Sodium azide is an inorganic compound with the formula NaN3. This colorless salt is the gas-forming component in some car airbag systems. It is used for the preparation of other azide compounds. It is highly soluble in water and is acutely poisonous.
Structure Sodium azide is an ionic solid. Two crystalline forms are known, rhombohedral and hexagonal. Both adopt layered structures. The azide anion is very similar in each form, being centrosymmetric with N–N distances of 1.18 Å. The Na+ ion has an octahedral geometry. Each azide is linked to six Na+ center ions, with three Na–N bonds to each terminal nitrogen center.
Preparation The common synthesis method is the "Wislicenus process", which proceeds in two steps in liquid ammonia. In the first step, ammonia is converted to sodium amide by metallic sodium:
2 Na + 2 NH3 → 2 NaNH2 + H2 The sodium amide is subsequently combined with nitrous oxide:
2 NaNH2 + N2O → NaN3 + NaOH + NH3 These reactions are the basis of the industrial route, which produces about 250 tons per year in 2004, with production increasing due to the increased use of airbags.
Laboratory methods Curtius and Thiele developed another production process, where a nitrite ester is converted to sodium azide using hydrazine. This method is suited for laboratory preparation of sodium azide:
2 NaNO2 + 2 C2H5OH + H2SO4 → 2 C2H5ONO + Na2SO4 + 2 H2O C2H5ONO + N2H4·H2O + NaOH → NaN3 + C2H5OH + 3 H2O Alternatively the salt can be obtained by the reaction of sodium nitrate with sodium amide.
3 NaNH2 + NaNO3 → NaN3 + 3 NaOH + NH3
Chemical reactions
Acid formation of hydrazoic acid Treatment of sodium azide with strong acids gives hydrazoic acid (hydrogen azide; HN3):
H+ + N−3 → HN3 Hydrazoic acid, which is also extremely toxic, is especially dangerous because it is a volatile liquid at room temperature. Otherwise, aqueous solutions contain only minute amounts of hydrazoic acid, as described by the following equilibrium reaction:
N−3 + H2O ⇌ HN3 + OH−, K = 10−4.6
Destruction Sodium azide can be destroyed by treatment with nitrous acid (HNO2) generated in situ from a solution of NaN3 with a metal nitrite by acidification with a mineral acid.
2 NaN3 + 2 HNO2 → 3 N2 + 2 NO + 2 NaOH A safer modification to the above method that avoids the potential production of hydrazoic acid or nitrogen oxide fumes is that of W. F. Rinkenbach. A solution of 2.5 oz (71 g) sodium nitrite in 1 US pt (470 mL) of water is added to a stirring dispersion of 1 oz (28 g) sodium azide in 1.5 US gal (5.7 L) 10% ammonium acetate, followed by addition of 7 US fl oz (210 mL) of glacial acetic acid. The solution is allowed to stand in a warm place for an hour and disposed of.
Applications
Automobile airbags and aircraft evacuation slides Airbag formulations through late 1990s to early 2000s contained mixtures of oxidizers, sodium azide and other agents including ignitors and accelerants. An electronic controller detonates this mixture during an automobile crash:
2 NaN3 → 2 Na + 3 N2 The same reaction occurs upon heating the salt to approximately 300 °C. The sodium that is formed is a potential hazard alone and, in automobile airbags, it is converted by reaction with other ingredients, such as potassium nitrate and silica. In the latter case, innocuous sodium silicates are generated. While sodium azide is still used in evacuation slides on modern aircraft, newer-generation automotive air bags contain less sensitive explosives such as nitroguanidine or guanidine nitrate.
Organic and inorganic synthesis Due to its explosion hazard, sodium azide is of only limited value in industrial-scale organic synthesis. In the laboratory, it is used to introduce the azide functional group by displacement of halides. The azide functional group can thereafter be converted to an amine by reduction with either SnCl2 in ethanol or lithium aluminium hydride or a tertiary phosphine, such as triphenylphosphine in the Staudinger reaction, with Raney nickel or with hydrogen sulfide in pyridine. Oseltamivir, an antiviral medication, is currently produced in commercial scale by a method which utilizes sodium azide. Sodium azide is a versatile precursor to other inorganic azide compounds, e.g., lead azide and silver azide, which are used in detonators as primary explosives. These azides are significantly more sensitive to premature detonation than sodium azide and thus have limited applications. Lead and silver azide can be made via double displacement reaction with sodium azide and their respective nitrate (most commonly) or acetate salts. Sodium azide also can react with the chloride salts of certain alkaline earth metals in aqueous solution, such as barium chloride or strontium chloride to respectively produce barium azide and strontium azide, which are also relatively sensitive primarily explosive materials. These azides can be recovered from solution through careful desiccation.
Biochemistry and biomedical uses Sodium azide is a useful probe reagent, and an antibacterial preservative for biochemical solutions. In the past merthiolate and chlorobutanol were also used as an alternative to azide for preservation of biochemical solutions. Sodium azide is an instantaneous inhibitor of lactoperoxidase, which can be useful to stop lactroperoxidase catalyzed 125I protein radiolabeling experiments. 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; however, some gram-positive bacteria (streptococci, pneumococci, lactobacilli) are intrinsically resistant.
Agricultural uses It is used in agriculture for pest control of soil-borne pathogens such as Meloidogyne incognita or Helicotylenchus dihystera. It is also used as a mutagen for crop selection of plants such as rice, barley or oats.
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