Potassium azide
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| Molar mass | 81.1184 g/mol |
| Appearance | Colorless crystals[1] |
| Density | 2.038 g/cmScript error: No such module "Su". [1] |
| Melting point | Template:Chembox CalcTemperatures |
| Boiling point | Template:Chembox CalcTemperatures |
| Solubility | 0.1375 g/100 g in ethanol (16 °C)[2] insoluble in ether |
| Template:Longitem | −1.7 kJ/mol |
| NFPA 704 (fire diamond) | Template:NFPA 704 diamond |
| Template:Longitem | Sodium azide, copper(II) azide, lead(II) azide, silver azide |
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Potassium azide is the inorganic compound having the formula Template:Chem2. It is a white, water-soluble salt. It is used as a reagent in the laboratory.
It has been found to act as a nitrification inhibitor in soil.[4]
Structure
Template:Chem2, Template:Chem2, Template:Chem2, and Template:Chem2 adopt the same structures. They crystallize in a tetragonal habit.[5] The azide is bound to eight cations in an eclipsed orientation. The cations are bound to eight terminal N centers.[6]
Synthesis and reactions
Template:Chem2 is prepared by treating potassium carbonate with hydrazoic acid, which is generated in situ.[7] In contrast, the analogous sodium azide is prepared (industrially) by the "Wislicenus process," which proceeds via the reaction sodium amide with nitrous oxide.[8]
Upon heating or upon irradiation with ultraviolet light, it decomposes into potassium metal and nitrogen gas.[9] The decomposition temperatures of the alkali metal azides are: Template:Chem2 (275 °C), Template:Chem2 (355 °C), Template:Chem2 (395 °C), Template:Chem2 (390 °C).[10]
Under high pressures and high temperatures, potassium azide was found to transform into the K2N6 and K9N56 compounds, both containing hexazine rings: NScript error: No such module "Su". and N64-, respectively.[11][12]
Health hazards
Like sodium azide, potassium azide is very toxic. The threshold limit value of the related sodium azide is 0.07 ppm. The toxicity of azides arise from their ability to inhibit cytochrome c oxidase.[8]
References
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- ↑ Ulrich Müller "Verfeinerung der Kristallstrukturen von KN3, RbN3, CsN3 und TIN3" Zeitschrift für anorganische und allgemeine Chemie 1972, Volume 392, 159–166. Script error: No such module "CS1 identifiers".
- ↑ P. W. Schenk "Alkali Azides from Carbonates" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 475.
- ↑ a b Horst H. Jobelius, Hans-Dieter Scharff "Hydrazoic Acid and Azides" in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim. Script error: No such module "CS1 identifiers".
- ↑ Script error: No such module "Citation/CS1".
- ↑ E. Dönges "Alkali Metals" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 475
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