Disulfidobis(tricarbonyliron): Difference between revisions
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== Synthesis and properties == |
== Synthesis and properties == |
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The synthesis of Fe<sub>2</sub>(μ-S<sub>2</sub>)(CO)<sub>6</sub> was first reported in 1958 from [[iron pentacarbonyl]] and [[sodium polysulfide]].<ref name="onlinelibrary.wiley.com">{{Cite journal |last1=Hieber |first1=W. |last2=Gruber |first2=J. |date=August 1958 |title=Zur Kenntnis der Eisencarbonylchalkogenide |url=https://onlinelibrary.wiley.com/doi/10.1002/zaac.19582960111 |journal=Zeitschrift für anorganische und allgemeine Chemie |language= |
The synthesis of Fe<sub>2</sub>(μ-S<sub>2</sub>)(CO)<sub>6</sub> was first reported in 1958 from [[iron pentacarbonyl]] and [[sodium polysulfide]].<ref name="onlinelibrary.wiley.com">{{Cite journal |last1=Hieber |first1=W. |last2=Gruber |first2=J. |date=August 1958 |title=Zur Kenntnis der Eisencarbonylchalkogenide |url=https://onlinelibrary.wiley.com/doi/10.1002/zaac.19582960111 |journal=Zeitschrift für anorganische und allgemeine Chemie |language=de |volume=296 |issue=1–6 |pages=91–103 |doi=10.1002/zaac.19582960111 |issn=0044-2313}}</ref> |
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[[File:Original synthesis of Fe2S2(CO)6.png|frameless|493x493px]] |
[[File:Original synthesis of Fe2S2(CO)6.png|frameless|493x493px]] |
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Revision as of 17:24, 26 March 2024
6.png)
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| Names | |
|---|---|
| Systematic IUPAC name
μ-η2:η2-disulfido-bis(tricarbonyliron) | |
| Identifiers | |
| Structure | |
| P1, No. 2 | |
a = 6.538, b = 7.743, c = 11.413 α = 83.87°, β = 75.66°, γ = 78.73°[1]
| |
Lattice volume (V)
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547.942 |
| octahedral at Fe | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Disulfidobis(tricarbonyliron), or Fe2(μ-S2)(CO)6, is an organometallic molecule used as a precursor in the synthesis of iron-sulfur compounds. Popularized as a synthetic building block by Dietmar Seyferth, Fe2(μ-S2)(CO)6 is commonly used to make mimics of the H-cluster in [FeFe]-hydrogenase.[2] Much of the reactivity of Fe2(μ-S2)(CO)6 proceeds through its sulfur-centered dianion, [Fe2(μ-S)2(CO)2]2-.
Synthesis and properties
The synthesis of Fe2(μ-S2)(CO)6 was first reported in 1958 from iron pentacarbonyl and sodium polysulfide.[3]
6.png)
The vibrant red, air-stable product is formed alongside Fe3S2(CO)9.[4] The molecule has an Fe2S2 core with a distorted tetrahedron shape. The compound sublimes at 40 °C, melts at 46.5 °C, and decomposes at 70 °C.[4] Fe2(μ-S2)(CO)6 has three peaks in its infrared spectrum corresponding to three distinct carbonyl stretching frequencies, indicating that the carbonyl ligands are inequivalent.[3] There are multiple peaks in the ultraviolet-visible spectrum, with a peak at 449 nm corresponding to a metal-to-ligand charge transfer band.[5] The dianion [Fe2(μ-S)2(CO)2]2- is most easily prepared by reduction of Fe2(μ-S2)(CO)6 with LiBEt3H, also known as Super-Hydride.[6]
In the neutral cluster, the sulfur atoms are bound to each other, forming a disulfide ligand. In the sulfur-centered dianion, the sulfur-sulfur bond is broken, forming two anionic sulfide ligands. Therefore, the bridging unit in the neutral cluster is a S22- ligand, while the bridging unit in the dianion is a single S2- ion.
