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Dimethylmercury

(Redirected from (CH3)2Hg)

Dimethylmercury is an extremely toxic organomercury compound with the formula (CH3)2Hg. A volatile, flammable, dense and colorless liquid, dimethylmercury is one of the strongest known neurotoxins. Less than 0.1 mL is capable of inducing severe mercury poisoning resulting in death.[2]

Dimethylmercury
Skeletal formula of dimethylmercury with all hydrogens added
Space-filling model of dimethylmercury
Names
IUPAC name
Dimethylmercury[1]
Other names
Mercury dimethanide
Identifiers
3D model (JSmol)
3600205
ChEBI
ChemSpider
ECHA InfoCard 100.008.916 Edit this at Wikidata
EC Number
  • 209-805-3
25889
MeSH dimethyl+mercury
RTECS number
  • OW3010000
UNII
UN number 2929
  • InChI=1S/2CH3.Hg/h2*1H3; checkY
    Key: ATZBPOVXVPIOMR-UHFFFAOYSA-N checkY
  • C[Hg]C
Properties
C
2H
6Hg
(CH
3)
2Hg
Molar mass 230.66 g mol−1
Appearance Colorless liquid
Odor Sweet
Density 2.961 g mL−1
Melting point −43 °C (−45 °F; 230 K)
Boiling point 93 to 94 °C (199 to 201 °F; 366 to 367 K)
1.543
Thermochemistry
57.9–65.7 kJ mol−1
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Extremely flammable, extremely poisonous, persistent environmental pollutant
GHS labelling:
GHS06: ToxicGHS08: Health hazardGHS02: FlammableGHS09: Environmental hazard
Danger
H224, H300+H310+H330, H372, H410
P260, P264, P273, P280, P284, P301+P310
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 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g. hydrogen peroxideSpecial hazards (white): no code
4
4
3
Flash point 5 °C (41 °F; 278 K)
Related compounds
Other anions
Other cations
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 ?)

Synthesis, structure, and reactions

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The compound was one of the earliest organometallics reported, reflecting its considerable stability. The compound was first prepared by George Buckton in 1857 by a reaction of methylmercury iodide with potassium cyanide:[3]

2 CH3HgI + 2 KCN → Hg(CH3)2 + 2 KI + (CN)2 + Hg

Later, Edward Frankland discovered that it could be synthesized by treating sodium amalgam with methyl halides:

Hg + 2 Na + 2 CH3I → Hg(CH3)2 + 2 NaI

It can also be obtained by alkylation of mercuric chloride with methyllithium:

HgCl2 + 2 LiCH3 → Hg(CH3)2 + 2 LiCl

The molecule adopts a linear structure with Hg–C bond lengths of 2.083 Å.[4]

Reactivity and physical properties

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Dimethylmercury is stable in water and reacts with mineral acids at a significant rate only at elevated temperatures,[5][6] whereas the corresponding organocadmium and organozinc compounds (and most metal alkyls in general) hydrolyze rapidly. The difference reflects the high electronegativity of Hg (Pauling EN = 2.00) and the low affinity of Hg(II) for oxygen ligands. The compound undergoes a redistribution reaction with mercuric chloride to give methylmercury chloride:

(CH3)2Hg + HgCl2 → 2 CH3HgCl

Whereas dimethylmercury is a volatile liquid, methylmercury chloride is a crystalline solid.[7]

Use

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Dimethylmercury has few applications because of the risks involved. It has been studied for reactions involving bonding methylmercury cations to target molecules, forming potent bactericides, but methylmercury's bioaccumulation and ultimate toxicity has led to it being largely abandoned in favor of the less toxic ethylmercury and diethylmercury compounds, which perform a similar function without the bioaccumulation hazard.

