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IUPAC name
Other names
3D model (JSmol)
ECHA InfoCard 100.005.803
Molar mass 42.04 g/mol
Appearance Yellow gas
Odor musty
Density 1.4 (air=1)
Melting point −145 °C (−229 °F; 128 K)
Boiling point −23 °C (−9 °F; 250 K)
linear C=N=N
Main hazards toxic and explosive
R-phrases (outdated) R12 R19 R22 R66 R67
S-phrases (outdated) S9 S16 S29 S33
NFPA 704
Flammability code 3: Liquids and solids that can be ignited under almost all ambient temperature conditions. Flash point between 23 and 38 °C (73 and 100 °F). E.g., gasolineHealth code 4: Very short exposure could cause death or major residual injury. E.g., VX gasReactivity code 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g., fluorineSpecial hazards (white): no codeNFPA 704 four-colored diamond
Lethal dose or concentration (LD, LC):
175 ppm (cat, 10 min)[3]
US health exposure limits (NIOSH):
PEL (Permissible)
TWA 0.2 ppm (0.4 mg/m3)[2]
REL (Recommended)
TWA 0.2 ppm (0.4 mg/m3)[2]
IDLH (Immediate danger)
2 ppm[2]
Related compounds
Related functional groups;
R-N=N=N (azide),
R-N=N-R (azo);
R2CN2 R = Ph, tms, CF3
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Diazomethane is the chemical compound CH2N2, discovered by German chemist Hans von Pechmann in 1894. It is the simplest diazo compound. In the pure form at room temperature, it is an extremely sensitive explosive yellow gas; thus, it is almost universally used as a solution in diethyl ether. The compound is a popular methylating agent in the laboratory, but it is too hazardous to be employed on an industrial scale without special precautions.[4] Use of diazomethane has been significantly reduced by the introduction of the safer and equivalent reagent trimethylsilyldiazomethane.[5]


For safety and convenience diazomethane is always prepared as needed as a solution in ether and used as such. It converts carboxylic acids into their methyl esters or into their homologues (see Arndt-Eistert synthesis). In the Büchner–Curtius–Schlotterbeck reaction diazomethane reacts with an aldehyde to form ketones.[6][7]

Büchner-Curtius-Schlotterbeck Reaction.

When diazomethane reacts with alcohols or phenols in presence of boron trifluoride (BF3), methyl ethers are obtained.

Diazomethane is also frequently used as a carbene source. It readily takes part in 1,3-dipolar cycloadditions.


Diazomethane laboratory preparation

Diazomethane is prepared by hydrolysis of an ethereal solution of an N-methyl nitrosamide with aqueous base. The traditional precursor is N-nitroso-N-methylurea, but this compound is itself somewhat unstable, and nowadays compounds such as N-methyl-N'-nitro-N-nitrosoguanidine (MNNG) and N-methyl-N-nitroso-p-toluenesulfonamide (Diazald) are preferred.[8]

Preparation of Diazomethane.

CH2N2 reacts with basic solutions of D2O to give the deuterated derivative CD2N2.[9]

The concentration of CH2N2 can be determined in either of two convenient ways. It can be treated with an excess of benzoic acid in cold Et2O. Unreacted benzoic acid is then back-titrated with standard NaOH. Alternatively, the concentration of CH2N2 in Et2O can be determined spectrophotometrically at 410 nm where its extinction coefficient, ε, is 7.2.[citation needed] The gas-phase concentration of diazomethane can be determined using photoacoustic spectroscopy.[4]

Related compounds[edit]

Diazomethane is both isomeric and isoelectronic with the more stable cyanamide, but they cannot interconvert. Many substituted derivatives of diazomethane have been prepared:


Diazomethane is toxic by inhalation or by contact with the skin or eyes (TLV 0.2ppm). Symptoms include chest discomfort, headache, weakness and, in severe cases, collapse.[14] Symptoms may be delayed. Deaths from diazomethane poisoning have been reported. In one instance a laboratory worker consumed a hamburger near a fumehood where he was generating a large quantity of diazomethane, and died four days later from fulminating pneumonia.[15] Like any other alkylating agent it is expected to be carcinogenic, but such concerns are overshadowed by its serious acute toxicity.

