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Ethenone - Wikipedia
Wikipedia

Ethenone

Ethenone is the formal name for ketene, an organic compound with formula C2H2O or H2C=C=O. It is the simplest member of the ketene class. It is an important reagent for acetylations.[4][5]

Ethenone
Structural formula
Space-filling model
Names
Preferred IUPAC name
Ethenone[1]
Other names
Ketene
Carbomethene
Keto-ethylene
Identifiers
3D model (JSmol)
1098282
ChEBI
ChemSpider
ECHA InfoCard 100.006.671 Edit this at Wikidata
EC Number
  • 207-336-9
RTECS number
  • OA7700000
UNII
  • InChI=1S/C2H2O/c1-2-3/h1H2 checkY
    Key: CCGKOQOJPYTBIH-UHFFFAOYSA-N checkY
  • InChI=1/C2H2O/c1-2-3/h1H2
    Key: CCGKOQOJPYTBIH-UHFFFAOYSA-N
  • InChI=1/C2H2O/c1-2-3/h1H2
    Key: CCGKOQOJPYTBIH-UHFFFAOYAO
  • O=C=C
Properties
C2H2O
Molar mass 42.037 g/mol
Appearance Colourless gas
Odor penetrating
Density 1.93 g/cm3
Melting point −150.5 °C (−238.9 °F; 122.6 K)
Boiling point −56.1 °C (−69.0 °F; 217.1 K)
decomposes
Solubility soluble in acetone
ethanol
ethyl ether
aromatic solvents
halocarbons
Vapor pressure >1 atm (20°C)[2]
1.4355
Thermochemistry
51.75 J/K mol
Std enthalpy of
formation (ΔでるたfH⦵298)
 -87.24 kJ/mol
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 4: Will rapidly or completely vaporize at normal atmospheric pressure and temperature, or is readily dispersed in air and will burn readily. Flash point below 23 °C (73 °F). E.g. propaneInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
4
4
1
Flash point −107 °C (−161 °F; 166 K)
Explosive limits 5.5-18%
Lethal dose or concentration (LD, LC):
1300 mg/kg (oral, rat)
17 ppm (mouse, 10 min)[3]
23 ppm (mouse, 30 min)
53 ppm (rabbit, 2 hr)
53 ppm (guinea pig, 2 hr)
750 ppm (cat, 10 min)
200 ppm (monkey, 10 min)
50 ppm (mouse, 10 min)
1000 ppm (rabbit, 10 min)[3]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 0.5 ppm (0.9 mg/m3)[2]
REL (Recommended)
 TWA 0.5 ppm (0.9 mg/m3) ST 1.5 ppm (3 mg/m3)[2]
IDLH (Immediate danger)
 5 ppm[2]
Safety data sheet (SDS) External MSDS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Properties

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Ethenone is a highly reactive gas (at standard conditions) and has a sharp irritating odour. It is only reasonably stable at low temperatures (−80 °C). It must therefore always be prepared for each use and processed immediately, otherwise a dimerization to diketene occurs or it reacts to polymers that are difficult to handle. The polymer content formed during the preparation is reduced, for example, by adding sulfur dioxide to the ketene gas.[6] Because of its cumulative double bonds, ethenone is highly reactive and reacts in an addition reaction H-acidic compounds to the corresponding acetic acid derivatives. It does for example react with water to acetic acid or with primary or secondary amines to the corresponding acetamides.

Preparation

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Ethenone is produced by thermal dehydration of acetic acid at 700–750 °C in the presence of triethyl phosphate as a catalyst:[7][8]

CH3CO2H → CH2=C=O + H2O

It has also been produced on a laboratory scale by the thermolysis of acetone at 600–700 °C.[9][10]

CH3COCH3 →CH2=C=O + CH4

This reaction is called the Schmidlin ketene synthesis.[11]

On a laboratory scale it can be produced by the thermal decomposition of Meldrum's acid at temperatures greater than 200 °C.[citation needed]

History

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When passed through heated pipes or electrically heated metal (like copper) wires at 500-600 °C in the presence of carbon disulfide, acetone decomposes into methane and ethenone, with 95% yield.[12][13] Ethenone was discovered at the same time by Hermann Staudinger (by reaction of bromoacetyl bromide with metallic zinc)[14][15] The dehydration of acetic acid was reported in 1910.[16]

 

The thermal decomposition of acetic anhydride was also described.[17]

 
 
 

Natural occurrence

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Ethenone has been observed to occur in space, in comets or in gas as part of the interstellar medium.[18]

