Bromine azide

Summary

Bromine azide
Bromine azide.svg
Names
IUPAC name
Bromine azide
Other names
Bromine nitride, Nitrogen bromide, Azidobromide
Identifiers
  • 13973-87-0
3D model (JSmol)
  • Interactive image
  • Interactive image
ChemSpider
  • 24562
  • 26364
  • DTXSID50161155 Edit this at Wikidata
  • InChI=1S/BrN3/c1-3-4-2
    Key: KFCUPNHUPHDVJC-UHFFFAOYSA-N
  • InChI=1/BrN3/c1-3-4-2
    Key: KFCUPNHUPHDVJC-UHFFFAOYAE
  • [N-]=[N+]=N\Br
  • [N-]=[N+]=NBr
Properties
BrN3
Molar mass 121.924 g/mol
Appearance Red liquid
Density N/A
Melting point -45 degrees C (-49 F°)
Boiling point Explodes
Structure[1]
tetragonal
I4cd
16
Hazards
Main hazards This is a poison that can spontaneously explode.[2] It explodes on contact with arsenic, sodium, silver foil, or phosphorus. It has a hazard class of 1.1A.
Related compounds
Related compounds
Fluorine azide
Chlorine azide
Iodine azide
Hydrazoic acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Bromine azide is an explosive inorganic compound with the formula BrN3. It has been described as a crystal or a red liquid at room temperature.[citation needed] It is extremely sensitive to small variations in temperature and pressure, with explosions occurring at Δp ≥ 0.05 Torr and also upon crystallization, thus extreme caution must be observed when working with this reagent.

Preparation

Bromine azide may be prepared by the reaction of sodium azide with Br2. This reaction forms bromine azide and sodium bromide:[1]

NaN3 + Br2 → BrN3 + NaBr

Structure

The high sensitivity of bromine azide has led to difficulty in discerning its crystal structure. Despite this, a crystal structure of bromine azide has been obtained using a miniature zone-melting procedure with focused infrared laser radiation. In contrast to IN3, which forms an endless chain-like structure upon crystallization, BrN3 forms a helical structure. Each molecule adopts a trans-bent structure, which is also found in the gas phase.[1]

Reactions

Bromium azide adds to alkenes both through ionic and free-radical addition, each giving an opposite orientation in the products. The ionic addition occurs stereospecifically in trans.[3] Reactions involving bromine azide are difficult to work with. The molecule is very reactive and is known to explode easily. This makes it a key reagent in explosives.[4] Photochemistry experiments with bromine azide have found that UV photolysis of a small sample of bromine azide resulted in dissociation of the entire sample, making it unstable. Similar samples with azide molecules did not show such an effect. This shows bromine azide's unstable tendencies in that even in the presence of sunlight, bromine azide will be a reactive molecule.[5]

Safety

Great care must be taken when handling bromine azide as it is potentially toxic and is able to explode under various conditions. Concentrated solutions in organic solvents may also explode. The liquid explodes on contact with arsenic, sodium, silver foil, or phosphorus. When heated to decomposition it emits highly toxic fumes of bromine and explodes. The amount of compound used during experimentation should be limited to 2 mmol. It also poses a potential moderate fire hazard in the form of vapor by chemical reaction. It is also a powerful oxidant.[1]

It has been banned from transport in the United States by the US Department of Transportation.

References

  1. ^ a b c d Lyhs, Benjamin; Bläser, Dieter; Wölper, Christoph; Schulz, Stephan; Jansen, Georg (20 February 2012). "Solid-State Structure of Bromine Azide". Angewandte Chemie International Edition. 51 (8): 1970–1974. doi:10.1002/anie.201108092. PMID 22250068.
  2. ^ Patnaik, Pradyot (2007). A Comprehensive Guide to the Hazardous Properties of Chemical Substances. 615: Wiley-Interscience. p. 615. ISBN 0-471-71458-5.CS1 maint: location (link)
  3. ^ Liu, Robert (1968). "2,3-Bis(perfluormethyl)bicyclo2.2.2]octa-2,5,7-trienes and their photorearrangement reactions". J. Am. Chem. Soc. 90 (1): 215–216. doi:10.1021/ja01003a041.
  4. ^ Perry, Dale L., ed. (1995). Handbook of inorganic compounds. Boca Raton: CRC Press. p. 74. ISBN 0-8493-8671-3.
  5. ^ Henshaw, T. L.; David, S. J.; MacDonald, M. A.; Gilbert, J. V.; Stedman, D. H.; Coombe, R. D. (1987). "Collisional decomposition of bromine azide". J. Phys. Chem. 91 (9): 2287–2293. doi:10.1021/j100293a016.