|Jmol-3D images||Image 1|
|Molar mass||62.13 g mol−1|
|Density||0.846 g cm-3|
-98 °C, 175 K, -145 °F
35-41 °C, 308-314 K, 95-106 °F
|Vapor pressure||53.7 kPa (at 20 °C)|
|Refractive index (nD)||1.435|
|Std enthalpy of
|-66.9--63.9 kJ mol-1|
|Std enthalpy of
|-2.1818--2.1812 MJ mol-1|
|GHS signal word||DANGER|
|GHS hazard statements||H225, H315, H318, H335|
|GHS precautionary statements||P210, P261, P280, P305+351+338|
|EU classification||F Xn|
|R-phrases||R11, R22, R37/38, R41|
|S-phrases||S7, S9, S16, S26, S29, S33, S36/39|
|Flash point||-36 °C|
| (what is: / ?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Dimethyl sulfide (DMS) or methylthiomethane is an organosulfur compound with the formula (CH3)2S. Dimethyl sulfide is a water-insoluble flammable liquid that boils at 37 °C (99 °F) and has a characteristic disagreeable odor. It is a component of the smell produced from cooking of certain vegetables, notably maize, cabbage, beetroot and seafoods. It is also an indication of bacterial infection in malt production and brewing. It is a breakdown product of dimethylsulfoniopropionate (DMSP), and is also produced by the bacterial metabolism of methanethiol.
Natural occurrence 
DMS originates primarily from DMSP, a major secondary metabolite in some marine algae. DMS is the most abundant biological sulfur compound emitted to the atmosphere. Emission occurs over the oceans by phytoplankton. DMS is also produced naturally by bacterial transformation of dimethyl sulfoxide (DMSO) waste that is disposed of into sewers, where it can cause environmental odor problems.
DMS is oxidized in the marine atmosphere to various sulfur-containing compounds, such as sulfur dioxide, dimethyl sulfoxide (DMSO), dimethyl sulfone, methanesulfonic acid and sulfuric acid. Among these compounds, sulfuric acid has the potential to create new aerosols which act as cloud condensation nuclei. Through this interaction with cloud formation, the massive production of atmospheric DMS over the oceans may have a significant impact on the Earth's climate. The CLAW hypothesis suggests that in this manner DMS may play a role in planetary homeostasis.
Dimethyl sulfide is said to have a characteristic cabbage-like smell that becomes highly disagreeable at higher concentrations. While some report that DMS has a low olfactory threshold that varies from 0.02 to 0.1 ppm between different persons, it has been suggested that the odor attributed to dimethyl sulfide may in fact be due to di- and polysulfides and thiol impurities, since the odor of dimethyl sulfide is much less disagreeable after it is freshly washed with saturated aqueous mercuric chloride. Dimethyl sulfide is also available as a food additive to impart a savory flavor; in such use, its concentration is low. Beetroot, asparagus, cabbage, corn and seafoods produce dimethyl sulfide when cooked.
Marine phytoplankton also produces dimethyl sulfide. Andrew Johnston, of the University of East Anglia, has characterized DMS as being the "smell of the sea". It would be more accurate to say that DMS is a component of the "smell of the sea," another being pheromones of algae called dictyopterenes.
Dimethyl sulfide, dimethyl disulfide and dimethyl trisulfide have been confirmed as volatiles given off by the fly-attracting plant known as dead-horse arum (Helicodiceros muscivorus). The plant fools flies into pollinating it by emitting an odor like rotting meat, which is an attractive food source for flies.
Industrial uses 
||This section needs additional citations for verification. (October 2012)|
Dimethyl sulfide has been used in petroleum refining to presulfide hydrodesulfurization catalysts, although other disulfides or polysulfides are preferred and easier to handle. It is as a presulfiding agent to control the formation of coke and carbon monoxide in ethylene production. DMS is also used in a range of organic syntheses, including as a reducing agent in ozonolysis reactions. It also has a use as a food flavoring component. It can also be oxidized to dimethyl sulfoxide, (DMSO), which is an important industrial solvent.
The largest single commercial producer of DMS in the world is Gaylord Chemical Corporation, which until mid-2010 was a significant economic component of the paper industry of Bogalusa, Louisiana. The Bogalusa DMS plant operated continuously until this date, since its startup in 1961 by the now defunct Crown Zellerbach Corporation. The process technology practiced at the Bogalusa plant (alkylation of sulfur using Kraft lignin) is no longer in operation anywhere in the world. All DMS manufacturers currently use hydrocarbon-based feedstocks. Gaylord has no production of any kind at the old Louisiana site after opening its expanded DMS / Dimethyl sulfoxide operation in Tuscaloosa, Alabama in 2010.
ChevronPhillips Chemical Company is another major manufacturer of DMS. CP Chem produces this material at their facilities in Borger, Texas, USA and Tesserndelo, Belgium.
Other uses 
Dimethyl sulfide finds a niche use as a displaceable ligand in chloro(dimethyl sulfide)gold(I) and other coordination compounds.Dimethyl sulfide is also used in the ozonolysis of alkenes getting itself oxidized to DMSO.