In toxicology, it still finds limited use as a reference toxin. It is also used to calibrate NMR instruments for detection of mercury (δ 0 ppm for 199Hg NMR), although diethylmercury and less toxic mercury salts are now preferred.[8][9][10]

Around 1960, Phil Pomerantz, a man working at the Bureau of Naval Weapons, suggested that dimethylmercury be used as a fuel mix with red fuming nitric acid.[11] This was never done although it did lead to testing a red fuming nitric acid-Unsymmetrical dimethylhydrazine rocket with elemental mercury being injected into the combustion chamber at the Naval Ordnance Test Station.[11]

Safety

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Dimethylmercury is extremely toxic and dangerous to handle. Absorption of doses as low as 0.1 mL can result in severe mercury poisoning.[2] The risks are enhanced because of the compound's high vapor pressure.[2] Since it is highly lipophilic, it absorbs through the skin and into body fat very easily and can permeate many materials, including many plastics and rubber compounds.

Permeation tests showed that several types of disposable latex or polyvinyl chloride gloves (typically, about 0.1 mm thick), commonly used in most laboratories and clinical settings, had high and maximal rates of permeation by dimethylmercury within 15 seconds.[12] The American Occupational Safety and Health Administration advises handling dimethylmercury with highly resistant laminated gloves with an additional pair of abrasion-resistant gloves worn over the laminate pair, and also recommends using a face shield and working in a fume hood.[2][13]

Dimethylmercury is metabolized after several days to methylmercury.[12] Methylmercury crosses the blood–brain barrier easily, probably owing to formation of a complex with cysteine.[13] It easily absorbs into the body, and has a tendency to bioaccumulate. The symptoms of poisoning may be delayed by months, resulting in cases in which a diagnosis is ultimately discovered, but only at a point in which it is too late or almost too late for an effective treatment regimen to be successful.[13] Methylmercury poisoning is also known as Minamata disease.

Incidents

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  • As early as 1865, two workers in the laboratory of Edward Frankland died after exhibiting progressive neurological symptoms following accidental exposure to the compound.[3]
  • Karen Wetterhahn, a professor of chemistry at Dartmouth College, died in 1997, ten months after spilling only a few drops of dimethylmercury onto her latex gloves.[2][14] This incident resulted in improved awareness of the substance's extreme toxicity, and its ability to easily penetrate latex, compared to less porous materials such as nitrile. New OSHA material-handling guidelines were published, many institutions purged their supplies of the compound, and it became almost impossible to buy.[15]
  • Christoph Bulwin, a 40-year-old German database administrator for IG Bergbau, Chemie, Energie, claimed to have been attacked with a syringe-tipped umbrella on 15 July 2011 in Hanover, Germany. Bulwin, who died a year later from mercury poisoning, had said he confiscated the syringe, which was later found to contain dimethylmercury.[16][17][18] According to a 2020 article in Forensic Science, Medicine and Pathology, police investigations revealed a syringe containing a typical mercury thallium compound in Bulwin's car, and mercury and thallium in thermometers at his workplace. Inconclusive antemortem and postmortem blood, urine, and tissue analysis cast doubts on the assault account. The absence of an identified assailant or motive, as well as the presence of different mercury compounds in Bulwin's car, led police to conclude that the intoxication was likely self-administered, thereby terminating the preliminary investigation.[19] The Forensic Science, Medicine and Pathology account is contradicted by other reports, including the 2022 episode of the German TV program Aktenzeichen XY .. ungelöst that was co-edited by the Hannover criminal police.[20]

