Dicobalt octacarbonyl

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Dicobalt octacarbonyl

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UN number	3281
Template:Longitem	Template:Chem2
Molar mass	341.95 g/mol
Appearance	red-orange crystals
Density	1.87 g/cm3
Melting point	Template:Chembox CalcTemperatures
Boiling point	Template:Chembox CalcTemperatures
Vapor pressure	0.7 mmHg (20 °C)
Template:Longitem	1.33 D (C2v isomer) 0 D (D3d isomer)
Template:Longitem	Iron pentacarbonyl Diiron nonacarbonyl Nickel tetracarbonyl

Dicobalt octacarbonyl is an organocobalt compound with composition Template:Chem2. This metal carbonyl is used as a reagent and catalyst in organometallic chemistry and organic synthesis, and is central to much known organocobalt chemistry. It is the parent member of a family of hydroformylation catalysts. Each molecule consists of two cobalt atoms bound to eight carbon monoxide ligands, although multiple structural isomers are known. Some of the carbonyl ligands are labile.

Synthesis, structure, properties

Dicobalt octacarbonyl an orange-colored, pyrophoric solid. It is synthesised by the high pressure carbonylation of cobalt(II) salts:

Template:Chem2

The preparation is often carried out in the presence of cyanide, converting the cobalt(II) salt into a pentacyanocobaltate(II) complex that reacts with carbon monoxide to yield Template:Chem2. Acidification produces cobalt tetracarbonyl hydride, Template:Chem2, which degrades near room temperature to dicobalt octacarbonyl and hydrogen. It can also be prepared by heating cobalt metal to above 250 °C in a stream of carbon monoxide gas at about 200 to 300 atm:

Template:Chem2

It exists as a mixture of rapidly interconverting isomers. In solution, there are two isomers known that rapidly interconvert:

File:Co2(CO)8NoCo-Co.png

The major isomer (on the left in the above equilibrium process) contains two bridging carbonyl ligands linking the cobalt centres and six terminal carbonyl ligands, three on each metal. It can be summarised by the formula Template:Chem2 and has C_2v symmetry. This structure resembles diiron nonacarbonyl (Template:Chem2) but with one fewer bridging carbonyl. The Co–Co distance is 2.52 Å, and the Co–CO_terminal and Co–CO_bridge distances are 1.80 and 1.90 Å, respectively. Analysis of the bonding suggests the absence of a direct cobalt–cobalt bond.

The minor isomer has no bridging carbonyl ligands, but instead has a direct bond between the cobalt centres and eight terminal carbonyl ligands, four on each metal atom. It can be summarised by the formula Template:Chem2 and has D_4d symmetry. It features an unbridged cobalt–cobalt bond that is 2.70 Å in length in the solid structure when crystallized together with C₆₀.

Reactions

Reduction

Dicobalt octacarbonyl is reductively cleaved by alkali metals and related reagents, such as sodium amalgam. The resulting sodium tetracarbonylcobaltate protonates to give tetracarbonyl cobalt hydride:

Template:Chem2

Template:Chem2

Salts of this form are also intermediates in the cyanide synthesis pathway for dicobalt octacarbonyl.

Reactions with electrophiles

Halogens and related reagents cleave the Co–Co bond to give pentacoordinated halotetracarbonyls:

Template:Chem2

Cobalt tricarbonyl nitrosyl is produced by treatment of dicobalt octacarbonyl with nitric oxide:

Template:Chem2

Reactions with alkynes

The Nicholas reaction is a substitution reaction whereby an alkoxy group located on the α-carbon of an alkyne is replaced by another nucleophile. The alkyne reacts first with dicobalt octacarbonyl, from which is generated a stabilized propargylic cation that reacts with the incoming nucleophile and the product then forms by oxidative demetallation.

The Nicholas reaction

The Nicholas reaction

The Pauson–Khand reaction, in which an alkyne, an alkene, and carbon monoxide cyclize to give a cyclopentenone, can be catalyzed by Template:Chem2, though newer methods that are more efficient have since been developed:

File:Pauson Khand reaction original.svg

Template:Chem2 reacts with alkynes to form a stable covalent complex, which is useful as a protective group for the alkyne. This complex itself can also be used in the Pauson–Khand reaction.

Intramolecular Pauson–Khand reactions, where the starting material contains both the alkene and alkyne moieties, are possible. In the asymmetric synthesis of the Lycopodium alkaloid huperzine-Q, Takayama and co-workers used an intramolecular Pauson–Khand reaction to cyclise an enyne containing a tert-butyldiphenylsilyl (TBDPS) protected primary alcohol. The preparation of the cyclic siloxane moiety immediately prior to the introduction of the dicobalt octacarbonyl ensures that the product is formed with the desired conformation.

File:Pauson-Khand reaction in synthesis of huperzine-Q.jpg

Dicobalt octacarbonyl can catalyze alkyne trimerisation of diphenylacetylene and its derivatives to hexaphenylbenzenes. Symmetrical diphenylacetylenes form 6-substituted hexaphenylbenzenes, while asymmetrical diphenylacetylenes form a mixture of two isomers.

Symmetric diphenylacetylene cyclotrimerization using dicobalt octacarbonyl

Symmetric diphenylacetylene cyclotrimerization using dicobalt octacarbonyl

Asymmetric diphenylacetylene cyclotrimerization using dicobalt octacarbonyl

Asymmetric diphenylacetylene cyclotrimerization using dicobalt octacarbonyl

Hydroformylation

File:Hydroformylation Mechanism V.1.svg

Catalytic cycle for the hydroformylation of a terminal alkene (Template:Chem2) to an aldehyde (Template:Chem2):Template:Ordered list

Hydrogenation of Template:Chem2 produces cobalt tetracarbonyl hydride Template:Chem2:

Template:Chem2

This hydride is a catalyst for hydroformylation – the conversion of alkenes to aldehydes. The catalytic cycle for this hydroformylation is shown in the diagram.

Substitution reactions

The CO ligands can be replaced with tertiary phosphine ligands to give Template:Chem2. These bulky derivatives are more selective catalysts for hydroformylation reactions. "Hard" Lewis bases, e.g. pyridine, cause disproportionation:

Template:Chem2

Conversion to higher carbonyls

File:HCCo3(CO)9.png

Methylidynetricobaltnonacarbonyl, Template:Chem2, an organocobalt cluster compound structurally related to tetracobalt dodecacarbonyl

Heating causes decarbonylation and formation of tetracobalt dodecacarbonyl:

Template:Chem2

Like many metal carbonyls, dicobalt octacarbonyl abstracts halides from alkyl halides. Upon reaction with bromoform, it converts to methylidynetricobaltnonacarbonyl, Template:Chem2, by a reaction that can be idealised as:

Template:Chem2

Safety

Template:Chem2 a volatile source of cobalt(0), is pyrophoric and releases carbon monoxide upon decomposition. The National Institute for Occupational Safety and Health has recommended that workers should not be exposed to concentrations greater than 0.1 mg/m³ over an eight-hour time-weighted average, without the proper respiratory gear.