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Phosgene

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"COCl2" redirects here. For the compound CoCl2, see Cobalt(II) chloride.
Not to be confused with phosphine, phosphene, oxalyl chloride, or phosgene oxime.
Phosgene[1]
Full structural formula with dimensions
Full structural formula with dimensions
Space-filling model
Space-filling model
A bag of toxic gases use in chemical warfare; the leftmost one is phosgene
Names
Preferred IUPAC name
Carbonyl dichloride[2]
Other names
Carbonyl chloride
CG
Carbon dichloride oxide
Carbon oxychloride
Chloroformyl chloride
Dichloroformaldehyde
Dichloromethanone
Dichloromethanal
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.000.792 Edit this at Wikidata
EC Number
  • 200-870-3
RTECS number
  • SY5600000
UNII
UN number 1076
  • InChI=1S/CCl2O/c2-1(3)4 checkY
    Key: YGYAWVDWMABLBF-UHFFFAOYSA-N checkY
  • InChI=1/CCl2O/c2-1(3)4
    Key: YGYAWVDWMABLBF-UHFFFAOYAH
  • ClC(Cl)=O
Properties
COCl2, also CCl2O
Molar mass 98.92 g/mol
Appearance Colorless gas
Odor Suffocating, like musty hay[3]
Density 4.248 g/L (15 °C, gas)
1.432 g/cm3 (0 °C, liquid)
Melting point −118 °C (−180 °F; 155 K)
Boiling point 8.3 °C (46.9 °F; 281.4 K)
Insoluble, reacts[4]
Solubility Soluble in benzene, toluene, acetic acid
Decomposes in alcohol and acid
Vapor pressure 1.6 atm (20°C)[3]
−48·10−6 cm3/mol
Structure
Planar, trigonal
1.17 D
Hazards
GHS labelling:
GHS04: Compressed Gas GHS05: Corrosive GHS06: Toxic[5]
Danger
H280, H314, H330[5]
P260, P280, P303+P361+P353+P315, P304+P340+P315, P305+P351+P338+P315, P403, P405[5]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
4
0
1
Flash point Non-flammable
0.1 ppm
Lethal dose or concentration (LD, LC):
500 ppm (human, 1 min)
340 ppm (rat, 30 min)
438 ppm (mouse, 30 min)
243 ppm (rabbit, 30 min)
316 ppm (guinea pig, 30 min)
1022 ppm (dog, 20 min)
145 ppm (monkey, 1 min)[6]
3 ppm (human, 2.83 h)
30 ppm (human, 17 min)
50 ppm (mammal, 5 min)
88 ppm (human, 30 min)
46 ppm (cat, 15 min)
50 ppm (human, 5 min)
2.7 ppm (mammal, 30 min)[6]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 0.1 ppm (0.4 mg/m3)[3]
REL (Recommended)
 TWA 0.1 ppm (0.4 mg/m3) C 0.2 ppm (0.8 mg/m3) [15-minute][3]
IDLH (Immediate danger)
 2 ppm[3]
Safety data sheet (SDS) [1]
Related compounds
Related compounds
 Thiophosgene
Formaldehyde
Carbonic acid
Urea
Carbon monoxide
Chloroformic acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Phosgene is the organic chemical compound with the formula COCl2. It is a colorless gas; in low concentrations, its odor resembles that of freshly cut hay or grass.[7] Phosgene is a valued industrial building block, especially for the production of precursors of polyurethanes and polycarbonate plastics.

Phosgene is very poisonous and was used as a chemical weapon during World War I, where it was responsible for 85,000 deaths.

In addition to its industrial production, small amounts occur from the breakdown and the combustion of organochlorine compounds.[8]

Structure and basic properties

Phosgene is a planar molecule as predicted by VSEPR theory. The C=O distance is 1.18 Å, the C−Cl distance is 1.74 Å and the Cl−C−Cl angle is 111.8°.[9] It is one of the simplest acyl chlorides, being formally derived from carbonic acid.

Production

Industrially, phosgene is produced by passing purified carbon monoxide and chlorine gas through a bed of porous activated carbon, which serves as a catalyst:[8]

CO + Cl2 → COCl2 (ΔHrxn = −107.6 kJ/mol)

This reaction is exothermic and is typically performed between 50 and 150 °C. Above 200 °C, phosgene reverts to carbon monoxide and chlorine, Keq(300 K) = 0.05. World production of this compound was estimated to be 2.74 million tonnes in 1989.[8]

Phosgene is fairly simple to produce, but as a scheduled chemical weapon is usually considered too dangerous to transport in bulk quantities. Instead, phosgene is usually produced and consumed within the same plant, as part of an "on demand" process. This involves maintaining equivalent rates of production and consumption, which keeps the amount of phosgene in the system at any one time fairly low, reducing the risks in the event of an accident.

