Bismuth pentafluoride
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| Names | |
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| Other names
bismuth(V) fluoride
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| Identifiers | |
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3D model (Jmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.029.205 |
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PubChem CID
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| Properties | |
| BiF5 | |
| Molar mass | 303.97 g mol−1 |
| Appearance | long white needles, colourless crystalline solid |
| Density | 5.40 g cm−3 |
| Melting point | 151.4 °C (304.5 °F; 424.5 K) , 154.4 °C |
| Boiling point | 230 °C (446 °F; 503 K) |
| Structure | |
| octahedral Bi | |
| Hazards | |
| NFPA 704 | |
| Related compounds | |
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Other anions
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bismuth trichloride, bismuth tribromide, bismuth triiodide, pentamethylbismuth |
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Other cations
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phosphorus pentafluoride, arsenic pentafluoride, antimony pentafluoride |
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Related compounds
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bismuth trifluoride |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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| Infobox references | |
Bismuth pentafluoride is the inorganic compound with the formula BiF5. It is a white solid that is highly reactive. The compound is of interest to researchers but of not particular value.
BiF5 is polymeric and consists of linear chains of trans-bridged corner sharing BiF6 octahedra. This is the same structure as α-UF5.
BiF5 can be prepared by treating BiF3 with F2 at 500 °C.
In an alternative synthesis, ClF3 is the fluorinating agent at 350 °C.
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.
BiF5 also reacts with alkali metal fluorides, MF, to form hexafluorobismuthates, M[BiF6], containing the hexafluorobismuthate anion, [BiF6]−.
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