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dimethylformamide

{{chembox

| Watchedfields = changed

| verifiedrevid = 458446617

| ImageFile = Dimethylformamide-2D-skeletal.svg

| ImageFile_Ref = {{chemboximage|correct|??}}

| ImageSize = 100

| ImageName = Skeletal formula of dimethylformamide with one explicit hydrogen added

| ImageFileL1 = DMF-3D-balls.png

| ImageFileL1_Ref = {{chemboximage|correct|??}}

| ImageNameL1 = Ball and stick model of dimethylformamide

| ImageFileR1 = Dimethylformamide-3D-vdW.png

| ImageNameR1 = Spacefill model of dimethylformamide

| PIN = N,N-Dimethylformamide{{cite book | title = Nomenclature of Organic Chemistry : IUPAC Recommendations and Preferred Names 2013 (Blue Book) | publisher = The Royal Society of Chemistry | date = 2014 | location = Cambridge | pages = 841, 844 | doi = 10.1039/9781849733069-FP001 | isbn = 978-0-85404-182-4 | quote = The traditional name ‘formamide’ is retained for HCO-NH2 and is the preferred IUPAC name. Substitution is permitted on the –NH2 group.}}

| SystematicName = N,N-Dimethylmethanamide[http://wtt-pro.nist.gov/wtt-pro/index.html?cmp=n.n-dimethylmethanamide N,N-Dimethylmethanamide], NIST web thermo tables

| OtherNames = Dimethylformamide
DMF

| IUPACName =

| Section1 = {{Chembox Identifiers

|CASNo = 68-12-2

|CASNo_Ref = {{cascite|correct|CAS}}

|PubChem = 6228

|ChemSpiderID = 5993

|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

|UNII = 8696NH0Y2X

|UNII_Ref = {{fdacite|correct|FDA}}

|EINECS = 200-679-5

|UNNumber = 2265

|DrugBank = DB01844

|DrugBank_Ref = {{drugbankcite|correct|drugbank}}

|KEGG = C03134

|KEGG_Ref = {{keggcite|correct|kegg}}

|MeSHName = Dimethylformamide

|ChEBI = 17741

|ChEBI_Ref = {{ebicite|correct|EBI}}

|ChEMBL = 268291

|ChEMBL_Ref = {{ebicite|correct|EBI}}

|RTECS = LQ2100000

|Beilstein = 605365

|3DMet = B00545

|SMILES = CN(C)C=O

|StdInChI = 1S/C3H7NO/c1-4(2)3-5/h3H,1-2H3

|StdInChI_Ref = {{stdinchicite|correct|chemspider}}

|StdInChIKey = ZMXDDKWLCZADIW-UHFFFAOYSA-N

|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

}}

| Section2 = {{Chembox Properties

|C=3|H=7|N=1|O=1

|Appearance = Colourless liquid

|Odor = Odorless, fishy if impure

|Density = 0.948 g/mL

|MeltingPtC = -61

|BoilingPtC = 153

|pKa = −0.3 (for the conjugate acid) (H2O){{cite web | title = Hazardous Substances Data Bank (HSDB) - N,N-DIMETHYLFORMAMIDE | url = https://pubchem.ncbi.nlm.nih.gov/source/hsdb/78}}

|Solubility = Miscible

|LogP = −0.829

|VaporPressure = 516 Pa

|LambdaMax = 270 nm

|Absorbance = 1.00

|RefractIndex = 1.4305 (at 20 °C)

|Viscosity = 0.92 mPa·s (at 20 °C)

}}

| Section3 = {{Chembox Structure

|Dipole = 3.86 D

}}

| Section4 = {{Chembox Thermochemistry

|DeltaHf = −239.4 ± 1.2 kJ/mol

|DeltaHc = −1.9416 ± 0.0012 MJ/mol

|HeatCapacity = 146.05 J/(K·mol)

}}

| Section5 = {{Chembox Hazards

|GHSPictograms = {{gHS flame}} {{gHS exclamation mark}} {{gHS health hazard}}

|GHSSignalWord = DANGER

|HPhrases = {{h-phrases|226|312|319|332|360}}

|PPhrases = {{p-phrases|280|305+351+338|308+313}}

|NFPA-H = 2

|NFPA-F = 2

|NFPA-R = 0

|FlashPtC = 58

|AutoignitionPtC = 445

|ExploLimits = 2.2–15.2%

|TLV-TWA = 30 mg/m3

|LD50 = {{unbulleted list|1.5 g/kg (rabbit, dermal)|2.8 g/kg (rat, oral)|3.7 g/kg (mouse, oral)|3.5 g/kg (rat, oral)}}

|PEL = TWA 10 ppm (30 mg/m3) [skin]{{PGCH|0226}}

|IDLH = 500 ppm

|REL = TWA 10 ppm (30 mg/m3) [skin]

|LC50 = 3092 ppm (mouse, 2 h){{IDLH|68122|Dimethylformamide}}

|LCLo = 5000 ppm (rat, 6 h)