Inadvertent generation

Upon ultraviolet (UV) radiation in the presence of oxygen simple organochlorides such as chloroform slowly convert into phosgene.[10] Phosgene is also formed as a metabolite of chloroform, likely via the action of cytochrome P-450.[11]

History

Phosgene was synthesized by the Cornish chemist John Davy (1790–1868) in 1812 by exposing a mixture of carbon monoxide and chlorine to sunlight. He named it "phosgene" from Greek φῶς (phos, light) and γεννάω (gennaō, to give birth) in reference of the use of light to promote the reaction.[12] It gradually became important in the chemical industry as the 19th century progressed, particularly in dye manufacturing.

Reactions and uses

The reaction of an organic substrate with phosgene is called phosgenation.[8]

Synthesis of carbonates

Diols react with phosgene to give either linear or cyclic carbonates (R = H, alkyl, aryl):

HOCR2−X−CR2OH + COCl2 → 1⁄n [OCR2−X−CR2OC(O)−]n + 2 HCl
One example is the reaction of phosgene with bisphenol A.[8] to form Polycarbonates.

Synthesis of isocyanates

The synthesis of isocyanates from amines illustrates the electrophilic character of this reagent and its use in introducing the equivalent synthon "CO2+":[13]

RNH2 + COCl2 → RN=C=O + 2 HCl (R = alkyl, aryl)

Such reactions are conducted on laboratory scale in the presence of a base such as pyridine that neutralizes the hydrogen chloride side-product.

On an industrial scale, phosgene is used in excess to increase yield and avoid side reactions. The phosgene excess is separated during the work-up of resulting end products and recycled into the process, with any remaining phosgene decomposed in water using activated carbon as the catalyst.

Laboratory uses

In the research laboratory, due to safety concerns phosgene nowadays finds limited use in organic synthesis. A variety of substitutes have been developed, notably trichloromethyl chloroformate ("diphosgene"), a liquid at room temperature, and bis(trichloromethyl) carbonate ("triphosgene"), a crystalline substance.[14] Aside from the previous reactions that are widely practiced industrially, phosgene is also used to produce acyl chlorides and carbon dioxide from carboxylic acids:

RCO2H + COCl2 → RC(O)Cl + HCl + CO2

Such acid chlorides react with amines and alcohols to give, respectively, amides and esters, which are commonly used intermediates. Thionyl chloride is more commonly and more safely employed for this application. A specific application for phosgene is the production of chloroformic esters such as benzyl chloroformate:

ROH + COCl2 → ROC(O)Cl + HCl

In the synthesis of choroformates phosgene is used in excess to prevent formation of the corresponding carbonate ester.

Phosgene is stored in bulks and metal cylinders. The outlet of cylinders is always standard, a tapered thread that is known as CGA 160.

Industrial use

Phosgene is used in industry for the production of aromatic di-isocyanates like toluene diisocyanate (TDI) and methylene diphenyl diisocyanate (MDI), which are precursors for production of polyurethanes and some polycarbonates. More than 90% of the worldwide produced phosgene is used in these processes, with the biggest production units located in the United States (Texas and Louisiana), Germany, Shanghai, Japan, and South Korea. The most important producers are Dow Chemical, Covestro, and BASF. Phosgene is used in the production of aliphatic diisocyanates such as hexamethylene diisocyanate (HDI) and isophorone diisocyanate (IPDI), which are precursors for the production of advanced coatings. Phosgene is also used to produce monoisocanates, used as pesticide precursors (e.g. methylisocyanate.)

Other reactions

Phosgene reacts with water to release hydrogen chloride and carbon dioxide:

COCl2 + H2O → CO2 + 2 HCl

Analogously, upon contact with ammonia, it converts to urea:

COCl2 + 4 NH3 → CO(NH2)2 + 2 NH4Cl

Halide exchange with nitrogen trifluoride and aluminium tribromide gives COF2 and COBr2, respectively.[8]

Chemical warfare

US Army phosgene identification poster from World War II
Further information: Chemical weapons in World War I and Second Italo-Ethiopian War

It is listed on Schedule 3 of the Chemical Weapons Convention: All production sites manufacturing more than 30 tonnes per year must be declared to the OPCW.[15] Although less toxic than many other chemical weapons such as sarin, phosgene is still regarded as a viable chemical warfare agent because of its simpler manufacturing requirements when compared to that of more technically advanced chemical weapons such as the first-generation nerve agent tabun.[16]

Phosgene was first deployed as a chemical weapon by the French in 1915 in World War I.[17] It was also used in a mixture with an equal volume of chlorine, with the chlorine helping to spread the denser phosgene.[18][19] Phosgene was more potent than chlorine, though some symptoms took 24 hours or more to manifest.

