Barium azide

From Wikipedia, the free encyclopedia
Jump to navigation Jump to search
Barium azide
Barium azide.svg
Barium azide, Ba(N3)2.png
Names
Other names
barium dinitride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.038.706
EC Number 242-594-6
UN number 1687
Properties
BaN6
Molar mass 221.37 g/mol
Appearance white crystalline solid
Odor odourless
Density 2.936 g cm−3[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/100mL (15.7 °C)
15.36 g/100mL (20 °C)
22.73 g/100mL (52.1 °C)
24.75 g/100mL (70 °C)[4]
Solubility in alcohol 0.017 g/100 mL (16 °C)[5]
Solubility in acetone insoluble
Solubility in ether insoluble
Hazards
Safety data sheet [1]
Highly toxic (T+)
Dangerous for the environment (N)
R-phrases (outdated) R1, R23, R25, R36, R37, R38
Lethal dose or concentration (LD, LC):
mg/kg (oral, rats/mice)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☑Y verify (what is ☑Y☒N ?)
Infobox references

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

Uses[edit]

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 → 2LiN3 + BaSO4

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

Ba(N3)2 → Ba + 3N2

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

See also[edit]

References[edit]

  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. 1. US Army Research and Development Command TACOM, ARDEC http://www.dtic.mil/get-tr-doc/pdf?AD=AD0257189. 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. 1. New York and London: Plenum Press. doi:10.1002/prac.19770811124 (inactive 2019-08-21). 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.