BETA SAÚDE
Dinitrogen dioxide
Texto da Wikipédia (en), licença CC BY-SA. O BETARUBI mostra o verbete inteiro nesta página — a leitura não continua fora do site.
 | |
| Identifiers | |
|---|---|
| |
3D model (JSmol) |
|
| ChEBI |
|
| ChemSpider | |
| 1035 | |
PubChem CID |
|
| UNII | |
| |
| |
| Properties | |
| N2O2 | |
| Molar mass | 60.012 g·mol−1 |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Dinitrogen dioxide is an inorganic compound having molecular formula N
2O
2. Many structural isomers are possible. The covalent bonding pattern O=N–N=O (a non-cyclic dimer of nitric oxide (NO)) is predicted to be the most stable isomer based on ab initio calculations and is the only one that has been experimentally produced.[1] In the solid form, the molecules have C2v symmetry: the entire structure is planar, with the two oxygen atoms cis across the N–N bond. The O–N distance is 1.15 Å, the N–N distance is 2.33 Å, and the O=N–N angle is 95°.[2]
It is an intermediate in the high-pressure disproportionation of nitric oxide:[3][4]
- 2NO ⇌ N2O2
- N2O + NO2"}},"i":0}}]}' id="mwLg"/>N2O2 + NO → N2O + NO2
References
- ↑ Nguyen, Kiet A.; Gordon, Mark S.; Montgomery, John A. Jr.; Michels, H. Harvey (October 1994). "Structures, Bonding, and Energetics of N2O2 Isomers". The Journal of Physical Chemistry. 98 (40): 10072–10078. doi:10.1021/j100091a021.
- ↑ 2</sub>"},"journal":{"wt":"Bulletin of the Korean Chemical Society"},"date":{"wt":"1999"},"volume":{"wt":"20"},"issue":{"wt":"12"},"pages":{"wt":"1399–1408"},"url":{"wt":"http://www.koreascience.or.kr/article/JAKO199913464470127.page"},"language":{"wt":"ko"},"issn":{"wt":"0253-2964"}},"i":0}}]}' id="mwRQ"/>Park, Jong Keun; Sun, Hosung (1999). "Theoretical Determination of Geometrical Structures of the Nitric Oxide Dimer, (NO)2". Bulletin of the Korean Chemical Society (in Korean). 20 (12): 1399–1408. ISSN 0253-2964.
- ↑ Agnew, Stephan F.; Swanson, B. I.; Jones, L. H.; Mills, R. L. (April 1985). "Disproportionation of Nitric Oxide at High Pressure". The Journal of Physical Chemistry. 89 (9): 1678–1682. doi:10.1021/j100255a026.
- ↑ Tsukahara, Hirokazu; Ishida, Takanobu; Todoroki, Yukiko; Hiraoka, Masahiro; Mayumi, Mitsufumi (January 2003). "Gas-phase Disproportionation of Nitric Oxide at Elevated Pressures". Free Radical Research. 37 (2): 171–177. doi:10.1080/1071576021000036489.
- 2</sub>"},"first":{"wt":"Allan L. L."},"last":{"wt":"East"},"journal":{"wt":"Journal of Chemical Physics"},"volume":{"wt":"109"},"issue":{"wt":"6"},"date":{"wt":"August 8, 1998"},"pages":{"wt":"2185–2193"},"doi":{"wt":"10.1063/1.476786"},"doi-access":{"wt":"free"},"bibcode":{"wt":"1998JChPh.109.2185E"}},"i":0}}]}' id="mwZg"/>East, Allan L. L. (August 8, 1998). "The 16 valence electronic states of nitric oxide dimer (NO)2". Journal of Chemical Physics. 109 (6): 2185–2193. Bibcode:1998JChPh.109.2185E. doi:10.1063/1.476786.
- 2</sub>O<sub>2</sub>: an ab initio valence bond study"},"first":{"wt":"Richard D."},"last":{"wt":"Harcourt"},"journal":{"wt":"Journal of Molecular Structure: THEOCHEM"},"volume":{"wt":"206"},"issue":{"wt":"3–4"},"date":{"wt":"April 1990"},"pages":{"wt":"253–264"},"doi":{"wt":"10.1016/0166-1280(90)85140-I"}},"i":0}}]}' id="mwaQ"/>Harcourt, Richard D. (April 1990). "The origin of the long N–N bond in N2O2: an ab initio valence bond study". Journal of Molecular Structure: THEOCHEM. 206 (3–4): 253–264. doi:10.1016/0166-1280(90)85140-I.
- Dkhissi, Ahmed; Soulard, Pascale; Perrin, Agnès; Lacome, Nelly (May 1997). "The NO Dimer". Journal of Molecular Spectroscopy. 183 (1): 12–17. Bibcode:1997JMoSp.183...12D. doi:10.1006/jmsp.1996.7249.