Parathion

Parathion, also called parathion-ethyl or diethyl parathion and locally known as "Folidol", is an organophosphate insecticide and acaricide. It was originally developed by IG Farben in the 1940s. It is highly toxic to non-target organisms, including humans, so its use has been banned or restricted in most countries. The basic structure is shared by parathion methyl.[5]

Parathion
Names
Preferred IUPAC name
O,O-Diethyl O-(4-nitrophenyl) phosphorothioate
Other names
E605
Identifiers
3D model (JSmol)
2059093
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.000.247
EC Number
  • 200-271-7
KEGG
RTECS number
  • TF4550000
UNII
UN number 3018 2783
  • InChI=1S/C10H14NO5PS/c1-3-14-17(18,15-4-2)16-10-7-5-9(6-8-10)11(12)13/h5-8H,3-4H2,1-2H3 checkY
    Key: LCCNCVORNKJIRZ-UHFFFAOYSA-N checkY
  • InChI=1/C10H14NO5PS/c1-3-14-17(18,15-4-2)16-10-7-5-9(6-8-10)11(12)13/h5-8H,3-4H2,1-2H3
    Key: LCCNCVORNKJIRZ-UHFFFAOYAR
  • S=P(Oc1ccc(cc1)[N+]([O-])=O)(OCC)OCC
Properties
C10H14NO5PS
Molar mass 291.26 g·mol−1
Appearance White crystals (pure form)
Melting point 6 °C (43 °F; 279 K)
24 mg/L
Solubility in other solvents high solubility

in xylene and butanol

Hazards
GHS labelling:
GHS06: ToxicGHS08: Health hazardGHS09: Environmental hazard
Danger
H300, H311, H330, H372, H410
P260, P264, P270, P271, P273, P280, P284, P301+P310, P302+P352, P304+P340, P310, P312, P314, P320, P321, P322, P330, P361, P363, P391, P403+P233, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamond
4
1
2
Flash point 120 °C (248 °F; 393 K)
Lethal dose or concentration (LD, LC):
5 mg/kg (mouse, oral)
10 mg/kg (rabbit, oral)
3 mg/kg (dog, oral)
0.93 mg/kg (cat, oral)
5 mg/kg (horse, oral)
8 mg/kg (guinea pig, oral)
2 mg/kg (rat, oral)[1]
84 mg/m3 (rat, 4 hr)[1]
50 mg/m3 (rabbit, 2 hr)
14 mg/m3 (guinea pig, 2 hr)
15 mg/m3 (mouse)[1]
NIOSH (US health exposure limits):
PEL (Permissible)
 none (methyl parathion),[2] TWA 0.1 mg/m3 [skin] (ethyl parathion)[3]
REL (Recommended)
 TWA 0.2 mg/m3 [skin] (methyl parathion)[2] TWA 0.05 mg/m3 [skin] (ethyl parathion)[3]
IDLH (Immediate danger)
 N.D. (methyl parathion)[2] 10 mg/m3 (ethyl parathion)[3]
Safety data sheet (SDS)
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 ?)
Infobox references

History
Bottle with E605

Parathion was developed by Gerhard Schrader for the German trust IG Farben in the 1940s. After World War II and the collapse of IG Farben due to the war crime trials, the Western allies seized the patent, and parathion was marketed worldwide by different companies and under different brand names. The most common German brand was E605 (banned in Germany after 2002); this was not a food-additive "E number" as used in the EU today. "E" stands for Entwicklungsnummer (German for "development number"). It is an irreversible acetylcholinesterase inhibitor.

Safety concerns have later led to the development of parathion methyl, which is somewhat less toxic.

In the EU, Parathion was banned after 2001. [6] In Switzerland, the substance is no longer approved as a pesticide.

Handling properties

Pure parathion is a white crystalline solid. It is commonly distributed as a brown liquid that smells of rotting eggs or garlic. The insecticide is somewhat stable, although it darkens when exposed to sunlight.

Industrial synthesis

Parathion is synthesized from diethyl dithiophosphoric acid (C2H5O)2PS2H by chlorination to generate diethylthiophosphoryl chloride ((C2H5O)2P(S)Cl), and then the chloride is treated with sodium 4-nitrophenolate (the sodium salt of 4-nitrophenol).[7]

2 (C2H5O)2P(S)SH + 3 Cl2 → 2 (C2H5O)2P(S)Cl + S2Cl2 + 2 HCl
(C2H5O)2P(S)Cl + NaOC6H4NO2 → (C2H5O)2P(S)OC6H4NO2 + NaCl

Applications

As a pesticide, parathion is generally applied by spraying. It is often applied to cotton, rice and fruit trees. The usual concentrations of ready-to-use solutions are 0.05 to 0.1%. The chemical is banned for use on many food crops.

Insecticidal activity

Parathion acts on the enzyme acetylcholinesterase indirectly. After an insect (or a human) ingests parathion, an oxidase replaces the double bonded sulfur with oxygen to give paraoxon.[8]

(C2H5O)2P(S)OC6H4NO2 + 1/2 O2 → (C2H5O)2P(O)OC6H4NO2 + S

The phosphate ester is more reactive in organisms than the phosphorothiolate ester, as the phosphorus atoms become much more electropositive.[8]

Parathion resistance is a special case of acetylcholinesterase inhibitor resistance.