}}

| Section6 = {{Chembox Related

|OtherFunction_label = alkanamides

|OtherFunction = {{unbulleted list|N-Methylformamide|Diethylformamide|Deuterated DMF}}

|OtherCompounds = {{unbulleted list|N-Nitroso-N-methylurea|ENU}}

}}

}}

Dimethylformamide, DMF is an organic compound with the chemical formula {{chem2|HCON(CH3)2|auto=1}}. Its structure is {{chem2|HC(\dO)\sN(\sCH3)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.

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.{{cite web | publisher = AIST | location = Japan | work = Spectral Database for Organic Compounds | url = http://www.aist.go.jp/RIODB/SDBS/cgi-bin/cre_frame_disp.cgi?sdbsno=324 | title = Dimethylformamide | access-date = 2012-06-28}}{{Dead link|date=July 2019 |bot=InternetArchiveBot |fix-attempted=yes}}

DMF is a classic example of a fluxional molecule.{{cite journal | author1 = H. S. Gutowsky | author2 = C. H. Holm | title = Rate Processes and Nuclear Magnetic Resonance Spectra. II. Hindered Internal Rotation of Amides | journal = J. Chem. Phys. | year = 1956 | volume = 25 | pages = 1228–1234 | doi=10.1063/1.1743184 | issue = 6|bibcode = 1956JChPh..25.1228G}}

Image:DmfDNMR.png

The ambient temperature 1H NMR spectrum shows two methyl signals, indicative of hindered rotation about the (O)C−N bond. 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.{{Ullmann | author = Bipp, H. | author2 = Kieczka, H. | title = Formamides | doi = 10.1002/14356007.a12_001.pub2}} The vapour pressure at 20 °C is 3.5 hPa.IPCS (International Programme on Chemical Safety) (1991). Environmental Health Criteria 114 "Dimethylformamide" United Nations Environment Programme, International Labour Organisation, World Health Organization; 1–124. 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.{{cite journal |author1=Taft, R. W. |author2=Abraham, M. H. |author3=Doherty, R. M. |author4=Kamlet, M. J. | title = The molecular properties governing solubilities of organic nonelectrolytes in water | journal = Nature | year = 1985 | volume = 313 | issue = 6001 | pages = 384–386 | doi = 10.1038/313384a0 |bibcode=1985Natur.313..384T |s2cid=36740734}} The partition coefficient log POW is measured to −0.85.(BASF AG, department of analytical, unpublished data, J-No. 124659/08, 27.11.1987) Since the density of DMF (0.95 g·cm−3 at 20 °C) is similar to that of water, significant flotation or stratification in surface waters in case of accidental losses is not expected.

File:DMF resonances.png{{Clear left}}

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.{{Cite encyclopedia|title = N,N-Dimethylformamide|encyclopedia = Encyclopedia of Reagents for Organic Synthesis|last1 = Comins|first1 = Daniel L.|last2 = Joseph|first2 = Sajan P.|year = 2001|publisher = John Wiley & Sons|isbn = 9780470842898|doi = 10.1002/047084289x.rd335|chapter = N,N-Dimethylformamide}}

