Thiophene

Thiophene

Names
IUPAC name Thiophene
Other names Thiofuran Thiacyclopentadiene Thiole
Identifiers
CAS Number	110-02-1
ChEBI	CHEBI:30856
ChEMBL	ChEMBL278958
ChemSpider	7739
Jmol 3D model	Interactive image
PubChem	8030
RTECS number	XM7350000
UNII	SMB37IQ40B
InChI InChI=1S/C4H4S/c1-2-4-5-3-1/h1-4H Key: YTPLMLYBLZKORZ-UHFFFAOYSA-N InChI=1/C4H4S/c1-2-4-5-3-1/h1-4H Key: YTPLMLYBLZKORZ-UHFFFAOYAY
SMILES c1ccsc1
Properties
Chemical formula	C4H4S
Molar mass	84.14 g/mol
Appearance	colorless liquid
Density	1.051 g/mL, liquid
Melting point	−38 °C (−36 °F; 235 K)
Boiling point	84 °C (183 °F; 357 K)
Refractive index (nD)	1.5287
Viscosity	0.8712 cP at 0.2 °C 0.6432 cP at 22.4 °C
Hazards
Safety data sheet	External MSDS, External MSDS
EU classification (DSD)	not listed
NFPA 704	3 2
Flash point	−1 °C (30 °F; 272 K)
Related compounds
Related thioethers	Tetrahydrothiophene Diethyl sulfide
Related compounds	Furan Pyrrole
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Thiophene, also commonly called thiofuran, is a heterocyclic compound with the formula C₄H₄S. Consisting of a flat five-membered ring, it is aromatic as indicated by its extensive substitution reactions. Related to thiophene are benzothiophene and dibenzothiophene, containing the thiophene ring fused with one and two benzene rings, respectively. Compounds analogous to thiophene include furan (C₄H₄O) and pyrrole (C₄H₄NH).

Isolation, occurrence

Thiophene was discovered as a contaminant in benzene.^[1] It was observed that isatin forms a blue dye if it is mixed with sulfuric acid and crude benzene. The formation of the blue indophenin was long believed to be a reaction with benzene. Victor Meyer was able to isolate the substance responsible for this reaction from benzene. This new heterocyclic compound was thiophene.^[2]

Thiophene and its derivatives occur in petroleum, sometimes in concentrations up to 1–3%. The thiophenic content of oil and coal is removed via the hydrodesulfurization (HDS) process. In HDS, the liquid or gaseous feed is passed over a form of molybdenum disulfide catalyst under a pressure of H₂. Thiophenes undergo hydrogenolysis to form hydrocarbons and hydrogen sulfide. Thus, thiophene itself is converted to butane and H₂S. More prevalent and more problematic in petroleum are benzothiophene and dibenzothiophene.

Synthesis and production

Reflecting their high stabilities, thiophenes arise from many reactions involving sulfur sources and hydrocarbons, especially unsaturated ones, e.g. acetylenes and elemental sulfur, which was the first synthesis of thiophene by Viktor Meyer in the year of its discovery. Thiophenes are classically prepared by the reaction of 1,4-diketones, diesters, or dicarboxylates with sulfidizing reagents such as P₄S₁₀ such as in the Paal-Knorr thiophene synthesis. Specialized thiophenes can be synthesized similarly using Lawesson's reagent as the sulfidizing agent, or via the Gewald reaction, which involves the condensation of two esters in the presence of elemental sulfur. Another method is the Volhard–Erdmann cyclization.

Thiophene is produced on a scale of around 2,000,000 kilograms per year worldwide. Production involves the vapor phase reaction of a sulfur source, typically carbon disulfide, and butanol. These reagents are contacted with an oxide catalyst at 500–550 °C.^[3]

Properties

At room temperature, thiophene is a colorless liquid with a mildly pleasant odor reminiscent of benzene, with which thiophene shares some similarities. The high reactivity of thiophene toward sulfonation is the basis for the separation of thiophene from benzene, which are difficult to separate by distillation due to their similar boiling points (4 °C difference at ambient pressure). Like benzene, thiophene forms an azeotrope with ethanol.

The molecule is flat; the bond angle at the sulphur is around 93°, the C–C–S angle is around 109°, and the other two carbons have a bond angle around 114°. The C–C bonds to the carbons adjacent to the sulphur are about 1.34 Å, the C–S bond length is around 1.70 Å, and the other C–C bond is about 1.41 Å (figures from the Cambridge Structural Database).

Reactivity

Thiophene is considered aromatic, although theoretical calculations suggest that the degree of aromaticity is less than that of benzene. The "electron pairs" on sulfur are significantly delocalized in the pi electron system. As a consequence of its aromaticity, thiophene does not exhibit the properties seen for conventional thioethers. For example the sulfur atom resists alkylation and oxidation. However, oxidation of a thiophene ring is thought to play a crucial role in the metabolic activation of various thiophene-containing drugs, such as tienilic acid and the investigational anticancer drug OSI-930. In these cases oxidation can occur both at sulfur, giving a thiophene S-oxide, as well as at the 2,3-double bond, giving the thiophene 2,3-epoxide, followed by subsequent NIH shift rearrangement.^{[4][5][6][7][8]}

Toward electrophiles

Although the sulfur atom is relatively unreactive, the flanking carbon centers, the 2- and 5-positions, are highly susceptible to attack by electrophiles. Halogens give initially 2-halo derivatives followed by 2,5-dihalothiophenes; perhalogenation is easily accomplished to give C₄X₄S (X = Cl, Br, I).^[9] Thiophene brominates 10⁷ times faster than does benzene.^[3]

Chloromethylation and chloroethylation occur readily at the 2,5-positions. Reduction of the chloromethyl product gives 2-methylthiophene. Hydrolysis followed by dehydration of the chloroethyl species gives 2-vinylthiophene.^[10][11]

Desulfurization by Raney nickel

Desulfurization of thiophene by Raney nickel

Desulfurization of thiophene with Raney nickel affords butane. When coupled with the easy 2,5-difunctionalization of thiophene, desulfurization provides a route to 1,4-disubstituted butanes.

