![antimony trifluoride antimony trifluoride](https://www.webelements.com/_media/compounds/Sb/F3Sb1-7783564.jpg)
It is used as a fluorination reagent in organic chemistry. With fluorine, it is oxidized to give antimony pentafluoride. The compound is a mild Lewis acid, hydrolyzing slowly in water. SbF 3 is prepared by treating antimony trioxide with hydrogen fluoride: Sb 2O 3 + 6 HF → 2 SbF 3 + 3 H 2O Because it is a polymer, SbF 3 is far less volatile than related compounds AsF 3 and SbCl 3. Three Sb–F bonds are short (192 pm) and three are long (261 pm). In solid SbF 3, the Sb centres have octahedral molecular geometry and are linked by bridging fluoride ligands. "Chemical Database - Antimony Pentafluoride". Commission of the European Communities (CEC). ^ International Programme on Chemical Safety (2005)."Dioxygenyl Salts" Inorganic Syntheses 1973, XIV, 109-122. "Inorganic Chemistry" Academic Press: San Diego, 2001. "Crystal structure of Antimony Pentafluoride" Journal of the Chemical Society, Chemical Communications 1971, pp. ^ Handbook of Preparative Inorganic Chemistry, 2nd Ed.Breunig, Hans Uwe Wolf "Antimony and Antimony Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2006, Wiley-VCH, Weinheim. Li, X.-y."Antimony(V) Fluoride" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. National Institute for Occupational Safety and Health (NIOSH). ^ a b NIOSH Pocket Guide to Chemical Hazards.CRC Handbook of Chemistry and Physics (87th ed.). SbF 5 reacts violently with many compounds, often releasing dangerous hydrogen fluoride. − is a weakly coordinating anion akin to PF 6 −.Īlthough it is only weakly basic, − does react with additional SbF 5 to give a centrosymmetric adduct: SbF 5 is a strong Lewis acid, exceptionally so toward sources of F − to give the very stable anion −, called hexafluoroantimonate.
![antimony trifluoride antimony trifluoride](https://i.pinimg.com/originals/b3/8e/94/b38e94daf4fb26f848f557ad9c4bf899.jpg)
, which is the same property that recommends the use of SbF 5 to generate superacids. The driving force for this reaction is the high affinity of SbF 5 for F − This effect is illustrated by the oxidation of oxygen: 2 SbF 5 + F 2 + 2 O 2 → 2 + −Īntimony pentafluoride has also been used in the first discovered chemical reaction that produces fluorine gas from fluoride compounds: In the same way that SbF 5 enhances the Brønsted acidity of HF, it augments the oxidizing power of F 2. The related species PF 5 and AsF 5 are monomeric in the solid and liquid states, probably due to the smaller sizes of the central atom, which limits their coordination number. The Sb-F bonds are 2.02 Å within the eight-membered Sb 4F 4 ring the remaining fluoride ligands radiating from the four Sb centers are shorter at 1.82 Å. The crystalline material is a tetramer, meaning that it has the formula 4. The liquid contains polymers wherein each Sb is octahedral, the structure being described with the formula n ((μ-F) denotes the fact that fluoride centres bridge two Sb centres). The material adopts a more complicated structure in the liquid and solid states. In the gas phase, SbF 5 adopts a trigonal bipyramidal structure of D 3h point group symmetry (see picture). It can also be prepared from antimony trifluoride and fluorine.
![antimony trifluoride antimony trifluoride](https://66.media.tumblr.com/c9546e6f94c40921f114d0cb88032e2b/tumblr_o5r36wnd7W1rszmkso1_500.jpg)
Antimony pentafluoride is prepared by the reaction of antimony pentachloride with anhydrous hydrogen fluoride: SbCl 5 + 5 HF → SbF 5 + 5 HCl