References

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  1. ^ "dimethylmercury – Compound Summary". PubChem Compound. US: National Center for Biotechnology Information. 16 September 2004. Identification and Related Records. Retrieved 29 January 2021.
  2. ^ a b c d e "OSHA Hazard Information Bulletins – Dimethylmercury". OSHA.gov. Retrieved 29 January 2021.
  3. ^ a b The Chemistry of mercury. C. A. McAuliffe. London: Macmillan. 1977. ISBN 978-1-349-02489-6. OCLC 1057702183.{{cite book}}: CS1 maint: others (link)
  4. ^ Holleman, A. F.; Wiberg, Egon; Wiberg, Nils (2001). Inorganic Chemistry. San Diego: Academic Press. ISBN 0-12-352651-5.
  5. ^ Crabtree, Robert H. (2005). The Organometallic Chemistry of the Transition Metals (4th ed.). Hoboken, N.J.: John Wiley. p. 424. ISBN 0471662569. OCLC 61520528.
  6. ^ Baughman, George L.; Gordon, John A.; Wolfe, N. Lee; Zepp, Richard G. (September 1973). Chemistry of Organomercurials in Aquatic Systems. United States Environmental Protection Agency Ecological Research Series. U.S. Govt. Print. Off. pp. 34–40. Retrieved 29 January 2021.
  7. ^ "Methylmercury chloride". PubChem. National Center for Biotechnology Information, United States National Institutes of Health. Retrieved 29 January 2021.
  8. ^ O'Halloran, T. V.; Singer, C. P. (10 March 1998). "199Hg Standards". Northwestern University. Archived from the original on 14 May 2005. Retrieved 20 January 2021.
  9. ^ Hoffman, R. (1 August 2011). "(Hg) Mercury NMR". Jerusalem: The Hebrew University. Retrieved 29 January 2021.
  10. ^ "Delayed Toxic Syndromes" (PDF). Terrorism by Fear and Uncertainty. ORAU. Archived from the original (PDF) on 23 April 2012. Retrieved 29 January 2021.
  11. ^ a b Clark, John Drury (23 May 2018). Ignition!. New Brunswick: Rutgers University Press Classics. pp. 162–164. ISBN 978-0-8135-9583-2.
  12. ^ a b Nierenberg, David W.; Nordgren, Richard E.; Chang, Morris B.; Siegler, Richard W.; Blayney, Michael B.; Hochberg, Fred; Toribara, Taft Y.; Cernichiari, Elsa; Clarkson, Thomas (1998). "Delayed Cerebellar Disease and Death after Accidental Exposure to Dimethylmercury". New England Journal of Medicine. 338 (23): 1672–1676. doi:10.1056/NEJM199806043382305. PMID 9614258.
  13. ^ a b c Cotton, Simon (October 2003). "Dimethylmercury and Mercury Poisoning: The Karen Wetterhahn story". Molecule of the Month. Bristol University School of Chemistry. doi:10.6084/m9.figshare.5245807. Retrieved 29 January 2021.
  14. ^ "DimethylMercury and Mercury poisoning". Molecule of the Month www.chm.bris.ac.uk. October 2003. Retrieved 25 August 2022.
  15. ^ Cavanaugh, Ray (19 February 2019). "The dangers of dimethylmercury". Chemistry World. Royal Society of Chemistry. Retrieved 29 January 2021.
  16. ^ Albers, Anne; Gies, Ursula; Raatschen, Hans-Jurgen; Klintschar, Michael (1 September 2020). "Another umbrella murder? – A rare case of Minamata disease". Forensic Science, Medicine and Pathology. 16 (3): 504–509. doi:10.1007/s12024-020-00247-y. ISSN 1556-2891. PMC 7449996. PMID 32323188.
  17. ^ "Umbrella stab victim dies of mercury poisoning". www.thelocal.de. 11 May 2012. Retrieved 13 June 2022.
  18. ^ "Quecksilbervergiftung" [Mercury poisoning]. Der Spiegel (in German). 11 May 2012. Retrieved 3 September 2020.
  19. ^ Albers, Anne; Gies, Ursula; Raatschen, Hans-Jurgen; Klintschar, Michael (1 September 2020). "Another umbrella murder? – A rare case of Minamata disease". Forensic Science, Medicine and Pathology. 16 (3): 504–509. doi:10.1007/s12024-020-00247-y. ISSN 1556-2891. PMC 7449996. PMID 32323188.
  20. ^ "Heimtückischer Mord - Familienvater stirbt nach Spritzenattacke - ZDFmediathek". 30 August 2022. Archived from the original on 30 August 2022. Retrieved 27 October 2024.
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