Chemistry:Ethanethiol
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| Names | |
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| Preferred IUPAC name
Ethanethiol | |
| Other names
Ethyl mercaptan
Mercaptoethane Ethyl sulfhydrate | |
| Identifiers | |
3D model (JSmol)
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| ChEBI | |
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PubChem CID
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| UNII | |
| UN number | 2363 |
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| Properties | |
| C2H6S | |
| Molar mass | 62.13404 g·mol−1 |
| Appearance | Colorless liquid[3] |
| Odor | Rotten cabbage, flatulence, skunk-like[3] |
| Density | 0.8617 g·cm−3 |
| Melting point | −148 °C (−234 °F; 125 K) |
| Boiling point | 35 °C (95 °F; 308 K) |
| 0.7% (20 °C)[3] | |
| Vapor pressure | 442 mmHg (20 °C)[3] |
| Acidity (pKa) | 10.6 |
| −47.0×10−6 cm3/mol | |
| Hazards | |
| Main hazards | Nauseating |
| GHS pictograms |   
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| GHS Signal word | Danger |
| H225, H332, H410 | |
| P210, P233, P240, P241, P242, P243, P261, P271, P273, P280, P303+361+353, P304+312, P304+340, P312, P370+378, P391, P403+235, P501 | |
| NFPA 704 (fire diamond) | |
| Flash point | −48 °C; −55 °F; 225 K[3] |
| Explosive limits | 2.8–18.0%[3] |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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682 mg/kg (rat, oral)[4] |
LC50 (median concentration)
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4410 ppm (rat, 4 hr) 2770 (mouse, 4 hr)[4] |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
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C 10 ppm (25 mg/m3)[3] |
REL (Recommended)
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C 0.5 ppm (1.3 mg/m3) [15-minute][3] |
IDLH (Immediate danger)
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500 ppm[3] |
| Related compounds | |
Related compounds
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Methanethiol Butanethiol Ethanol thiophenol |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Ethanethiol, commonly known as ethyl mercaptan, is an organosulfur compound with the formula CH3CH2SH.[5] is a colorless liquid with a distinct odor. Abbreviated EtSH, it consists of an ethyl group (Et), CH3CH2, attached to a thiol group, SH. Its structure parallels that of ethanol, but with sulfur in place of oxygen. The odor of EtSH is infamous. Ethanethiol is more volatile than ethanol due to a diminished ability to engage in hydrogen bonding. Ethanethiol is toxic in high concentrations. It occurs naturally as a minor component of petroleum, and may be added to otherwise odorless gaseous products such as liquefied petroleum gas (LPG) to help warn of gas leaks. At these concentrations, ethanethiol is not harmful.
Preparation
Ethanethiol is prepared by the reaction of ethylene with hydrogen sulfide in the presence of various catalysts. It is also prepared commercially by the reaction of ethanol with hydrogen sulfide gas over an acidic solid catalyst, such as alumina.[6]
Historic methods
Ethanethiol was originally reported by Zeise in 1834.[7] Zeise treated calcium ethyl sulfate with a suspension of barium sulfide saturated with hydrogen sulfide. He is credited with naming the C2H5S- group as mercaptum.
Ethanethiol can also be prepared by a halide displacement reaction, where ethyl halide is treated with aqueous sodium bisulfide. This conversion was demonstrated as early as 1840 by Henri Victor Regnault.[8]
Odor
Ethanethiol has a strongly disagreeable odor that humans can detect in minute concentrations. The threshold for human detection is as low as one part in 2.8 billion parts of air (0.36 parts per billion). Its odor resembles that of leeks, onions, durian or cooked cabbage.[9]
Employees of the Union Oil Company of California reported first in 1938 that turkey vultures would gather at the site of any gas leak. After finding that this was caused by traces of ethanethiol in the gas it was decided to boost the amount of ethanethiol in the gas, to make detection of leaks easier. [10][11]
Uses
Ethanethiol is intentionally added to butane and propane (see: LPG) to impart an easily noticed smell to these normally odorless fuels that pose the threat of fire, explosion, and asphyxiation.
