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Iron–sulfur cluster - Wikipedia

From Wikipedia, the free encyclopedia

Molecular structures and ubiquitous inorganic cofactors found in all domains of life

Structure of [Fe4S4(SMe)4]2−, a synthetic analogue of 4Fe–4S cofactors.[1]

Iron–sulfur clusters are molecular ensembles of iron and sulfide. They are most often discussed in the context of the biological role for iron–sulfur proteins, which are pervasive.[2] Many Fe–S clusters are known in the area of organometallic chemistry and as precursors to synthetic analogues of the biological clusters. It is supposed that the last universal common ancestor had many iron-sulfur clusters.[3]

Iron–sulfur clusters occur in many biological systems, often as components of electron transfer proteins. The ferredoxin proteins are the most common Fe–S proteins in nature. They feature either 2Fe–2S or 4Fe–4S centers. They occur in all branches of life.[4]

Fe–S clusters can be classified according to their Fe:S stoichiometry [2Fe–2S], [4Fe–3S], [3Fe–4S], and [4Fe–4S].[5] The [4Fe–4S] clusters occur in two forms: normal ferredoxins and high potential iron proteins (HiPIP). Both adopt cuboidal structures, but they utilize different oxidation states. They are found in all forms of life.[6]

The relevant redox couple in all Fe–S proteins is Fe(II)/Fe(III).[6]

Many clusters have been synthesized in the laboratory with the formula [Fe4S4(SR)4]2−, which are known for many R substituents, and with many cations. Variations have been prepared including the incomplete cubanes [Fe3S4(SR)3]3−.[7]

Synthetic Fe–S clusters[edit]

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(May 2025) Organometallic clusters[edit]

Organometallic Fe–S clusters include the sulfido carbonyls with the formula Fe2S2(CO)6, H2Fe3S(CO)9, and Fe3S2(CO)9. Compounds are also known that incorporate cyclopentadienyl ligands, such as (C5H5)4Fe4S4.[8]

Figure. Illustrative synthetic Fe–S clusters. From left to right: Fe3S2(CO)9, [Fe3S(CO)9]2−, (C5H5)4Fe4S4, and [Fe4S4Cl4]2−. Inorganic materials[edit]

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(November 2022) Structure of potassium dithioferrate, which features infinite chains of Fe(III) centers.
  1. ^ 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.
  2. ^ Lippard, S. J. and Berg, J. M. (1994). "Principles of Bioinorganic Chemistry". University Science Books: Mill Valley, CA. ISBN 0-935702-73-3.
  3. ^ Weiss, Madeline C., et al. (2016). "The physiology and habitat of the last universal common ancestor." Nature Microbiology 1 (9): 1–8.
  4. ^ Johnson, D. C.; Dean, D. R.; Smith, A. D.; Johnson, M. K. (2005). "Structure, function, and formation of biological iron-sulfur clusters". Annual Review of Biochemistry. 74 (1): 247–281. doi:10.1146/annurev.biochem.74.082803.133518. PMID 15952888.
  5. ^ Lill, Roland (2015). "Issue of iron-sulfur protein". Biochimica et Biophysica Acta (BBA) - Molecular Cell Research. 1853 (6): 1251–1252. doi:10.1016/j.bbamcr.2015.03.001. PMC 5501863. PMID 25746719.
  6. ^ a b Fisher, N (1998). "Intramolecular electron transfer in [4Fe–4S)]". The EMBO Journal: 849–858.
  7. ^ Rao, P. V.; Holm, R. H. (2004). "Synthetic Analogues of the Active Sites of Iron-Sulfur Proteins". Chem. Rev. 104 (2): 527─559. doi:10.1021/Cr020615+. PMID 14871134.
  8. ^ Ogino, H.; Inomata, S.; Tobita, H. (1998). "Abiological Iron-Sulfur Clusters". Chem. Rev. 98 (6): 2093–2122. doi:10.1021/cr940081f. PMID 11848961.

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