Dimethylformamide is an organic compound with the chemical formulaHCON(CH3)2. Its structure is HC(=O)−N(−CH3)2. Commonly abbreviated as DMF (although this initialism is sometimes used for dimethylfuran, or dimethyl fumarate), this colourless liquid is miscible with water and the majority of organic liquids. DMF is a common solvent for chemical reactions. Dimethylformamide is odorless, but technical-grade or degraded samples often have a fishy smell due to impurity of dimethylamine. Dimethylamine degradation impurities can be removed by sparging samples with an inert gas such as argon or by sonicating the samples under reduced pressure. As its name indicates, it is structurally related to formamide, having two methyl groups in the place of the two hydrogens. DMF is a polar (hydrophilic) aprotic solvent with a high boiling point. It facilitates reactions that follow polar mechanisms, such as SN2 reactions.
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Yverify (what is YN ?)
Infobox references
Structure and propertiesedit
As for most amides, the spectroscopic evidence indicates partial double bond character for the C−N and C−O bonds. Thus, the infrared spectrum shows a C=O stretching frequency at only 1675 cm−1, whereas a ketone would absorb near 1700 cm−1.[6]
The ambient temperature 1H NMR spectrum shows two methyl signals, indicative of hindered rotation about the (O)C−N bond.[6] At temperatures near 100 °C, the 500 MHz NMR spectrum of this compound shows only one signal for the methyl groups.
DMF is miscible with water.[8] The vapour pressure at 20 °C is 3.5 hPa.[9] A Henry's law constant of 7.47 × 10−5 hPa·m3/mol can be deduced from an experimentally determined equilibrium constant at 25 °C.[10] The partition coefficient log POW is measured to −0.85.[11] Since the density of DMF (0.95 g·cm−3 at 20 °C[8]) is similar to that of water, significant flotation or stratification in surface waters in case of accidental losses is not expected.
Reactionsedit
DMF is hydrolyzed by strong acids and bases, especially at elevated temperatures. With sodium hydroxide, DMF converts to formate and dimethylamine. DMF undergoes decarbonylation near its boiling point to give dimethylamine. Distillation is therefore conducted under reduced pressure at lower temperatures.[12]
In one of its main uses in organic synthesis, DMF is a reagent in the Vilsmeier–Haack reaction, which is used to formylate aromatic compounds.[13][14] The process involves initial conversion of DMF to a chloroiminium ion, [(CH3)2N=CH(Cl)]+, known as a Vilsmeier reagent,[15] which attacks arenes.
Dimethylformamide forms 1:1 adducts with a variety of Lewis acids such as the soft acid I2, and the hard acid phenol. It is classified as a hard Lewis base and its ECW model base parameters are EB = 2.19 and CB = 1.31.[17] Its relative donor strength toward a series of acids, versus other Lewis bases, can be illustrated by C-B plots.[18][19]
Productionedit
DMF was first prepared in 1893 by the French chemist Albert Verley (8 January 1867 – 27 November 1959), by distilling a mixture of dimethylamine hydrochloride and potassium formate.[20]
The primary use of DMF is as a solvent with low evaporation rate. DMF is used in the production of acrylic fibers and plastics. It is also used as a solvent in peptide coupling for pharmaceuticals, in the development and production of pesticides, and in the manufacture of adhesives, synthetic leathers, fibers, films, and surface coatings.[8]
It is used in the manufacturing of solvent dyes as an important raw material. It is consumed during reaction.
Pure acetylene gas cannot be compressed and stored without the danger of explosion. Industrial acetylene is safely compressed in the presence of dimethylformamide, which forms a safe, concentrated solution. The casing is also filled with agamassan, which renders it safe to transport and use.
As a cheap and common reagent, DMF has many uses in a research laboratory.
DMF-d7 in the presence of a catalytic amount of potassium tert-butoxide under microwave heating is a reagent for deuteration of polyaromatic hydrocarbons.
Safetyedit
Dimethylformamide vapor exposure has shown reduced alcohol tolerance and skin irritation in some cases.[30]
On 20 June 2018, the Danish Environmental Protective Agency published an article about DMF's use in squishies. The density of the compound in the toy resulted in all squishies being removed from the Danish market. All squishies were recommended to be thrown out as household waste.
[31]
Toxicityedit
The acute LD50 (oral, rats and mice) is 2.2–7.55 g/kg.[8] Hazards of DMF have been examined.[32]
^Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. pp. 841, 844. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4. The traditional name 'formamide' is retained for HCO-NH2 and is the preferred IUPAC name. Substitution is permitted on the –NH2 group.
^"Hazardous Substances Data Bank (HSDB) - N,N-DIMETHYLFORMAMIDE".
^ ab"Dimethylformamide". Spectral Database for Organic Compounds. Japan: AIST. Retrieved 2012-06-28.[permanent dead link]
^H. S. Gutowsky; C. H. Holm (1956). "Rate Processes and Nuclear Magnetic Resonance Spectra. II. Hindered Internal Rotation of Amides". J. Chem. Phys. 25 (6): 1228–1234. Bibcode:1956JChPh..25.1228G. doi:10.1063/1.1743184.
^IPCS (International Programme on Chemical Safety) (1991). Environmental Health Criteria 114 "Dimethylformamide" United Nations Environment Programme, International Labour Organisation, World Health Organization; 1–124.
^Taft, R. W.; Abraham, M. H.; Doherty, R. M.; Kamlet, M. J. (1985). "The molecular properties governing solubilities of organic nonelectrolytes in water". Nature. 313 (6001): 384–386. Bibcode:1985Natur.313..384T. doi:10.1038/313384a0. S2CID 36740734.