CH2N2 may explode in contact with sharp edges, such as ground-glass joints, even scratches in glassware.[16] Glassware should be inspected before use and preparation should take place behind a blast shield. Specialized kits to prepare diazomethane with flame-polished joints are commercially available.

The compound explodes when heated beyond 100 °C, exposed to intense light, alkali metals, or calcium sulfate. Use of a blast shield is highly recommended while using this compound.

Proof-of-concept work has been done with microfluidics, in which continuous point-of-use synthesis from N-methyl-N-nitrosourea and 0.93M potassium hydroxide in water was followed by point-of-use conversion with benzoic acid, resulting in a 65% yield of the methyl benzoate ester within seconds at temperatures ranging from 0-50 C. The yield was better than under capillary conditions; the microfluidics were credited with "suppression of hot spots, low holdup, isothermal conditions, and intensive mixing."[17]


  2. ^ a b c "NIOSH Pocket Guide to Chemical Hazards #0182". National Institute for Occupational Safety and Health (NIOSH). 
  3. ^ "Diazomethane". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). 
  4. ^ a b Proctor, Lee D.; Warr, Antony J. (November 2002). "Development of a Continuous Process for the Industrial Generation of Diazomethane". Organic Process Research & Development. 6 (6): 884–892. doi:10.1021/op020049k. 
  5. ^ Shioiri, Takayuki; Aoyama, Toyohiko; Snowden, Timothy (2001). "Trimethylsilyldiazomethane". e-EROS Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rt298.pub2. 
  6. ^ Buchner, E.; Curtius, Th. (1885). "Synthese von Ketonsäureäthern aus Aldehyden und Diazoessigäther". Berichte der Deutschen Chemischen Gesellschaft. 18: 2371–2377. doi:10.1002/cber.188501802118. 
  7. ^ Schlotterbeck, F. (1907). "The conversion of aldehydes and ketones through diazomethane". Berichte der Deutschen Chemischen Gesellschaft. 40: 479–483. doi:10.1002/cber.19070400179. 
  8. ^ Reed, Donald E.; James A. Moore (1961). "DIAZOMETHANE". Organic Syntheses. 41: 16. doi:10.15227/orgsyn.041.0016. 
  9. ^ P. G. Gassman and W. J. Greenlee (1988). "Dideuterodiazomethane". Organic Syntheses. ; Collective Volume, 6, p. 432 
  10. ^ W. J. Middleton; D. M. Gale (1988). "Bis(Trifluoromethyl)diazomethane". Organic Syntheses. ; Collective Volume, 6, p. 161 
  11. ^ L. I. Smith, K. L. Howard (1955). "Diphenyldiazomethane"". Organic Syntheses. ; Collective Volume, 3, p. 351 
  12. ^ T. Shioiri, T. Aoyama, S. Mori. "Trimethylsilyldiazomethane". Organic Syntheses. ; Collective Volume, 8, p. 612 
  13. ^ X. Creary (1990). "Tosylhydrazone Salt Pyrolyses: Phenydiazomethanes". Organic Syntheses. ; Collective Volume, 7, p. 438 
  14. ^ Muir, GD (ed.) 1971, Hazards in the Chemical Laboratory, The Royal Institute of Chemistry, London.
  15. ^ LeWinn, E.B. "Diazomethane Poisoning: Report of a fatal case with autopsy", The American Journal of the Medical Sciences, 1949, 218, 556-562.
  16. ^ de Boer, Th. J.; Backer, H. J. (1956). "DIAZOMETHANE". Organic Syntheses. 36: 16. doi:10.15227/orgsyn.036.0016. 
  17. ^ Wladimir Reschetilowski (2013-09-13). "Microreactors in Preparative Chemistry: Practical Aspects in Bioprocessing, Nanotechnology, Catalysis and more". Wiley. p. 6-15. 

External links[edit]