Silver azide

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Silver azide
Names
IUPAC name
Silver(I) azide
Other names
Argentous azide
Identifiers
3D model (
JSmol
)
ChemSpider
ECHA InfoCard
 100.034.173 Edit this at Wikidata
UNII
  • InChI=1S/Ag.N3/c;1-3-2/q+1;-1 checkY
    Key: QBFXQJXHEPIJKW-UHFFFAOYSA-N checkY
  • InChI=1/Ag.N3/c;1-3-2/q+1;-1
    Key: QBFXQJXHEPIJKW-UHFFFAOYAJ
  • InChI=1S/Ag.N3/c;1-3-2/q+1;-1
    Key: QBFXQJXHEPIJKW-UHFFFAOYSA-N
  • [Ag+].[N-]=[N+]=[N-]
Properties
AgN3
Molar mass 149.888 g/mol
Appearance colorless crystals
Density 4.42 g/cm3
Melting point 250 °C (482 °F; 523 K) explosive
Boiling point decomposes
Solubility in other solvents 2.0×10−8 g/L
Structure
Orthorhombic oI16[1]
Ibam, No 72
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Very toxic, explosive
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 4: Readily capable of detonation or explosive decomposition at normal temperatures and pressures. E.g. nitroglycerinSpecial hazards (white): no code
3
0
4
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Silver azide is the

primary explosive
.

Structure and chemistry

Silver azide can be prepared by treating an

aqueous solution of silver nitrate with sodium azide.[2] The silver azide precipitates as a white solid, leaving sodium nitrate
in solution.

AgNO3(aq) + NaN3(aq) → AgN3(s) + NaNO3(aq)

square planar Ag+ coordinated by four azide ligands. Correspondingly, each end of each azide ligand is connected to a pair of Ag+ centers. The structure consists of two-dimensional AgN3 layers stacked one on top of the other, with weaker Ag–N bonds between layers. The coordination of Ag+ can alternatively be described as highly distorted 4 + 2 octahedral, the two more distant nitrogen atoms being part of the layers above and below.[3]

Part of a layer Layer stacking 4 + 2 coordination of Ag+ 2 + 1 coordination of N in N−3

In its most characteristic reaction, the solid decomposes explosively, releasing nitrogen gas:

2 AgN3(s) → 3 N2(g) + 2 Ag(s)

The first step in this decomposition is the production of free electrons and azide radicals; thus the reaction rate is increased by the addition of

lead azide.[6]

Safety

AgN3, like most heavy

primary explosive. Decomposition can be triggered by exposure to ultraviolet light or by impact.[2] Ceric ammonium nitrate [NH4]2[Ce(NO3)6] is used as an oxidising agent to destroy AgN3 in spills.[5]

See also

References

  1. doi:10.1107/S0365110X62003497
    .
  2. ^
    ISBN 978-3-642-28435-9.[1]
  3. PMID 17257034.{{cite journal}}: CS1 maint: multiple names: authors list (link
    )
  4. ISBN 978-0-444-82437-0
    .
  5. ^
    ISBN 978-1-56670-567-7
    .
  6. ISBN 978-0-471-96562-6
    .
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