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{{Chembox |
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{{Chembox |
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| verifiedrevid = 450791932 |
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| verifiedrevid = 450793307 |
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| IUPACName = Disulfur |
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| Name = |
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| OtherNames = Diatomic sulfur<br /> |
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| ImageFile = Disulfur-2D-dimensions.png |
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Sulfur<br /> |
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| ImageFile1 = Disulfur-3D-balls.png |
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Sulfur dimer |
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| ImageFile_Ref = {{Chemboximage|correct|??}} |
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| Section1 = {{Chembox Identifiers |
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| ImageName = Ball and stick model of disulfur molecule |
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| CASNo = 23550-45-0 |
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| IUPACName = Disulfur<ref>ebi.ac.uk/chebi/searchId.do?chebiId=29387</ref> |
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| PubChem = 5460602 |
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| SystematicName = Disulfene |
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| PubChem_Ref = {{Pubchemcite|correct|pubchem}} |
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| OtherNames = Diatomic sulfur<br /> |
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| ChemSpiderID = 4574100 |
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Sulfur dimer <br /> |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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Disulphur |
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| Gmelin = 753 |
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| Section1 = {{Chembox Identifiers |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| CASNo_Ref = {{cascite|correct|??}} |
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| CASNo = 23550-45-0 |
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| PubChem = 5460602 |
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| ChemSpiderID = 4574100 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| Gmelin = 753 |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| ChEBI = 29387 |
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| ChEBI = 29387 |
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| SMILES = |
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| SMILES = S=S |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChI = 1S/S2/c1-2 |
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| StdInChI = 1S/S2/c1-2 |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = MAHNFPMIPQKPPI-UHFFFAOYSA-N |
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| StdInChIKey = MAHNFPMIPQKPPI-UHFFFAOYSA-N |
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}} |
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| Section2 = {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| S = 2 |
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| S=2 |
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| Dipole = 0 D |
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| ExactMass = 63.944141380 g mol<sup>-1</sup> |
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| Dipole = 0 D |
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| Section3 = {{Chembox Thermochemistry |
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| Section3 = {{Chembox Thermochemistry |
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| DeltaHf = 128.60 kJ mol<sup>-1</sup> |
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| DeltaHf = 128.60 kJ mol<sup>−1</sup> |
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| Entropy = 228.17 kJ K<sup>-1</sup> mol<sup>-1</sup> |
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| Entropy = 228.17 J K<sup>−1</sup> mol<sup>−1</sup> |
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| HeatCapacity = 32.51 kJ K<sup>-1</sup> mol<sup>-1</sup> |
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| HeatCapacity = 32.51 kJ K<sup>−1</sup> mol<sup>−1</sup> |
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| Section4 = {{chembox Related |
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| Section4 = {{Chembox Related |
