Chemistry:Tetramethylammonium chloride
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| Names | |||
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| Preferred IUPAC name
N,N,N-Trimethylmethanaminium chloride | |||
| Other names
Tetramethylammonium chloride
Tetramethylazanium chloride | |||
| Identifiers | |||
3D model (JSmol)
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PubChem CID
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| Properties | |||
| C4H12NCl | |||
| Molar mass | 109.60 g/mol | ||
| Appearance | White crystals | ||
| Density | 1.17 g/cm3 | ||
| Melting point | 425 °C (797 °F; 698 K) (decomposes) | ||
| Soluble in water and methanol. Slightly soluble in ethanol. Insoluble in ether, benzene, chloroform. | |||
| Hazards | |||
| Safety data sheet | External MSDS | ||
| Related compounds | |||
Other anions
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tetramethylammonium hydroxide | ||
Other cations
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tetraethylammonium chloride | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |||
 verify (what is   ?)
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| Infobox references | |||
Tetramethylammonium chloride is one of the simplest quaternary ammonium salts, with four methyl groups tetrahedrally attached to the central N. The chemical formula (CH3)4N+Cl− is often abbreviated further as Me4N+Cl−. It is a hygroscopic colourless solid that is soluble in water and polar organic solvents. Tetramethylammonium chloride is a major industrial chemical, being used widely as a chemical reagent[1] and also as a low-residue bactericide in such processes as hydrofracking.[2] In the laboratory, it has fewer synthetic chemical applications than quaternary ammonium salts containing longer N-alkyl substituents, which are used extensively as phase-transfer catalysts.
Preparation and laboratory uses
Tetramethylammonium chloride is efficiently produced by the reaction of trimethylamine and methyl chloride.[3]
- N(CH3)3 + CH3Cl → N(CH3)4+Cl−
It is produced by the alkylation of ammonium chloride with dimethyl carbonate in the presence of an ionic liquid catalyst.[4]
Except under extraordinary conditions,[5] it is typically employed as a source of the inert counter cation Me4N+. Similarly it serves as a lipophilic precipitating agent.[6]
In low concentrations, it is used in polymerase chain reactions to increase yields and specificity. It has been shown to enhance yields 5–10 fold at 60mM by stabilizing the AT base pairs.[7]
Toxicity
LD50 = 25 mg/kg (mouse, i.p.); 40 mg/kg (mouse, s.c.); 50 mg/kg (rat, p.o.). Very toxic to aquatic organisms.[8]
Diverse data on human exposure, environmental toxicology and environmentally-related chemistry is available through the NIH Toxnet database.[1]
See also
- Quaternary ammonium cation
- Tetraethylammonium chloride
- Tetramethylammonium hydroxide
- Tetramethylammonium
References
- ↑ 1.0 1.1 http://toxnet.nlm.nih.gov/cgi-bin/sis/search/a?dbs+hsdb:@term+@DOCNO+7987[|permanent dead link|dead link}}]
- ↑ http://fracfocus.org/chemical-use/what-chemicals-are-used
- ↑ Van Gysel, August B.; Musin, Willy (2000). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a16_535.
- ↑ Zheng, Z. et al. (2007). "Alkylation of Ammonium Salts Catalyzed by Imidazolium-Based Ionic Liquid Catalysts". Advanced Synthesis & Catalysis 349 (7): 1095–1101. doi:10.1002/adsc.200600451.
- ↑ Nenad, Maraš; Polanc, Slovenko; Kočevar, Marijan (2008). "Microwave-assisted methylation of phenols with tetramethylammonium chloride in the presence of K2CO3 or Cs2CO3". Tetrahedron 64 (51): 11618–11624. doi:10.1016/j.tet.2008.10.024.
- ↑ W. J. Middleton and D. W. Wiley (1973). "tetramethylammonium 1-Propene-1,1,2,3,3-pentacarbonitrile". Organic Syntheses. doi:10.15227/orgsyn.041.0099.; Collective Volume, 5, pp. 1013
- ↑ Chevet E. et al. (1995). "Low concentrations of tetramethylammonium chloride increase yield and specificity of PCR". Nucleic Acids Research 23 (16) 3343–344.
- ↑ https://datasheets.scbt.com/sc-251199.pdf
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