Physiology of dimethyl sulfide 
See also 
- Coccolithophore, a marine unicellular planktonic photosynthetic algae, producer of DMS
- Dimethylsulfoniopropionate, a parent molecule of DMS and methanethiol in the oceans
- Dimethyl selenide, a selenium analogue of DMS produced by bacteria and phytoplankton
- Dimethyl telluride, a tellurium analogue of DMS
- Emiliania huxleyi, a coccolithophorid producing DMS
- Swern oxidation
- Gaia hypothesis
- "dimethyl sulfide (CHEBI:17437)". Chemical Entities of Biological Interest. UK: European Bioinformatics Institute. 17 October 2009. Main. Retrieved 19 October 2011.
- Simpson, D.; Winiwarter, W.; Börjesson, G.; Cinderby, S.; Ferreiro, A.; Guenther, A.; Hewitt, C. N.; Janson, R.; Khalil, M. A. K.; Owen, S.; Pierce, T. E.; Puxbaum, H.; Shearer, M.; Skiba, U.; Steinbrecher, R.; Tarrasón, L.; Öquist, M. G. (1999). "Inventorying emissions from nature in Europe". Journal of Geophysical Research 104 (D7): 8113–8152. Bibcode:1999JGR...104.8113S. doi:10.1029/98JD02747.
- Glindemann, D.; Novak, J.; Witherspoon, J. (2006). "Dimethyl Sulfoxide (DMSO) Waste Residues and Municipal Waste Water Odor by Dimethyl Sulfide (DMS): the North-East WPCP Plant of Philadelphia". Environmental Science and Technology 40 (1): 202–207. doi:10.1021/es051312a. PMID 16433352.
- Lucas, D. D.; Prinn, R. G. (2005). "Parametric sensitivity and uncertainty analysis of dimethylsulfide oxidation in the clear-sky remote marine boundary layer". Atmospheric Chemistry and Physics 5 (6): 1505–1525. doi:10.5194/acp-5-1505-2005.
- Malin, G.; Turner, S. M.; Liss, P. S. (1992). "Sulfur: The plankton/climate connection". Journal of Phycology 28 (5): 590–597. doi:10.1111/j.0022-3646.1992.00590.x.
- Charlson, R. J.; Lovelock, J. E.; Andreae, M. O.; Warren, S. G. (1987). "Oceanic phytoplankton, atmospheric sulphur, cloud albedo and climate". Nature 326 (6114): 655–661. Bibcode:1987Natur.326..655C. doi:10.1038/326655a0.
- Morton, T. H. (2000). "Archiving Odors". In Bhushan, N.; Rosenfeld, S. Of Molecules and Mind. Oxford: Oxford University Press. pp. 205–216.
- Parliment, T. H.; Kolor, M. G.; Maing, I. Y. (1977). "Identification of the Major Volatile Components of Cooked Beets". Journal of Food Science 42 (6): 1592–1593. doi:10.1111/j.1365-2621.1977.tb08434.x.
- http://www.springerlink.com.libproxy.tkk.fi/content/djbrepd4mjpjqgwn/[dead link]
- "Cloning the smell of the seaside". University of East Anglia. 2007-02-02.
- Itoh, T.; Inoue, H.; Emoto, S. (2000). "Synthesis of Dictyopterene A: Optically Active Tributylstannylcyclopropane as a Chiral Synthon". Bulletin of the Chemical Society of Japan 73 (2): 409–416. doi:10.1246/bcsj.73.409. ISSN 1348-0634.
- Stensmyr, M. C.; Urru, I.; Collu, I.; Celander, M.; Hansson, B. S.; Angioy, A.-M. (2002). "Rotting Smell of Dead-Horse Arum Florets". Nature 420 (6916): 625–626. doi:10.1038/420625a. PMID 12478279.
- "Locations". Gaylord Chemicals.
- Gahl, WA; Bernardini, I; Finkelstein, JD; Tangerman, A; Martin, JJ; Blom, HJ; Mullen, KD; Mudd, SH (1988 Feb). "Transsulfuration in an adult with hepatic methionine adenosyltransferase deficiency.". The Journal of Clinical Investigation 81 (2): 390–7. doi:10.1172/JCI113331. PMC 329581. PMID 3339126.
- Tangerman, A (2009 Oct 15). "Measurement and biological significance of the volatile sulfur compounds hydrogen sulfide, methanethiol and dimethyl sulfide in various biological matrices.". Journal of chromatography. B, Analytical technologies in the biomedical and life sciences 877 (28): 3366–77. doi:10.1016/j.jchromb.2009.05.026. PMID 19505855.
- "Intra- and extra-oral halitosis: finding of a new form of extra-oral blood-borne halitosis caused by dimethyl sulphide". J. Clin. Periodontol. 34 (9): 748–55. September 2007. doi:10.1111/j.1600-051X.2007.01116.x. PMID 17716310.
- Tangerman, A; Winkel, EG (2008 Mar). "The portable gas chromatograph OralChroma™: a method of choice to detect oral and extra-oral halitosis.". Journal of breath research 2 (1): 017010. doi:10.1088/1752-7155/2/1/017010. PMID 21386154.
- Tangerman, A; Winkel, EG (2010 Mar 2). "Extra-oral halitosis: an overview.". Journal of breath research 4 (1): 017003. Bibcode:2010JBR.....4a7003T. doi:10.1088/1752-7155/4/1/017003. PMID 21386205.
|Wikimedia Commons has media related to: Dimethyl sulfide|