Disulfur
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| Names | |
|---|---|
| IUPAC name
Disulfur
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| Other names
Diatomic sulfur
Sulfur | |
| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| 753 | |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| S2 | |
| Molar mass | 64.12 g·mol−1 |
| 0 D | |
| Thermochemistry | |
Heat capacity (C)
|
32.51 kJ K−1 mol−1 |
Std molar
entropy (S⦵298) |
228.17 J K−1 mol−1 |
Std enthalpy of
formation (ΔfH⦵298) |
128.60 kJ mol−1 |
| Related compounds | |
Related compounds
|
Triplet oxygen |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Disulfur is the diatomic molecule with the formula S2.[1] It is analogous to the dioxygen molecule but rarely occurs at room temperature. This violet gas is the dominant species in hot sulfur vapors. S2 is one of the minor components of the atmosphere of Io, which is predominantly composed of SO2.[2] The instability of S2 is usually described in the context of the double bond rule.
Synthesis
This violet gas is generated by heating sulfur above 720 °C, comprising 99% of the vapor at low pressure (1 mm Hg) at 530 °C.
Disulfur can be produced when an atmosphere of COS is irradiated with UV light using a mercury photosensitizer or when CS2, H2S2, S2Cl2 or C2H4S, PSF3 or COS are irradiated.[3]
Natural occurrence
Gaseous disulfur has been detected emanating from the surface of Jupiter's moon Io, from the vicinity of Pele volcano.[4]
Properties
The ground state of S2 is a triplet: it is a diradical, with two unpaired electrons) like O2 and SO. It has the S-S bond length of 189 pm, much shorter than the S-S single bonds in S8, which are 206 pm long. Its Raman spectrum consists of a band at 715 cm−1.[5] The corresponding O-O band for O2 is found at 1122 cm−1. The S-S bond energy is 265 kJ/mol compared to 498 kJ/mol for O2.
Sulfur has a large number of allotropes, perhaps as many as thirty. Their specific properties are distinguishable by various types of spectroscopy. The most stable form of sulfur at normal conditions is S8.[6]
Disulfur readily photodissociates,[7] with a mean lifespan of 7.5 min in sunlight.[8]
References
- ^ Steudel, Ralf; Eckert, Bodo (2003). "Solid Sulfur Allotropes". Elemental Sulfur and Sulfur-Rich Compounds I. Topics in Current Chemistry. Vol. 230. pp. 58–68. doi:10.1007/b12110. ISBN 978-3-540-40191-9.
- ^ Lellouch, E. (January 2005). "Io's Atmosphere and Surface-Atmosphere Interactions". Space Science Reviews. 116 (1–2): 211–224. Bibcode:2005SSRv..116..211L. doi:10.1007/s11214-005-1957-z.
- ^ Tardif, Sylvie L.; Rys, Andrzej Z.; Abrams, Charles B.; Abu-Yousef, Imad A.; Lesté-Lasserre, Pierre B. F.; Schultz, Erwin K. V.; Harpp, David N. (1997). "Recent chemistry of the chalcogen diatomics". Tetrahedron. 53 (36): 12225–12236. doi:10.1016/S0040-4020(97)00555-3.
- ^ Spencer, J. R. (2000). "Discovery of Gaseous S2 in Io's Pele Plume". Science. 288 (5469): 1208–1210. Bibcode:2000Sci...288.1208S. doi:10.1126/science.288.5469.1208. ISSN 0036-8075. PMID 10817990.
- ^ Eckert, Bodo; Steudel, Ralf (2003). "Molecular Spectra of Sulfur Molecules and Solid Sulfur Allotropes". Elemental Sulfur and Sulfur-Rich Compounds II. Topics in Current Chemistry. Vol. 231. pp. 181–191. doi:10.1007/b13181. ISBN 978-3-540-40378-4.
- ^ A. F. Holleman, N. Wiberg. Inorganic Chemistry. Academic Press; Berlin; New York: De Gruyter, 2001.ISBN 0-12-352651-5
- ^ Frederix, Pim W. J. M.; Yang, Chung-Hsin; Groenenboom, Gerrit C.; Parker, David H.; Alnama, Koutayba; Western, Colin M.; Orr-Ewing, Andrew J. (2009). "Photodissociation Imaging of Diatomic Sulfur (S2)†". The Journal of Physical Chemistry A. 113 (52): 14995–15005. Bibcode:2009JPCA..11314995F. CiteSeerX 10.1.1.511.5087. doi:10.1021/jp905104u. ISSN 1089-5639. PMID 19754091.
- ^ Ahearn, M. F.; Schleicher, D. G.; Feldman, P. D. (1983). "The discovery of S2 in comet IRAS-Araki-Alcock 1983d". The Astrophysical Journal. 274: L99. Bibcode:1983ApJ...274L..99A. doi:10.1086/184158. ISSN 0004-637X.
External links
Media related to Disulfur at Wikimedia Commons