Lithiation

Not only is thiophene reactive toward electrophiles, it is also readily lithiated with butyl lithium to give 2-lithiothiophene, which is a precursor to a variety of derivatives, including dithienyl.^[12]

Coordination chemistry

Thiophene exhibits little thioether-like character, but it does serve as a pi-ligand forming piano stool complexes such as Cr(η⁵-C₄H₄S)(CO)₃.^[13]

Uses

Thiophenes are important heterocyclic compounds that are widely used as building blocks in many agrochemicals and pharmaceuticals.^[3] The benzene ring of a biologically active compound may often be replaced by a thiophene without loss of activity.^[14] This is seen in examples such as the NSAID lornoxicam, the thiophene analog of piroxicam.

Polythiophene

The polymer formed by linking thiophene through its 2,5 positions is called polythiophene. Polythiophene itself has poor processing properties. More useful are polymers derived from thiophenes substituted at the 3- and 3- and 4- positions. Polythiophenes become electrically conductive upon partial oxidation, i.e. they become "organic metals."^[15]

References

1. Meyer, Viktor (1883). "Ueber den Begleiter des Benzols im Steinkohlenteer" [On a substance that accompanies benzene in coal tar]. Berichte der Deutschen chemischen Gesellschaft 16: 1465–1478. doi:10.1002/cber.188301601324.
2. Ward C., Sumpter (1944). "The Chemistry of Isatin". Chemical Reviews 34 (3): 393–434. doi:10.1021/cr60109a003.
3. Swanston, Jonathan (2006). "Thiophene". Ullmann’s Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a26_793.pub2..
4. Mansuy, D., Valadon, P., Erdelmeier, I., López García, P., Amar, C., Girault, J. P., and Dansette, P. M. (1991). "Thiophene S-oxides as new reactive metabolites: Formation by cytochrome-P450 dependent oxidation and reaction with nucleophiles". J. Am. Chem. Soc. 113 (20): 7825–7826. doi:10.1021/ja00020a089.
5. Treiber, A., Dansette, P. M., Amri, H. E., Girault, J.-P., Ginderow, D., Mornon, J.-P., Mansuy, D.; Dansette; El Amri; Girault; Ginderow; Mornon; Mansuy (1997). "Chemical and Biological Oxidation of Thiophene:  Preparation and Complete Characterization of Thiophene S-Oxide Dimers and Evidence for Thiophene S-Oxide as an Intermediate in Thiophene Metabolism in Vivo and in Vitro". J. Am. Chem. Soc. 119 (7): 1565–1571. doi:10.1021/ja962466g.
6. Rademacher P. M., Woods C. M., Huang Q., Szklarz G. D., Nelson S. D.; Woods; Huang; Szklarz; Nelson (2012). "Differential Oxidation of Two Thiophene-Containing Regioisomers to Reactive Metabolites by Cytochrome P450 2C9". Chem. Res. Toxicol. 25 (4): 895–903. doi:10.1021/tx200519d. PMC 3339269. PMID 22329513.
7. Mansuy D., Dansette P. M.; Dansette (2011). "Sulfenic acids as reactive intermediates in xenobiotic metabolism". Archives of Biochemistry and Biophysics 507 (1): 174–185. doi:10.1016/j.abb.2010.09.015. PMID 20869346.
8. Dansette, PM, Rosi, J, Debernardi, J, Bertho G, Mansuy D; Rosi; Debernardi; Bertho; Mansuy (2012). "Metabolic Activation of Prasugrel: Nature of the Two Competitive Pathways Resulting in the Opening of Its Thiophene Ring". Chem. Res. Toxicol. 25 (5): 1058–1065. doi:10.1021/tx3000279.
9. Henry Y. Lew and C. R. Noller (1963). "2-Iodolthiophene". Org. Synth.; Coll. Vol. 4, p. 545
10. W. S. Emerson and T. M. Patrick, Jr. (1963). "2-Vinylthiophene". Org. Synth.; Coll. Vol. 4, p. 980
11. K. B. Wiberg and H. F. McShane (1955). "2-Chloromethylthiophene". Org. Synth.; Coll. Vol. 3, p. 1
12. E. Jones and I. M. Moodie (1988). "2-Thiophenethiol". Org. Synth.; Coll. Vol. 6, p. 979
13. Rauchfuss, T. B., "The Coordination Chemistry of Thiophenes", Progress in Inorganic Chemistry 1991, volume 39, pp. 259-311. ISBN 978-0-471-54489-0
14. Daniel Lednicer (1999). The Organic Chemistry of Drug Synthesis 6. New York: Wiley Interscience. p. 187. ISBN 0-471-24510-0.
15. J. Roncali (1992). "Conjugated poly(thiophenes): synthesis, functionalization, and applications". Chem. Rev. 92 (4): 711–738. doi:10.1021/cr00012a009.

External links

• International Chemical Safety Card 1190
•  Chisholm, Hugh, ed. (1911). "Thiophen". Encyclopædia Britannica 26 (11th ed.). Cambridge University Press.