Dimethylformamide
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Names | |||
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Preferred IUPAC name
N,N-Dimethylformamide[2] | |||
Other names | |||
Identifiers | |||
3D model (
JSmol ) |
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3DMet | |||
605365 | |||
ChEBI | |||
ChEMBL | |||
ChemSpider | |||
DrugBank | |||
ECHA InfoCard
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100.000.617 | ||
EC Number |
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KEGG | |||
MeSH | Dimethylformamide | ||
PubChem CID
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RTECS number
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UNII | |||
UN number | 2265 | ||
CompTox Dashboard (EPA)
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Properties | |||
C3H7NO | |||
Molar mass | 73.095 g·mol−1 | ||
Appearance | Colourless liquid | ||
Odor | Odorless, fishy if impure | ||
Density | 0.948 g/mL | ||
Melting point | −61 °C (−78 °F; 212 K) | ||
Boiling point | 153 °C (307 °F; 426 K) | ||
Miscible | |||
log P | −0.829 | ||
Vapor pressure | 516 Pa | ||
Acidity (pKa) | −0.3 (for the conjugate acid) (H2O)[3] | ||
UV-vis (λmax) | 270 nm | ||
Absorbance | 1.00 | ||
Refractive index (nD)
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1.4305 (at 20 °C) | ||
Viscosity | 0.92 mPa·s (at 20 °C) | ||
Structure | |||
3.86 D | |||
Thermochemistry | |||
Heat capacity (C)
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146.05 J/(K·mol) | ||
Std enthalpy of (ΔfH⦵298)formation |
−239.4 ± 1.2 kJ/mol | ||
Std enthalpy of (ΔcH⦵298)combustion |
−1.9416 ± 0.0012 MJ/mol | ||
Hazards | |||
GHS labelling: | |||
Danger | |||
H226, H312, H319, H332, H360 | |||
P280, P305+P351+P338, P308+P313 | |||
NFPA 704 (fire diamond) | |||
Flash point | 58 °C (136 °F; 331 K) | ||
445 °C (833 °F; 718 K) | |||
Explosive limits
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2.2–15.2% | ||
Threshold limit value (TLV)
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30 mg/m3 (TWA) | ||
Lethal dose or concentration (LD, LC): | |||
LD50 (median dose)
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LC50 (median concentration)
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3092 ppm (mouse, 2 h)[5] | ||
LCLo (lowest published)
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5000 ppm (rat, 6 h)[5] | ||
NIOSH (US health exposure limits): | |||
PEL (Permissible)
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TWA 10 ppm (30 mg/m3) [skin][4] | ||
REL (Recommended)
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TWA 10 ppm (30 mg/m3) [skin][4] | ||
IDLH (Immediate danger) |
500 ppm[4] | ||
Related compounds | |||
Related alkanamides
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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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Dimethylformamide is an
Structure and properties
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]
DMF is a classic example of a fluxional molecule.[7]
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.
Reactions
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
Production
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]
DMF is prepared by combining methyl formate and dimethylamine or by reaction of dimethylamine with carbon monoxide.[21]
Although currently impractical, DMF can be prepared from supercritical carbon dioxide using ruthenium-based catalysts.[22]
Applications
The primary use of DMF is as a solvent with low evaporation rate. DMF is used in the production of
- It is used as a reagent in the aldehydes.
- It is a common solvent in the Heck reaction.[26]
- It is a common catalyst used in the synthesis of carboxylic acids using oxalyl or thionyl chloride. The catalytic mechanism entails reversible formation of an imidoyl chloride (also known as the 'Vilsmeier reagent'):[27][28]
- DMF penetrates most paint strippers.
- DMF is used as a solvent to recover 1,3-butadiene via extractive distillation.
- 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 is effective at separating and suspending near infrared spectroscopy of such.[29]
- DMF can be utilized as a standard in proton NMR spectroscopy allowing for a quantitative determination of an unknown compound.
- In the synthesis of organometallic compounds, it is used as a source of carbon monoxide ligands.
- DMF is a common solvent used in electrospinning.
- DMF is commonly used in the solvothermal synthesis of metal–organic frameworks.
- DMF-d7 in the presence of a catalytic amount of potassium tert-butoxide under microwave heating is a reagent for deuteration of polyaromatic hydrocarbons.
Safety
Dimethylformamide vapor exposure has shown reduced alcohol tolerance and skin irritation in some cases.[30]
On 20 June 2018, the
Toxicity
The acute
References
- ^ N,N-Dimethylmethanamide, NIST web thermo tables
- 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".
- ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0226". National Institute for Occupational Safety and Health (NIOSH).
- ^ a b "Dimethylformamide". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
- ^ a b "Dimethylformamide". Spectral Database for Organic Compounds. Japan: AIST. Retrieved 2012-06-28.[permanent dead link]
- .
- ^ ISBN 978-3527306732.
- ^ IPCS (International Programme on Chemical Safety) (1991). Environmental Health Criteria 114 "Dimethylformamide" United Nations Environment Programme, International Labour Organisation, World Health Organization; 1–124.
- S2CID 36740734.
- ^ (BASF AG, department of analytical, unpublished data, J-No. 124659/08, 27.11.1987)
- ISBN 9780470842898.
- ^ .
- ^ ISBN 9780080405933.
- .
- ISBN 9780471704508.
- .
- ^ 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
- 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.
- ISBN 3-527-30578-5.
- 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.
- ISBN 978-3-319-03979-4.
- ISBN 9780470716069.
- 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.
- 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.
- PMID 3358569.
External links
- International Chemical Safety Card 0457
- NIOSH Pocket Guide to Chemical Hazards. "#0226". National Institute for Occupational Safety and Health (NIOSH).
- Concise International Chemical Assessment Document 31: N,N-Dimethylformamide