbook.cgi?ID=C7783564 WebBook page for SbF3]
{{Antimony compounds}}
{{fluorides}}
{{DEFAULTSORT:Antimony Trifluoride}}