Use

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Ethenone is used to make acetic anhydride from acetic acid. Generally it is used for the acetylation of chemical compounds.[19]

 
Reactions with ammonia, water, ethanol, and acetic acid
 
Mechanism of the above reactions

Ethenone reacts with methanal in the presence of catalysts such as Lewis acids (AlCl3, ZnCl2 or BF3) to give βべーた-propiolactone.[20] The technically most significant use of ethenone is the synthesis of sorbic acid by reaction with 2-butenal (crotonaldehyde) in toluene at about 50 °C in the presence of zinc salts of long-chain carboxylic acids. This produces a polyester of 3-hydroxy-4-hexenoic acid, which is thermally[21] or hydrolytically depolymerized to sorbic acid.

Ethenone is very reactive, tending to react with nucleophiles to form an acetyl group. For example, it reacts with water to form acetic acid;[22] with acetic acid to form acetic anhydride; with ammonia and amines to form ethanamides;[23] and with dry hydrogen halides to form acetyl halides.[24]

The formation of acetic acid likely occurs by an initial formation of 1,1-dihydroxyethene, which then tautomerizes to give the final product.[25]

Ethenone will also react with itself via [2 + 2] photocycloadditions to form cyclic dimers known as diketenes. For this reason, it should not be stored for long periods.[26]

Hazards

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Exposure to concentrated levels causes humans to experience irritation of body parts such as the eye, nose, throat and lungs. Extended toxicity testing on mice, rats, guinea pigs and rabbits showed that ten-minute exposures to concentrations of freshly generated ethenone as low as 0.2 mg/liter (116 ppm) may produce a high percentage of deaths in small animals. These findings show ethenone is toxicologically identical to phosgene.[27][19]

The formation of ketene in the pyrolysis of vitamin E acetate, an additive of some e-liquid products, is one possible mechanism of the reported pulmonary damage[28] caused by electronic cigarette use.[29] A number of patents describe the catalytic formation of ketene from carboxylic acids and acetates, using a variety of metals or ceramics, some of which are known to occur in e-cigarette devices from patients with e-cigarette or vaping product-use associated lung injury (EVALI).[30][31]

Occupational exposure limits are set at 0.5 ppm (0.9 mg/m3) over an eight-hour time-weighted average.[32] An IDLH limit is set at 5 ppm, as this is the lowest concentration productive of a clinically relevant physiologic response in humans.[33]

