Chemistry:Nitrosyl azide
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| Properties | |
| N 3–N=O | |
| Molar mass | 72.027 g·mol−1 |
| Appearance | Pale yellow solid below −50 °C (−58 °F). Above that temperature it decomposes. |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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Nitrosyl azide is an inorganic compound of nitrogen and oxygen with the chemical formula N
3–N=O. It is a highly labile nitrogen oxide with the empirical formula N
4O.
Synthesis
Nitrosyl azide can be synthesized via the following reaction of sodium azide and nitrosyl chloride at low temperatures:
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Properties
Below −50 °C, nitrosyl azide exists as a pale yellow solid. Above this temperature, it decomposes into nitrous oxide N
2O and molecular nitrogen N
2:[1]
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Characterization of the compound with IR and Raman spectroscopy show absorption bands that agree well with calculated values for a trans-structure.[1][2] Quantum chemical calculations show a cis-form higher in energy by 4.2 kJ/mol and an aromatic ring form (oxatetrazole N
4O) that is more stable by 205 kJ/mol. However, the cyclization to the ring form would have to exceed the 205 kJ/mol activation energy barrier required to bend the azide group, which might explain why nitrosyl azide is stable enough to be isolated at low temperature.[1]
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References
- ↑ 1.0 1.1 1.2 Schulz, Axel; Tornieporth-Oetting, Inis C.; Klapötke, Thomas M. (1993). "Nitrosyl Azide, N4O, an Intrinsically Unstable Oxide of Nitrogen" (in en). Angewandte Chemie International Edition in English 32 (11): 1610–1612. doi:10.1002/anie.199316101.
- ↑ Lucien, Harold W. (1958). "The Preparation and Properties of Nitrosyl Azide" (in en). Journal of the American Chemical Society 80 (17): 4458–4460. doi:10.1021/ja01550a004.
- Cotton, F. Albert & Geoffrey Wilkinson (1999). Advanced Inorganic Chemistry (6th ed.). New York: John Wiley & Sons. p. 331. ISBN 0-471-19957-5.
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 | |||
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| 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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