Disulfur monoxide

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Disulfur monoxide
Structure of S2O
solid ball model of S2O
Names
Other names
sulfur suboxide; Sulfuroxide;
Identifiers
20901-21-7 [1]
ChemSpider 124163
Properties
S2O
Molar mass 80.1294 g/mol[1]
Appearance colourless gas or dark red solid[2]
Structure
bent
Hazards
Main hazards toxic
Related compounds
Related compounds
trisulfur
SO,
Ozone,
SO2
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Disulfur monoxide or sulfur suboxide is an inorganic compound with formula S2O. It is one of the lower sulfur oxides. It is a colourless gas and condenses to give a pale coloured solid that is unstable at room temperature.[3] It is a bent molecule with an S-S-O angle of 117.88°, S-S bond length of 188.4pm, and S-O bond length of 146.5pm.[4]

Disulfur monoxide was discovered by Peter W. Schenk in 1933.[5][6] However only when Myers and Meschi studied it, did the actual composition and shape of the molecule become known.[6]

Preparation[edit]

It can be formed by many methods, including combustion of sulfur vapour in a deficiency of oxygen. It arises by oxidizing sulfur with copper oxide:[7]

3/4 S8 + 3 CuO → 3 CuS + S2O + SO2

Other routes include the reaction of thionyl chloride with silver sulfide:

SOCl2 + Ag2S → 2 AgCl + S2O

It also arises via thermal decomposition of sulfur dioxide in a glow discharge.[8]

Disulfur monoxide forms a yellow solution in carbon tetrachloride.[7] The solid can be obtained at liquid nitrogen temperatures, often appearing dark colored owing to impurities. On decomposition at room temperature it forms SO2 via the formation of polysulfur oxides.[8]

Discovery[edit]

Disulfur monoxide was first produced by P. W. Schenk in 1933[3] with a glow discharge though sulfur vapour and sulfur dioxide. He discovered that the gas could survive for hours at single digit pressures of mercury in clean glass, but decomposed near 30mm Hg Schenk assigned the formula as SO and called it sulfur monoxide. In 1940 K Kondrat'eva and V Kondrat'ev proposed the formula as S2O2, disulfur dioxide. In 1956, D. J. Meschi and R. J. Myers established the formula as S2O.[9]

Natural occurrence[edit]

Desulfovibrio desulfuricans is claimed to produce S2O.[10] S2O can be found coming from volcanoes on Io. It can form from 1 to 6% when hot 100 bar S2 and SO2 gas erupts from volcanoes. It is believed that Pele on Io is surrounded by solid S2O.[11]

Properties[edit]

Condensed solid S2O displays absorption bands at 420 and 530 nm. These are likely to be due to S3 and S4.[12]

The microwave spectrum of S2O has the following rotational parameters: A=41915.44, B=5059.07, and C=4507.19 MHz.[13]

In the ultraviolet S2O has absorption band systems in the ranges 2500 to 3400 Å, and 1900 to 2400 Å. There are bands at 3235 and 3278 Å.[6] The band in the 3150 to 3400 Å range is due to C1A'-X1A'(π*←π) transition.[14]

The bond angle S-S-O is 109°.[6] The harmonic frequency for S-S stretching is 415.2 cm−1.[14]

Reactions[edit]

A self decomposition of S2O can form trithio-ozone (S3) and SO2. Also 5,6-di-tert-butyl-2,3,7-trithiabicyclo[2.2.1]hept-5-ene 2-endo-7-endo-dioxide when heated can form S2O.[15] It reacts with diazoalkanes to form dithiirane 1-oxides.[16]

Disulfur monoxide is a ligand bound to transition metals. These are formed by oxidation peroxide oxidation of a disulfur ligands. Excessive oxygen can yield a dioxygendisulfur ligand, which can be reduced in turn with triphenylphosphine. Examples are: [Ir(dppe)2S2O]+, OsCl(NO)(PPh3)2S2O, NbCl(η-C5H5)2S2O, Mn(CO)2(η-C5Me5)S2O, Re(CO)2(η-C5Me5)S2O, Re(CO)2(η-C5H5)S2O.[17]

The molybdenum compound Mo(CO)2(S2CNEt2)2 reacts with elemental sulfur and air to form a compound Mo2(S2O)2(S2CNEt2)4.[17] Another way to form these complexes is to combine sulfonyliminooxo-λ4-sulfurane (OSNSO2.R) complexes with hydrogen sulfide.[17] Complexes formed in this way are: IrCl(CO)(PPh3)2S2O; Mn(CO)2(η-C5H5)S2O. With hydrosulfide and a base followed by oxygen, OsCl(NO)(PPh3)2S2O can be made.[17]

References[edit]

