tert-Butylthiol
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| Names | |
|---|---|
| Preferred IUPAC name
2-Methylpropane-2-thiol | |
| Other names
t-BuSH 2-Methylpropane-2-thiol 2-Methyl-2-propanethiol tert-Butyl mercaptan | |
| Identifiers | |
75-66-1  | |
| 3D model (Jmol) | Interactive image |
| Abbreviations | TBM |
| ChemSpider | 6147 |
| ECHA InfoCard | 100.000.810 |
| PubChem | 6387 |
| |
| |
| Properties | |
| C4H10S | |
| Molar mass | 90.18 g·mol−1 |
| Appearance | Colorless, clear liquid |
| Density | 0.8 g/mL |
| Melting point | −0.50 °C (31.10 °F; 272.65 K) |
| Boiling point | 62 to 65 °C (144 to 149 °F; 335 to 338 K) |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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| Infobox references | |
tert-Butylthiol, also known as 2-methylpropane-2-thiol, 2-methyl-2-propanethiol, tert-butyl mercaptan (TBM), and t-BuSH, is an organosulfur compound with the formula (CH3)3CSH. This thiol may have been used as a flavoring agent,[1] as an odorant for natural gas (which is odorless), and also in a wide range of organic reactions.
Preparation
At least one publication has listed tert-butylthiol as a very minor component of cooked potatoes,[2] but because the tert-butyl moiety is very rare in natural products, other sources doubt the existence of natural sources of the compound. The compound was first prepared in 1890 by Leonard Dobbin[3] by the reaction of zinc sulfide and t-butyl chloride.
The compound was later prepared in 1932 by the reaction of the Grignard reagent, t-BuMgCl, with sulfur to give the corresponding thiolate, followed by hydrolysis.[4] This preparation is shown below:
- t-BuMgCl + S → t-BuSMgCl
- t-BuSMgCl + H2O → t-BuSH + Mg(OH)Cl
It is currently prepared industrially by the reaction of isobutylene with hydrogen sulfide over a clay (silica alumina) catalyst.[5]
Reactions
tert-Butylthiol can react with metal alkoxides and acyl chlorides to form thiol esters, as shown in the equation:[6]
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_2-methylpropane-2-thiolate_reaction.svg.png)
In the reaction above, thallium(I) ethoxide converts to thallium(I) t-butylthiolate. In the presence of diethyl ether, thallium(I) t-butylthiolate reacts with acyl chlorides to give the corresponding tert-butyl thioesters.[6] Like other thioesters, it reverts to tert-butylthiol by hydrolysis.[7]
Lithium 2-methylpropane-2-thiolate can be prepared by treatment of tert-butylthiol with lithium hydride in an aprotic solvent such as hexamethylphosphoramide (HMPA). The resulting thiolate salt is a useful demethylating reagent. For example, treatment with 7-methylguanosine gives guanosine. Other N-methylated nucleosides in tRNA are not demethylated by this reagent.[8]
Metal complexes
The anion derived from tert-butylthiol forms complexes with various metals. One example is tetrakis(tert-butylthiolato)molybdenum(IV), Mo(t-BuS)4. This complex was prepared by treating MoCl4 with t-BuSLi:[9]
- MoCl4 + 4 t-BuSLi → Mo(t-BuS)4 + 4 LiCl
Mo(t-BuS)4 is a dark red diamagnetic complex that is sensitive to air and moisture. The molybdenum center has a distorted tetrahedral coordination to four sulfur atoms, with overall D2 symmetry.[9]
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Safety
Even in well ventilated areas, extreme caution must be made when handling tert-butylthiol as it is a highly odorous chemical with an odor threshold of <0.33 ppb.[10] Extreme caution is not due to toxicity, but due to the significant odor and the concern this odor could cause to individuals that might be exposed. The PEL for thiols of most types is 500 ppb, primarily due to reaction of nausea at levels of 2–3 ppm. The LC50 of tert-butylthiol is much, much higher.
Commercial use
tert-Butylthiol is the main ingredient in many gas odorant blends. It is always utilized as a blend of other compounds, typically dimethyl sulfide, methyl ethyl sulfide, tetrahydrothiophene or other mercaptans such as isopropyl mercaptan, sec-butyl mercaptan and/or n-butyl mercaptan, due to its rather high melting point of −0.5 °C (31.1 °F). These blends are used only with natural gas and not propane, as the boiling points of these blends and propane are quite different. As propane is delivered as a liquid and vaporizes to gas when being delivered to the appliance, the vapor liquid equilibrium would substantially reduce the amount of odorant blend in the vapor.
tert-Butylthiol has been listed on the European Food Safety Authority (FL-no: 12.174) as a flavor additive. There is no indication of what flavor(s) in which it may have been used. It has been removed from this list.[11]
See also
- Butanethiol (butyl mercaptan)
References
- ↑ "tert-butyl mercaptan". thegoodscentscompany.com.
- ↑ Gumbmann, M. R.; Burr, H. K. (1964). "Volatile Sulfur Compounds in Potatoes". Journal of Food and Agricultural Chemistry. 12 (5): 404–408. doi:10.1021/jf60135a004.
- ↑ Dobbin, Leonard (1890). "On tertiary Butyl Mercaptan". Journal of the Chemical Society, Transactions. 57: 639–643. doi:10.1039/ct8905700639.
- ↑ Rheinboldt, Heinrich; Mott, Friedrich; Motzkus, Erwin; A. D. McMaster; B. M. Mattson; S. T. Michel (1932). "Tertiäres Butylmercaptan". Journal fuer Praktische Chemie (Leipzig). 134 (9–12): 257–281. doi:10.1002/prac.19321340901.
- ↑ Schulze, W.A.; Lyon, J.P. & Short, G.H. (1948). "Synthesis of Tertiary Alkyl Mercaptans". Industrial and Engineering Chemistry. American Chemical Society. 40 (12): 2308–2313. doi:10.1021/ie50468a019.
- 1 2 Spessard, Gary O.; Chan, Wan Kit; Masamune, S. (1990). "Preparation of thiol esters: s-tert-butyl cyclohexanecarbothioate and s-tert-butyl 3α,7α,12α-trihydroxy-5β-cholane-24-thioate". Organic Syntheses. 7: 87.
- ↑ "2-propanethiol, 2-methyl-". National Institute of Standards and Technology.
- ↑ Ho, Tse-Lok; Fieser, Mary; Fieser, Louis (2006). "Lithium 2-methylpropane-2-thiolate". Fieser and Fieser's Reagents for Organic Synthesis. doi:10.1002/9780471264194.fos06530. ISBN 0471264199.
- 1 2 Otsuka, Sei; Kamata, Masato; Hirotsu, Ken; Higuchi, Taiichi (1981). "A Novel Molybdenum Thiolato Compound, Tetrakis(tert-butylthiolato)molybdenum(IV). Preparation and Crystal and Molecular Structure". J. Am. Chem. Soc. 103 (11): 3011–3014. doi:10.1021/ja00401a017.
- ↑ Devos, M; Patte, F.; Rouault, J.; Lafort, P.; Van Gemert, L. J. (1990). Standardized Human Olfactory Thresholds. Oxford: IRL Press at Oxford University Press. p. 118. ISBN 0199631468.
- ↑ "Scientific Opinion on Flavouring Group Evaluation 8, Revision 3 (FGE.08Rev3): Aliphatic and alicyclic mono-, di-, tri-, and polysulphides with or without additional oxygenated functional groups from chemical groups 20 and 30". EFSA. Retrieved 15 April 2013.