Methyl azide is an organic compound with the formula CH3N3. It is a white solid and it is the simplest organic azide.

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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Preparation and properties

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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

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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

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  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.
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  • Graner, G.; Hirota, E.; Iijima, T.; Kuchitsu, K.; Ramsay, D. A.; Vogt, J.; Vogt, N. (1999). "CH3N3 Methyl azide". In Kuchitsu, K. (ed.). Group II Molecules and Radicals: Numerical Data and Functional Relationships in Science and Technology. Landolt-Börnstein - Group II Molecules and Radicals. Vol. 25 B. p. 1. doi:10.1007/10653318_320. ISBN 3-540-63645-5.
  • "Methyl azide". NIST Webbook. National Institute for Standards and Technology.