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Lower sulfur oxides
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<h2 id="sulfur-monoxide-disulfur-dioxide-disulfur-monoxide">Sulfur monoxide, disulfur dioxide, disulfur monoxide</h2> <p>These species are well characterized in the gas phase, but they cannot be isolated as solids or liquids. Instead, when condensed, they undergo dimerization and oligomerization, usually yielding sulfur dioxide and elemental sulfur. At a few <a href="/facts/Millibar/wwFWTTkT">millibars</a> pressure, the relative stabilities are S2O > S2O2 > SO.<a class="footnote-ref" id="fnref:3" href="#fn:3"><sup>3</sup></a> <a href="/facts/Sulfur_monoxide/CI8PbSJX">Sulfur monoxide</a> (SO) and its dimer (S2O2) have been trapped at low temperature. <a href="/facts/Disulfur_dioxide/WJDkS1oU">Disulfur dioxide</a> (S2O2) is a dimer of sulfur monoxide. It has C2v structure (planar). </p><p><a href="/facts/Disulfur_monoxide/ez5v6KrH">Disulfur monoxide</a> (S2O) is an analogue of <a href="/facts/Sulfur_dioxide/jDK1fIDs">sulfur dioxide</a>. Like SO2 as well as <a href="/facts/Ozone/o0E5gn2p">ozone</a> (O3), and <a href="/facts/Trisulfur/3jn3RdcG">trisulfur</a> (S3), it adopts a bent structure. The S-S bond length is 188.4 pm, the S-O bond is 146.5 pm and the SSO angle is 117.88°. The two dipole moment components are μa = 0.875 D and μb = 1.18 D.<a class="footnote-ref" id="fnref:4" href="#fn:4"><sup>4</sup></a> This species decomposes to give a polymeric sulfur oxides ("PSO's") with the approximate formula [S3O]<i>n</i>. PSO's decompose at room temperature to elemental sulfur and SO2. PSO's have been proposed to be responsible for the colour of <a href="/facts/Io_(moon)/p3Uc8FmK">Io</a>.<a class="footnote-ref" id="fnref:5" href="#fn:5"><sup>5</sup></a> </p><p>Trisulfur monoxide, S3O is an unstable molecule. It has been detected in the gas phase using neutralization-reionization <a href="/facts/Mass_spectrometry/RH5WBHJ2">mass spectrometry</a>. Both cyclic and chain structures were found.<a class="footnote-ref" id="fnref:6" href="#fn:6"><sup>6</sup></a> </p> <h2 id="cyclic-snoxx-1-2">Cyclic SnO<i>x</i> (<i>x</i> = 1, 2)</h2> <p>A number of monoxides S<i>n</i>O are known where <i>n</i> = 5-10. The oxygen atom is exocyclic.<a class="footnote-ref" id="fnref:7" href="#fn:7"><sup>7</sup></a> They can be prepared by oxidising the homocycles with <a href="/facts/Trifluoroperoxyacetic_acid/YDHkVHud">trifluoroperoxyacetic acid</a>:<a class="footnote-ref" id="fnref:8" href="#fn:8"><sup>8</sup></a> </p> S<i>n</i> + CF3C(O)OOH → S<i>n</i>O + CF3C(O)OH <p>The compounds are yellow or orange-coloured and thermally unstable near room temperature.<a class="footnote-ref" id="fnref:9" href="#fn:9"><sup>9</sup></a> </p> <table><tbody><tr><th>formula</th><th>color (25 °C)</th><th><a href="/facts/Melting_point/MY0w0h0k">m.p.</a> (°C)<a class="footnote-ref" id="fnref:10" href="#fn:10"><sup>10</sup></a></th></tr><tr><td>S6O</td><td>yellow</td><td>39</td></tr><tr><td>S7O</td><td>orange</td><td>55</td></tr><tr><td>S7O2</td><td>intense orange</td><td>60–62 (decomp.)</td></tr><tr><td><a href="/facts/Octasulfur_monoxide/NqqNKho3">S8O</a></td><td>orange</td><td>78 (decomposition)</td></tr><tr><td>S9O</td><td>intensely yellow</td><td>32-34</td></tr><tr><td>S10O</td><td>orange</td><td>51 (decomp.)