Cobaltocene

Cobaltocene, Co(C₅H₅)₂, is known as bis(cyclopentadienyl)cobalt(II) or even "bis Cp cobalt." This dark purple compound is solid at room temperature that sublimes at 40 °C in a good vacuum, ca. 0.1 mm. Cobaltocene was discovered shortly after ferrocene, the first "metallocene." The compound must be handled and stored in the absence of air due to the ease with which it reacts with O₂.

Cobaltocene is prepared by the reaction of sodium cyclopentadienide, NaC₅H₅, with anhydrous CoCl₂ in THF solution. Sodium chloride is generated, and the organometallic product is usually purified by vacuum sublimation.^[1]

Additional recommended knowledge

Daily Sensitivity Test

Daily Visual Balance Check

What is the Correct Way to Check Repeatability in Balances?

Structure and bonding

Co(C₅H₅)₂ belongs to a group of organometallic compounds called metallocenes that consist of a metal atom sandwiched between two cyclopentadienyl (Cp) rings.^[2] Thus, metallocenes are sometimes referred as sandwich compounds.

Cobaltocene has 19 valence electrons, one more than usually found in organotransition metal complexes, such as its very stable relative ferrocene. This additional electron occupies an orbital that is antibonding with respect to the Co-C bonds. Consequently, the Co-C distances are slightly longer than the Fe-C bonds in ferrocene. Many chemical reactions of Co(C₅H₅)₂ are characterized by its tendency lose this "extra" electron, yielding 18-electron cation known as cobaltocenium:

Redox properties

Co(C₅H₅)₂ is a common one-electron reducing agent in the laboratory.^[3] In fact, the reversibility of the Co(C₅H₅)₂ redox couple is so well behaved that Co(C₅H₅)₂ may be used in cyclic voltammetry as an internal standard. One of its analogues called decamethylcobaltocene Co(C₅Me₅)₂ is an especially powerful reducing agent, due to inductive donation of electron density from the 10 methyl groups, prompting the cobalt to give up its "extra" electron even more so. These two compounds are rare examples of reductants that dissolve in non-polar organic solvents. The reduction potentials of these compounds follow, using the ferrocene-ferrocenium couple as the reference:

We can see from this data that the decamethyl compounds are ca. 600 mV more reducing than the parent metallocenes. This substituent effect is, however, overshadowed by the influence of the metal: changing from Fe to Co renders the reduction more favorable by over 1.3 volts.

Other reactions

Treatment of Co(C₅H₅)₂ with carbon monoxide gives the cobalt(I) derivative Co(C₅H₅)(CO)₂, concomitant with loss of one Cp ligand. This air-stable, distillable liquid has "two-legged piano-stool" structure.

References

1. ^ King, R. B. “Organometallic Syntheses” Volume 1: Academic Press: New York, 1965.
2. ^ C. Elschenbroich, A. Salzer ”Organometallics : A Concise Introduction” (2nd Ed) (1992) from Wiley-VCH: Weinheim. ISBN 3-527-28165-7
3. ^ Connelly, N. G. and Geiger, W. E., "Chemical Redox Agents for Organometallic Chemistry", Chemical Reviews, 1996, volume 96, 877-922