| 词条 | Disulfur dioxide | ||||||||||||||||||||||
| 释义 |
| Name = Disulfur dioxide | ImageFile = Disulfur-dioxide-2D-dimensions.png | ImageName = structure of disulfur dioxide, S2O2 | ImageFile1 = Disulfur-dioxide-3D-vdW-A.png | ImageName1 = space-filling model of the disulfur dioxide molecule | IUPACName = | OtherNames = disulfur(II)oxide SO dimer |Section1={{Chembox Identifiers | SMILES = O=[S][S]=O | CASNo = 126885-21-0 | CASNo_Comment = [1] | ChemSpiderID = | RTECS = | InChI = 1/O2S2/c1-3-4-2 | InChI_Comment = | InChIKey = AXYLJRYHRATPSG-UHFFFAOYNA-N |Section2={{Chembox Properties | Formula = S2O2 | MolarMass = 96.1299 g/mol | Appearance = gas | Density = | Solubility = | Solvent = other solvents | SolubleOther = | MeltingPt = | BoilingPt = | Viscosity = |Section3={{Chembox Structure | Coordination = bent | CrystalStruct = | Dipole = |Section7={{Chembox Hazards | ExternalSDS = | MainHazards = toxic | RPhrases = | SPhrases = | NFPA-H = | NFPA-F = | NFPA-R = | NFPA-S = |Section8={{Chembox Related | OtherCompounds = tetrasulfur SO, S3O S2O }}Disulfur dioxide, dimeric sulfur monoxide or SO dimer is an oxide of sulfur.[1] The solid is unstable with a lifetime of a few seconds at room temperature.[2] StructureDisulfur dioxide adopts 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 OSS angle is 112.7°. S2O2 has a dipole moment of 3.17 D.[4] an asymmetric top molecule.[3][4] FormationSulfur monoxide (SO) converts to disulfur dioxide (S2O2) spontaneously and reversibly.[5] 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.[4] Another laboratory procedure is to react oxygen atoms with carbon oxysulfide 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 S2O2 ⇌ 2SO Disulfur dioxide is also produced upon a microwave discharge in sulfur dioxide diluted in helium.[11] At a pressure of 0.1 mm Hg,five percent of the result is S2O2.[8] Disulfur dioxide is formed transiently when hydrogen sulfide and oxygen undergo flash photolysis.[9] PropertiesThe ionisation energy of disulfur dioxide is 9.93±0.02 eV.[6] Disulfur dioxide absorbs at 320–400 nm, as observed of the Venusian atmosphere,[10] and is believed to have contributed to the greenhouse effect on that planet.[11] ReactionsAlthough disulfur dioxide exists in equilibrium with sulfur monoxide, it also reacts with sulfur monoxide to form sulfur dioxide and disulfur monoxide.[12][13] ComplexesS2O2 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)2PtS2O2.[15] Iridium atoms can also form a complex: cis-[(dppe)2IrS2]Cl with sodium periodate oxidises 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 triphenyl phosphine to form triphenyl phosphine oxide, and triphenyl phosphine sulfide.[16] AnionThe S2O2− anion has been observed in the gas phase. It may adopt a trigonal shape akin to SO3.[18] SpectrumMicrowave
