Disulfur dioxide

From Wikipedia, the free encyclopedia
Disulfur dioxide
structure of disulfur dioxide, S2O2
space-filling model of the disulfur dioxide molecule
Names
Other names
disulfur(II)oxide
SO dimer
Identifiers
3D model (JSmol)
  • InChI=1/O2S2/c1-3-4-2
    Key: AXYLJRYHRATPSG-UHFFFAOYNA-N
  • O=[S][S]=O
Properties
S2O2
Molar mass 96.1299 g/mol
Appearance gas
Structure
bent
Hazards
Main hazards toxic
Related compounds
Related compounds
 tetrasulfur
SO,

S2O
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Disulfur dioxide, dimeric sulfur monoxide or SO dimer is an oxide of sulfur with the formula S2O2.[2] The solid is unstable with a lifetime of a few seconds at room temperature.[3]

Structure[]

Disulfur dioxide adopts a cis planar structure with C2v symmetry. The S−O bond length is 145.8 pm, shorter than in sulfur monoxide. The S−S bond length is 202.45 pm and the O−S−S angle is 112.7°. S2O2 has a dipole moment of 3.17 D.[4] It is an asymmetric top molecule.[1][5]

Formation[]

Sulfur monoxide (SO) converts to disulfur dioxide (S2O2) spontaneously and reversibly.[4] So the substance can be generated by methods that produce sulfur monoxide. Disulfur dioxide has also been formed by an electric discharge in sulfur dioxide.[5] Another laboratory procedure is to react oxygen atoms with carbonyl sulfide or carbon disulfide vapour.[6]

Although most forms of elemental sulfur (S8 and other rings and chains) do not combine with SO2, atomic sulfur does so to form sulfur monoxide, which dimerizes:[7]

S + SO2 → S2O2 ⇌ 2 SO

Disulfur dioxide is also produced upon a microwave discharge in sulfur dioxide diluted in helium.[8] At a pressure of 0.1 mmHg (13 Pa), five percent of the result is S2O2.[9]

Disulfur dioxide is formed transiently when hydrogen sulfide and oxygen undergo flash photolysis.[10]

Properties[]

The ionization energy of disulfur dioxide is 9.93±0.02 eV.[6]

Disulfur dioxide absorbs at 320–400 nm, as observed of the Venusian atmosphere,[11] and is believed to have contributed to the greenhouse effect on that planet.[12]

Reactions[]

Although disulfur dioxide exists in equilibrium with sulfur monoxide, it also reacts with sulfur monoxide to form sulfur dioxide and disulfur monoxide.[8][13]

Complexes[]

S2O2 can be a ligand with transition metals. It binds in the η2-S–S position with both sulfur atoms linked to the metal atom.[14] This was first shown in 2003. The bis(trimethylphosphine) thiirane S-oxide complex of platinum, when heated in toluene at 110 °C loses ethylene, and forms a complex with S2O2: (Ph3P)2Pt(S2O2).[15] Iridium atoms can also form a complex: cis-[(dppe)2IrS2]Cl with sodium periodate oxidizes to [(dppe)2IrS2O] and then to [(dppe)2IrS2O2], with dppe being 1,2-bis(diphenylphosphino)ethane.[16][17] This substance has the S2O2 in a cis position. The same conditions can make a trans complex, but this contains two separate SO radicals instead. The iridium complex can be decomposed with triphenylphosphine to form triphenylphosphine oxide and triphenylphosphine sulfide.[16]

Anion[]

The S
2O−
2 anion has been observed in the gas phase. It may adopt a trigonal shape akin to SO3.[18]

Spectrum[]

Microwave[]

Transition Frequency (MHz)[5]
21,1−20,2 11013.840
41,3−40,4 14081.640
11,1−00,0 15717.946
40,4−31,3 16714.167
31,3−20,2 26342.817
42,2−41,3 26553.915
22,0−21,1 28493.046
60,6−51,5 30629.283
52,4−51,5 35295.199
51,5−40,4 35794.527

In the Solar System[]

There is a some evidence that disulfur dioxide may be a small component in the atmosphere of Venus, and that it may substantially contribute of the planet's severe greenhouse effect.[11] It is not found in any substantive quantity in Earth's atmosphere.

References[]

