Methylarsonic acid: Difference between revisions
m Smokefoot moved page Methanearsonic acid to Methylarsonic acid: more common name |
→Synthesis and biosynthesis: redirect hatnote |
||
(21 intermediate revisions by 17 users not shown) | |||
Line 1: | Line 1: | ||
{{Chembox |
{{Chembox |
||
| ImageFile = |
| ImageFile = MeAsO3H2.png |
||
| ImageSize = |
| ImageSize = 144 |
||
| ImageAlt = |
| ImageAlt = |
||
| PIN = Methylarsonic acid<ref>{{cite book |author=[[International Union of Pure and Applied Chemistry]] |date=2014 |title=Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 |publisher=[[Royal Society of Chemistry|The Royal Society of Chemistry]] |pages=916, 918 |doi=10.1039/9781849733069 |isbn=978-0-85404-182-4}}</ref> |
|||
| IUPACName = |
|||
| OtherNames = |
| OtherNames = Methanearsonic acid<br/>Monomethylarsonic acid |
||
|Section1={{Chembox Identifiers |
|Section1={{Chembox Identifiers |
||
| CASNo = 124-58-3 |
| CASNo = 124-58-3 |
||
| PubChem = |
| PubChem = 8948 |
||
| InChI=1S/CH5AsO3/c1-2(3,4)5/h1H3,(H2,3,4,5) |
|||
⚫ | |||
| InChIKey=QYPPRTNMGCREIM-UHFFFAOYSA-N |
|||
| EC_number=204-705-6 |
|||
| RTECS=PA1575000 |
|||
| UNNumber=1557 |
|||
| UNII=J37VJ5709S |
|||
| Beilstein=4-04-00-03682 |
|||
| ChemSpiderID=8604 |
|||
⚫ | |||
|Section2={{Chembox Properties |
|Section2={{Chembox Properties |
||
| C=1|H=5|As=1|O=3 |
| C=1|H=5|As=1|O=3 |
||
Line 24: | Line 31: | ||
}} |
}} |
||
''' |
'''Methylarsonic acid''' is an [[organoarsenic compound]] with the formula CH<sub>3</sub>AsO<sub>3</sub>H<sub>2</sub>. It is a colorless, water-soluble solid. Salts of this compound, e.g. [[disodium methyl arsonate]], have been widely used in as herbicides and fungicides in growing cotton and rice.<ref name=Ullmann>{{Ullmann | author = Grund, S. C. | author2 = Hanusch, K. | author3 = Wolf, H. U. | title = Arsenic and Arsenic Compounds | doi = 10.1002/14356007.a03_113.pub2 }}</ref> |
||
==Reactions== |
|||
Near physiological pH, methanearsonic acid converts to its conjugate bases, the '''methylarsonates'''. These include CH<sub>3</sub>AsO<sub>3</sub>H<sup>−</sup> and {{chem|CH|3|AsO|3|2−}}. |
|||
==Synthesis and biosynthesis== |
|||
{{Confuse|Meyer synthesis}} |
|||
Reaction of [[arsenous acid]] with [[methyl iodide]] gives methylarsonic acid. This historically significant conversion is called the '''Meyer reaction''':<ref>{{cite journal|title=Ueber einige anomale Reaktionen|author=G. Meyer|journal=Berichte der deutschen chemischen Gesellschaft|pages=1439–1443|volume=13|year=1883|doi=10.1002/cber.188301601316}}</ref> |
|||
:As(OH)<sub>3</sub> + CH<sub>3</sub>I + NaOH → CH<sub>3</sub>AsO(OH)<sub>2</sub> + NaI + H<sub>2</sub>O |
|||
The then-novel aspect of the reaction was that alkylation occurs at arsenic, leading to oxidation of arsenic from [[oxidation state]] +3 to +5. |
|||
The [[biomethylation]] of arsenic compounds is thought to start with the formation of methanearsonates. Thus, trivalent arsenic compounds are methylated to give methanearsonate. [[S-Adenosylmethionine|''S''-Adenosylmethionine]] is the methyl donor. The methanearsonates are the precursors to [[cacodylate]]s, again by the cycle of reduction (to methylarsonous acid) followed by a second methylation.<ref name=Cullen/> |
|||
==Safety== |
==Safety== |