In the Solar SystemThere 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.[10] It is not found in any substantive quantity in Earth's atmosphere. References1. ^{{cite book|editor1=Arnold F. Holleman |editor2=Egon Wiber |editor3=Nils Wiberg |title=Inorganic Chemistry|chapter-url=https://books.google.com/books?id=Mtth5g59dEIC&pg=PA530|year=2001|publisher=Academic Press|page=530|chapter=Oxides of sulfur|isbn=9780123526519 }} {{Oxides}}2. ^{{cite book|last=Mitchell|first=Stephen C. |title=Biological Interactions Of Sulfur Compounds|date=3 September 2004|publisher=CRC Press|isbn=978-0203362525|page=7}} 3. ^1 {{cite book|last1=Demaison|first1=Jean|last2=Vogt|first2=Jürgen|title=Asymmetric Top Molecules, Part 3|chapter-url=https://link.springer.com/content/pdf/10.1007%2F978-3-642-14145-4_258.pdf|series=Landolt-Börnstein - Group II Molecules and Radicals|doi=10.1007/978-3-642-14145-4_258|volume=29D3|year=2011|publisher=Springer|isbn=978-3-642-14145-4|pages=492 |chapter=836 O2S2 Disulfur dioxide}} 4. ^1 2 {{cite journal|last=Thorwirth|first=Sven|author2=P. Theulé|author3=C. A. Gottlieb |author4=H. S. P. Müller|author5=M. C. McCarthy|author6=P. Thaddeus|date=23 February 2006|title=Rotational spectroscopy of S2O: vibrational satellites, 33 S isotopomers, and the submillimeter-wave spectrum|pages=219–229|volume=795|issue=1–3|journal=Journal of Molecular Structure|url=http://hera.ph1.uni-koeln.de/~sthorwirth/pdf/s2o_JMSt_2006.pdf|doi=10.1016/j.molstruc.2006.02.055|bibcode=2006JMoSt.795..219T}} 5. ^1 Spectroscopic studies of the SO2 discharge system. II. Microwave spectrum of the SO dimer Lovas F. J., Tiemann E., Johnson D.R. The Journal of Chemical Physics (1974), 60, 12, 5005-5010 {{doi|10.1063/1.1681015}} 6. ^1 {{cite journal|last=Cheng|first=Bing-Ming|author2=Wen-Ching Hung|year=1999|title=Photoionization efficiency spectrum and ionization energy of S[sub 2]O[sub 2]|journal=The Journal of Chemical Physics|volume=110|issue=1|page=188|issn=0021-9606|doi=10.1063/1.478094|bibcode=1999JChPh.110..188C}} 7. ^{{cite journal|last=Murakami|first=Yoshinori |author2=Shouichi Onishi |author3=Takaomi Kobayashi |author4=Nobuyuki Fujii |author5=Nobuyasu Isshiki |author6=Kentaro Tsuchiya |author7=Atsumu Tezaki |author8=Hiroyuki Matsui|year=2003|title=High Temperature Reaction of S + SO2→ SO + SO: Implication of S2O2Intermediate Complex Formation|journal=The Journal of Physical Chemistry A|volume=107|issue=50|pages=10996–11000|issn=1089-5639|doi=10.1021/jp030471i|bibcode=2003JPCA..10710996M }} 8. ^{{cite book|last1=Pujapanda|first1=Balaram Sahoo, Nimain C. Nayak, Asutosh Samantaray, Prafulla K.|last2=Balaram|first2=Sahoo|last3=Charan|first3=nayak Nimai |author4=samantaray Asutosh |author5=pujapanda Prafulla Kumar|title=Inorganic Chemistry|url=https://books.google.com/books?id=8KAemlQzOj8C|accessdate=16 May 2013|publisher=PHI Learning Pvt. Ltd.|isbn=9788120343085|page=461|year=2012}} 9. ^{{cite book|last1=Compton|first1=R. G.|last2=Bamford|first2=C.H. |last3=Tipper|first3=C.F.H. |title=Reactions of Non-Metallic Inorganic Compounds|chapter-url=https://books.google.com/books?id=GwhMyI_tZO4C|series=Comprehensive Chemical Kinetics|year=1972|publisher=Elsevier|isbn=978-0080868011|page=50|chapter=Oxidation of H2S}} 10. ^1 {{cite journal|title=Identification of OSSO as a near-UV absorber in the Venusian atmosphere|author1=BN Frandsen|author2=PO Wennberg|author3=HG Kjaergaard|year=2016|journal=Geophys. Res. Lett.