Bromine monofluoride
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| IUPAC name Bromine monofluoride | |
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| UN number | 1745 |
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InChI
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| Properties | |
Chemical formula | BrF |
| Molar mass | 98.903 g/mol |
| Density | 4.403 g/L [1] |
| Melting point | −33 °C (−27 °F; 240 K)[1] |
| Boiling point | 20 °C (68 °F; 293 K) (decomposes)[1] |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references | |
Chemical compound
Bromine monofluoride is a quite unstable interhalogen compound with the chemical formula BrF. It can be produced through the reaction of bromine trifluoride (or bromine pentafluoride) and bromine. Due to its lability, the compound can be detected but not isolated:[2]
- BrF3 + Br2 → 3 BrF
- BrF5 + 2 Br2 → 5 BrF
- Br2(l) + F2(g) → 2 BrF(g)
It is usually generated in the presence of caesium fluoride.[3]
Bromine monofluoride decomposes at normal temperature through dismutation to bromine trifluoride, bromine pentafluoride, and free bromine.
The molecular structure in the gas phase was determined by microwave spectroscopy; the bond length is re = 1.758981(50) Å.[4]
The bond length in a cocrystal with methylchloride is 1.822(2) Å; the lengthening relative to the free molecule is due to an interaction of the type F-Br···ClMe with a distance of 2.640(1) Å.[5]
See also
- Bromine trifluoride, BrF3
- Bromine pentafluoride, BrF5
References
- ^ a b c David R. Lide: CRC Handbook of Chemistry and Physics. 89. Auflage, Taylor & Francis, 2008, ISBN 978-1-4200-6679-1, S. 4–53.
- ^ Macintyre, J. E.; Daniel, F. M.; Stirling, V. M. (1992). Dictionary of Inorganic Compounds. CRC Press. p. 285. ISBN 978-0-412-30120-9.
- ^ Winter, Rolf; Terjeson, Robin J.; Gard, Gary L. (1998). "An Improved and Facile Preparation of SF5Br". Journal of Fluorine Chemistry. 89: 105–106. doi:10.1016/S0022-1139(98)00094-3.
- ^ Nair, K. P. R. (1979). "Electric dipole moment of diatomic interhalogen molecules,". Kem. Kozl. 52: 431.
- ^ Drews, Thomas; Seppelt, Konrad (October 2012). "Bromine Monofluoride". Zeitschrift für anorganische und allgemeine Chemie. 638 (12–13): 2106–2110. doi:10.1002/zaac.201200293.
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Salts and covalent derivatives of the fluoride ion
| HF | ?HeF2 | |||||||||||||||||
| LiF | BeF2 | BF BF3 B2F4 +BO3 | CF4 CxFy +CO3 | NF3 FN3 N2F2 NF N2F4 NF2 ?NF5 | OF2 O2F2 OF O3F2 O4F2 ?OF4 | F2 | Ne | |||||||||||
| NaF | MgF2 | AlF AlF3 | SiF4 | P2F4 PF3 PF5 | S2F2 SF2 S2F4 SF3 SF4 S2F10 SF6 +SO4 | ClF ClF3 ClF5 | ?ArF2 ?ArF4 | |||||||||||
| KF | CaF CaF2 | ScF3 | TiF2 TiF3 TiF4 | VF2 VF3 VF4 VF5 | CrF2 CrF3 CrF4 CrF5 ?CrF6 | MnF2 MnF3 MnF4 ?MnF5 | FeF2 FeF3 FeF4 | CoF2 CoF3 CoF4 | NiF2 NiF3 NiF4 | CuF CuF2 ?CuF3 | ZnF2 | GaF2 GaF3 | GeF2 GeF4 | AsF3 AsF5 | Se2F2 SeF4 SeF6 +SeO3 | BrF BrF3 BrF5 | KrF2 ?KrF4 ?KrF6 | |
| RbF | SrF SrF2 | YF3 | ZrF3 ZrF4 | NbF4 NbF5 | MoF4 MoF5 MoF6 | TcF4 TcF 5 TcF6 | RuF3 RuF 4 RuF5 RuF6 | RhF3 RhF4 RhF5 RhF6 | PdF2 Pd[PdF6] PdF4 ?PdF6 | Ag2F AgF AgF2 AgF3 | CdF2 | InF InF3 | SnF2 SnF4 | SbF3 SbF5 | TeF4 ?Te2F10 TeF6 +TeO3 | IF IF3 IF5 IF7 +IO3 | XeF2 XeF4 XeF6 ?XeF8 | |
| CsF | BaF2 | LuF3 | HfF4 | TaF5 | WF4 WF5 WF6 | ReF4 ReF5 ReF6 ReF7 | OsF4 OsF5 OsF6 ?OsF 7 ?OsF 8 | IrF2 IrF3 IrF4 IrF5 IrF6 | PtF2 Pt[PtF6] PtF4 PtF5 PtF6 | AuF AuF3 Au2F10 ?AuF6 AuF5•F2 | Hg2F2 HgF2 ?HgF4 | TlF TlF3 | PbF2 PbF4 | BiF3 BiF5 | ?PoF2 PoF4 PoF6 | AtF ?AtF3 ?AtF5 | RnF2 ?RnF 4 ?RnF 6 | |
| FrF | RaF2 | LrF3 | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |
| ↓ | ||||||||||||||||||
| LaF3 | CeF3 CeF4 | PrF3 PrF4 | NdF2 NdF3 NdF4 | PmF3 | SmF2 SmF3 | EuF2 EuF3 | GdF3 | TbF3 TbF4 | DyF2 DyF3 DyF4 | HoF3 | ErF3 | TmF2 TmF3 | YbF2 YbF3 | |||||
| AcF3 | ThF3 ThF4 | PaF4 PaF5 | UF3 UF4 UF5 UF6 | NpF3 NpF4 NpF5 NpF6 | PuF3 PuF4 PuF5 PuF6 | AmF2 AmF3 AmF4 ? AmF6 | CmF3 CmF4 ?CmF6 | BkF3 BkF 4 | CfF3 CfF4 | EsF3 EsF4 ?EsF6 | Fm | Md | No | |||||
