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]
References
- ↑
- ↑ 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.
- 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.
- 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.