  1. ^ a b Demaison, Jean; Vogt, Jürgen (2011). "836. O2S2 Disulfur dioxide" (PDF). Asymmetric Top Molecules, Part 3. Landolt–Börnstein: Group II Molecules and Radicals. 29D3. Springer. p. 492. doi:10.1007/978-3-642-14145-4_258. ISBN 9783642141454.
  2. ^ Holleman, Arnold F.; Wiber, Egon; Wiberg, Nils, eds. (2001). "Oxides of sulfur". Inorganic Chemistry. Academic Press. p. 530. ISBN 9780123526519.
  3. ^ Mitchell, Stephen C. (2004). Biological Interactions Of Sulfur Compounds. CRC Press. p. 7. ISBN 9780203362525.
  4. ^ a b Lovas, F. J. (1974). "Spectroscopic studies of the SO2 discharge system. II. Microwave spectrum of the SO dimer". The Journal of Chemical Physics. 60 (12): 5005. doi:10.1063/1.1681015.
  5. ^ a b c Thorwirth, Sven; Theulé, P.; Gottlieb, C. A.; Müller, H. S. P.; McCarthy, M. C.; Thaddeus, P. (2006). "Rotational spectroscopy of S2O: vibrational satellites, 33S isotopomers, and the submillimeter-wave spectrum" (PDF). Journal of Molecular Structure. 795 (1–3): 219–229. Bibcode:2006JMoSt.795..219T. doi:10.1016/j.molstruc.2006.02.055.
  6. ^ a b Cheng, Bing-Ming; Hung, Wen-Ching (1999). "Photoionization efficiency spectrum and ionization energy of S2O2". The Journal of Chemical Physics. 110 (1): 188. Bibcode:1999JChPh.110..188C. doi:10.1063/1.478094. ISSN 0021-9606.
  7. ^ Murakami, Yoshinori; Onishi, Shouichi; Kobayashi, Takaomi; Fujii, Nobuyuki; Isshiki, Nobuyasu; Tsuchiya, Kentaro; Tezaki, Atsumu; Matsui, Hiroyuki (2003). "High Temperature Reaction of S + SO2 → SO + SO: Implication of S2O2 Intermediate Complex Formation". The Journal of Physical Chemistry A. 107 (50): 10996–11000. Bibcode:2003JPCA..10710996M. doi:10.1021/jp030471i. ISSN 1089-5639.
  8. ^ a b Field, T. A.; Slattery, A. E.; Adams, D. J.; Morrison, D. D. (2005). "Experimental observation of dissociative electron attachment to S2O and S2O2 with a new spectrometer for unstable molecules" (PDF). Journal of Physics B: Atomic, Molecular and Optical Physics. 38 (3): 255–264. Bibcode:2005JPhB...38..255F. doi:10.1088/0953-4075/38/3/009. ISSN 0953-4075. Archived from the original (PDF) on 2015-09-24. Retrieved 2013-05-13.
  9. ^ Sahoo, Balaram; Nayak, Nimai Charan; Samantaray, Asutosh; Pujapanda, Prafulla Kumar (2012). Inorganic Chemistry. PHI Learning. p. 461. ISBN 9788120343085. Retrieved 2013-05-16.
  10. ^ Compton, R. G.; Bamford, C. H.; Tipper, C. F. H. (1972). "Oxidation of H2S". Reactions of Non-Metallic Inorganic Compounds. Comprehensive Chemical Kinetics. Elsevier. p. 50. ISBN 9780080868011.
  11. ^ a b Frandsen, B. N.; Wennberg, P. O.; Kjærgaard, H. G. (2016). "Identification of OSSO as a near-UV absorber in the Venusian atmosphere" (PDF). Geophysical Research Letters. 43 (21): 11146–11155. Bibcode:2016GeoRL..4311146F. doi:10.1002/2016GL070916.
  12. ^ "Rare molecule on Venus may help explain planet's weather". CBC News. Retrieved 2016-11-11.
  13. ^ Herron, J. T.; Huie, R. E. (1980). "Rate constants at 298 K for the reactions SO + SO + M → (SO)2 + M and SO + (SO)2 → SO2 + S2O". Chemical Physics Letters. 76 (2): 322–324. Bibcode:1980CPL....76..322H. doi:10.1016/0009-2614(80)87032-1.
  14. ^ Halcrow, Malcolm A.; Huffman, John C.; Christou, George (1994). "Synthesis, Characterization, and Molecular Structure of the New S2O Complex Mo(S2O)(S2CNEt2)3·1/2Et2O" (PDF). Inorganic Chemistry. 33 (17): 3639–3644. doi:10.1021/ic00095a005. ISSN 0020-1669.
  15. ^ Lorenz, Ingo-Peter; Kull, Jürgen (1986). "Complex Stabilization of Disulfur Dioxide in the Fragmentation of Thiirane S-Oxide on Bis(triphenylphosphane)platinum(0)". Angewandte Chemie International Edition in English. 25 (3): 261–262. doi:10.1002/anie.198602611. ISSN 0570-0833.
  16. ^ a b Schmid, Günter; Ritter, Günter; Debaerdemaeker, Tony (1975). "Die Komplexchemie niederer Schwefeloxide. II. Schwefelmonoxid und Dischwefeldioxid als Komplexliganden" [The complex chemistry of lower sulfur oxides. II. Sulfur monoxide and disulfur dioxide as complex ligands]. Chemische Berichte. 108 (9): 3008–3013. doi:10.1002/cber.19751080921. ISSN 0009-2940.
  17. ^ Nagata, K.; Takeda, N.; Tokitoh, N. (2003). "Unusual Oxidation of Dichalcogenido Complexes of Platinum". Chemistry Letters. 32 (2): 170–171. doi:10.1246/cl.2003.170. ISSN 0366-7022.
  18. ^ Clements, Todd G.; Hans-Jürgen Deyerl; Robert E. Continetti (2002). "Dissociative Photodetachment Dynamics of S
    2    O−
    2    "     (PDF). The Journal of Physical Chemistry A. 106 (2): 279–284. Bibcode:2002JPCA..106..279C. doi:10.1021/jp013329v. ISSN 1089-5639. Retrieved 2013-05-13.
Retrieved from ""