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.{{cite journal|author-link1 = Anton Vilsmeier|last1 = Vilsmeier|first1 = Anton|last2 = Haack|first2 = Albrecht|title = Über die Einwirkung von Halogenphosphor auf Alkyl-formanilide. Eine neue Methode zur Darstellung sekundärer und tertiärer p-Alkylamino-benzaldehyde|language = de|trans-title=On the reaction of phosphorus halides with alkyl formanilides. A new method for the preparation of secondary and tertiary p-alkylamino-benzaldehyde|year = 1927|journal = Ber. Dtsch. Chem. Ges. A/B|volume = 60|issue = 1|pages = 119–122|doi = 10.1002/cber.19270600118}}{{cite book|last1 = Meth-Cohn|first1 = Otto|last2 = Stanforth|first2 = Stephen P.|chapter = The Vilsmeier-Haack Reaction|title = Additions to CX π-Bonds, Part 2|series = Comprehensive Organic Synthesis: Selectivity, Strategy and Efficiency in Modern Organic Chemistry|year = 1993|volume = 2|editor1-first = Barry M.|editor1-last = Trost|editor1-link = Barry M. Trost|editor2-first = Clayton H.|editor2-last = Heathcock|editor2-link = Clayton H. Heathcock|pages = 777–794|doi = 10.1016/B978-0-08-052349-1.00049-4|publisher = Elsevier|isbn = 9780080405933}} The process involves initial conversion of DMF to a chloroiminium ion, [(CH3)2N=CH(Cl)]+, known as a Vilsmeier reagent,{{cite journal|title = The Vilsmeier Reaction of Non-Aromatic Compounds|first1 = Gurnos|last1 = Jones|first2 = Stephen P.|last2 = Stanforth|journal = Org. React.|year = 2000|volume = 56|issue = 2|pages = 355–686|doi = 10.1002/0471264180.or056.02}} which attacks arenes.

Organolithium compounds and Grignard reagents react with DMF to give aldehydes after hydrolysis in a reaction called Bouveault aldehyde synthesis.{{cite book |last1=Wang |first1=Zerong |title=Comprehensive organic name reactions and reagents |date=2009 |publisher=John Wiley |location=Hoboken, N.J. |isbn=9780471704508 |pages=490–492}}

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.{{cite journal|author1=Vogel G. C. |author2=Drago, R. S. |year=1996|journal=Journal of Chemical Education|volume=73|pages=701–707|title=The ECW Model|issue=8 |bibcode=1996JChEd..73..701V|doi=10.1021/ed073p701}} Its relative donor strength toward a series of acids, versus other Lewis bases, can be illustrated by C-B plots.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{{cite journal|author1=Cramer, R. E. |author2=Bopp, T. T. |year=1977|title= Graphical display of the enthalpies of adduct formation for Lewis acids and bases |journal= Journal of Chemical Education |volume=54|pages=612–613|doi= 10.1021/ed054p612}} The plots shown in this paper used older parameters. Improved E&C parameters are listed in ECW model.

History and synthesis

DMF was first obtained in 1893 by the French chemist Albert Verley (1867–1959), by distilling a mixture of dimethylamine hydrochloride and potassium formate.{{cite journal|last1=Verley|first1=A.|title=Sur la préparation des amides en général|journal=Bulletin de la Société Chimique de Paris|date=1893|volume=9|pages=690–692|url=https://babel.hathitrust.org/cgi/pt?id=uc1.a0008581456;view=1up;seq=700|series=3rd series|trans-title=On the preparation of amides in general|language=fr}} 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.

It is now industrially manufactured by combining methyl formate and dimethylamine or by reaction of dimethylamine with carbon monoxide.{{cite book |author1=Weissermel, K. |author2=Arpe, H.-J. | title = Industrial Organic Chemistry: Important Raw Materials and Intermediates | publisher = Wiley-VCH | isbn = 3-527-30578-5 | pages = 45–46 |year=2003}}

Although currently impractical, DMF can be prepared from supercritical carbon dioxide using ruthenium-based catalysts.{{cite book|author1=Walter Leitner|author2=Philip G. Jessop|title=Chemical synthesis using supercritical fluids|url=https://books.google.com/books?id=-9yqpBozUuYC&pg=PA408|access-date=27 June 2011|year=1999|publisher=Wiley-VCH|isbn=978-3-527-29605-7|pages=408–}}

Applications

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.

