Bismuth pentafluoride
Other names
bismuth(V) fluoride
3D model (JSmol)
ECHA InfoCard 100.029.205 Edit this at Wikidata
  • InChI=1/Bi.5FH.3H/h;5*1H;;;/q+3;;;;;;;;/p-5/rBiH3.5FH/h1H3;5*1H/q+3;;;;;/p-5
  • F[Bi](F)(F)(F)F
Molar mass 303.97 g mol−1
Appearance long white needles,[1] colourless crystalline solid[2]
Density 5.40 g cm−3[1]
Melting point 151.4 °C (304.5 °F; 424.5 K) ,[2] 154.4 °C[1]
Boiling point 230 °C (446 °F; 503 K)[1][2]
octahedral Bi
GHS labelling:
GHS03: Oxidizing GHS05: Corrosive
H272, H314
P210, P220, P221, P260, P264, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P370+P378, P405, P501
NFPA 704 (fire diamond)
Flash point non-combustible
Safety data sheet (SDS) MSDS
Related compounds
Other anions
bismuth trichloride, bismuth tribromide, bismuth triiodide, pentamethylbismuth
Other cations
phosphorus pentafluoride, arsenic pentafluoride, antimony pentafluoride
Related compounds
bismuth trifluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Bismuth pentafluoride is an inorganic compound with the formula BiF5. It is a white solid that is highly reactive. The compound is of interest to researchers but not of particular value.


BiF5 is polymeric and consists of linear chains of trans-bridged corner sharing BiF6 octahedra.[1][3] This is the same structure as α-UF5.[1]

(BiF5) chain packing of chains


BiF5 can be prepared by treating BiF3 with F2 at 500 °C.[2]

BiF3 + F2 → BiF5

In an alternative synthesis, ClF3 is the fluorinating agent at 350 °C.[4]

BiF3 + ClF3 → BiF5 + ClF


Bismuth pentafluoride is the most reactive of the pnictogen pentafluorides and is an extremely strong fluorinating agent. It reacts vigorously with water to form ozone and oxygen difluoride, and with iodine or sulfur at room temperature. BiF5 fluorinates paraffin oil (hydrocarbons) to fluorocarbons above 50 °C and oxidises UF4 to UF6 at 150 °C. At 180 °C, bismuth pentafluoride fluorinates Br2 to BrF3 and Cl2 to ClF.[1]

BiF5 also reacts with alkali metal fluorides, MF, to form hexafluorobismuthates, M[BiF6], containing the hexafluorobismuthate anion, [BiF6].[2] Bismuth pentafluorude in hydrofluoric acid solvent also reacts with nickel fluoride to form the nickel salt of this anion, which can be incorporated into a complex with acetonitrile.[5]


  1. ^ a b c d e f g Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 561–563. ISBN 978-0-08-037941-8.
  2. ^ a b c d e Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils (ed.), Inorganic Chemistry, translated by Eagleson, Mary; Brewer, William, San Diego/Berlin: Academic Press/De Gruyter, pp. 769–770, ISBN 0-12-352651-5
  3. ^ C. Hebecker (1971). "Zur Kristallstruktur von Wismutpentafluorid". Z. anorg. allg. Chem. 384 (2): 111–114. doi:10.1002/zaac.19713840204.
  4. ^ A. I. Popov; A. V. Scharabarin; V. F. Sukhoverkhov; N. A. Tchumaevsky (1989). "Synthesis and properties of pentavalent antimony and bismuth fluorides". Z. Anorg. Allg. Chem. 576 (1): 242–254. doi:10.1002/zaac.19895760128.
  5. ^ Roland Bougon; Pierrette Charpin; Karl O. Christe; Jacques Isabey; Monique Lance; Martine Nierlich; Julien Vigner; William W. Wilson (1988). "Preparation and characterization of nickel(2+) hexafluorobismuthate(1-) and of the ternary adducts [Ni(CH3CN)6](BiF6)2 and [Ni(CH3CN)6](SbF6)2. Crystal structure of hexakis(acetonitrile-d3)nickel(2+) hexafluoroantimonate". Inorganic Chemistry. 27 (8): 1389–1393. doi:10.1021/ic00281a018.