Studies of the coupling between iron-57 and carbon-13 atoms in carbon-13 NMR spectroscopy indicate rapid intermolecular exchange of carbonyl ligands between clusters.[7]
Structure and bonding
The crystal structure of Fe2(μ-S2)(CO)6 was first reported in 1965.[8] The Fe2S2 core forms a tetrahedron, though calculations show that the 'butterfly' structure with a broken S–S bond and diradical character is not substantially higher in energy.[5][9] Seeking to explain the compound's diamagnetism, both an iron–iron and a sulfur–sulfur bond were proposed. In early works, to comport with a d2sp3 hybrid orbital interpretation of the bonding in octahedral metal complexes, the metal–metal bond was proposed to be "bent." However, the directionality of this bond faced some controversy.[10] With the advent of computational chemistry programs such as density functional theory (DFT) and the quantum theory of atoms in molecules (QTAIM), this bond and its topology have been thoroughly investigated, and some calculations support a nonlinear iron–iron bond.[5][10][11] However, these calculations indicate that the bond angle is likely closer to 15° than the 130° originally proposed.[10]
Computational work indicates that the highest occupied molecular orbital (HOMO) of the compound is Fe–Fe bonding in nature and substantially delocalized, while the lowest unoccupied molecular orbital (LUMO) is a localized S–S sigma bond. Much of the sulfur-centered reactivity of this compound can thus be understood in terms of frontier orbital theory.[5]
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6_LUMO.png)
Reactivity
The Fe2(μ-S2)(CO)6 molecule is a useful synthetic precursor to a variety of Fe–S multinuclear compounds. Reactivity frequently begins with reductive cleavage of the sulfur–sulfur bond to [Fe2(μ-S)2(CO)2]2-, though syntheses directly from the neutral cluster are also known.
Reactivity through the dianion
The first step in many reactions with Fe2(μ-S2)(CO)6 is reduction to the dianion, which is easily performed with lithium triethylborohydride.[6]
6.png)
The resulting dianion can then be reacted with a dihaloalkane to form a cyclic alkane thiolate.[12] Cyclic alkane thiolates have been used as precursors to active catalysts for electrocatalytic hydrogen evolution, which can be considered a model reaction for the all-iron hydrogenase.[13]
The dianion can also be treated with two different haloalkanes to form an asymmetric alkylated species.[2]
In addition to electrophilic organic reagents, [Fe2(μ-S)2(CO)2]2- can be treated with inorganic or organometallic reagents to insert a variety of heterometals.[4][14]
Reactivity directly from the neutral compound
The neutral compound is electrophilic at the sulfur–sulfur bond, meaning that it can be treated with carbanionic reagents (for example, Grignard or organolithium reagents). Use of carbanionic reagents (RM) allows for asymmetric functionalization of the two sulfur atoms.
Reactivity mimicking that of the dianion can be achieved directly from the neutral species through photochemistry. Fe2(μ-S2)(CO)6 absorbs light at 450 nm, corresponding to a metal-to-ligand charge transfer (MLCT) from the Fe-centered HOMO to the S-centered LUMO. As the HOMO is bonding with respect to the Fe–Fe bond, and the LUMO is antibonding with respect to the S–S bond, promotion of an electron from the HOMO to the LUMO weakens both bonds. This can be treated as reduction of the sulfur bridge by the iron core.
Temporary sulfur-centered dianion character allows the formally neutral molecule to perform oxidative addition reactions with organic small molecules:[5][15]
Reactivity through the dithiol derivative
Synthetic models of the H-cluster of the all-iron hydrogenase have been synthesized. Treating the dianion [Fe2(μ-S)2(CO)2]2- with trifluoroacetic acid produces the dithiol derivative Fe2(μ-SH)2(CO)6, which can then be reacted with ammonium carbonate in paraformaldehyde to form a structural model of the H-cluster.[14]
Precatalyst for electrocatalytic H2 production
In addition to structural mimics of the H-cluster, work has been done to model the reactivity of the all-Fe hydrogenase. The cyclic propyl thiolate cluster derived from Fe2(μ-S2)(CO)6 (see above) acts as a precatalyst, and when treated with acid in an electrolysis cell, hydrogen gas is produced.[13] As a result, this system can be used as a model to better understand the mechanism of hydrogen production in the all-Fe hydrogenase.
Applications beyond chemical synthesis
The synthesis of Fe2(μ-S2)(CO)6 has been proposed as an educational experiment in upper-level undergraduate inorganic laboratory courses.[16]
References
- ^ doi.org/10.1021/om2011744
- ^ a b Li, Yulong; Rauchfuss, Thomas B. (2016-06-22). "Synthesis of Diiron(I) Dithiolato Carbonyl Complexes". Chemical Reviews. 116 (12): 7043–7077. doi:10.1021/acs.chemrev.5b00669. ISSN 0009-2665. PMC 4933964. PMID 27258046.
- ^ a b Hieber, W.; Gruber, J. (August 1958). "Zur Kenntnis der Eisencarbonylchalkogenide". Zeitschrift für anorganische und allgemeine Chemie (in German). 296 (1–6): 91–103. doi:10.1002/zaac.19582960111. ISSN 0044-2313.
