Nitrosyl azide
{{Chembox
| ImageFile= Nitrosylazide.png
|Section1={{Chembox Identifiers
| CASNo = 62316-46-5
| PubChem = 18974641
| SMILES = [N-]=[N+]=NN=O
| StdInChI = 1S/N4O/c1-2-3-4-5
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = LHKVDVFVJMYULK-UHFFFAOYSA-N
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| ChemSpiderID = 13917998
}}
|Section2={{Chembox Properties
| Formula = {{chem2|N3\sN\dO}}
| N=4|O=1
| Appearance = Pale yellow solid below {{cvt|−50|C|F}}. Above that temperature it decomposes.
}}
|Section8={{Chembox Related
| OtherCompounds = {{ubl|Nitrogen monoxide|Nitrous oxide|Nitryl azide|Oxatetrazole}}
}}
}}
Nitrosyl azide is an inorganic compound of nitrogen and oxygen with the chemical formula {{chem2|N3\sN\dO|auto=1}}. It is a highly labile nitrogen oxide with the empirical formula {{chem2|N4O}}.
Synthesis
Nitrosyl azide can be synthesized via the following reaction of sodium azide and nitrosyl chloride at low temperatures:
Properties
Below −50 °C, nitrosyl azide exists as a pale yellow solid. Above this temperature, it decomposes into nitrous oxide {{chem2|N2O}} and molecular nitrogen {{chem2|N2}}:{{Cite journal|last1=Schulz|first1=Axel|last2=Tornieporth-Oetting|first2=Inis C.|last3=Klapötke|first3=Thomas M.|date=1993|title=Nitrosyl Azide, N4O, an Intrinsically Unstable Oxide of Nitrogen|journal=Angewandte Chemie International Edition in English |language=en|volume=32|issue=11|pages=1610–1612|doi=10.1002/anie.199316101}}
Characterization of the compound with IR and Raman spectroscopy show absorption bands that agree well with calculated values for a trans-structure.{{Cite journal|last=Lucien|first=Harold W.|date=1958|title=The Preparation and Properties of Nitrosyl Azide|journal=Journal of the American Chemical Society|language=en|volume=80|issue=17|pages=4458–4460|doi=10.1021/ja01550a004}} Quantum chemical calculations show a cis-form higher in energy by 4.2 kJ/mol and an aromatic ring form (oxatetrazole {{chem2|N4O}}) that is more stable by 205 kJ/mol. However, the cyclization to the ring form would have to surpass the 205 kJ/mol activation energy barrier to bend the azide group, which might explain why nitrosyl azide is stable enough to be isolated at low temperature.
References
- {{cite book | author = Cotton, F. Albert & Geoffrey Wilkinson | title = Advanced Inorganic Chemistry | edition = 6th | location = New York | publisher = John Wiley & Sons | date = 1999 | isbn = 0-471-19957-5 | page = 331}}
{{Azides}}