Metal sulfur dioxide complex

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In organometallic chemistry, metal sulfur dioxide complexes are complexes that contain sulfur dioxide, SO2, bonded to a transition metal. [1] Such compounds are common but are mainly of theoretical interest. Historically, the study of these compounds has provided insights into the mechanisms of migratory insertion reactions.

Contents

Bonding modes

Portion of the structure of [Ni(SO2)6](AsF6)2, showing the dication and one of two AsF6 anions. EntryWithCollCode80473.png
Portion of the structure of [Ni(SO2)6](AsF6)2, showing the dication and one of two AsF6 anions.

Sulfur dioxide forms complexes with many transition metals. Most numerous are complexes with metals in oxidation state 0 or +1. [1]

In most cases SO2 binds in monodentate fashion, attaching to the metal through sulfur. Such complexes are further subdivided according to the planarity or pyramidalization at sulfur. The various bonding modes are:

More exotic bonding modes are known for clusters.

Illustrative SO2 complexes of soft metal centers. From the left, Fe(CO)2[P(OPh)3]2(e -SO2), IrCl(CO)(PPh3)2(e -SO2), Mo(CO)2(PMe3)3(e -SO2), and the A-frame complex Rh2(bis(diphenylphosphino)methane)2Cl(CO)2(m-SO2). SO2CmpxesUpgrade.png
Illustrative SO2 complexes of soft metal centers. From the left, Fe(CO)2[ P(OPh)3 ]2(η -SO2), IrCl(CO)(PPh3)2(η -SO2), Mo(CO)2(PMe3)3(η -SO2), and the A-frame complex Rh2(bis(diphenylphosphino)methane)2Cl(CO)2(μ-SO2).

Preparation

Complexes of the transition metals are usually generated simply by treating the appropriate metal complex with SO2. The adducts are often weak. In some cases, SO2 displaces other ligands. [3]

A large number of labile O-bonded SO2 complexes arise from the oxidation of a suspension of the metals in liquid SO2, an excellent solvent. [2]

Reactions

The main reaction of sulfur dioxide promoted by transition metals is its reduction by hydrogen sulfide. Known as the Claus process, this reaction is conducted on a large scale as a way to remove hydrogen sulfide that arises in hydrotreating processes in refineries.

Insertion of SO2 into metal-ligand bonds

Of academic interest, SO2 acts like a Lewis acid towards the alkyl ligand. [4] The pathway for the insertion of SO2 into metal alkyl bond begins with attack of the alkyl nucleophile on the sulfur centre in SO2. The "insertion" proceed the sulfur dioxide between the metal and the alkyl ligand leads to the O, O'-sulphinate. Alternatively an O-sulphinate can arise. Both of these intermediates commonly convert to an S-sulphinate. [5] S-sulphinate has sulfur–oxygen stretching frequencies from 1250–1000 cm−1 and 1100–1000 cm−1. The O, O'-sulphinate and O-sulphinate are difficult to distinguish as they have stretching frequencies from 1085–1050 cm−1 and 1000–820 cm−1 or lower. The pathway involving the O, O' sulphinate can generally be ruled out if the original metal complex fulfilled the 18-electron rule because the two metal–oxygen bonds would exceed the 18 electron rule. [6] The pathway by which SO2 inserts into a square planar alkyl complexes involves the formation of an adduct. Thereafter, the alkyl ligand migrates to the SO2. [7]

Pathway for insertion of SO2 into Au-methyl bonds of a square planar Au(III)) complex. AuMe+SO2Insn.png
Pathway for insertion of SO2 into Au-methyl bonds of a square planar Au(III)) complex.