  • It is used as a reagent in the Bouveault aldehyde synthesis{{cite journal|last = Bouveault|first = Louis|author-link = Louis Bouveault|journal = Bulletin de la Société Chimique de Paris|year = 1904|series=3rd series|volume = 31|pages = 1306–1322|title = Modes de formation et de préparation des aldéhydes saturées de la série grasse|language = fr|trans-title = Methods of preparation of saturated aldehydes of the aliphatic series|url=https://babel.hathitrust.org/cgi/pt?id=uc1.a0004784781;view=1up;seq=1410}}{{cite journal|last = Bouveault|first = Louis|author-link = Louis Bouveault|journal = Bulletin de la Société Chimique de Paris|year = 1904|series=3rd series|volume = 31|pages = 1322–1327|title = Nouvelle méthode générale synthétique de préparation des aldéhydes|trans-title = Novel general synthetic method for preparing aldehydes|language = fr|url=https://babel.hathitrust.org/cgi/pt?id=uc1.a0004784781;view=1up;seq=1426}}{{cite book|last = Li|first = Jie Jack|title = Name Reactions: A Collection of Detailed Mechanisms and Synthetic Applications|edition = 5th|chapter = Bouveault aldehyde synthesis|pages = 72–73|chapter-url = https://books.google.com/books?id=HoXBBAAAQBAJ&pg=PA72|year = 2014|publisher = Springer Science & Business Media|isbn = 978-3-319-03979-4}} and in the Vilsmeier-Haack reaction, another useful method of forming aldehydes.
  • It is a common solvent in the Heck reaction.{{cite book|title = The Mizoroki–Heck Reaction|editor-first = Martin|editor-last = Oestreich|publisher = John Wiley & Sons|year = 2009|isbn = 9780470716069}}
  • It is a common catalyst used in the synthesis of acyl halides, in particular the synthesis of acyl chlorides from carboxylic acids using oxalyl or thionyl chloride. The catalytic mechanism entails reversible formation of an imidoyl chloride (also known as the 'Vilsmeier reagent'):{{cite book | author = Clayden, J. | title = Organic Chemistry | publisher = Oxford University Press | location = Oxford | year = 2001 | pages = [https://archive.org/details/organicchemistry00clay_0/page/276 276–296] | isbn = 0-19-850346-6 | url-access = registration | url = https://archive.org/details/organicchemistry00clay_0/page/276}}Ansell, M. F. in "The Chemistry of Acyl Halides"; S. Patai, Ed.; John Wiley and Sons: London, 1972; pp 35–68.

File:Acyl chloride via amide catalysis.png

  • DMF penetrates most plastics and makes them swell. Because of this property DMF is suitable for solid phase peptide synthesis and as a component of paint strippers.
  • DMF is used as a solvent to recover olefins such as 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 carbon nanotubes, and is recommended by the NIST for use in near infrared spectroscopy of such.{{cite book |author1=Haddon, R. |author2=Itkis, M. |editor1=Freiman, S. |editor2=Hooker, S. |editor3=Migler |editor4=K. |editor5=Arepalli, S. | title = Publication 960-19 Measurement Issues in Single Wall Carbon Nanotubes | chapter = 3. Near-Infrared (NIR) Spectroscopy | publisher = NIST |date=March 2008 | chapter-url = https://www.nist.gov/customcf/get_pdf.cfm?pub_id=852726 | chapter-format = pdf | page = 20 | access-date = 2012-06-28}}
  • 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.{{cite journal | pmc=1008494 | year=1979 | last1=Lyle | first1=W. H. | last2=Spence | first2=T. W. | last3=McKinneley | first3=W. M. | last4=Duckers | first4=K. | title=Dimethylformamide and alcohol intolerance | journal=British Journal of Industrial Medicine | volume=36 | issue=1 | pages=63–66 | doi=10.1136/oem.36.1.63 | pmid=444443}}

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.

{{cite web | title = Skumlegetøj afgiver farlige kemikalier (in English- Squishies giving dangerous chemicals) | url = https://mst.dk/service/nyheder/nyhedsarkiv/2018/jun/skumlegetoej-afgiver-farlige-kemikalier/ | author1 = Magnus Løfstedt | access-date = 2019-06-13 | archive-date = 2021-09-03 | archive-url = https://web.archive.org/web/20210903082250/https://mst.dk/service/nyheder/nyhedsarkiv/2018/jun/skumlegetoej-afgiver-farlige-kemikalier/ | url-status = dead}}

Toxicity

The acute LD50 (oral, rats and mice) is 2.2–7.55 g/kg. Hazards of DMF have been examined.{{cite journal |author1=Redlich, C. |author2=Beckett, W. S. |author3=Sparer, J. |author4=Barwick, K. W. |author5=Riely, C. A. |author6=Miller, H. |author7=Sigal, S. L. |author8=Shalat, S. L. |author9=Cullen, M. R. | title = Liver disease associated with occupational exposure to the solvent dimethylformamide | journal = Annals of Internal Medicine | year = 1988 | volume = 108 | issue = 5 | pages = 680–686 | pmid = 3358569 | doi=10.7326/0003-4819-108-5-680}}

References

{{Reflist|35em}}

External links

  • {{ICSC|0457|04}}
  • {{PGCH|0226}}
  • [http://www.inchem.org/documents/cicads/cicads/cicad31.htm Concise International Chemical Assessment Document 31: N,N-Dimethylformamide]

{{Authority control}}

Category:Formamides

Category:Amide solvents

Category:Hepatotoxins

Category:IARC Group 2A carcinogens