Following the extensive use of phosgene during World War I, it was stockpiled by various countries.[20][21][22]

Phosgene was then only infrequently used by the Imperial Japanese Army against the Chinese during the Second Sino-Japanese War.[23] Gas weapons, such as phosgene, were produced by Unit 731.

Toxicology and safety

Phosgene is an insidious poison as the odor may not be noticed and symptoms may be slow to appear.[24]

The odor detection threshold for phosgene is 0.4 ppm, four times the threshold limit value. Its high toxicity arises from the action of the phosgene on the –OH, –NH2 and –SH groups of the proteins in pulmonary alveoli (the site of gas exchange), respectively forming ester, amide and thioester functional groups in accord with the reactions discussed above. This results in disruption of the blood–air barrier, eventually causing pulmonary edema. The extent of damage in the alveoli does not primarily depend on phosgene concentration in the inhaled air, with the dose (amount of inhaled phosgene) being the critical factor.[25] Dose can be approximately calculated as "concentration" × "duration of exposure".[25][26] Therefore, persons in workplaces where there exists risk of accidental phosgene release usually wear indicator badges close to the nose and mouth.[27] Such badges indicate the approximate inhaled dose, which allows for immediate treatment if the monitored dose rises above safe limits. [27]

In case of low or moderate quantities of inhaled phosgene, the exposed person is to be monitored and subjected to precautionary therapy, then released after several hours. For higher doses of inhaled phosgene (above 150 ppm × min) a pulmonary edema often develops which can detected by X-ray imaging and regressive blood oxygen concentration. Inhalation of such high doses can eventually result in fatality within hours up to 2–3 days of the exposure.

The risk connected to a phosgene inhalation is based not so much on its toxicity (which is much lower in comparison to modern chemical weapons like sarin or tabun) but rather on its typical effects: the affected person may not develop any symptoms for hours until an edema appears, at which point it could be too late for medical treatment to assist.[28] All fatalities as a result of accidental releases from the industrial handling of phosgene occurred in this fashion. On the other hand, pulmonary edemas treated in a timely manner usually heal in the mid- and longterm, without major consequences once some days or weeks after exposure have passed.[29][30] Nonetheless, the detrimental health effects on pulmonary function from untreated, chronic low-level exposure to phosgene should not be ignored; although not exposed to concentrations high enough to immediately cause an edema, many synthetic chemists (e.g. Leonidas Zervas) working with the compound were reported to experience chronic respiratory health issues and eventual respiratory failure from continuous low-level exposure.

If accidental release of phosgene occurs in an industrial or laboratory setting, it can be mitigated with ammonia gas; in the case of liquid spills (e.g. of diphosgene or phosgene solutions) an absorbent and sodium carbonate can be applied.[31]

Accidents

  • The first major phosgene-related incident happened in May 1928 when eleven tons of phosgene escaped from a war surplus store in central Hamburg.[32] Three hundred people were poisoned, of whom ten died.[32]
  • In the second half of 20th century several fatal incidents implicating phosgene occurred in Europe, Asia and the US. Most of them have been investigated by authorities and the outcome made accessible to the public. For example, phosgene was initially blamed for the Bhopal disaster, but investigations proved methyl isocyanate to be responsible for the numerous poisonings and fatalities.
  • Recent major incidents happened in January 2010 and May 2016. An accidental release of phosgene gas at a DuPont facility in West Virginia killed one employee in 2010.[33] The US Chemical Safety Board released a video detailing the accident.[34] Six years later, a phosgene leak occurred in a BASF plant in South Korea, where a contractor inhaled a lethal dose of phosgene.[35]