Dithionite complexes

Dithionite, the reductively coupled derivative of sulfur dioxide is observed as a ligand when some reduced metals are treated with sulfur dithioxide. One example is [(C5(CH3)5)2Sm]2(S2O4). [8] [9]

S2O complexes

Several complexes of disulfur monoxide are known. Most are formed by oxidation peroxide oxidation of a disulfur ligand. In these complexes, the S2O ligand is invariably bound in an η2-S,S manner. Selected examples: [Ir(dppe)2S2O]+, OsCl(NO)(PPh3)2S2O, NbCl(η-C5H5)2S2O, Mn(CO)2(η-C5Me5)S2O, Re(CO)2(η-C5Me5)S2O, Re(CO)2(η-C5H5)S2O. [10]

Mo2(S2O)2(S2CNEt2)4 arises when the dithiocarbamate complex Mo(CO)2(S2CNEt2)2 is oxidized with elemental sulfur in air. Another way to form these complexes is to combine OSNSO2·R complexes with hydrogen sulfide. Complexes formed in this way are: IrCl(CO)(PPh3)2S2O; Mn(CO)2(η-C5H5)S2O. With hydrosulfide and a base followed by oxygen, OsCl(NO)(PPh3)2S2O can be made.

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References

  1. 1 2 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN   978-0-08-037941-8.
  2. 1 2 3 Mews, R.; Lork, E.; Watson, P. G.; Görtler, B. (2000). "Coordination Chemistry in and of Sulfur Dioxide". Coord. Chem. Rev. 197 (1): 277–320. doi:10.1016/S0010-8545(99)00191-5.
  3. ↑ Schenk, W. A. (1987). "Sulfur Oxides as Ligands in Coordination Compounds". Angew. Chem. Int. Ed. 26 (2): 98–109. doi:10.1002/anie.198700981.
  4. ↑ Douglas, B. E.; McDaniel, D. H.; Alexander, J. J. (1994). Concepts and Models of Inorganic Chemistry (3rd ed.). New York: John Wiley & Sons, Inc. ISBN   978-0-471-62978-8.
  5. ↑ Wojcicki, A. (1974). "Insertion Reactions of Transition Metal–Carbon σ-Bonded Compounds II. Sulfur Dioxide and Other Molecules". In Stone, F. G. A.; West, R. (eds.). Advances in Organometallic Chemistry . Vol. 12. pp. 31–81. doi:10.1016/S0065-3055(08)60450-5. ISBN   9780120311125.
  6. ↑ Alexander, J. J. (1985). Hartley, F. R.; Patai, S. (eds.). The Chemistry of the Metal-Carbon Bond, Vol. 2: The Nature and Cleavage of Metal-Carbon Bonds. New York: John Wiley & Sons.
  7. ↑ Puddephatt, R. J.; Stalteri, M. A. (1980). "Competition between Insertion of Sulfur Dioxide into the Methyl– or Phenyl–Transition Metal Bond". J. Organomet. Chem. 193 (1): C27–C29. doi:10.1016/S0022-328X(00)86091-X.
  8. ↑ Klementyeva, Svetlana V.; Arleth, Nicholas; Meyer, Karsten; Konchenko, Sergey N.; Roesky, Peter W. (2015). "Dithionite and Sulfinate Complexes from the Reaction of SO2with Decamethylsamarocene". New Journal of Chemistry. 39 (10): 7589–7594. doi:10.1039/C5NJ00318K.
  9. ↑ Tennent, Norman H.; Su, Sophia R.; Poffenberger, Craig A.; Wojcicki, Andrew (1975). "Synthesis of a Transition Metal-Dithionite Complex, (η5-C5H5)(CO)2Fe-S(O)2S(O)2-Fe(CO)2(η5-C5H5)". Journal of Organometallic Chemistry. 102 (4): C46–C48. doi:10.1016/S0022-328X(00)89402-4.
  10. ↑ Hill, Anthony F. (1994). Organotransition Metallic Chemistry of Sulfur Dioxide Analogs. Advances in Organometallic Chemistry. Vol. 36. pp. 159–227. doi:10.1016/S0065-3055(08)60391-3. ISBN   9780120311361.
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