Degradation

Degradation of parathion leads to more water-soluble products. Hydrolysis, which deactivates the molecule, occurs at the aryl ester bond resulting in diethyl thiophosphate and 4-nitrophenol.[8]

(C2H5O)2P(S)OC6H4NO2 + H2O → HOC6H4NO2 + (C2H5O)2P(S)OH

Degradation proceeds differently under anaerobic conditions: the nitro group on parathion is reduced to the amine.

(C2H5O)2P(S)OC6H4NO2 + 6 H → (C2H5O)2P(S)OC6H4NH2 + 2 H2O

Safety

Parathion is a cholinesterase inhibitor. It generally disrupts the nervous system by inhibiting acetylcholinesterase. It is absorbed via skin, mucous membranes, and orally. Absorbed parathion is rapidly metabolized to paraoxon, as described in Insecticidal activity. Paraoxon exposure can result in headaches, convulsions, poor vision, vomiting, abdominal pain, severe diarrhea, unconsciousness, tremor, dyspnea, and finally pulmonary edema as well as respiratory arrest. Symptoms of poisoning are known to last for extended periods, sometimes months. The most common and very specific antidote is atropine, in doses of up to 100 mg daily. Because atropine may also be toxic, it is recommended that small frequently repeated doses be used in treatment. If human poisoning is detected early and the treatment is prompt (atropine and artificial respiration), fatalities are infrequent. Insufficient oxygen will lead to cerebral hypoxia and permanent brain damage. Peripheral neuropathy including paralysis is noticed as late sequelae after recovery from acute intoxication. Parathion and related organophosphorus pesticides are used in hundreds of thousands of poisonings annually, especially suicides.[9] It is known as Schwiegermuttergift (mother-in-law poison) in Germany. For this reason, most formulations contain a blue dye providing warning.

Parathion was used as a chemical warfare agent, most notably by an element of the British South Africa Police attached to the Selous Scouts during the Rhodesian Bush War. They used it to poison clothing that was then supplied to anti-government guerrillas. When the enemy soldiers put on the clothes, they were poisoned by absorption through the skin.[10][11][12]

Based on animal studies, parathion is considered by the U.S. Environmental Protection Agency to be a possible human carcinogen.[13] Studies show that parathion is toxic to fetuses, but does not cause birth defects.[14]

It is classified by the United Nations Environment Programme as a persistent organic pollutant and by the World Health Organization as Toxicity Class Ia (extremely hazardous).

Parathion is toxic to bees, fish, birds, and other forms of wildlife.[14]

Protection against poisoning

To provide the end user with a minimum standard of protection, suitable protective gloves, clothing, and a respirator with organic-vapour cartridges is normally worn. Industrial safety during the production process requires special ventilation and continuous measurement of air contamination in order not to exceed PEL levels, as well as careful attention to personal hygiene. Frequent analysis of workers' serum acetylcholinesterase activity is also helpful with regards to occupational safety, because the action of parathion is cumulative. Also, atropine has been used as a specific antidote.

Use in suicides

A chemist swallowed .00424 ounces (0.120 g) of parathion to find the most lethal means of exposure to humans, intending to take an antidote afterwards, but was paralyzed and so died before he could reach it.[15]

Parathion was commonly used for suicides in the 1950s and 1960s.[15]

See also

References
  1. "Parathion". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  2. NIOSH Pocket Guide to Chemical Hazards. "#0427". National Institute for Occupational Safety and Health (NIOSH).
  3. NIOSH Pocket Guide to Chemical Hazards. "#0479". National Institute for Occupational Safety and Health (NIOSH).
  4. "Hazard Rating Information for NFPA Fire Diamonds". Archived from the original on 2015-02-17. Retrieved 2015-03-13.
  5. "Parathion". www.fao.org. Retrieved 2020-04-17.
  6. Non-inclusion of parathion in Annex I to Council Directive 91/414/EEC
  7. Fee, D. C.; Gard, D. R.; Yang, C. (2005). "Phosphorus Compounds". Kirk-Othmer Encyclopedia of Chemical Technology. New York: John Wiley & Sons. doi:10.1002/0471238961.16081519060505.a01.pub2. ISBN 978-0471238966.
  8. Metcalf, R. L. (2002). "Insect Control". Ullmann's Encyclopedia of Industrial Chemistry. New York: Wiley-VCH Verlag GmbH & Co. KGaA. doi:10.1002/14356007.a14_263. ISBN 978-3527306732.
  9. Litchfield, M.H. "Estimates of acute pesticide poisoning in agricultural workers in less developed countries" Toxicology Reviews 2005, volume 24, pp. 271-8. PMID 16499408
  10. "Poison in Rhodesia" (PDF). 31 January 2019.
  11. "Dirty War: Rhodesia and Chemical Biological Warfare 1975-1980 (Book Review)". PRISM | National Defense University.
  12. Cross, Glenn (2017). Dirty War: Rhodesia and Chemical Biological Warfare, 1975–1980. Solihull, UK: Helion & Company. ISBN 978-1-911512-12-7.
  13. "Parathion". Integrated Risk Information System. U. S. Environmental Protection Agency. 26 January 2007.
  14. "Pesticide Information Profiles - Parathion". Extension Toxicology Network. Oregon State University. September 1993.
  15. Carson, Rachel (1962). Silent Spring. ISBN 978-0-547-52762-8. OCLC 1346358856.
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