See also

References

  1. ^ Merck Index, 11th Edition, 7310.
  2. ^ Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. p. 798. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4.
  3. ^ a b c d e NIOSH Pocket Guide to Chemical Hazards. "#0504". National Institute for Occupational Safety and Health (NIOSH).
  4. ^ "PHOSGENE (cylinder)". Inchem (Chemical Safety Information from Intergovernmental Organizations). International Programme on Chemical Safety and the European Commission.
  5. ^ a b c Record of Phosgene in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on 16 March 2021.
  6. ^ a b "Phosgene". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  7. ^ CBRNE - Lung-Damaging Agents, Phosgene May 27, 2009
  8. ^ a b c d e f Wolfgang Schneider; Werner Diller. "Phosgene". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_411. ISBN 978-3527306732.
  9. ^ Nakata, M.; Kohata, K.; Fukuyama, T.; Kuchitsu, K. (1980). "Molecular Structure of Phosgene as Studied by Gas Electron Diffraction and Microwave Spectroscopy. The rz Structure and Isotope Effect". Journal of Molecular Spectroscopy. 83: 105–117. doi:10.1016/0022-2852(80)90314-8.
  10. ^ Singh, Hanwant Bir (December 1976). "Phosgene in the ambient air". Nature. 264 (5585): 428–429. doi:10.1038/264428a0.
  11. ^ Pohl, Lance R.; Bhooshan, B.; Whittaker, Noel F.; Krishna, Gopal (December 1977). "Phosgene: A metabolite of chloroform". Biochemical and Biophysical Research Communications. 79 (3): 684–691. doi:10.1016/0006-291X(77)91166-4.
  12. ^ John Davy (1812). "On a gaseous compound of carbonic oxide and chlorine". Philosophical Transactions of the Royal Society of London. 102: 144–151. doi:10.1098/rstl.1812.0008. JSTOR 107310. Phosgene was named on p. 151: " ... it will be necessary to designate it by some simple name. I venture to propose that of phosgene, or phosgene gas; from φως, light, γινομαι, to produce, which signifies formed by light; ... "
  13. ^ R. L. Shriner, W. H. Horne, and R. F. B. Cox (1943). "p-Nitrophenyl Isocyanate". Organic Syntheses{{cite journal}}: CS1 maint: multiple names: authors list (link); Collected Volumes, vol. 2, p. 453.
  14. ^ Hamley, P. "Phosgene" Encyclopedia of Reagents for Organic Synthesis, 2001 John Wiley, New York. doi:10.1002/047084289X.rp149
  15. ^ Annex on Implementation and Verification ("Verification Annex") Archived 2006-05-15 at the Wayback Machine.
  16. ^ https://itportal.decc.gov.uk/cwc_files/S2AAD_guidance.pdf.
  17. ^ Nye, Mary Jo (1999). Before big science: the pursuit of modern chemistry and physics, 1800–1940. Harvard University Press. p. 193. ISBN 0-674-06382-1.
  18. ^ Staff (2004). "Choking Agent: CG". CBWInfo. Archived from the original on 2006-02-18. Retrieved 2007-07-30.
  19. ^ Kiester, Edwin; et al. (2007). An Incomplete History of World War I. Vol. 1. Murdoch Books. p. 74. ISBN 978-1-74045-970-9.
  20. ^ Base's phantom war reveals its secrets, Lithgow Mercury, 7/08/2008
  21. ^ Chemical warfare left its legacy, Lithgow Mercury, 9/09/2008
  22. ^ Chemical bombs sit metres from Lithgow families for 60 years, The Daily Telegraph, September 22, 2008
  23. ^ Yuki Tanaka, "Poison Gas, the Story Japan Would Like to Forget", Bulletin of the Atomic Scientists, October 1988, pp. 16–17
  24. ^ Borak J.; Diller W. F. (2001). "Phosgene exposure: mechanisms of injury and treatment strategies". Journal of Occupational and Environmental Medicine. 43 (2): 110–9. doi:10.1097/00043764-200102000-00008. PMID 11227628. S2CID 41169682.
  25. ^ a b Werner F. Diller, Early Diagnosis of Phosgene Overexposure.Toxicology and Industrial Health, Vol.1, Nr.2, April 1985, p. 73 -80
  26. ^ W. F. Diller, R. Zante : Zentralbl. Arbeitsmed. Arbeitsschutz Prophyl. Ergon. 32, (1982) 60 -368
  27. ^ a b W. F.Diller, E.Drope, E. Reichold: Ber. Int. Kolloq. Verhütung von Arbeitsunfällen und Berufskrankheiten Chem. Ind.6 th (1979) Chem. Abstr. 92 (1980) 168366x
  28. ^ W. F. Diller: Radiologische Untersuchungen zur verbesserten Frühdiagnose von industriellen Inhalationsvergiftungen mit verzögertem Wirkungseintritt, Verlag für Medizin Dr. E. Fischer, Heidelberg. Zentralbatt für Arbeitsmedizin, Arbeitsschutz und Ergonomie, Nr. 3, Mai 2013, p. 160 - 163
  29. ^ W.F. Diller, F. Schnellbächer, F. Wüstefeld : Zentralbl. Arbeitsmed. Arbeitsschutz Prophyl. 29 (1979) p.5-16
  30. ^ Results From the US Industry-Wide Phosgene Surveillance "The Diller Registry" : Journal of Occ. and Env. Med., March 2011-Vol.53-iss. 3 p.239- 244
  31. ^ "Phosgene: Health and Safety Guide". International Programme on Chemical Safety. 1998.
  32. ^ a b Ryan, T.Anthony (1996). Phosgene and Related Carbonyl Halides. Elsevier. pp. 154–155. ISBN 0444824456.
  33. ^ https://www.csb.gov/dupont-corporation-toxic-chemical-releases/
  34. ^ Fatal Exposure: Tragedy at DuPont, retrieved 2021-07-02
  35. ^ https://www.youtube.com/watch?v=ISNGimMXL7M
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