Thioacetone
Names
Preferred IUPAC name
Propane-2-thione[1]
Systematic IUPAC name
Thiopropan-2-one
Other names
  • Propanethione
  • Thiopropanone
  • Thioacetone
  • Dimethyl thioketone
  • Sulfocarbon dimethanide
  • (Dimethyl)methylene sulfide
  • Sulfoacetone
  • Sulfopropanone
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/C3H6S/c1-3(2)4/h1-2H3
    Key: JTNXQVCPQMQLHK-UHFFFAOYSA-N
  • InChI=1/C3H6S/c1-3(2)4/h1-2H3
    Key: JTNXQVCPQMQLHK-UHFFFAOYAT
  • CC(=S)C
Properties
C3H6S
Molar mass 74.14 g·mol−1
Appearance Orange to brown liquid
Odor Putrid and intensely foul
Melting point −55°C(218.15k/-67°F)[2]
Boiling point 70°C(343.15k/158°F)[2]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Odor, skin irritant
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Thioacetone is an organosulfur compound belonging to the -thione group called thioketones with a chemical formula (CH3)2CS. It is an unstable orange or brown substance that can be isolated only at low temperatures.[3] Above −20 °C (−4 °F), thioacetone readily converts to a polymer and a trimer, trithioacetone.[4] It has an extremely potent, unpleasant odor, and is considered one of the worst-smelling chemicals known to humanity.[5]

Thioacetone was first obtained in 1889 by Baumann and Fromm, as a minor impurity in their synthesis of trithioacetone.[2]

Preparation

Thioacetone is usually obtained by cracking the cyclic trimer trithioacetone, [(CH3)2CS]3. The trimer is prepared by pyrolysis of allyl isopropyl sulfide or by treating acetone with hydrogen sulfide in the presence of a Lewis acid.[6][7] The trimer cracks at 500–600 °C (932–1,112 °F) to give the thione.[3][8][2]

Polymerization

Unlike its oxygen analogue acetone, which does not polymerise easily, thioacetone spontaneously polymerizes even at very low temperatures, pure or dissolved in ether or ethylene oxide, yielding a white solid that is a varying mixture of a linear polymer ···–[C(CH
3)
2–S–]
n–··· and the cyclic trimer trithioacetone. Infrared absorption of this product occurs mainly at 2950, 2900, 1440, 1150, 1360, and 1375 cm−1 due to the geminal methyl pairs, and at 1085 and 643 cm−1 due to the C–S bond. The 1H NMR spectra shows a single peak at x = 8.1.[2]

The mean molecular weight of the polymer varies from 2000 to 14000 depending on the preparation method, temperature, and presence of the thioenol tautomer. The polymer melts in the range of about 70 °C to 125 °C. Polymerization is promoted by free radicals and light.[2]

The cyclic trimer of thioacetone (trithioacetone) is a white or colorless compound with a melting point of 24 °C (75 °F), near room temperature. It also has a disagreeable odor.[4]

Odour

Thioacetone has an intensely foul odour. Like many low molecular weight organosulfur compounds, the smell is potent and can be detected even when highly diluted.[5] In 1889, an attempt to distill the chemical in the German city of Freiburg was followed by cases of vomiting, nausea, and unconsciousness in an area with a radius of 0.75 kilometres (0.47 mi) around the laboratory due to the smell.[9] In an 1890 report, British chemists at the Whitehall Soap Works in Leeds noted that dilution seemed to make the smell worse and described the smell as "fearful".[10] In 1967, Esso researchers repeated the experiment of cracking trithioacetone at a laboratory south of Oxford, UK. They reported their experience as follows:

Recently we found ourselves with an odour problem beyond our worst expectations. During early experiments, a stopper jumped from a bottle of residues, and, although replaced at once, resulted in an immediate complaint of nausea and sickness from colleagues working in a building two hundred yards [180 m] away. Two of our chemists who had done no more than investigate the cracking of minute amounts of trithioacetone found themselves the object of hostile stares in a restaurant and suffered the humiliation of having a waitress spray the area around them with a deodorant. The odours defied the expected effects of dilution since workers in the laboratory did not find the odours intolerable ... and genuinely denied responsibility since they were working in closed systems. To convince them otherwise, they were dispersed with other observers around the laboratory, at distances up to a quarter of a mile [0.40 km], and one drop of either acetone gem-dithiol or the mother liquors from crude trithioacetone crystallisations were placed on a watch glass in a fume cupboard. The odour was detected downwind in seconds.[5]

Thioacetone is sometimes considered a dangerous chemical due to its extremely foul odour and its supposed ability to render people unconscious, induce vomiting, and be detected over long distances.[citation needed]

See also

References

  1. ^ International Union of Pure and Applied Chemistry (2014). Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013. The Royal Society of Chemistry. p. 739. doi:10.1039/9781849733069. ISBN 978-0-85404-182-4.
  2. ^ a b c d e f William H. Sharkey (1979): "Polymerization through the carbon-sulfur double bond". Polymerization, series Advances in Polymer Science, volume 17, pages 73–103. doi:10.1007/3-540-07111-3_2
  3. ^ a b V.C.E. Burnop; K.G. Latham (1967). "Polythioacetone Polymer". Polymer. 8: 589–607. doi:10.1016/0032-3861(67)90069-9.
  4. ^ a b R.D. Lipscomb; W.H. Sharkey (1970). "Characterization and polymerization of thioacetone". Journal of Polymer Science Part A: Polymer Chemistry. 8 (8): 2187–2196. Bibcode:1970JPoSA...8.2187L. doi:10.1002/pol.1970.150080826.
  5. ^ a b c Derek Lowe (June 11, 2009). "Things I Won't Work With: Thioacetone". In The Pipeline.
  6. ^ Bailey, William J.; Chu, Hilda (1965). "Synthesis of polythioacetone". ACS Polymer Preprints. 6: 145–155.
  7. ^ Bohme, Horst; Pfeifer, Hans; Schneider, Erich (1942). "Dimeric thioketones". Berichte der Deutschen Chemischen Gesellschaft. 75B (7): 900–909. doi:10.1002/cber.19420750722. Note: This early report mistakes the trimer for the monomer
  8. ^ Kroto, H.W.; Landsberg, B.M.; Suffolk, R.J.; Vodden, A. (1974). "The photoelectron and microwave spectra of the unstable species thioacetaldehyde, CH3CHS, and thioacetone, (CH3)2CS". Chemical Physics Letters. 29 (2): 265–269. Bibcode:1974CPL....29..265K. doi:10.1016/0009-2614(74)85029-3. ISSN 0009-2614.
  9. ^ E. Baumann & E. Fromm (1889). "Ueber Thioderivate der Ketone". Berichte der Deutschen Chemischen Gesellschaft. 22 (2): 2592–2599. doi:10.1002/cber.188902202151.
  10. ^ Chemical News and Journal of Industrial Science. Chemical news office. 1890. p. 219.

External links

source: http://en.wikipedia.org/wiki/Thioacetone