| 词条 | Antimony pentafluoride |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 441020860 | ImageFileL1 = Antimony-pentafluoride-2D.png | ImageNameL1 = Antimony pentafluoride | ImageFileR1 = Antimony-pentafluoride-monomer-3D-balls.png | ImageNameR1 = Antimony pentafluoride | IUPACName = antimony(V) fluoride | OtherNames = antimony pentafluoride pentafluoridoantimony |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 | InChIKey = VBVBHWZYQGJZLR-NMXCDXEPAW | StdInChI = 1S/5FH.Sb/h5*1H;/q;;;;;+5/p-5 | StdInChIKey = VBVBHWZYQGJZLR-UHFFFAOYSA-I | StdInChI_Ref = {{stdinchicite|changed|chemspider}} | StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} | CASNo = 7783-70-2 | CASNo_Ref = {{cascite|correct|CAS}} | PubChem = 24557 | ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} | ChemSpiderID = 22963 | RTECS = CC5800000 | UNNumber = 1732 |Section2={{Chembox Properties | Formula = SbF5 | MolarMass = 216.74 g/mol | Appearance = colorless oily liquid hygroscopic | Odor = pungent | Density = 2.99 g/cm3 [1] | MeltingPtC = 8.3 | BoilingPtC = 149.5 | Solubility = Reacts | SolubleOther = soluble in KF, liquid SO2 |Section7={{Chembox Hazards | ExternalSDS = ICSC 0220 | EUClass = Harmful (Xn) Dangerous for the environment (N) | NFPA_ref = [2] | NFPA-H = 4 | NFPA-F = 0 | NFPA-R = 1 | NFPA-S = W | RPhrases = {{R20/22}}, {{R51/53}} | SPhrases = {{S2}}, {{S61}} | FlashPt = | REL = TWA 0.5 mg/m3 (as Sb)[3] | PEL = TWA 0.5 mg/m3 (as Sb)[3] |Section8={{Chembox Related | OtherCompounds = Antimony trifluoride | OtherAnions = Antimony pentachloride | OtherCations = Phosphorus pentafluoride Arsenic pentafluoride Bismuth pentafluoride }}Antimony pentafluoride is the inorganic compound with the formula SbF5. 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 acidity and its ability to react with almost all known compounds.[4] PreparationAntimony 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 reactionsIn 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] In the same way that SbF5 enhances the Brønsted acidity of HF, it augments the oxidizing power of F2. This effect is illustrated by the oxidation of oxygen:[9] 2 SbF5 + F2 + 2 O2 → 2 [O2]+[SbF6]− Antimony pentafluoride has also been used in the first discovered chemical reaction that produces fluorine 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}} The driving force for this reaction is the high affinity of SbF5 for {{chem|F|-}}, which is the same property that recommends the use of SbF5 to generate superacids. HexafluoroantimonateSbF5 is a strong Lewis acid, exceptionally so toward sources of F− to give the very stable anion [SbF6]−, called hexafluoroantimonate. [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]− SafetySbF5 reacts violently with many compounds, often releasing dangerous hydrogen fluoride. It is corrosive to the skin and eyes.[10][11] References1. ^{{RubberBible87th}} 2. ^[https://www.worldofchemicals.com/chemicals/chemical-properties/antimony-pentafluoride%20.html World of Chemicals SDS] 3. ^1 {{PGCH|0036}} 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|10.1002/047084289}}. 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. ^{{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 }} 11. ^{{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 }} External links
4 : Superacids|Antimony compounds|Fluorides|Metal halides |
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