Barium azide

Barium azide
Names


Other names Barium dinitride
Identifiers
CAS Number	18810-58-7^Y
3D model (JSmol)	Interactive image
ChemSpider	56472^Y
ECHA InfoCard	100.038.706
EC Number	242-594-6
PubChem CID	62728
UN number	1687
CompTox Dashboard (EPA)	DTXSID60908174
InChI InChI=1S/Ba.2N3/c;21-3-2/q+2;2-1^Y Key: UUXFWHMUNNXFHD-UHFFFAOYSA-N^Y
SMILES [Ba+2].[N-]=[N+]=[N-].[N-]=[N+]=[N-]
Properties
Chemical formula	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
Solubility in water	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
Crystal structure	Monoclinic
Hazards
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H200, H301, H315, H319, H331, H335
Precautionary statements	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). Y verify (what is ^YN ?) Infobox references

Chemical compound

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.

Preparation

Barium azide 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.^{[citation needed]}

Uses

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 purity nitrogen by heating:

Ba(N₃)₂ → Ba + 3 N₂

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

References

^ 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)^{[dead link]}
^ 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.
^ Audrieth, L. F. (1934). "Hydrazoic Acid and Its Inorganic Derivatives". Chem. Rev. 15 (2): 169–224. doi:10.1021/cr60051a002.
^ ^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.
^ 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.