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Barium azide

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Barium azide
Names
Other names barium dinitride
Identifiers
CAS Number
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.038.706 Edit this at Wikidata
EC Number
  • 242-594-6
PubChem CID
UN number 1687
CompTox Dashboard (EPA)
InChI
  • InChI=1S/Ba.2N3/c;2*1-3-2/q+2;2*-1Key: UUXFWHMUNNXFHD-UHFFFAOYSA-N
SMILES
  • .==.==
Properties
Chemical formula BaN6
Molar mass 194.23 g/mol
Appearance white crystalline solid
Odor odorless
Density 2.936 g/cm
Melting point 126 °C
Boiling point 160°C(initial decomposition), >217°C (deflagrates)
180°C(initial decomposition), 225°C explosion
Solubility in water 11.5 g/100 mL (0°C)
14.98 g/100mL (15.7°C)
15.36 g/100mL (20°C)
22.73 g/100mL (52.1°C)
24.75 g/100mL (70°C)
Solubility in alcohol 0.017 g/100 mL (16°C)
Solubility in acetone , ether insoluble
Hazards
Lethal dose or concentration (LD, LC):
LD50 (median dose) mg/kg (oral, rats/mice)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). checkY verify (what is  ?) Infobox references
Chemical compound

Barium azide Ba(N3)2 is an inorganic azide, is explosive, but less sensitive to mechanical shock than lead azide.

Preparation

Barium azide can be prepared by action of hydrazoic acid in barium hydroxide, barium oxide or barium carbonate. The salt has also been synthesized with hydrazine and nitrite: 3.5 g barium hydroxide and 200 mL aqueous hydrazine (5% w/w) were cooled and 15 g ethyl nitrite added dropwise with stirring. After 24 hours, excess hydroxide was removed with carbon dioxide; the filtrate yield was 8g (30% yield).

Uses

Can be used to make azides of magnesium (but its hydrolytic tendency frustrated efforts to isolate it), sodium, potassium, lithium, rubidium and zinc with their respective sulfates.

Ba(N3)2 + Li2SO4 → 2 LiN3 + BaSO4

References

  1. Fedoroff, Basil T. (1960). Encyclopedia of Explosives and Related Items (Vol. 1). US Army Research and Development Command TACOM, ARDEC. {{cite book}}: Unknown parameter |coauthors= ignored (|author= suggested) (help)
  2. Tiede, E. (1916). "Die Zersetzung der Alkali- und Erdalkali-azide im Hochvakuum zur Reindarstellung von Stickstoff". Ber. Dtsch. Chem. Ges. 49: p. 1742–1745. doi:10.1002/cber.19160490234. {{cite journal}}: |pages= has extra text (help)
  3. Audrieth, L. F. (1934). "Hydrazoic Acid and Its Inorganic Derivatives". Chem. Rev. 15: p. 169–224. doi:10.1021/cr60051a002. {{cite journal}}: |pages= has extra text (help)
  4. ^ H. D. Fair and R. F. Walker (1977). Energetic Materials, Vol. 1. Physics and Chemistry of the Inorganic Azides. New York and London: Plenum Press. doi:10.1002/prac.19770811124.
  5. Curtius, T.; Rissom, J. (1898). "Neue Untersuchungen über den Stickstoffwasserstoff N3H". J. Prakt. Chem. 58: p. 261–309. doi:10.1002/prac.18980580113. {{cite journal}}: |pages= has extra text (help)
  6. Hoth, W.; Pyl, G. (1916). "Über die Darstellung der Stickstoffwasserstoffsäure und ihrer Salze". Angew. Chem. 49: p. 1742–1745. doi:10.1002/cber.19160490234. {{cite journal}}: |pages= has extra text (help)
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