</td></tr></tbody></table> <p>One dioxide is well characterized: the deep orange S7O2 (m.p. 60–62 °C with decomposition), which arises using trifluoroperoxoacetic acid.<a class="footnote-ref" id="fnref:11" href="#fn:11"><sup>11</sup></a> </p> <h2 id="references">References</h2> <ol> <li id="fn:1"><p>Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. <a href="978-0-08-037941-8" target="_blank">978-0-08-037941-8</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li> <li id="fn:2"><p>Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. <a href="978-0-08-037941-8" target="_blank">978-0-08-037941-8</a> <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li> <li id="fn:3"><p>R. Steudel (2003). "Sulfur-Rich Oxides SnO and SnO2". In Steudel, R. (ed.). Elemental Sulfur und Sulfur-Rich Compounds II. Berlin-Heidelberg: Springer. doi:10.1007/b13185. ISBN 9783540449515. <a href="9783540449515" target="_blank">9783540449515</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li> <li id="fn:4"><p>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. <a href="/wiki/Journal_of_Molecular_Spectroscopy" target="_blank">/wiki/Journal_of_Molecular_Spectroscopy</a> <a href="#fnref:4" class="footnote-back-ref">↩</a></p></li> <li id="fn:5"><p>Baklouti D., D; Schmitt, B.; Brissaud, O. (November 2004). "Infrared study of lower sulfur oxides on Io's surface". Bulletin of the American Astronomical Society. 36: 1099. Bibcode:2004DPS....36.1607B. <a href="/wiki/Bulletin_of_the_American_Astronomical_Society" target="_blank">/wiki/Bulletin_of_the_American_Astronomical_Society</a> <a href="#fnref:5" class="footnote-back-ref">↩</a></p></li> <li id="fn:6"><p>de Petris, G; Rosi M Troiani A (2006). "S3O and S3O+ in the gas phase: ring and open-chain structures". Chemical Communications (42): 4416–4418. doi:10.1039/b609646h. PMID 17057862. <a href="/wiki/Chemical_Communications" target="_blank">/wiki/Chemical_Communications</a> <a href="#fnref:6" class="footnote-back-ref">↩</a></p></li> <li id="fn:7"><p>R. Steudel (2003). "Sulfur-Rich Oxides SnO and SnO2". In Steudel, R. (ed.). Elemental Sulfur und Sulfur-Rich Compounds II. Berlin-Heidelberg: Springer. doi:10.1007/b13185. ISBN 9783540449515. <a href="9783540449515" target="_blank">9783540449515</a> <a href="#fnref:7" class="footnote-back-ref">↩</a></p></li> <li id="fn:8"><p>Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. <a href="978-0-08-037941-8" target="_blank">978-0-08-037941-8</a> <a href="#fnref:8" class="footnote-back-ref">↩</a></p></li> <li id="fn:9"><p>Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. <a href="978-0-08-037941-8" target="_blank">978-0-08-037941-8</a> <a href="#fnref:9" class="footnote-back-ref">↩</a></p></li> <li id="fn:10"><p>R. Steudel (2003). "Sulfur-Rich Oxides SnO and SnO2". In Steudel, R. (ed.). Elemental Sulfur und Sulfur-Rich Compounds II. Berlin-Heidelberg: Springer. doi:10.1007/b13185. ISBN 9783540449515. <a href="9783540449515" target="_blank">9783540449515</a> <a href="#fnref:10" class="footnote-back-ref">↩</a></p></li> <li id="fn:11"><p>Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8. <a href="978-0-08-037941-8" target="_blank">978-0-08-037941-8</a> <a href="#fnref:11" class="footnote-back-ref">↩</a></p></li> </ol>