Lewisite
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| Names | |
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| IUPAC name
2-chloroethenylarsonous dichloride
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| Other names
2-chloroethenyldichloroarsine
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| MeSH | lewisite |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| C2H2AsCl3 | |
| Molar mass | 207.32 g/mol |
| Density | 1.89 g/cm3 |
| Melting point | –18 °C |
| Boiling point | 190 °C |
| Hazards | |
| NFPA 704 (fire diamond) | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Lewisite is an organoarsenic compound, specifically an arsine. It was once manufactured in the U.S. and Japan as a chemical weapon, acting as a vesicant (blister agent) and lung irritant. Although colorless and odorless, impure samples of lewisite are a yellow or brown liquid with a distinctive odor that has been described as similar to scented geraniums.[2]
Chemical reactions
The compound is prepared by the addition of arsenic trichloride to acetylene:
- AsCl3 + C2H2 → ClCHCHAsCl2
Lewisite, like other arsenous chlorides, hydrolyses in water to form hydrochloric acid:
- ClCHCHAsCl2 + 2 H2O → "ClCHCHAs(OH)2" + 2 HCl
This reaction is accelerated in alkaline solutions, with poisonous (but non-volatile) sodium arsenite being the coproduct.
Mode of action as chemical weapon
It can easily penetrate ordinary clothing and even rubber; upon skin contact it causes immediate pain and itching with a rash and swelling. Large, fluid-filled blisters (similar to those caused by mustard gas exposure) develop after approximately 12 hours.[2] These are severe chemical burns. Sufficient absorption can cause systemic poisoning leading to liver necrosis or death.
Inhalation causes a burning pain, sneezing, coughing, vomiting, and possibly pulmonary edema.[2] Ingestion results in severe pain, nausea, vomiting, and tissue damage.[2] The results of eye exposure can range from stinging and strong irritation to blistering and scarring of the cornea.[3] Generalised symptoms also include restlessness, weakness, subnormal temperature and low blood pressure.
Chemical composition
Lewisite is usually found as a mixture, of 2-chlorovinylarsonous dichloride as well as bis(2-chloroethenyl)arsinous chloride ("lewisite 2"), and tris(2-chlorovinyl)arsine ("lewisite 3").
History
Lewisite is named after the US chemist and soldier Winford Lee Lewis (1878–1943). In 1918 he found the thesis of Julius Arthur Nieuwland at Maloney Hall, a chemical laboratory at The Catholic University of America, Washington DC in which Nieuwland detailed the synthesis by allowing arsenic trichloride to react with acetylene in the presence of a hydrochloric acid solution of mercuric chloride.
It was developed into a secret weapon at Nela Park (a facility located in Cleveland, Ohio at East 131st Street and Taft Avenue[4]) and given the name "the new G-34" to confuse its development with mustard gas.[citation needed] It was not used in World War I, but experimented with in the 1920s as the "Dew of Death."[5]
After World War I, the US became interested in lewisite because it was not flammable. It had the military symbol of M1 up into World War II, when it was changed to L. Field trials with lewisite during World War II demonstrated that casualty concentrations were not achievable under high humidity due to its rate of hydrolysis and its charactistic odor and lacrymation forced troops to don masks and avoid contaminated areas. The United States produced about 20,000 tons of lewisite, keeping it on hand primarily as an antifreeze for mustard gas or to penetrate protective clothing in special situations. It was replaced by the mustard gas variant HT (a 60:40 mixture of sulfur mustard and O Mustard), and declared obsolete in the 1950s. It is effectively treated with British anti-lewisite (dimercaprol). Most stockpiles of lewisite were neutralized with bleach and dumped into the Gulf of Mexico,[6] but some remain at the Deseret Chemical Depot. In 2010, lewisite was found in a World War I weapons dump in Washington, DC,[7]
Controversy over Japanese depots of lewisite in China
In mid 2006, China and Japan were negotiating disposal of stocks of lewisite in northeastern China, left by Japanese military during World War II. Residents of China have died over the past twenty years from accidental exposure to these stockpiles.[8]
References
- ^ Lewisite I - Compound Summary, PubChem.
- ^ a b c d Committee on Review and Evaluation of the Army Non-Stockpile Chemical Materiel Disposal Program, U.S. National Research Council (1999). National Academies Press. p. 16. ISBN 0309068797.
- ^ Lewisite. Emergency Response Database. National Institute for Occupational Safety and Health. Retrieved January 7, 2009.
- ^ Upton native's role was the best defense; WWI masks thwarted
- ^ Domingo Tabangcura, Jr. and G. Patrick Daubert, MD. British anti-Lewisite Development Molecule of the Month, University of Bristol School of Chemistry
- ^ Code Red - Weapons of Mass Destruction [Online Resource] - Blister Agents
- ^ Buried in a DC yard: WWI chemicals, weapons
- ^ Abandoned Chemical Weapons (ACW) in China