|volume=43|issue=21|pages=11,146|doi=10.1002/2016GL070916|bibcode=2016GeoRL..4311146F|url=https://authors.library.caltech.edu/73255/1/Frandsen_et_al-2016-Geophysical_Research_Letters.pdf}} 11. ^{{cite web |url=http://www.cbc.ca/news/technology/rare-molecule-venus-weather-1.3843428 |title=Rare molecule on Venus may help explain planet's weather - Technology & Science - CBC News |newspaper=Cbc.ca |date= |author= |accessdate= November 11, 2016}} 12. ^1 {{cite journal|last=Field|first=T A|author2=A E Slattery|author3=D J Adams|author4=D D Morrison|year=2005|title=Experimental observation of dissociative electron attachment to S2O and S2O2 with a new spectrometer for unstable molecules|journal=Journal of Physics B: Atomic, Molecular and Optical Physics|volume=38|issue=3|pages=255–264|issn=0953-4075|doi=10.1088/0953-4075/38/3/009|url=http://www.qub.ac.uk/schools/SchoolofMathematicsandPhysics/ampr/tfield/reprint-eric1.pdf|bibcode=2005JPhB...38..255F}} 13. ^{{cite journal|last=Herron|first=J. T.|author2=R. E. Huie|year=1980|title=Rate constants at 298 K for the reactions sulfur monoxide + sulfur monoxide + M -> dimeric sulfur monoxi de + M and sulfur monoxide + dimeric sulfur monoxide -> sulfur dioxide + sulfur oxide (S2O)|journal=Chemical Physics Letters|volume=76|issue=2|pages=322–324|doi=10.1016/0009-2614(80)87032-1|bibcode=1980CPL....76..322H}} 14. ^{{cite journal|last=Halcrow|first=Malcolm A.|author2=John C. Huffman|author3=George Christou|year=1994|title=Synthesis, Characterization, and Molecular Structure of the New S2O Complex Mo(S2O)(S2CNEt2)3.cntdot.1/2Et2O|journal=Inorganic Chemistry|volume=33|issue=17|pages=3639–3644|issn=0020-1669|doi=10.1021/ic00095a005|url=http://www.chem.ufl.edu/~christou/group/ChristouGroupPapers/138%20Mo%20S2O%20full%20IC.pdf}} 15. ^{{cite journal|last=Lorenz|first=Ingo-Peter|author2=Jürgen Kull|year=1986|title=Complex Stabilization of Disulfur Dioxide in the Fragmentation of ThiiraneS-Oxide on Bis(triphenylphosphane)platinum(0)|journal=Angewandte Chemie International Edition in English|volume=25|issue=3|pages=261–262|issn=0570-0833|doi=10.1002/anie.198602611}} 16. ^1 {{cite journal|last=Schmid|first=Günter|author2=Günter Ritter|author3=Tony Debaerdemaeker|year=1975|title=Die Komplexchemie niederer Schwefeloxide, II. Schwefelmonoxid und Dischwefeldioxid als Komplexliganden|journal=Chemische Berichte|volume=108|issue=9|pages=3008–3013|issn=0009-2940|doi=10.1002/cber.19751080921}} 17. ^{{cite journal|last=Nagata|first=K|author2=N. Takeda|author3=N Tokitoh N|year=2003|title=Unusual Oxidation of Dichalcogenido Complexes of Platinum|journal=Chemical Letters|volume=32|issue=2|pages=170–171|issn=0366-7022|doi=10.1246/cl.2003.170}} 18. ^{{cite journal|last=Clements|first=Todd G. |author2=Hans-Jürgen Deyerl |author3=Robert E. Continetti|year=2002|title=Dissociative Photodetachment Dynamics of S2O2-|journal=The Journal of Physical Chemistry A|volume=106|issue=2|pages=279–284|issn=1089-5639|doi=10.1021/jp013329v|url=http://checont6.ucsd.edu/pdf/051.clements.2002.pdf|accessdate=2013-05-13|bibcode=2002JPCA..106..279C }} 1 : Sulfur oxides |
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