My watch list  

Sodium azide

Sodium azide
Other names Sodium trinitride
CAS number 26628-22-8
Molecular formula NaN3
Molar mass 65.01 g/mol
Appearance White solid.
Density 1.85 g/cm³, solid
Melting point

275 °C decomp.

Solubility in water 41.7 g/100 mL (17°C)
MSDS External MSDS
EU classification Highly toxic (T+)
Dangerous for
the environment (N)
R-phrases R21, R26, R28,
R32, R50, R53
S-phrases (S1), (S2), S28, S45,
S60, S61
Related Compounds
Other cations Potassium azide
Related compounds Sodium cyanide
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)

Infobox disclaimer and references

Sodium azide is the chemical compound with the formula NaN3. This colourless salt is a common reagent in organic synthesis, and it is a component in many car airbag systems.


Structure, synthesis, and principal reactions


Sodium azide is ionic. The N3 group is centrosymmetric with N-N distances of 1.18 Å.[1] Sodium azide is highly soluble in water. Such solutions contain minute amounts of hydrogen azide, as described by the following equilibrium:

N3 + H2O \overrightarrow{\leftarrow} HN3 K = 10−4.6


The common synthesis method is the "Wislicenus process," which proceeds in two steps from ammonia. In the first step, ammonia is converted to sodium amide:

2 Na + 2 NH3 → 2 NaNH2 + H2

The sodium amide is subsequently combined with nitrous oxide.

2 NaNH2 + N2O → NaN3 + NaOH + NH3

Alternatively the salt can be obtained by the reaction of sodium nitrate with sodium amide.[2]


Treatment of sodium azide with strong acids gives the corresponding acid, hydrazoic acid:

H2SO4 + NaN3 → HN3 + NaHSO4

Sodium azide cannot be melted, but decomposes vigorously to sodium metal and nitrogen gas at approximately 300 °C. An electrical charge triggered by automobile impact heats the salt to explosively release nitrogen gas inside the airbag:

2 NaN3 → 2 Na + 3 N2

The sodium that is formed is a potential hazard itself and, in automobile airbags, it is converted by reaction with other ingredients, such as potassium nitrate (KNO3) and silica (SiO2), into an inert alkaline silicate 'glass'.[3]

Sodium azide is used in organic synthesis to introduce the azide functional group by displacement of a halide.[4] The azide functional group can thereafter be converted to an amine by reduction with either lithium aluminum hydride, or a tertiary phosphine such as triphenylphosphine in the Staudinger reaction.

Sodium azide can be destroyed by treatment with acidic sodium nitrite solution:[5]

2 NaN3 + 2 HNO2 → 3 N2 + 2 NO + 2 NaOH

Biochemistry and biomedical uses

Sodium azide is a useful probe reagent, mutagen, and preservative. In hospitals and laboratories, it is a biocide; it is especially important in bulk reagents and stock solutions which may otherwise support bacterial growth where the sodium azide acts as a bacteriostatic by inhibiting cytochrome oxidase in gram-negative bacteria; gram-positive (streptococci, pneumococci, lactobacilli) are resistant[6] (a characteristic similar to antibiotic resistance). It is also used in agriculture (farming) for pest control.

Azide inhibits cytochrome oxidase by binding irreversibly to the heme cofactor in a process similar to the action of carbon monoxide. Sodium azide is particularly affects organs that undergo high rates of respiration, such as the heart and the brain.

Toxic effects

Sodium azide is often comparable with cyanide, as they give similar symptoms.[citation needed] Exposure to sodium azide has some or all of the following symptoms within minutes: rapid breathing, restlessness, dizziness, weakness, headache, nausea and vomiting, rapid heart rate, red eyes (gas or dust exposure), clear drainage from the nose (gas or dust exposure), cough (gas or dust exposure), skin burns and blisters (explosion or direct skin contact. Exposure to a large amount of sodium azide may cause these other health effects as well: convulsions, low blood pressure, low heart rate, loss of consciousness, and lung injury, respiratory failure leading to death.


  1. ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
  2. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  3. ^ Eric A. Betterton (2003). "Environmental Fate of Sodium Azide Derived from Automobile Airbags". Critical Reviews in Environmental Science and Technology 33 (4): 423–458. doi:10.1080/10643380390245002.
  4. ^ Asher Kalir and David Balderman "2-Phenyl-2-Adamantanamine Hydrochloride" Organic Syntheses, Collected Volume 7, p.433 (1990).
  5. ^ (1995) Prudent practices in the laboratory: handling and disposal of chemicals. National Academy Press. ISBN 0309052297. 
  6. ^ Lichstein, Herman C.; Malcolm H. Soule (1943-06-19). "Studies of the Effect of Sodium Azide on Microbic Growth and Respiration" (PDF). Journal of Bacteriology 47 (3): 221-230. the American Society for Microbiology. ISSN 0343-6993. Retrieved on 2006-10-03.
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Sodium_azide". A list of authors is available in Wikipedia.
Your browser is not current. Microsoft Internet Explorer 6.0 does not support some functions on Chemie.DE