Ferrocenium tetrafluoroborate

Ferrocenium tetrafluoroborate
Names
	Other names dicyclopentadienyl iron tetrafluoroborate
Identifiers
CAS Number	1282-37-7 ;
ECHA InfoCard	100.156.161
Properties
Chemical formula	C10H10BFeF4
Molar mass	272.84 g/mol
Appearance	dark blue powder
Melting point	178 °C (352 °F; 451 K) (decomposes)
Solubility in acetonitrile	Soluble
Hazards
Safety data sheet	External MSDS
EU classification (DSD) (outdated)	C
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

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

↑ 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.

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[1] Bard, A.J.; Parsons, R.; Jordan, J. (1985). Standard Potentials in Aqueous Solution. New York: IUPAC.

[Geiger-2] 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.

[3] 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.

[4] 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.