In the underground mining industry, ethanethiol or ethyl mercaptan is referred to as "stench gas".[12] The gas is released into mine ventilation systems during an emergency to alert mine workers. In Ontario, mining legislation dictates that "The alarm system in an underground mine shall, consist of the introduction into all workplaces of sufficient quantities of ethyl mercaptan gas or similar gas to be readily detectable by all workers".[13]
Reactions
Ethanethiol is a reagent in organic synthesis. In the presence of sodium hydroxide, it gives the powerful nucleophile EtS−. The salt can be generated quantitatively by reaction with sodium hydride.[14]
Ethanethiol can be oxidized to ethyl sulfonic acid, using strong oxidizing agents. Weaker oxidants, such as ferric oxide or hydrogen peroxide give the disulfide, diethyl disulfide:
- 2 EtSH + H2O2 → EtS-SEt + 2 H2O
Like other thiols, it behaves comparably to hydrogen sulfide. For example, it binds, concomitant with deprotonation to "soft" transition metal cations, such as Hg2+, Cu+, and Ni2+ to give polymeric thiolato complexes, Hg(SEt)2, CuSEt, and Ni(SEt)2, respectively.
See also
- tert-Butylthiol (tert-butyl mercaptan)
- Butanethiol (butyl mercaptan)
References
- ↑ Merck Index, 12th edition, hEllon and 3771
- ↑ "ICSC 0470 - ETHANETHIOL". http://www.inchem.org/documents/icsc/icsc/eics0470.htm.
- ↑ 3.0 3.1 3.2 3.3 3.4 3.5 3.6 3.7 3.8 NIOSH Pocket Guide to Chemical Hazards. "#0280". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0280.html.
- ↑ 4.0 4.1 "Ethyl mercaptan". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/75081.html.
- ↑ Staley, Dennis; Wilbraham, Antony; Matta, Michael; Waterman, Edward (2017). Pearson Chemistry. United States: Pearson Education, Inc.. pp. R25. ISBN 978-1-32-320590-7.
- ↑ Norell, John; Louthan, Rector P. (1988). "Thiols". Kirk-Othmer Concise Encyclopedia of Chemical Technology (3rd ed.). New York: John Wiley & Sons, Inc.. pp. 946–963. ISBN 978-0471801047.
- ↑ Zeise, William Christopher (1834). "Sur le Mercaptan; avec des Observations sur d'autres produits resultant de l'action des sulfovinates ainsi que de l'huile de vin, sur des sulfures metalliques" (in fr). Annales de Chimie et de Physique. 2nd series 56: 87–97. https://babel.hathitrust.org/cgi/pt?id=hvd.hx3dwt;view=1up;seq=93.
- ↑ Regnault, V (1840). "Ueber die Einwirkung des Chlors auf die Chlorwasserstoffäther des Alkohols und Holzgeistes und über mehrere Punkte der Aethertheorie" (in de). Annalen der Chemie und Pharmacie 34: 24–52. doi:10.1002/jlac.18400340103. https://babel.hathitrust.org/cgi/pt?id=hvd.hx3bgj;view=1up;seq=418. From p. 24: "Das Aethylsulfür war bis jetzt noch nicht dargestellt worden. Man erhält es sehr leicht durch wechselseitige Zersetzung, wenn man Aethylchlorür mit einer weingeistigen Auflösung von einfach Schwefelkalium zusammenbringt." (Ethanethiol still has not been prepared – until now. One obtains it very easily by reciprocal decomposition [i.e., salt metathesis reaction ], if one brings together ethyl chloride with a solution, in ethanol, of simple potassium hydrogen sulfide.)
- ↑ "Ethanethiol price,buy Ethanethiol - chemicalbook". https://www.chemicalbook.com/Price/Ethanethiol.htm#Properties.
- ↑ Gooley, Tristan (21 May 2015). The Walker's Guide to Outdoor Signs. Sceptre. pp. 242. ISBN 9781444780109.
- ↑ Nicholls, Henry. "The truth about vultures". http://www.bbc.com/earth/story/20150713-the-truth-about-vultures.
- ↑ "Stench Gas". Zacon Ltd.. http://www.zacon.ca/stench-gas.asp.
- ↑ "Occupational Health and Safety Act: R.R.O. 1990, REGULATION 854 MINES AND MINING PLANTS Sect. 26(6)(a)". Ontario Ministry of Labour. http://www.e-laws.gov.on.ca/html/regs/english/elaws_regs_900854_e.htm.
- ↑ Mirrington, R. N.; Feutrill, G. I. (1988). "Orcinol Monomethyl Ether". Organic Syntheses. http://www.orgsyn.org/demo.aspx?prep=CV6P0859.; Collective Volume, 6, pp. 859
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