Biology:Transition metal thiolate complex

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Transition metal thiolate complexes are metal complexes containing thiolate ligands. Thiolates are ligands that can be classified as soft Lewis bases. Therefore, thiolate ligands coordinate most strongly to metals that behave as soft Lewis acids as opposed to those that behave as hard Lewis acids. Most complexes contain other ligands in addition to thiolate, but many homoleptic complexes are known with only thiolate ligands. The amino acid cysteine has a thiol functional group, consequently many cofactors in proteins and enzymes feature cysteinate-metal cofactors.[1]

The zinc finger motif, which is found in transcription factors, is a metal thiolate complex.
Structure of [Fe4S4(SMe)4]2−, a synthetic analogue of 4Fe-4S cofactors.[2]

Synthesis

Metal thiolate complexes are commonly prepared by reactions of metal complexes with thiols (RSH), thiolates (RS−), and disulfides (R2S2). The salt metathesis reaction route is common. In this method, an alkali metal thiolate is treated with a transition metal halide to produce an alkali metal halide and the metal thiolate complex:

LiSC6H5 + CuI → Cu(SC6H5) + LiI

Lithium tert-butylthiolate reacts with MoCl4 to give the tetrathiolate complex:[3]

MoCl4 + 4 t-BuSLi → Mo(t-BuS)4 + 4 LiCl

Mo(t-BuS)4 is a dark red diamagnetic complex that is sensitive to air and moisture. The molybdenum center has a distorted tetrahedral coordination to four sulfur atoms, with overall D2 symmetry.[3]

Mo(t-BuS)4.

Nickelocene and ethanethiol give a dimeric thiolate, one cyclopentadienyl ligand serving as a base:

2 HSC2H5 + 2 Ni(C5H5)2 → [Ni(SC2H5)(C5H5)]2 + 2 C5H6
Thiomersal, a disinfectant, is a metal thiolate complex, being derived from Hg(II) and thiosalicylic acid.

Regarding their mechanism of formation from thiols, metal thiolate complexes can arise via deprotonation of thiol complexes.[4][5]

Redox routes

Many thiolate complexes are prepared by redox reactions. Organic disulfides oxidize low valence metals, as illustrated by the oxidation of titanocene dicarbonyl:

(C
5H
5)
2Ti(CO)
2 + (C
6H
5S)
2 → (C
5H
5)
2Ti(SC
6H
5)
2 + 2 CO

Some metal centers are oxidized by thiols, the coproduct being hydrogen gas:

Fe
3(CO)
12 + 2 C
2H
5SH → Fe
2(SC
2H
5)
2(CO)
6 + Fe(CO)
5 + CO + H
2

These reactions may proceed by the oxidative addition of the thiol to Fe(0).

Thiols and especially thiolate salts are reducing agents. Consequently, they induce redox reactions with certain transition metals. This phenomenon is illustrated by the synthesis of cuprous thiolates from cupric precursors:

4 HSC6H5 + 2 CuO → 2 Cu(SC6H5) + (C6H5S)2 + 2 H2O

Thiolate clusters of the type [Fe4S4(SR)4]2− occur in iron–sulfur proteins. Synthetic analogues can be prepared by combined redox and salt metathesis reactions:[6]

4 FeCl3 + 6 NaSR + 6 NaSH → Na2[Fe4S4(SR)4] + 10 NaCl + 4 HCl + H2S + R2S2

Structure

Divalent sulfur exhibits bond angles approaching 90°. Such acute angles are also seen in the M-S-C angles of metal thiolates. Having filled p-orbitals of suitable symmetry, thiolates are pi-donor ligands. This property plays a role in the stabilization of Fe(IV) states in the enzyme cytochrome P450.

Structure of the quasi-two-coordinate ferrous dithiolate Fe[SC6H3-2,6-(C6H2-2,4,6-(iPr)3)2]2. A weak Fe-C(ipso) bond is indicated by the Fe---C distance of 2.427(1) Å. The structure illustrates the low coordination numbers enabled by bulky ligands.[7]

Reactions

Thiolates are relatively basic ligands, being derived from conjugate acids with pKa's of 6.5 (thiophenol) to 10.5 (butanethiol). Consequently, thiolate ligand often bridge pairs of metals. One example is Fe2(SCH3)2(CO)6. Thiolate ligands, especially when nonbridging, are susceptible to attack by electrophiles including acids, alkylating agents, and oxidants.

Structure of Fe2(SCH3)2(CO)6.

Occurrence and applications

Metal thiolate functionality is pervasive in metalloenzymes. Iron-sulfur proteins, blue copper proteins, and the zinc-containing enzyme liver alcohol dehydrogenase feature thiolate ligands. Commonly thiolate is ligand is provided from the cysteine residue. All molybdoproteins feature thiolates in the form of cysteinyl and/or molybdopterin.[8] thumb|The copper site in plastocyanin features two [[imidazole, a thioether, and a thiolate ligand.]]

References

  1. ↑ Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5 
  2. ↑ Axel Kern; Christian Näther; Felix Studt; Felix Tuczek (2004). "Application of a Universal Force Field to Mixed Fe/Mo−S/Se Cubane and Heterocubane Clusters. 1. Substitution of Sulfur by Selenium in the Series [Fe4X4(YCH3)4]2-; X = S/Se and Y = S/Se". Inorg. Chem. 43 (16): 5003–5010. doi:10.1021/ic030347d. PMID 15285677. 
  3. ↑ 3.0 3.1 Otsuka, Sei; Kamata, Masato; Hirotsu, Ken; Higuchi, Taiichi (1981). "A Novel Molybdenum Thiolato Compound, Tetrakis(tert-butylthiolato)molybdenum(IV). Preparation and Crystal and Molecular Structure". Journal of the American Chemical Society 103 (11): 3011–3014. doi:10.1021/ja00401a017. 
  4. ↑ Jessop, Philip G.; Morris, Robert H. (1993). "Hydrogen/Deuterium exchange reactions of an iridium dithiol complex". Inorganic Chemistry 32 (11): 2236–2237. doi:10.1021/ic00063a006. 
  5. ↑ Heller, M.; Sheldrick, W. S. (2004). "Copper(I) Coordination Polymers with Alkanedithiol and -dinitrile Bridging Ligands". Zeitschrift für anorganische und allgemeine Chemie 630 (12): 1869–1874. doi:10.1002/zaac.200400165. 
  6. ↑ Lee, S. C.; Lo, W.; Holm, R. H. (2014). "Developments in the Biomimetic Chemistry of Cubane-Type and Higher Nuclearity Iron–Sulfur Clusters". Chemical Reviews 114 (7): 3579–3600. doi:10.1021/cr4004067. PMID 24410527. 
  7. ↑ Nguyen, T.; Panda, A.; Olmstead, M. M.; Richards, A. F.; Stender, M.; Brynda, M.; Power, P. P. (2005). "Synthesis and Characterization of Quasi-Two-Coordinate Transition Metal Dithiolates M(SAr)2 (M = Cr, Mn, Fe, Co, Ni, Zn; Ar = C6H3-2,6(C6H2-2,4,6-Pri3)2).". J. Am. Chem. Soc. 127 (23): 8545–8552. doi:10.1021/ja042958q. PMID 15941290. 
  8. ↑ S. J. Lippard, J. M. Berg "Principles of Bioinorganic Chemistry" University Science Books: Mill Valley, CA; 1994. ISBN:0-935702-73-3.



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