Chemistry:Ammonium azide
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| Names | |
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| IUPAC name
Ammonium azide
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| Other names
Ammonium trinitride
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| Identifiers | |
3D model (JSmol)
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PubChem CID
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| Properties | |
| [NH 4]N 3 | |
| Molar mass | 60.060 g·mol−1 |
| Appearance | Colorless or white crystalline solid |
| Odor | Odorless |
| Density | 1.3459 g/cm3 |
| Melting point | 160[1] °C (320 °F; 433 K) |
| Boiling point | 400 °C (752 °F; 673 K) (decomposes) |
| 20.2 g/100 mL (30 °C)[1] | |
| Solubility | Insoluble in diethyl ether and benzene[2] |
| Solubility in methanol | 3.3 g/100 mL (20 °C)[2] |
| Solubility in ethanol | 1.06 g/100 mL (20 °C)[2] |
| Structure[3] | |
| Orthorhombic | |
| Pman | |
a = 8.930, b = 8.642, c = 3.800
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Formula units (Z)
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4 |
| Thermochemistry[1] | |
Std molar
entropy (S |
112.5 J/(mol·K) |
Std enthalpy of
formation (ΔfH⦵298) |
115.5 kJ/mol |
Gibbs free energy (ΔfG˚)
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274.2 kJ/mol |
| Hazards | |
| Main hazards | Very toxic, explosive |
| Related compounds | |
Other anions
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Other cations
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Related compounds
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Ammonium azide is the chemical compound with the formula [[[Chemistry:Nitrogen|N]]H
4]N
3, being the salt of ammonia and hydrazoic acid. Like other inorganic azides, this colourless crystalline salt is a powerful explosive, although it has a remarkably low sensitivity. [NH
4]N
3 is physiologically active and inhalation of small amounts causes headaches and palpitations. It was first obtained by Theodor Curtius in 1890, along with other azides.
Structure
Ammonium azide is ionic, meaning it is a salt consisting of ammonium cations [NH
4]+
and azide anions N−
3, therefore its formula is [NH
4]+
[N
3]−
. It is a structural isomer of tetrazene. Ammonium azide contains about 93% nitrogen by mass.
Preparation
There are two major methods of producing ammonium azide. Small quantities (grams) of ammonium azide are produced by bubbling ammonia gas through a solution of hydrazoic acid in diethyl ether:[2]
- NH3 + HN3 → [NH4]N3
Larger quantities are produced by the reaction of sodium azide and ammonium chloride in dimethylformamide at 100 °C.[4]
References
- ↑ 1.0 1.1 1.2 Haynes, William M.; Lide, David R.; Bruno, Thomas J. (2014). CRC Handbook of Chemistry and Physics, 95th Edition (95th ed.). CRC Press. ISBN 9781482208689. OCLC 908078665.
- ↑ 2.0 2.1 2.2 2.3 Frierson, W. J.; Filbert, W. F. (1946). "Ammonium Azide". Inorganic Syntheses. 2. Wiley. p. 136–138. doi:10.1002/9780470132333.ch39. ISBN 978-0-470-13161-9.
- ↑ Frevel, Ludo K. (1 January 1936). "The Crystal Structure of Ammonium Azide, NH4N3". Zeitschrift für Kristallographie - Crystalline Materials 94 (1–6): 197. doi:10.1524/zkri.1936.94.1.197.
- ↑ Evans, B. L.; Yoffe, A. D.; Gray, Peter (1959). "Physics And Chemistry Of The Inorganic Azides". Chemical Reviews 59 (4): 515–568. doi:10.1021/cr50028a001. ISSN 0009-2665.
- Yakovleva, G. S.; Kurbangalina, R. Kh.; Stesik, L. N. (1977). "Detonation properties of ammonium azide". Combustion, Explosion, and Shock Waves 13 (3): 405. doi:10.1007/BF00740326. Bibcode: 1977CESW...13..405Y.
- Salim de Amorim, Helio; do Amaral, M. R.; Pattison P.; Ludka I. P.; Mendes, J. C. (2002). "Ammonium azide: A Commented Example of an Ab Initio Structure (Re-)Determination From X-Ray Diffraction". Revista de la Sociedad Química de Mexico 45 (4): 313–319. https://www.redalyc.org/pdf/475/47546404.pdf.
- Curtius, Th. (1890). "Ueber Stickstoffwasserstoffsäure (Azoimid) N3H". Berichte der Deutschen Chemischen Gesellschaft 23 (2): 3023–3033. doi:10.1002/cber.189002302232. https://zenodo.org/record/1425592.
Further reading
- Schmidt, Eckart W. (2022). "Azides and Azido Compounds". Encyclopedia of Liquid Fuels. De Gruyter. pp. 893–900. doi:10.1515/9783110750287-011. ISBN 978-3-11-075028-7.
Salts and covalent derivatives of the azide ion
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| HN3 | He | ||||||||||||||||||
| LiN3 | Be(N3)2 | B(N3)3 | CH3N3, C(N3)4 |
N(N3)3,H2N—N3 | O | FN3 | Ne | ||||||||||||
| NaN3 | Mg(N3)2 | Al(N3)3 | Si(N3)4 | P | SO2(N3)2 | ClN3 | Ar | ||||||||||||
| KN3 | Ca(N3)2 | Sc(N3)3 | Ti(N3)4 | VO(N3)3 | Cr(N3)3, CrO2(N3)2 |
Mn(N3)2 | Fe(N3)3 | Co(N3)2, Co(N3)3 |
Ni(N3)2 | CuN3, Cu(N3)2 |
Zn(N3)2 | Ga(N3)3 | Ge | As | Se(N3)4 | BrN3 | Kr | ||
| RbN3 | Sr(N3)2 | Y | Zr(N3)4 | Nb | Mo | Tc | Ru(N3)63− | Rh(N3)63− | Pd(N3)2 | AgN3 | Cd(N3)2 | In | Sn | Sb | Te | IN3 | Xe(N3)2 | ||
| CsN3 | Ba(N3)2 | Hf | Ta | W | Re | Os | Ir(N3)63− | Pt(N3)62− | Au(N3)4− | Hg2(N3)2, Hg(N3)2 |
TlN3 | Pb(N3)2 | Bi(N3)3 |
Po | At | Rn | |||
| Fr | Ra(N3)2 | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |||
| ↓ | |||||||||||||||||||
| La | Ce(N3)3, Ce(N3)4 |
Pr | Nd | Pm | Sm | Eu | Gd(N3)3 | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||||
| Ac | Th | Pa | UO2(N3)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||||
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