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| OtherCpds = ] |
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| OtherCompounds = ] |
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| Section5 = |
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'''Disulfur''' is the ] with the formula S<sub>2</sub>.<ref>B. Eckert. R. Steudel “Solid Sulfur Allotropes”, Topic in Current Chemistry (2003) volume 231, pages 1-79. {{DOI|10. 1007/b12110B}}.</ref> It is analogous to the dioxygen molecule but rarely occurs at room temperature. This violet gas is commonly generated by heating sulfur above 720 °C and comprises 99% of vapor species at low pressure (1 mm Hg) at 530 °C. S<sub>2</sub> is one of minor components of the atmosphere of ], which is dominantly composed of ].<ref>Emmanuel Lellouch "Io’S Atmosphere and Surface-Atmosphere Interactions", LESIA, Observatoire de Paris, F-92195 Meudon. {{DOI|10.1 007/s11214-005-1957-z}}</ref> Diatomic molecules are common containing C, O, N and F, but for heavier elements they are often only stable at high temperatures. |
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'''Disulfur''' is the ] with the formula S<sub>2</sub>.<ref>{{Cite book| last1 = Steudel | first1 = Ralf| last2 = Eckert | first2 = Bodo| chapter = Solid Sulfur Allotropes| doi = 10.1007/b12110 | title = Elemental Sulfur and Sulfur-Rich Compounds I | series = ] | volume = 230 | pages = 58–68| year = 2003 | isbn = 978-3-540-40191-9 }}</ref> It is analogous to the ] molecule but rarely occurs at room temperature. This violet gas is the dominant species in hot sulfur vapors. S<sub>2</sub> is one of the minor components of the atmosphere of ], which is predominantly composed of ].<ref>{{Cite journal | last1 = Lellouch | first1 = E.| doi = 10.1007/s11214-005-1957-z | title = Io's Atmosphere and Surface-Atmosphere Interactions | journal = ] | volume = 116 | issue = 1–2| pages = 211–224 | date=January 2005 |bibcode = 2005SSRv..116..211L | s2cid = 121867974}}</ref> The instability of S<sub>2</sub> is usually described in the context of the ]. |
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==Production== |
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==Synthesis== |
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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. |
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Disulfur results when an atmosphere of ] is irradiated with UV light using a mercury ] or when CS<sub>2</sub>, H<sub>2</sub>S<sub>2</sub>, S<sub>2</sub>Cl<sub>2</sub> or C<sub>2</sub>H<sub>4</sub>S are photolyzed. Singlet S<sub>2</sub> is also formed when sulfur compounds such as H<sub>2</sub>S, PSF<sub>3</sub> or COS are photolyzed. S<sub>2</sub> can be generated by heating various organosulfur precursors.<ref>Sylvie L. Tardif, Andrzej Z. Rys, Charles B. Abrams, Imad A. Abu-Yousef, Pierre B. F. Leste-Lasserre, Erwin K. V. Schultz, and David N. Harpp “Recent Chemistry of the Chalcogen Diatomics” Terrahedron, Vol. 53, No 36, pp. 12225-12236. {{doi|10.1016/S0040-4020(97)00555-3}}</ref> |
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Disulfur can be produced when an atmosphere of ] is irradiated with UV light using a mercury ] or when CS<sub>2</sub>, H<sub>2</sub>S<sub>2</sub>, S<sub>2</sub>Cl<sub>2</sub> or C<sub>2</sub>H<sub>4</sub>S, PSF<sub>3</sub> or COS are irradiated.<ref>{{Cite journal | last1 = Tardif | first1 = Sylvie L.| last2 = Rys | first2 = Andrzej Z.| last3 = Abrams | first3 = Charles B.| last4 = Abu-Yousef | first4 = Imad A.| last5 = Lesté-Lasserre | first5 = Pierre B. F.| last6 = Schultz | first6 = Erwin K. V.| last7 = Harpp | first7 = David N.| doi = 10.1016/S0040-4020(97)00555-3 | title = Recent chemistry of the chalcogen diatomics | journal = ] | volume = 53 | issue = 36 | pages = 12225–12236 | year = 1997 }}</ref> |
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===Natural occurrence=== |
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Gaseous disulfur has been detected emanating from the surface of Jupiter's moon ], from the vicinity of ].<ref name="Spencer2000">{{cite journal|last1=Spencer|first1=J. R.|title=Discovery of Gaseous S2 in Io's Pele Plume|journal=Science|volume=288|issue=5469|year=2000|pages=1208–1210|issn=0036-8075|doi=10.1126/science.288.5469.1208|pmid=10817990|bibcode=2000Sci...288.1208S}}</ref> |
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==Properties== |
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==Properties== |
