Iron–sulfur cluster
Molecular structures and ubiquitous inorganic cofactors found in all domains of life
From Wikipedia, the free encyclopedia
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]
In biology
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
Synthetic Fe–S clusters are laboratory-prepared coordination compounds or chains, often designed to mimic the structural, electronic, or chemical properties of biological Fe–S clusters.
Roussin's black anion, [Fe4S3(NO)7]−, described in 1858, is the first synthetic Fe-S cluster.[8] It has the geometry of an incomplete cubane-type cluster with C3v symmetry. The dark color of the complex is attributed to a number of charge-transfer interactions.[9] Since the 1970s, many of these Fe-S clusters have been described.[10][11] A key property of Fe–S clusters is their ability to undergo redox.
Organometallic clusters
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.[12]
Inorganic materials
In maquettes and artificial proteins
It is possible to incorporate Fe–S clusters into maquettes (smaller minimal functional proteins designed from biological proteins) and artificial proteins, often abbreviated to MAPs. The first examples of Fe–S MAPs emerged in the early 1970s, as a means to mimic naturally occurring iron-containing proteins like rubredoxins. These contained [Fe(S-Cys)4] motifs.[10] Further research into [4Fe–4S] MAPs has led to the development of ambidoxins: de novo maquettes that consist of 12 residues with the sequence X-Cys-X2-Cys-X2-Cys-X2-Cys-X (X = Arg, Lys), which can successfully perform hundreds of redox cycles. However, Fe–S MAPs are limited by their lower solubility and exposed Fe–S cluster core that is susceptible to degradation by solvents.[10][11][13]