Phosgene

"COCl2" redirects here. For the compound CoCl₂, see Cobalt(II) chloride.

Not to be confused with phosphine, phosphene, oxalyl chloride, or phosgene oxime.

Phosgene

Names
IUPAC name Carbonyl dichloride
Other names CG; carbon dichloride oxide; carbon oxychloride; Chloroformyl chloride; dichloroformaldehyde; dichloromethanone; dichloromethanal
Identifiers
CAS Number	75-44-5 Y
ChEBI	CHEBI:29365 Y
ChemSpider	6131 Y
EC Number	200-870-3
Jmol 3D model	Interactive image
PubChem	6371
RTECS number	SY5600000
UNII	117K140075 Y
UN number	1076
InChI InChI=1S/CCl2O/c2-1(3)4 Y Key: YGYAWVDWMABLBF-UHFFFAOYSA-N Y InChI=1/CCl2O/c2-1(3)4 Key: YGYAWVDWMABLBF-UHFFFAOYAH
SMILES ClC(Cl)=O
Properties
Chemical formula	COCl2
Molar mass	98.92 g mol−1
Appearance	colorless gas
Odor	suffocating, like musty hay
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)
Solubility in water	decomposes in water
Solubility	soluble in benzene, toluene, acetic acid decomposes in alcohol and acid
Vapor pressure	1.6 atm (20°C)
Structure
Molecular shape	Planar, trigonal
Dipole moment	1.17 D
Vapor pressure	{{{value}}}
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).
Y verify (what is YN ?)
Infobox references

Phosgene is the chemical compound with the formula COCl₂. This colorless gas gained infamy as a chemical weapon during World War I where it was responsible for about 85% of the 100,000 deaths caused by chemical weapons. It is also a valued industrial reagent and building block in synthesis of pharmaceuticals and other organic compounds. In low concentrations, its odor resembles freshly cut hay or grass. In addition to its industrial production, small amounts occur naturally from the breakdown and the combustion of organochlorine compounds, such as those used in refrigeration systems. The chemical was named by combining the Greek words 'phos' (meaning light) and genesis (birth); it does not mean it contains any phosphorus (cf. phosphine).

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°. It is one of the simplest acid 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:

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

The reaction is exothermic, therefore the reactor must be cooled. Typically, the reaction is conducted between 50 and 150 °C. Above 200 °C, phosgene reverts to carbon monoxide and chlorine, K_eq (300K) = 0.05. World production of this compound was estimated to be 2.74 million tonnes in 1989.

Because of safety issues, phosgene is often produced and consumed within the same plant, and extraordinary measures are made to contain this toxic gas. 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. Although less dangerous than many other chemical weapons, such as sarin, phosgene is still regarded as a viable chemical warfare agent because it is so easy to manufacture when compared to the production requirements of more technically advanced chemical weapons such as the first-generation nerve agent tabun.

Adventitious occurrence

Upon ultraviolet (UV) radiation in the presence of oxygen, chloroform slowly converts into phosgene by a radical reaction. To suppress this photodegradation, chloroform is often stored in brown-tinted glass containers. Chlorinated compounds used to remove oil from metals, such as automotive brake cleaners, are converted to phosgene by the UV rays of arc welding processes.

Phosgene may also be produced during testing for leaks of older-style refrigerant gases. Chloromethanes (R12, R22 and others) were formerly leak-tested in situ by employing a small gas torch (propane, butane or propylene gas) with a sniffer tube and a copper reaction plate in the flame nozzle of the torch. If any refrigerant gas was leaking from a pipe or joint, the gas would be sucked into the flame via the sniffer tube and would cause a colour change of the gas flame to a bright greenish blue. In the process, phosgene gas would be created due to the thermal reaction. No valid statistics are available, but anecdotal reports suggest that numerous refrigeration technicians suffered the effects of phosgene poisoning due to their ignorance of the toxicity of phosgene, produced during such leak testing. Electronic sensing of refrigerant gases phased out the use of flame testing for leaks in the 1980s. Similarly, phosgene poisoning is a consideration for people fighting fires that are occurring in the vicinity of freon refrigeration equipment, smoking in the vicinity of a freon leak, or fighting fires using halon or halotron.

Uses

The great majority of phosgene is used in the production of isocyanates, the most important being toluene diisocyanate (TDI) and methylene diphenyl diisocyanate (MDI). These two isocyanates are precursors to polyurethanes.

Synthesis of carbonates

Significant amounts are also used in the production of polycarbonates by its reaction with bisphenol A. Polycarbonates are an important class of engineering thermoplastic found, for example, in lenses in eyeglasses. 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

Synthesis of isocyanates

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

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

Such reactions are conducted in the presence of a base such as pyridine that absorbs the hydrogen chloride.

Laboratory uses

In the research laboratory phosgene still 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. Aside from the above reactions that are widely practiced industrially, phosgene is also used to produce acid 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:

ROH + COCl₂ → ROC(O)Cl + HCl

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

Other chemistry

Although it is somewhat hydrophobic, phosgene reacts with water to release hydrogen chloride and carbon dioxide:

COCl₂ + H₂O → CO₂ + 2 HCl

Analogously, with ammonia, one obtains urea:

COCl₂ + 4 NH₃ → CO(NH₂)₂ + 2 NH₄Cl

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

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" in reference of the use of light to promote the reaction; from Greek, phos (light) and gene (born). It gradually became important in the chemical industry as the 19th century progressed, particularly in dye manufacturing.

Chemical warfare

Further information: Use of poison gas in World War I and Second Italo-Abyssinian War

Following the extensive use of phosgene gas in combat during World War I, it was stockpiled by various countries as part of their secret chemical weapons programs.

In May 1928, eleven tons of phosgene escaped from a war surplus store in central Hamburg. 300 people were poisoned of whom 10 died.

US Army phosgene identification poster from World War II

Phosgene was then only frequently used by the Imperial Japanese Army against the Chinese during the Second Sino-Japanese War. Gas weapons, such as phosgene, were produced by Unit 731 and authorized by specific orders given by Hirohito (Emperor Showa) himself, transmitted by the chief of staff of the army. For example, the Emperor authorized the use of toxic gas on 375 separate occasions during the Battle of Wuhan from August to October 1938.

Safety

Phosgene is an insidious poison as the odor may not be noticed and symptoms may be slow to appear. 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 proteins in the pulmonary alveoli, the site of gas exchange: their damage disrupts the blood–air barrier, causing suffocation. It reacts with the amines of the proteins, causing crosslinking by formation of urea-like linkages, in accord with the reactions discussed above. Phosgene detection badges are worn by those at risk of exposure.

Sodium bicarbonate may be used to neutralise liquid spills of phosgene. Gaseous spills may be mitigated with ammonia.

See also

• Diphosgene
• Triphosgene
• Bhopal disaster
• Carbonyl fluoride
• Carbonyl bromide
• Formaldehyde

External links

• Davy's account of his discovery of phosgene
• International Chemical Safety Card 0007
• CDC - Phosgene - NIOSH Workplace Safety and Health Topic
• NIOSH Pocket Guide to Chemical Hazards
• U.S. CDC Emergency Preparedness & Response
• U.S. EPA Acute Exposure Guideline Levels
• Regime For Schedule 3 Chemicals And Facilities Related To Such Chemicals, OPCW website
• CBWInfo website
• Use of Phosgene in WWII and in modern-day warfare (Refer to Section 4.C of the article)
• An experience with accidental poisoning by heated tetrachlorethylene solvent