Barium azide

Summary

Barium azide is an inorganic azide with the formula Ba(N3)2. It is a barium salt of hydrazoic acid. Like most azides, it is explosive. It is less sensitive to mechanical shock than lead azide.

Barium azide
Barium azide.svg
Barium azide, Ba(N3)2.png
Names
Other names
Barium dinitride
Identifiers
  • 18810-58-7 checkY
3D model (JSmol)
  • Interactive image
ChemSpider
  • 56472 checkY
ECHA InfoCard 100.038.706 Edit this at Wikidata
EC Number
  • 242-594-6
  • 62728
UN number 1687
  • DTXSID60908174 Edit this at Wikidata
  • InChI=1S/Ba.2N3/c;2*1-3-2/q+2;2*-1 checkY
    Key: UUXFWHMUNNXFHD-UHFFFAOYSA-N checkY
  • [Ba+2].[N-]=[N+]=[N-].[N-]=[N+]=[N-]
Properties
Ba(N3)2
Molar mass 221.37 g/mol
Appearance White crystalline solid
Odor Odourless
Density 2.936 g/cm3[1]
Melting point 126 °C (259 °F; 399 K)
Boiling point 160 °C (320 °F; 433 K) (initial decomposition)[2] >217 °C (deflagrates)
180 °C (initial decomposition),[3] 225 °C explosion
11.5 g/100 mL (0 °C)
14.98 g/100 mL (15.7 °C)
15.36 g/100 mL (20 °C)
22.73 g/100 mL (52.1 °C)
24.75 g/100 mL (70 °C)[4]
Solubility in ethanol 0.017 g/100 mL (16 °C)[5]
Solubility in acetone Insoluble
Solubility in ether Insoluble
Structure
Monoclinic
Hazards
GHS labelling:
GHS01: ExplosiveGHS06: Toxic
Danger
H200, H301, H315, H319, H331, H335
P210, P240, P264, P280, P305+P351+P338, P310
Safety data sheet (SDS) [1]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

PreparationEdit

Barium azine may be prepared by reacting sodium azide with a soluble barium salt. Care should be taken to prevent large crystals from forming in the solution as barium azide crystals will explode if subjected to friction/shock or if fully dried. The product should be stored submerged in ethanol.

UsesEdit

Barium azide can be used to make azides of magnesium, sodium, potassium, lithium, rubidium and zinc with their respective sulfates.[4]

Ba(N3)2 + Li2SO4 → 2 LiN3 + BaSO4

It can also be used as a source for high pure nitrogen by heating:

Ba(N3)2 → Ba + 3 N2

This reaction liberates metallic barium, which is used as a getter in vacuum applications.

See alsoEdit

ReferencesEdit

  1. ^ Fedoroff, Basil T.; Aaronson, Henry A.; Reese, Earl F.; Sheffield, Oliver E.; Clift, George D.; Dunkle, Cyrus G.; Walter, Hans; McLean, Dan C. (1960). Encyclopedia of Explosives and Related Items. Vol. 1. US Army Research and Development Command TACOM, ARDEC http://www.dtic.mil/get-tr-doc/pdf?AD=AD0257189. {{cite encyclopedia}}: Missing or empty |title= (help)
  2. ^ Tiede, Erich (1916). "Die Zersetzung der Alkali- und Erdalkali-azide im Hochvakuum zur Reindarstellung von Stickstoff". Ber. Dtsch. Chem. Ges. (in German). 49 (2): 1742–1745. doi:10.1002/cber.19160490234.
  3. ^ Audrieth, L. F. (1934). "Hydrazoic Acid and Its Inorganic Derivatives". Chem. Rev. 15 (2): 169–224. doi:10.1021/cr60051a002.
  4. ^ a b H. D. Fair; R. F. Walker, eds. (1977). Physics and Chemistry of the Inorganic Azides. Energetic Materials. Vol. 1. New York and London: Plenum Press. ISBN 9781489950093.
  5. ^ Curtius, T.; Rissom, J. (1898). "Neue Untersuchungen über den Stickstoffwasserstoff N3H". J. Prakt. Chem. (in German). 58 (1): 261–309. doi:10.1002/prac.18980580113.