  1. ^ a b c d "Disulfur monoxide". NIST. 2008. 
  2. ^ B Hapke and F Graham (May 1989). "Spectral properties of condensed phases of disulfur monoxide, polysulfur oxide, and irradiated sulfur". Icarus 79 (1): 47. Bibcode:1989Icar...79...47H. doi:10.1016/0019-1035(89)90107-3. 
  3. ^ a b R. Steudel: Sulfur-Rich Oxides SnO and SnO2" in Elemental Sulfur und Sulfur-Rich Compounds II, Steudel, R., 2003, Springer, Berlin-Heidelberg. ISBN 9783540449515
  4. ^ Meschi, D. J.; Myers, R. J. (1959). "The microwave spectrum, structure, and dipole moment of disulfur monoxide". Journal of Molecular Spectroscopy 3 (1–6): 405–416. Bibcode:1959JMoSp...3..405M. doi:10.1016/0022-2852(59)90036-0. 
  5. ^ Schenk, Peter W. (18 March 1933). "über das Schwefelmonoxyd". Zeitschrift für anorganische und allgemeine Chemie (in German) 211 (1-2): 150–160. doi:10.1002/zaac.19332110117. 
  6. ^ a b c d Hallin, K-E. J.; Merer, A. J.; Milton, D. J. (November 1977). "Rotational analysis of bands of the 3400 Å system of disulphur monoxide (S2O)". Canadian Journal of Physics 55 (21): 1858–1867. doi:10.1139/p77-226. 
  7. ^ a b Satyanarayana, S. R.; A. R. Vasudeva Murthy (1964). "Reactions with Disulphur monoxide Solutions Obtained by the Reduction of Cupric Oxide by Elemental Sulphur" (PDF). Proceedings of the Indian Academy of Sciences Section A 59 (4). 
  8. ^ a b Cotton and Wilkinson (1966). Advanced Inorganic Chemistry: A Comprehensive Treatise. p. 540. 
  9. ^ David J. Meschi and Rollie J. Myers (30 July 1956). "Disulfur Monoxide. I. Its Identification as the Major Constituent in Schenk's "Sulfur Monoxide"". Journal of the American Chemical Society 78 (24): 6220. doi:10.1021/ja01605a002. 
  10. ^ Iverson, WP (26 May 1967). "Disulfur monoxide: production by Desulfovibrio". Science 156 (3778): 1112–4. Bibcode:1967Sci...156.1112I. doi:10.1126/science.156.3778.1112. PMID 6024190. 
  11. ^ Mikhail Yu. Zolotov and Bruce Fegley (9 March 1998). "Volcanic Origin of Disulfur Monoxide (S2O) on Io" (PDF). Icarus 133 (2): 293. Bibcode:1998Icar..133..293Z. doi:10.1006/icar.1998.5930. 
  12. ^ Navizet, Isabelle; Komiha, Najia; Linguerri, Roberto; Chambaud, Gilberte; Rosmus, Pavel (November 2010). "On the formation of S2O at low energies: An ab initio study". Chemical Physics Letters 500 (4-6): 207–210. doi:10.1016/j.cplett.2010.10.012. 
  13. ^ Cook, Robert L; Winnewisser, Gisbert; Lindsey, D.C (May 1973). "The centrifugal distortion constants of disulfur monoxide". Journal of Molecular Spectroscopy 46 (2): 276–284. doi:10.1016/0022-2852(73)90042-8. 
  14. ^ a b Zhang, Qingguo; Dupré, Patrick; Grzybowski, Bartosz; Vaccaro, Patrick H. (1995). "Laser-induced fluorescence studies of jet-cooled S2O: Axis-switching and predissociation effects". The Journal of Chemical Physics 103 (1): 67. doi:10.1063/1.469623. 
  15. ^ Nakayama J; Aoki, S; Takayama, J; Sakamoto, A; Sugihara, Y; Ishii, A (28 July 2004). "Reversible disulfur monoxide (S2O)-forming retro-Diels-Alder reaction. disproportionation of S2O to trithio-ozone (S3) and sulfur dioxide (SO2) and reactivities of S2O and S3". Journal of the American Chemical Societ 126 (29): 9085–93. doi:10.1021/ja047729i. PMID 15264842. 
  16. ^ A Ishii; Kawai, T; Tekura, K; Oshida, H; Nakayama, J (18 May 2001). "A Convenient Method for the Generation of a Disulfur Monoxide Equivalent and Its Reaction with Diazoalkanes to Yield Dithiirane 1-Oxides". Angew Chem Int Ed Engl 40 (10): 1924–1926. doi:10.1002/1521-3773(20010518)40:10<1924::AID-ANIE1924>3.0.CO;2-F. PMID 11385674. 
  17. ^ a b c d F G A Stone (1994-03-07). Advances in Organometallic Chemistry, Volume 36. p. 168. ISBN 978-0-12-031136-1.