Ferrocenium tetrafluoroborate
| |
| Names | |
|---|---|
| Other names
dicyclopentadienyl iron tetrafluoroborate
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| Identifiers | |
| ECHA InfoCard | 100.156.161 |
| Properties | |
| C10H10BFeF4 | |
| Molar mass | 272.84 g/mol |
| Appearance | dark blue powder |
| Melting point | 178 °C (352 °F; 451 K) (decomposes) |
| Solubility in acetonitrile | Soluble[citation needed] |
| Hazards | |
| Safety data sheet | External MSDS |
EU classification (DSD) (outdated)
|
 C
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| Related compounds | |
Related compounds
|
Ferrocene |
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 | |
Ferrocenium tetrafluoroborate is an organometallic compound with the formula [Fe(C5H5)2]BF4. This salt is composed of the cation [Fe(C5H5)2]+ and the tetrafluoroborate anion (BF−
4). The related hexafluorophosphate is also a popular reagent with similar properties. The cation is often abbreviated Fc+ or Cp2Fe+. The salt is deep blue in color and paramagnetic.
Ferrocenium salts are sometimes used as one-electron oxidizing agents, and the reduced product, ferrocene, is inert and readily separated from ionic products. The ferrocene–ferrocenium couple is often used as a reference in electrochemistry. The standard potential of ferrocene-ferrocenium is 0.400 V vs. the normal hydrogen electrode (NHE)[1] and is often assumed to be invariant between different solvents.
Preparation[edit]
Commercially available, this compound may be prepared by oxidizing ferrocene typically with ferric salts followed by addition of fluoroboric acid.[2] A variety of other oxidants work well also, such as nitrosyl tetrafluoroborate.[3] Many analogous ferrocenium salts are known.[4]
References[edit]
- ^ Bard, A.J.; Parsons, R.; Jordan, J. (1985). Standard Potentials in Aqueous Solution. New York: IUPAC.
- ^ Connelly, N. G.; Geiger, W. E. (1996). "Chemical Redox Agents for Organometallic Chemistry". Chem. Rev. 96 (2): 877–910. doi:10.1021/cr940053x. PMID 11848774.
- ^ Nielson, Roger M.; McManis, George E.; Safford, Lance K.; Weaver, Michael J. (1989). "Solvent and electrolyte effects on the kinetics of ferrocenium-ferrocene self-exchange. A reevaluation". J. Phys. Chem. 93 (5): 2152. doi:10.1021/j100342a086.
- ^ Le Bras, J.; Jiao, H.; Meyer, W. E.; Hampel, F.; Gladysz, J. A. (2000). "Synthesis, Crystal Structure, and Reactions of the 17-Valence-Electron Rhenium Methyl Complex [(η5-C5Me5)Re(NO)(P(4-C6H4CH3)3)(CH3)]+ B(3,5-C
6H
3(CF
3)
2)−
4: Experimental and Computational Bonding Comparisons with 18-Electron Methyl and Methylidene Complexes". J. Organomet. Chem. 616: 54–66. doi:10.1016/S0022-328X(00)00531-3.