^(BASF AG, department of analytical, unpublished data, J-No. 124659/08, 27.11.1987)
^Comins, Daniel L.; Joseph, Sajan P. (2001). "N,N-Dimethylformamide". N,N-Dimethylformamide. Encyclopedia of Reagents for Organic Synthesis. John Wiley & Sons. doi:10.1002/047084289x.rd335. ISBN 9780470842898.
^ abVilsmeier, Anton; Haack, Albrecht (1927). "Über die Einwirkung von Halogenphosphor auf Alkyl-formanilide. Eine neue Methode zur Darstellung sekundärer und tertiärer p-Alkylamino-benzaldehyde" [On the reaction of phosphorus halides with alkyl formanilides. A new method for the preparation of secondary and tertiary p-alkylamino-benzaldehyde]. Ber. Dtsch. Chem. Ges. A/B (in German). 60 (1): 119–122. doi:10.1002/cber.19270600118.
^ abMeth-Cohn, Otto; Stanforth, Stephen P. (1993). "The Vilsmeier-Haack Reaction". In Trost, Barry M.; Heathcock, Clayton H. (eds.). Additions to CX π-Bonds, Part 2. Comprehensive Organic Synthesis: Selectivity, Strategy and Efficiency in Modern Organic Chemistry. Vol. 2. Elsevier. pp. 777–794. doi:10.1016/B978-0-08-052349-1.00049-4. ISBN 9780080405933.
^Jones, Gurnos; Stanforth, Stephen P. (2000). "The Vilsmeier Reaction of Non-Aromatic Compounds". Org. React.56 (2): 355–686. doi:10.1002/0471264180.or056.02.
^Wang, Zerong (2009). Comprehensive organic name reactions and reagents. Hoboken, N.J.: John Wiley. pp. 490–492. ISBN 9780471704508.
^Vogel G. C.; Drago, R. S. (1996). "The ECW Model". Journal of Chemical Education. 73 (8): 701–707. Bibcode:1996JChEd..73..701V. doi:10.1021/ed073p701.
^Laurence, C. and Gal, J-F. Lewis Basicity and Affinity Scales, Data and Measurement, (Wiley 2010) pp 50-51 ISBN 978-0-470-74957-9
^Cramer, R. E.; Bopp, T. T. (1977). "Graphical display of the enthalpies of adduct formation for Lewis acids and bases". Journal of Chemical Education. 54: 612–613. doi:10.1021/ed054p612. The plots shown in this paper used older parameters. Improved E&C parameters are listed in ECW model.
^Verley, A. (1893). "Sur la préparation des amides en général" [On the preparation of amides in general]. Bulletin de la Société Chimique de Paris. 3rd series (in French). 9: 690–692. On p. 692, Verley states that DMF is prepared by a procedure analogous to that for the preparation of dimethylacetamide (see p. 691), which would be by distilling dimethylamine hydrochloride and potassium formate.
^Weissermel, K.; Arpe, H.-J. (2003). Industrial Organic Chemistry: Important Raw Materials and Intermediates. Wiley-VCH. pp. 45–46. ISBN 3-527-30578-5.
^Walter Leitner; Philip G. Jessop (1999). Chemical synthesis using supercritical fluids. Wiley-VCH. pp. 408–. ISBN 978-3-527-29605-7. Retrieved 27 June 2011.
^Bouveault, Louis (1904). "Modes de formation et de préparation des aldéhydes saturées de la série grasse" [Methods of preparation of saturated aldehydes of the aliphatic series]. Bulletin de la Société Chimique de Paris. 3rd series (in French). 31: 1306–1322.
^Bouveault, Louis (1904). "Nouvelle méthode générale synthétique de préparation des aldéhydes" [Novel general synthetic method for preparing aldehydes]. Bulletin de la Société Chimique de Paris. 3rd series (in French). 31: 1322–1327.
^Li, Jie Jack (2014). "Bouveault aldehyde synthesis". Name Reactions: A Collection of Detailed Mechanisms and Synthetic Applications (5th ed.). Springer Science & Business Media. pp. 72–73. ISBN 978-3-319-03979-4.
^Oestreich, Martin, ed. (2009). The Mizoroki–Heck Reaction. John Wiley & Sons. ISBN 9780470716069.
^Clayden, J. (2001). Organic Chemistry. Oxford: Oxford University Press. pp. 276–296. ISBN 0-19-850346-6.
^Ansell, M. F. in "The Chemistry of Acyl Halides"; S. Patai, Ed.; John Wiley and Sons: London, 1972; pp 35–68.
^Haddon, R.; Itkis, M. (March 2008). "3. Near-Infrared (NIR) Spectroscopy" (pdf). In Freiman, S.; Hooker, S.; Migler; K.; Arepalli, S. (eds.). Publication 960-19 Measurement Issues in Single Wall Carbon Nanotubes. NIST. p. 20. Retrieved 2012-06-28.
^Lyle, W. H.; Spence, T. W.; McKinneley, W. M.; Duckers, K. (1979). "Dimethylformamide and alcohol intolerance". British Journal of Industrial Medicine. 36 (1): 63–66. doi:10.1136/oem.36.1.63. PMC1008494. PMID 444443.
^Magnus Løfstedt. "Skumlegetøj afgiver farlige kemikalier (in English- Squishies giving dangerous chemicals)". Archived from the original on 2021-09-03. Retrieved 2019-06-13.
^Redlich, C.; Beckett, W. S.; Sparer, J.; Barwick, K. W.; Riely, C. A.; Miller, H.; Sigal, S. L.; Shalat, S. L.; Cullen, M. R. (1988). "Liver disease associated with occupational exposure to the solvent dimethylformamide". Annals of Internal Medicine. 108 (5): 680–686. doi:10.7326/0003-4819-108-5-680. PMID 3358569.