Methyl azide
Skeletal formula of methyl azide
Ball-and-stick model of the methyl azide molecule
Space-filling model of the methyl azide molecule
Names
Preferred IUPAC name
Azidomethane
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/CH3N3/c1-3-4-2/h1H3 checkY
    Key: PBTHJVDBCFJQGG-UHFFFAOYSA-N checkY
  • [N-]=[N+]=N\C
Properties
CH3N3
Molar mass 57.056 g·mol−1
Appearance white powder
Boiling point 20–21 °C (68–70 °F; 293–294 K)
slightly soluble
Solubility alkane, ether
Explosive data
Shock sensitivity High
Friction sensitivity High
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Highly explosive
Related compounds
Related compounds
 Hydrazoic acid, Chlorine azide, Ethyl azide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Methyl azide is an organic compound with the formula CH3N3. It is a white solid and it is the simplest organic azide.

Preparation and properties

Methyl azide can be prepared by the methylation of sodium azide, for instance with dimethyl sulfate in alkaline solution, followed by passing through a tube of anhydrous calcium chloride or sodium hydroxide to remove contaminating hydrazoic acid.[1] The first synthesis was reported in 1905.[2]

Decomposition to a nitrene is a first-order reaction:

CH3N3 → CH3N + N2

The product, like its notional tautomer methanimine, polymerizes at room temperature.[3]

Methyl azide might be a potential precursor in the synthesis of prebiotic molecules via nonequilibrium reactions on interstellar ices initiated by energetic galactic cosmic rays (GCR) and photons.[4]

Safety precautions

Methyl azide is stable at ambient temperature but may explode when heated. Presence of mercury increases the sensitivity to shock and spark. It is incompatible with methanol and dimethyl malonate.[5] When heated to decomposition, it emits toxic fumes of NO
x.[citation needed] It can be stored indefinitely in the dark at −80 °C.[1]

References

  1. ^ a b Chae, Junghyun (2008-03-14), "Methyl Azide", in John Wiley & Sons, Ltd (ed.), Encyclopedia of Reagents for Organic Synthesis, Chichester, UK: John Wiley & Sons, Ltd, pp. rn00795, doi:10.1002/047084289x.rn00795, ISBN 978-0-471-93623-7
  2. ^ Dimroth, O.; Wislicenus, W. (1905). "Ueber das Methylazid". Berichte der Deutschen Chemischen Gesellschaft. 38 (2): 1573–1576. doi:10.1002/cber.19050380254.
  3. ^ O'Dell, M. S.; Darwent, B. (1970). "Thermal decomposition of methyl azide". Canadian Journal of Chemistry. 48 (7): 1140–1147. doi:10.1139/v70-187.
  4. ^ Quinto-Hernandez, A.; Wodtke, A. M.; Bennett, C. J.; Kim, Y. S.; Kaiser, R. I. (2011). "On the Interaction of Methyl Azide (CH3N3) Ices with Ionizing Radiation: Formation of Methanimine (CH2NH), Hydrogen Cyanide (HCN), and Hydrogen Isocyanide (HNC)". The Journal of Physical Chemistry A. 115 (3): 250–264. doi:10.1021/jp103028v. PMID 21162584.
  5. ^ Urben, P. G., ed. (2006). Bretherick's Handbook of Reactive Chemical Hazards (7th ed.). Elsevier. ISBN 9780123725639.

External links

Inorganic compounds of carbon and related ions
Salts and covalent derivatives of the azide ion
Categories