Triiron dodecacarbonyl

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Triiron dodecacarbonyl
Triiron dodecacarbonyl
Names
IUPAC names
dodecarbonyltriiron,
tetra-μ-carbonyl-1:2κ4C,1:3κ2C,2:3κ2C-
octacarbonyl-1κ3C,2κ3C,3κ2C-triangulo
-triiron(3 FeFe)
Other names
Iron tetracarbonyl trimer
Identifiers
17685-52-8 YesY
Properties
Fe3(CO)12
Molar mass 503.66 g/mol
Appearance dark black/green crystals
Melting point 165 °C (329 °F; 438 K)
Boiling point decomposes
insoluble
Structure
Point group C2v
Related compounds
Other cations
Triruthenium dodecacarbonyl
Triosmium dodecacarbonyl
Related iron carbonyls
Iron pentacarbonyl
Diiron nonacarbonyl
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Triiron dodecarbonyl is the organoiron compound with the formula Fe3(CO)12. It is a dark green solid that sublimes under vacuum. It is soluble in nonpolar organic solvents to give intensely green solutions. Most low-nuclearity clusters are pale yellow or orange. Hot solutions of Fe3(CO)12 decompose to an iron mirror, which can be pyrophoric in air. The solid decomposes slowly in air, and thus samples are typically stored cold under an inert atmosphere.[1] It is a more reactive source of iron(0) than iron pentacarbonyl.

Synthesis[edit]

It was one of the first metal carbonyl clusters synthesized. It was occasionally obtained from the thermolysis of Fe(CO)5:

3 Fe(CO)5 → Fe3(CO)12 + 3 CO

Traces of the compound are easily detected because of its characteristic deep green colour. UV-photolysis of Fe(CO)5 produces Fe2(CO)9, not Fe3(CO)12.

The usual synthesis of Fe3(CO)12 starts with the reaction of Fe(CO)5 with base:[2]

3 Fe(CO)5 + (C2H5)3N + H2O → [(C2H5)3NH][HFe3(CO)11] + 3 CO + CO2

followed by oxidation of the resulting hydrido cluster with acid:

[(C2H5)3NH][HFe3(CO)11] + HCl + CO → Fe3(CO)12 + H2 + [(C2H5)3NH]Cl

The original synthesis by Walter Hieber et al. entailed the oxidation of H2Fe(CO)4 with MnO2. The cluster was originally formulated incorrectly as "Fe(CO)4".[3]

Structure[edit]

Elucidation of the structure of Fe3(CO)12 proved to be challenging because the CO ligands are disordered in the crystals. Early evidence for its distinctive C2v structure came from Mössbauer spectroscopic measurements that revealed two quadrupole doublets with similar isomer shifts but different (1.13 and 0.13 mm s−1) quadrupolar coupling constants.

Fe3(CO)12 consists of a triangle of iron atoms surrounded by 12 CO ligands. Ten of the CO ligands are terminal and two span an Fe---Fe edge, resulting in C2v point group symmetry. By contrast, Ru3(CO)12 and Os3(CO)12 adopt D3h-symmetric structures, wherein all 12 CO ligands are terminally bound to the metals. Spectroscopic evidence indicates that the two carbonyl groups may be unsymmetrical, in which case the idealized C2v symmetry is reduced to C2.[citation needed] In solution Fe3(CO)12 is fluxional, resulting in equivalencing all 12 CO groups. Overall, it can be appreciated that these three clusters formally arise from condensation of three 16-electron M(CO)4 fragments, akin to the theoretical condensation of three methylene (:CH2) molecules into cyclopropane.

The anion [HFe3(CO)11] is structurally related to Fe3(CO)12, with the hydride replacing one bridging CO ligand. The bonding in the Fe-H-Fe subunit is described using concepts developed for diborane.

Reactions[edit]

Like most metal carbonyls, Fe3(CO)12 undergoes substitution reactions, making, for example, Fe3(CO)11{P(C6H5)3} forms upon reaction with triphenylphosphine.

Heating Fe3(CO)12 gives a low yield of the carbido cluster Fe5(CO)15C. Such reactions proceed via disproportionation of CO to give CO2 and carbon.

Fe3(CO)12 form "ferroles" upon reaction with heterocycles such as thiophenes.

Fe3(CO)12 reacts with thiols and disulfides to give thiolate-bridged complexes, such as methylthioirontricarbonyl dimer:[4]

2 Fe3(CO)12 + 3 (CH3)2S2 → 3 [Fe(CO)3SCH3]2 + 6 CO. These complexes are studied as hydrogenase mimics.[5]

Safety[edit]

Fe3(CO)12 is hazardous as a source of volatile iron and as a source of carbon monoxide. Solid samples, especially when finely divided, and residues from reactions can be pyrophoric, which can ignite the organic solvents used for such reactions.

References[edit]

  1. ^ Elschenbroich, C.; Salzer, A. ”Organometallics: A Concise Introduction” (2nd Ed) (1992) from Wiley-VCH: Weinheim. ISBN 3-527-28165-7
  2. ^ McFarlane, W.; Wilkinson, G. W. (1966). "Triiron dodecacarbonyl". Inorganic Syntheses 8: 181–3. doi:10.1002/9780470132395.ch47. 
  3. ^ Hieber, W.; Leutert, F. (1932). "Über Metallcarbonyle. XII. Die Basenreaktion des Eisenpentacarbonyls und die Bildung des Eisencarbonylwasserstoffs (Metal carbonyls. XII. The Reaction of Iron Pentacarbonyl with Bases and the Formation of Iron Hydrocarbonyl)". Zeitschrift für anorganische und allgemeine Chemie 204: 145–64. doi:10.1002/zaac.19322040115. 
  4. ^ King, R. B. "Organosulfur Derivatives of Metal Carbonyls. I. The Isolation of Two Isomeric Products in the Reaction of Triiron Dodecacarbonyl with Dimethyl Disulfide" J. Am. Chem. Soc. 1962, vol. 84, 2460. doi:10.1021/ja00871a045
  5. ^ Synthesis, Purification, and Characterization of a µ-(1,3-Propanedithiolato)-hexacarbonyldiiron Laboratory Experiment or Mini-Project for Inorganic Chemistry or Integrated Laboratory Carmen F. Works 836 Journal of Chemical Education Vol. 84 No. 5 May 2007 Abstract