Triethylamine
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| Names | |||
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| IUPAC name
N,N-Diethylethanamine
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Other names
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| Identifiers | |||
121-44-8  |
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| Abbreviations | TEA[1] | ||
| 605283 | |||
| ChEBI | CHEBI:35026 |
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| ChEMBL | ChEMBL284057 |
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| ChemSpider | 8158 |
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| EC Number | 204-469-4 | ||
| Jmol 3D model | Interactive image | ||
| KEGG | C14691 |
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| MeSH | triethylamine | ||
| PubChem | 8471 | ||
| RTECS number | YE0175000 | ||
| UNII | VOU728O6AY |
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| UN number | 1296 | ||
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| Properties[3] | |||
| C6H15N | |||
| Molar mass | 101.19 g·mol−1 | ||
| Appearance | Colourless liquid | ||
| Odor | Fishy, ammoniacal | ||
| Density | 0.7255 g mL−1 | ||
| Melting point | −114.70 °C; −174.46 °F; 158.45 K | ||
| Boiling point | 88.6 to 89.8 °C; 191.4 to 193.5 °F; 361.7 to 362.9 K | ||
| log P | 1.647 | ||
| Vapor pressure | 6.899–8.506 kPa | ||
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Henry's law
constant (kH) |
66 μmol Pa−1 kg−1 | ||
| Acidity (pKa) | 10.75 (for the conjugate acid) (H2O), 9.00 (DMSO) [2] | ||
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Refractive index (nD)
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1.401 | ||
| Thermochemistry | |||
| 216.43 J K−1 mol−1 | |||
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Std enthalpy of
formation (ΔfH |
−169 kJ mol−1 | ||
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Std enthalpy of
combustion (ΔcH |
−4.37763 to −4.37655 MJ mol−1 | ||
| Vapor pressure | {{{value}}} | ||
| Related compounds | |||
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Related amines
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Related compounds
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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 verify (what is  ?) |
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| Infobox references | |||
Triethylamine is the chemical compound with the formula N(CH2CH3)3, commonly abbreviated Et3N. It is also abbreviated TEA, yet this abbreviation must be used carefully to avoid confusion with triethanolamine or tetraethylammonium, for which TEA is also a common abbreviation. It is a colourless volatile liquid with a strong fishy odor reminiscent of ammonia and is also the smell of the hawthorn plant.[4] Like diisopropylethylamine (Hünig’s base), triethylamine is commonly encountered in organic synthesis.
Synthesis and properties
Triethylamine is prepared by the alkylation of ammonia with ethanol:[5]
- NH3 + 3 C2H5OH → N(C2H5)3 + 3 H2O
The pKa of protonated triethylamine is 10.75,[2] and it can be used to prepare buffer solutions for that pH. The hydrochloride salt, triethylamine hydrochloride (triethylammonium chloride), is a colorless, odorless, and hygroscopic powder, which decomposes when heated to 261 °C.
Applications
Triethylamine is commonly employed in organic synthesis as a base, most often in the preparation of esters and amides from acyl chlorides.[6] Such reactions lead to the production of hydrogen chloride which combines with triethylamine to form the salt triethylamine hydrochloride, commonly called triethylammonium chloride. This reaction removes the hydrogen chloride from the reaction mixture, which is required for these reactions to proceed to completion (R, R' = alkyl, aryl):
- R2NH + R'C(O)Cl + Et3N → R'C(O)NR2 + Et3NH+Cl−
Like other tertiary amines, it catalyzes the formation of urethane foams and epoxy resins. It is also useful in dehydrohalogenation reactions and Swern oxidations.
Triethylamine is used to give salts of various carboxylic acid-containing pesticides, e.g. Triclopyr and 2,4-dichlorophenoxyacetic acid
Triethylamine is readily alkylated to give the corresponding quaternary ammonium salt:
- RI + Et3N → Et3NR+I−
Triethylamine is mainly used in the production of quaternary ammonium compounds for textile auxiliaries and quaternary ammonium salts of dyes. It is also a catalyst and acid neutralizer for condensation reactions and is useful as an intermediate for manufacturing medicines, pesticides and other chemicals.
Niche uses
Triethylamine is the active ingredient in FlyNap, a product for anesthetizing Drosophila melanogaster. Triethylamine is used in mosquito and vector control labs to anesthetize mosquitoes. This is done to preserve any viral material that might be present during species identification.
Also, the bicarbonate salt of triethylamine (often abbreviated TEAB, triethylammonium bicarbonate) is useful in reverse phase chromatography, often in a gradient to purify nucleotides and other biomolecules.
References
- ↑ X. Bories-Azeau, S. P. Armes, and H. J. W. van den Haak, Macromolecules 2004, 37, 2348 PDF
- ↑ 2.0 2.1 David Evans Research Group
- ↑ Lua error in package.lua at line 80: module 'strict' not found.
- ↑ The Hawthorn, BBC
- ↑ Karsten Eller, Erhard Henkes, Roland Rossbacher, Hartmut Höke "Amines, Aliphatic" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005. doi:10.1002/14356007.a02_001
- ↑ Lua error in package.lua at line 80: module 'strict' not found.
