Barium azide
Names | |
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Other names
barium dinitride | |
Identifiers | |
3D model (JSmol) |
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ChemSpider | |
ECHA InfoCard | 100.038.706 |
EC Number | 242-594-6 |
PubChem CID |
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UN number | 1687 |
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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 | |
EU classification (DSD) (outdated) |
Highly toxic (T+) Dangerous for the environment (N) |
R-phrases (outdated) | R1, R23, R25, R36, R37, R38 |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose) |
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). | |
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
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 used as a getter in vacuum applications.
See also
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. 1. US Army Research and Development Command TACOM, ARDEC.
- ↑ 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.
- 1 2 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 2018-08-27). 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.
Salts and covalent derivatives of the azide ion | |||||||||||||||||||
---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|
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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