- ^ a b c Seyferth, Dietmar; Henderson, Richard S.; Song, Li Cheng (January 1982). "Chemistry of .mu.-dithio-bis(tricarbonyliron), a mimic of organic disulfides. 1. Formation of di-.mu.-thiolate-bis(tricarbonyliron) dianion". Organometallics. 1 (1): 125–133. doi:10.1021/om00061a022. ISSN 0276-7333.
- ^ a b c d e Bertini, Luca; Fantucci, Piercarlo; De Gioia, Luca (2011-02-14). "On the Photochemistry of the Low-Lying Excited State of Fe 2 (CO) 6 S 2 . A DFT and QTAIM Investigation". Organometallics. 30 (3): 487–498. doi:10.1021/om100799z. ISSN 0276-7333.
- ^ a b Seyferth, Dietmar; Henderson, Richard S; Song, Li-Cheng (June 1980). "The dithiobis(tricarbonyliron) dianion: Improved preparation and new chemistry". Journal of Organometallic Chemistry. 192 (1): C1–C5. doi:10.1016/S0022-328X(00)93341-2.
- ^ Aime, Silvio; Osella, Domenico (July 1981). "Iron-57 satellites in 13C NMR spectra: an aid to elucidation of "hidden-processes" in the dynamics of metal carbonyls". Journal of Organometallic Chemistry. 214 (2): C27–C30. doi:10.1016/S0022-328X(00)86637-1.
- ^ Wei, Chin Hsuan; Dahl, Lawrence F. (January 1965). "The Molecular Structure of a Tricyclic Complex, [SFe(CO) 3 ] 2". Inorganic Chemistry. 4 (1): 1–11. doi:10.1021/ic50023a001. ISSN 0020-1669.
- ^ Arrigoni, Federica; Zampella, Giuseppe; Zhang, Fanjun; Kagalwala, Husain N.; Li, Qian-Li; Woods, Toby J.; Rauchfuss, Thomas B. (2021-03-15). "Computational and Experimental Investigations of the Fe 2 (μ-S 2 )/Fe 2 (μ-S) 2 Equilibrium". Inorganic Chemistry. 60 (6): 3917–3926. doi:10.1021/acs.inorgchem.0c03709. ISSN 0020-1669. PMC 8100967. PMID 33650855.
- ^ a b c Hall, Michael B.; Fenske, Richard F.; Dahl, Lawrence F. (1975-12-01). "Nonparameterized molecular orbital calculations of ligand-bridge Fe2(CO)6X2-type dimers containing metal-metal interactions". Inorganic Chemistry. 14 (12): 3103–3117. doi:10.1021/ic50154a048. ISSN 0020-1669.
- ^ Farrugia, Louis J.; Evans, Cameron; Senn, Hans Martin; Hänninen, Mikko M.; Sillanpää, Reijo (2012-04-09). "QTAIM View of Metal–Metal Bonding in Di- and Trinuclear Disulfido Carbonyl Clusters". Organometallics. 31 (7): 2559–2570. doi:10.1021/om2011744. ISSN 0276-7333.
- ^ Kambe, N., ed. (2008). Category 5, Compounds with One Saturated Carbon Heteroatom Bond: Sulfur, Selenium, and Tellurium (1 ed.). Stuttgart: Georg Thieme Verlag. doi:10.1055/b-003-125755. ISBN 978-3-13-118921-9.
- ^ a b Gloaguen, Frédéric; Lawrence, Joshua D.; Rauchfuss, Thomas B. (2001-09-01). "Biomimetic Hydrogen Evolution Catalyzed by an Iron Carbonyl Thiolate". Journal of the American Chemical Society. 123 (38): 9476–9477. doi:10.1021/ja016516f. ISSN 0002-7863. PMID 11562244.
- ^ a b Song, Li-Cheng (2005-01-01). "Investigations on Butterfly Fe/S Cluster S-Centered Anions ( μ -S - ) 2 Fe 2 (CO) 6 , ( μ -S - )( μ -RS)Fe 2 (CO) 6 , and Related Species". Accounts of Chemical Research. 38 (1): 21–28. doi:10.1021/ar030004j. ISSN 0001-4842. PMID 15654733.
- ^ King, R.B; Bitterwolf, T.E (September 2000). "Metal carbonyl analogues of iron–sulfur clusters found in metalloenzyme chemistry". Coordination Chemistry Reviews. 206–207: 563–579. doi:10.1016/S0010-8545(99)00251-9.
- ^ Barrett, Jacob; Spentzos, Ariana; Works, Carmen (2015-04-14). "An Advanced Organometallic Lab Experiment with Biological Implications: Synthesis and Characterization of Fe 2 (μ-S 2 )(CO) 6". Journal of Chemical Education. 92 (4): 719–722. Bibcode:2015JChEd..92..719B. doi:10.1021/ed500393j. ISSN 0021-9584.