||
Like |
Like most arsenic compounds, it is highly toxic.<ref name=Cullen>{{cite journal|title=Comparative toxicity of trivalent and pentavalent inorganic and methylated arsenicals in rat and human cells|author1=Styblo, M. |author2=Del Razo, L. M. |author3=Vega, L. |author4=Germolec, D. R. |author5=LeCluyse, E. L. |author6=Hamilton, G. A. |author7=Reed, W. |author8=Wang, C. |author9=Cullen, W. R. |author10=Thomas, D. J. |journal=Archives of Toxicology|year=2000|volume=74|pages=289–299|doi=10.1007/s002040000134}}</ref> |
||
==References== |
==References== |
||
{{Reflist}} |
|||
<references /> |
|||
[[Category:Arsonic acids |
[[Category:Arsonic acids]] |
Revision as of 13:33, 20 September 2023
Names | |
---|---|
Preferred IUPAC name
Methylarsonic acid[1] | |
Other names
Methanearsonic acid
Monomethylarsonic acid | |
Identifiers | |
3D model (JSmol)
|
|
4-04-00-03682 | |
ChemSpider | |
ECHA InfoCard | 100.004.278 |
EC Number |
|
PubChem CID
|
|
RTECS number |
|
UNII | |
UN number | 1557 |
CompTox Dashboard (EPA)
|
|
| |
| |
Properties | |
CH5AsO3 | |
Molar mass | 139.970 g·mol−1 |
Appearance | white solid |
Melting point | 160.5 °C (320.9 °F; 433.6 K) |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|
Methylarsonic acid is an organoarsenic compound with the formula CH3AsO3H2. It is a colorless, water-soluble solid. Salts of this compound, e.g. disodium methyl arsonate, have been widely used in as herbicides and fungicides in growing cotton and rice.[2]
Reactions
Near physiological pH, methanearsonic acid converts to its conjugate bases, the methylarsonates. These include CH3AsO3H− and CH
3AsO2−
3.
Synthesis and biosynthesis
Reaction of arsenous acid with methyl iodide gives methylarsonic acid. This historically significant conversion is called the Meyer reaction:[3]
- As(OH)3 + CH3I + NaOH → CH3AsO(OH)2 + NaI + H2O
The then-novel aspect of the reaction was that alkylation occurs at arsenic, leading to oxidation of arsenic from oxidation state +3 to +5.
The biomethylation of arsenic compounds is thought to start with the formation of methanearsonates. Thus, trivalent arsenic compounds are methylated to give methanearsonate. S-Adenosylmethionine is the methyl donor. The methanearsonates are the precursors to cacodylates, again by the cycle of reduction (to methylarsonous acid) followed by a second methylation.[4]
Safety
Like most arsenic compounds, it is highly toxic.[4]
References
- ^ International Union of Pure and Applied Chemistry (2014). Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013. The Royal Society of Chemistry. pp. 916, 918. doi:10.1039/9781849733069. ISBN 978-0-85404-182-4.
- ^ Grund, S. C.; Hanusch, K.; Wolf, H. U. "Arsenic and Arsenic Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_113.pub2. ISBN 978-3527306732.
- ^ G. Meyer (1883). "Ueber einige anomale Reaktionen". Berichte der deutschen chemischen Gesellschaft. 13: 1439–1443. doi:10.1002/cber.188301601316.
- ^ a b Styblo, M.; Del Razo, L. M.; Vega, L.; Germolec, D. R.; LeCluyse, E. L.; Hamilton, G. A.; Reed, W.; Wang, C.; Cullen, W. R.; Thomas, D. J. (2000). "Comparative toxicity of trivalent and pentavalent inorganic and methylated arsenicals in rat and human cells". Archives of Toxicology. 74: 289–299. doi:10.1007/s002040000134.