References

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  1. ^ "Front Matter". Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. p. 723. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4.
  2. ^ a b c d NIOSH Pocket Guide to Chemical Hazards. "#0367". National Institute for Occupational Safety and Health (NIOSH).
  3. ^ a b "Ketene". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  4. ^ Miller, Raimund; Abaecherli, Claudio; Said, Adel; Jackson, Barry (2001). "Ketenes". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a15_063. ISBN 3527306730.
  5. ^ Mitzel, Thomas M.; Pigza, Julie A. (2009). "Ketene". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rk000.pub2. ISBN 978-0-471-93623-7.
  6. ^ EP 0377438, R. Bergamin et al., issued 1990-06-11, assigned to Lonza AG 
  7. ^ Miller, Raimund; Abaecherli, Claudio; Said, Adel; Jackson, Barry (2001). "Ketenes". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a15_063. ISBN 978-3-527-30385-4.
  8. ^ Arpe, Hans-Jürgen (2007), Industrielle organische Chemie: Bedeutende vor- und Zwischenprodukte (in German) (6th ed.), Weinheim: Wiley-VCH, pp. 200–201, ISBN 978-3-527-31540-6[permanent dead link]
  9. ^ Weygand C (1972). Hilgetag G, Martini A (eds.). Weygand/Hilgetag Preparative Organic Chemistry (4th ed.). New York: John Wiley & Sons, Inc. pp. 1031–1032. ISBN 978-0471937494.
  10. ^ Hurd CD, Kamm O (1941). "Ketene in Organic Syntheses". Organic Syntheses. Vol. Collective Vol. 1. p. 330.
  11. ^ Schmidlin J, Bergman M (1910). "Darstellung des Ketens aus Aceton" [Preparation of ketene from acetone]. Berichte der Deutschen Chemischen Gesellschaft (in German). 43 (3): 2821–2823. doi:10.1002/cber.19100430340.
  12. ^ K.-H. Lautenschläger, W. Schröter, A. Wanninger, "Taschenbuch der Chemie", 20. Aufl. 2006, ISBN 978-3-8171-1761-1.
  13. ^ "Ketene". Organic Syntheses. doi:10.15227/orgsyn.004.0039.
  14. ^ H. Staudinger H. W. Klever (1908): "Keten. Bemerkung zur Abhandlung zur Abhandlung der HHrn. V.T. Wilsmore und A. W. Stewart". Berichte der deutschen chemischen Gesellschaft, volume 41, issue 1, pages 1516-1517. doi:10.1002/cber.190804101275
  15. ^ Tidwell, T. T. (2005), "Ein Jahrhundert Ketene (1905–2005): die Entdeckung einer vielseitigen Klasse reaktiver Intermediate". Angewandte Chemie, volume 117, pages 5926–5933. doi:10.1002/ange.200500098
  16. ^ J. Schmidlin, M. Bergman (1910): Berichte der deutschen chemischen Gesellschaft, volume 43, pages 2821- doi:10.1002/cber.19100430340
  17. ^ Norman Thomas Mortimer Wilsmore (1907): "Keten". Journal of the Chemical Society, Transactions, volume 91, article CLXXXVIII (188), pages 1938-1941. doi:10.1039/ct9079101938
  18. ^ Hudson, Reggie L.; Loeffler, Mark J. (31 July 2013). "Ketene Formation in Interstellar Ices: A Laboratory Study". The Astrophysical Journal. 773 (2): 109. Bibcode:2013ApJ...773..109H. doi:10.1088/0004-637x/773/2/109. hdl:2060/20140010162. S2CID 37437108.
  19. ^ a b Entry on Diketen. at: Römpp Online. Georg Thieme Verlag, retrieved 16. Juni 2014.
  20. ^ Hans-Jürgen Arpe, "Industrielle Organische Chemie", 6. Aufl., 2007, WILEY-VCH Verlag, Weinheim, ISBN 978-3-527-31540-6.
  21. ^ EP 1295860, D. Decker et al., issued 26. März 2003-03-26, assigned to Nutrinova GmbH 
  22. ^ Tidwell, p. 11.
  23. ^ Tidwell, p. 560.
  24. ^ ChemSpider http://www.chemspider.com/Chemical-Structure.9643.html
  25. ^ Nguyen, Minh Tho; Raspoet, Greet (1999). "The hydration mechanism of ketene: 15 years later". Can. J. Chem. 77 (5–6): 817–829. doi:10.1139/v99-090.
  26. ^ Christoph Taeschler :Ketenes, Ketene Dimers, and Related Substances, Kirk-Othmer Encyclopedia of Chemical Technology, John Wiley & Sons, New York, 2010
  27. ^ H. A. Wooster; C. C. Lushbaugh; C. E. Redeman (1946). "The Inhalation Toxicity of Ketene and of Ketene Dimer". J. Am. Chem. Soc. 68 (12): 2743. doi:10.1021/ja01216a526.
  28. ^ "The Vaping-Related Lung Disease Outbreak May be Coming to an End". 20 December 2019.
  29. ^ Wu, Dan; O’Shea, Donal F. (24 March 2020). "Potential for release of pulmonary toxic ketene from vaping pyrolysis of vitamin E acetate". Proceedings of the National Academy of Sciences. 117 (12): 6349–6355. Bibcode:2020PNAS..117.6349W. doi:10.1073/pnas.1920925117. PMC 7104367. PMID 32156732.
  30. ^ Attfield, Kathleen R.; Chen, Wenhao; Cummings, Kristin J.; Jacob, Peyton; O’Shea, Donal F.; Wagner, Jeff; Wang, Ping; Fowles, Jefferson (15 October 2020). "Potential of Ethenone (Ketene) to Contribute to Electronic Cigarette, or Vaping, Product Use–associated Lung Injury". American Journal of Respiratory and Critical Care Medicine. 202 (8): 1187–1189. doi:10.1164/rccm.202003-0654LE. PMID 32551843. S2CID 219919028.
  31. ^ U.S. patent No. 5475144. Catalyst and process for synthesis of ketenes from carboxylic acids. Dec 12, 1995. https://patents.google.com/patent/US5475144A/en
  32. ^ Centers for Disease Control and Prevention (4 April 2013). "Ketene". NIOSH Pocket Guide to Chemical Hazards. Retrieved 13 November 2013.
  33. ^ Centers for Disease Control and Prevention (May 1994). "Ketene". Documentation for Immediately Dangerous To Life or Health Concentrations (IDLHs). Retrieved 13 November 2013.

Literature

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