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S<sub>2</sub> exists in the ] like O<sub>2</sub>, i.e. both are diradicals. It has S-S double bond length of 189 pm, much shorter than the S-S single bonds in S<sub>8</sub>, which are 206 pm. In its ], the S-S vibrational band is observed at 715 cm<sup>−1</sup>.<ref>B. Eckert, Ralf Steudel “Molecular Spectra of Sulfur Molecules and Solid Sulfur Allotropes”, Topics in Current Chemistry (2003) volume 231, pages 31–98. {{DOI|10.1007/b13181}}</ref> The corresponding vibrational band of O-O is found at 1122 cm<sup>−1</sup>. The S-S ] is 265 kJ/mol compared to 498 kJ/mol for O<sub>2</sub>. |
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The ground state of S<sub>2</sub> is a ]: a ], with two unpaired electrons like O<sub>2</sub> and ].<ref>{{cite book|first1=N. N.|last1=Greenwood|first2=A.|last2=Earnshaw|title=Chemistry of the Elements|publisher=Pergamon|location=New York|year=1986|postscript=;}} as cited in {{cite journal|doi=10.1080/10426509708545509|journal=Phosphorus, Sulfur, and Silicon|year=1997|volume=120|page=41|publisher=Gordon & Breach|location=Amsterdam, NL|title=The sulfur diatomics|first=David N.|last=Harpp}}</ref> It has the S-S bond length of 189 pm, much shorter than the S-S single bonds in S<sub>8</sub>, which are 206 pm long. Its ] consists of a band at 715 cm<sup>−1</sup>.<ref>{{Cite book| last1 = Eckert | first1 = Bodo| last2 = Steudel | first2 = Ralf| chapter = Molecular Spectra of Sulfur Molecules and Solid Sulfur Allotropes | doi = 10.1007/b13181 | title = Elemental Sulfur and Sulfur-Rich Compounds II | series = ] | volume = 231 | pages = 181–191| year = 2003 | isbn = 978-3-540-40378-4 }}</ref> The corresponding O-O band for O<sub>2</sub> is found at 1556 cm<sup>−1</sup>.<ref>{{Cite journal|last1=Hill|first1=R.A.|last2=Esherick|first2=P.|last3=Owyoung|first3=A.|date=1983|title=High-resolution stimulated Raman spectroscopy of O2|journal=Journal of Molecular Spectroscopy|language=en|volume=100|issue=1|pages=119–133|doi=10.1016/0022-2852(83)90029-2|bibcode=1983JMoSp.100..119H}}</ref> The S-S ] is 430 kJ/mol compared to 498 kJ/mol for O<sub>2</sub>.<ref>({{RubberBible87th}}</ref> |
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Singlet disulfur is believed to be the product of ]s with ], or the thermal decomposition of dialkoxy disulfides. However, the disulfur produced in that reaction is believed singlet because it undergoes formal hetero-] cycloadditions, not because of any spectroscopic evidence.<ref>{{cite book|doi=10.1002/9780470682531.pat0829|title=Peroxides|chapter=Sulfoxylic and thiosulfurous acids and their dialkoxy derivatives|first1=Sergei V.|last1=Makarov|first2=Anna S.|last2=Makarova|first3=Radu|last3=Silaghi-Dumitrescu|series=Chemistry of Functional Groups|year=2014|publisher=Wiley|page=297|isbn=978-0-470-68253-1 }}</ref> |
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Sulfur has a large number of ]s, perhaps as many as thirty. Their specific properties are distinguishable by various types of spectroscopy. The only stable form of sulfur at normal condition is S<sub>8</sub>.<ref>A. F. Holleman, N. Wiberg. Inorganic Chemistry. Academic Press; Berlin ; New York : De Gruyter, 2001.ISBN 0-12-352651-5.</ref> |
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Triplet disulfur readily ],<ref name="FrederixYang2009">{{cite journal|last1=Frederix|first1=Pim W. J. M.|last2=Yang|first2=Chung-Hsin|last3=Groenenboom|first3=Gerrit C.|last4=Parker|first4=David H.|last5=Alnama|first5=Koutayba|last6=Western|first6=Colin M.|last7=Orr-Ewing|first7=Andrew J.|title=Photodissociation Imaging of Diatomic Sulfur (S2)†|journal=The Journal of Physical Chemistry A|volume=113|issue=52|year=2009|pages=14995–15005|issn=1089-5639|doi=10.1021/jp905104u|pmid=19754091|bibcode=2009JPCA..11314995F|citeseerx=10.1.1.511.5087}}</ref> with a mean lifespan of 7.5 min in sunlight.<ref name="AhearnSchleicher1983">{{cite journal|last1=Ahearn|first1=M. F.|last2=Schleicher|first2=D. G.|last3=Feldman|first3=P. D.|title=The discovery of S2 in comet IRAS-Araki-Alcock 1983d|journal=The Astrophysical Journal|volume=274|year=1983|pages=L99|issn=0004-637X|doi=10.1086/184158|bibcode=1983ApJ...274L..99A}}</ref> |
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==References== |
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==References== |
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==External links== |
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*{{Commonscatinline}} |
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{{Diatomic elements}} |
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