From Wikipedia, the free encyclopedia
  (Redirected from Tert-Butyl mercaptan)
Jump to: navigation, search
Skeletal formula of tert-butylthiol
Ball-and-stick model of the tert-butylthiol molecule
IUPAC name
Other names
t-BuSH; 2-Methylpropane-2-thiol; 2-Methyl-2-propanethiol; tert-Butyl mercaptan
75-66-1 YesY
Abbreviations TBM
ChemSpider 6147 YesY
Jmol-3D images Image
PubChem 6387
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).
 YesY verify (what isYesY/N?)
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.


tert-Butylthiol likely does not occur naturally, but at least one publication has listed it as a very minor component of cooked potatoes.[2] 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]


tert-Butylthiol can react with metal alkoxides and acyl chlorides to form thiol esters, as shown in the equation:[6]

Reaction of tert-butylthiol with an acyl chloride.
Reaction of tert-butylthiol with an acyl chloride.

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 hexamethylphosphorous triamide (HMPT). 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]

Lithium 2-methylpropane-2-thiolate reaction with 7-methylguanosine.

Metal complexes[edit]

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]



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[edit]

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[edit]


  1. ^ "tert-butyl mercaptan". thegoodscentscompany.com. 
  2. ^ 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. 
  3. ^ Dobbin, Leonard (1890). "On tertiary Butyl Mercaptan". Journal of the Chemical Society, Transactions 57: 639–643. doi:10.1039/ct8905700639. 
  4. ^ 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. 
  5. ^ Schulze, W.A.; Lyon, J.P. and Short, G.H. (1948). "Synthesis of Tertiary Alkyl Mercaptans". Industrial and Engineering Chemistry (American Chemical Society) 40 (12): 2308–2313. doi:10.1021/ie50468a019. 
  6. ^ a b 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. 
  7. ^ "2-propanethiol, 2-methyl-". National Institute of Standards and Technology. 
  8. ^ 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. 
  9. ^ a b 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. 
  10. ^ 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. 
  11. ^ "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.