Sulfur monoxide
Chemical compound From Wikipedia, the free encyclopedia
Sulfur monoxide is an inorganic compound with formula SO. It is only found as a dilute gas phase. When concentrated or condensed, it converts to S2O2 (disulfur dioxide). It has been detected in space but is rarely encountered intact otherwise.
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| Names | |||
|---|---|---|---|
| IUPAC name | |||
| Systematic IUPAC name
Oxidosulfur[1] | |||
| Identifiers | |||
3D model (JSmol) |
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| 7577656 | |||
| ChEBI | |||
| ChEMBL | |||
| ChemSpider | |||
| 666 | |||
| MeSH | sulfur+monoxide | ||
PubChem CID |
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CompTox Dashboard (EPA) |
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| Properties | |||
| SO | |||
| Molar mass | 48.064 g mol−1 | ||
| Appearance | Colourless gas | ||
| Reacts | |||
| log P | 0.155 | ||
| Thermochemistry | |||
Std molar entropy (S⦵298) |
221.94 J K−1 mol−1 | ||
Std enthalpy of formation (ΔfH⦵298) |
5.01 kJ mol−1 | ||
| Related compounds | |||
Related compounds |
Triplet oxygen Disulfur | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Structure and bonding
The SO molecule has a triplet ground state similar to O2 and S2, that is, each molecule has two unpaired electrons.[2] The S−O bond length of 148.1 pm is similar to that found in lower sulfur oxides (e.g. S8O, S−O = 148 pm) but is longer than the S−O bond in gaseous S2O (146 pm), SO2 (143.1 pm) and SO3 (142 pm).[2]
The molecule is excited with near infrared radiation to the singlet state (with no unpaired electrons). The singlet state is believed to be more reactive than the ground triplet state, in the same way that singlet oxygen is more reactive than triplet oxygen.[3]
Production and reactions
Summarize
Perspective
The SO molecule is thermodynamically unstable, converting initially to S2O2.[2] Consequently controlled syntheses typically do not detect the presence of SO proper, but instead the reaction of a chemical trap or the terminal decomposition products of S2O2 (sulfur and sulfur dioxide).
Production of SO as a reagent in organic syntheses has centred on using compounds that "extrude" SO. Examples include the decomposition of the relatively simple molecule ethylene episulfoxide:[4]
- C2H4SO → C2H4 + SO
Yields directly from an episulfoxide are poor, and improve only moderately when the carbons are sterically shielded.[5] A much better approach decomposes a diaryl cyclic trisulfide oxide, C10H6S3O, produced from thionyl chloride and the dithiol.[6]
SO inserts into alkenes, alkynes and dienes producing thiiranes, molecules with three-membered rings containing sulfur.[7]
Sulfur monoxide may form transiently during the metallic reduction of thionyl bromide.[8]
Generation under extreme conditions
In the laboratory, sulfur monoxide can be produced by treating sulfur dioxide with sulfur vapor in a glow discharge.[2] It has been detected in single-bubble sonoluminescence of concentrated sulfuric acid containing some dissolved noble gas.[9]
Benner and Stedman developed a chemiluminescence detector for sulfur via the reaction between sulfur monoxide and ozone:[10]
- SO + O3 → SO2* + O2
- SO2* → SO2 + hν
(* indicates an excited state)
Occurrence
Ligand for transition metals
As a ligand SO can bond in a number different ways:[11][12]
- a terminal ligand, with a bent M−O−S arrangement, for example with titanium oxyfluoride[13]
- a terminal ligand, with a bent M−S−O arrangement, analogous to bent nitrosyl
- bridging across two or three metal centres (via sulfur), as in Fe3(μ3-S)(μ3-SO)(CO)9
- η2 sideways-on (d–π interaction) with vanadium, niobium, and tantalum.[14]
Astrochemistry
Sulfur monoxide has been detected around Io, one of Jupiter's moons, both in the atmosphere[15] and in the plasma torus.[16] It has also been found in the atmosphere of Venus,[17] in Comet Hale–Bopp,[18] in 67P/Churyumov–Gerasimenko,[19] and in the interstellar medium.[20]
On Io, SO is thought to be produced both by volcanic and photochemical routes. The principal photochemical reactions are proposed as follows:[21]
- O + S2 → S + SO
- SO2 → SO + O
Biological chemistry
Sulfur monoxide may have some biological activity. The formation of transient SO in the coronary artery of pigs has been inferred from the reaction products, carbonyl sulfide and sulfur dioxide.[23]
Safety measures
Because of sulfur monoxide's rare occurrence in our atmosphere and poor stability, it is difficult to fully determine its hazards. But when condensed and compacted, it forms disulfur dioxide, which is relatively toxic and corrosive. This compound is also highly flammable (similar flammability to methane) and when burned produces sulfur dioxide, a poisonous gas.
Sulfur monoxide dication
Sulfur dioxide SO2 in presence of hexamethylbenzene C6(CH3)6 can be protonated under superacidic conditions (HF·AsF5) to give the non-rigid π-complex C6(CH3)6SO2+. The SO2+ moiety can essentially move barrierless over the benzene ring. The S−O bond length is 142.4(2) pm.[24]
- C6(CH3)6 + SO2 + 3 HF·AsF5 → [C6(CH3)6SO][AsF6]2 + [H3O][AsF6]
Disulfur dioxide
SO converts to disulfur dioxide (S2O2).[25] Disulfur dioxide is a planar molecule with C2v symmetry. The S−O bond length is 145.8 pm, shorter than in the monomer, and the S−S bond length is 202.45 pm. The O−S−S angle is 112.7°. S2O2 has a dipole moment of 3.17 D.[25]
References
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