Tetrathiafulvalene

Tetrathiafulvalene
Names
	Preferred IUPAC name 2,2′-Bi(1,3-dithiolylidene)
	Other names Δ2,2-Bi-1,3-dithiole
Identifiers
CAS Number	31366-25-3 ;
3D model (JSmol)	Interactive image;
Beilstein Reference	1282106
ChEBI	CHEBI:52444 ;
ChemSpider	89848 ;
ECHA InfoCard	100.045.979
EC Number	250-593-7;
PubChem CID	99451;
UNII	HY1EN16W9T ;
CompTox Dashboard (EPA)	DTXSID6067620 ;
	InChI InChI=1S/C6H4S4/c1-2-8-5(7-1)6-9-3-4-10-6/h1-4H Key: FHCPAXDKURNIOZ-UHFFFAOYSA-N ; InChI=1/C6H4S4/c1-2-8-5(7-1)6-9-3-4-10-6/h1-4H Key: FHCPAXDKURNIOZ-UHFFFAOYAZ;
	SMILES S1C=CSC1=C2SC=CS2;
Properties
Chemical formula	C6H4S4
Molar mass	204.34 g·mol−1
Appearance	Yellow solid
Melting point	116 to 119 °C (241 to 246 °F; 389 to 392 K)
Boiling point	Decomposes
Solubility in water	Insoluble
Solubility in organic solvents	Soluble[vague]
Structure
Dipole moment	0 D
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	combustible
	GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H317
Precautionary statements	P261, P280, P302+P352, P333+P313, P363, P501
Related compounds
Related compounds	TCNQ; Thiophene; Tetracyanoethylene;
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Tetrathiafulvalene (TTF) is an organosulfur compound with the formula (C₃H₂S₂)₂. Studies on this heterocyclic compound contributed to the development of molecular electronics. TTF is related to the hydrocarbon fulvalene, (C₅H₄)₂, by replacement of four CH groups with sulfur atoms. Over 10,000 scientific publications discuss TTF and its derivatives.^[2]

Preparation

The high level of interest in TTFs has spawned the development of many syntheses of TTF and its analogues.^[2] Most preparations entail the coupling of cyclic C₃S₂ building blocks such as 1,3-dithiole-2-thion or the related 1,3-dithiole-2-ones. For TTF itself, the synthesis begins with the cyclic trithiocarbonate H₂C₂S₂C=S (1,3-dithiole-2-thione), which is S-methylated and then reduced to give H₂C₂S₂CH(SCH₃) (1,3-dithiole-2-yl methyl thioether), which is treated as follows:^[3]

H₂C₂S₂CH(SCH₃) + H[BF₄] → [H₂C₂S₂CH]⁺[BF₄]⁻ + CH₃SH

2 [H₂C₂S₂CH]⁺[BF₄]⁻ + 2 N(CH₂CH₃)₃ → (H₂C₂S₂C)₂ + 2 [NH(CH₂CH₃)₃]⁺[BF₄]⁻

Redox properties

Bulk TTF itself has unremarkable electrical properties. Distinctive properties are, however, associated with salts of its oxidized derivatives, such as salts derived from TTF⁺.

The high electrical conductivity of TTF salts can be attributed to the following features of TTF:

its planarity, which allows π-π stacking of its oxidized derivatives,
its high symmetry, which promotes charge delocalization, thereby minimizing coulombic repulsions, and
its ability to undergo oxidation at mild potentials to give a stable radical cation. Electrochemical measurements show that TTF can be oxidized twice reversibly:

TTF → TTF⁺ + e⁻ (E = 0.34 V)

TTF⁺ → TTF²⁺ + e⁻ (E = 0.78 V, vs. Ag/AgCl in CH₃CN solution)

Each dithiolylidene ring in TTF has 7π electrons: 2 for each sulfur atom, 1 for each sp² carbon atom. Thus, oxidation converts each ring to an aromatic 6π-electron configuration, consequently leaving the central double bond essentially a single bond, as all π-electrons occupy ring orbitals.

History

Edge-on view of portion of crystal structure of hexamethyleneTTF/TCNQ charge transfer salt, highlighting the segregated stacking.^[4]

The salt [TTF⁺
]Cl⁻
was reported to be a semiconductor in 1972.^[5] Subsequently, the charge-transfer salt [TTF]TCNQ was shown to be a narrow band gap semiconductor.^[6] X-ray diffraction studies of [TTF][TCNQ] revealed stacks of partially oxidized TTF molecules adjacent to anionic stacks of TCNQ molecules. This "segregated stack" motif was unexpected and is responsible for the distinctive electrical properties, i.e. high and anisotropic electrical conductivity. Since these early discoveries, numerous analogues of TTF have been prepared. Well studied analogues include tetramethyltetrathiafulvalene (Me₄TTF), tetramethylselenafulvalenes (TMTSFs), and bis(ethylenedithio)tetrathiafulvalene (BEDT-TTF, CAS [66946-48-3]).^[7] Several tetramethyltetrathiafulvalene salts (called Fabre salts) are of some relevance as organic superconductors.

References

^ "Tetrathiafulvalene". pubchem.ncbi.nlm.nih.gov.
^ ^a ^b Bendikov, M; Wudl, F; Perepichka, D F (2004). "Tetrathiafulvalenes, Oligoacenenes, and Their Buckminsterfullerene Derivatives: The Brick and Mortar of Organic Electronics". Chemical Reviews. 104 (11): 4891–4945. doi:10.1021/cr030666m. PMID 15535637.
^ Wudl, F.; Kaplan, M. L. (1979). "2,2′-Bi-L,3-Dithiolylidene (Tetrathiafulvalene, TTF) and its Radical Cation Salts". Inorganic Syntheses. Vol. 19. pp. 27–30. doi:10.1002/9780470132500.ch7. ISBN 978-0-470-13250-0. {{cite book}}: |journal= ignored (help)
^ D. Chasseau; G. Comberton; J. Gaultier; C. Hauw (1978). "Réexamen de la structure du complexe hexaméthylène-tétrathiafulvalène-tétracyanoquinodiméthane". Acta Crystallographica Section B. 34 (2): 689. Bibcode:1978AcCrB..34..689C. doi:10.1107/S0567740878003830.
^ Wudl, F.; Wobschall, D.; Hufnagel, E. J. (1972). "Electrical Conductivity by the Bis(1,3-dithiole)-bis(1,3-dithiolium) System". J. Am. Chem. Soc. 94 (2): 670–672. doi:10.1021/ja00757a079.
^ Ferraris, J.; Cowan, D. O.; Walatka, V. V. Jr.; Perlstein, J. H. (1973). "Electron transfer in a new highly conducting donor-acceptor complex". J. Am. Chem. Soc. 95 (3): 948–949. doi:10.1021/ja00784a066.
^ Larsen, J.; Lenoir, C. (1998). "2,2'-Bi-5,6-Dihydro-1,3-Dithiolo[4,5-b][1,4]dithiinylidene (BEDT-TTF)". Organic Syntheses{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 9, p. 72.

Tetrathiafulvalene

Preparation

Redox properties

History

See also

References

Further reading