Chlorine nitrate, with chemical formula ClONO2 is an important atmospheric gas present in the stratosphere. It is an important sink of reactive chlorine and nitrogen, and thus its formation and destruction play an important role in the depletion of ozone.[2]

Chemical properties

It explosively reacts with metals, metal chlorides, alcohols, ethers, and most organic materials. When it is heated to decomposition, it emits toxic fumes of Cl2 and NOx.[citation needed]

Synthesis and reactions

It can be produced by the reaction of dichlorine monoxide and dinitrogen pentoxide at 0 °C:[3]

Cl2O + N2O5 → 2 ClONO2

or by the reaction:[4]

ClF + HNO3 → HF + ClONO2

It can also react with alkenes:

(CH3)2C=CH2 + ClONO2 → O2NOC(CH3)2CH2Cl

Chlorine nitrate reacts with metal chlorides:[5]

4 ClONO2 + TiCl4 → Ti(NO3)4 + 4 Cl2

References

  1. ^ Obermeyer, Axel; Borrmann, Horst; Simon, Arndt (August 1995). "Crystal Structures and Bonding in NOCl, NO2Cl, and NO3Cl". Journal of the American Chemical Society. 117 (30): 7887–7890. doi:10.1021/ja00135a006.
  2. ^ von Clarmann, Thomas; Johansson, Sören (2018). "Chlorine nitrate in the atmosphere". Atmos. Chem. Phys. 18 (20): 15363–15386. Bibcode:2018ACP....1815363V. doi:10.5194/acp-18-15363-2018.
  3. ^ Schmeisser, M.; Ruff, J. K. & Lustig, M. Chlorine(1) Nitrate Inorganic Syntheses, Wiley-Blackwell, https://doi.org/10.1002/9780470132401.ch34, 1967, 127-130
  4. ^ Schack, Carl J. (1967-10-01). "New synthesis of chlorine nitrate". Inorganic Chemistry. 6 (10): 1938–1939. doi:10.1021/ic50056a047. ISSN 0020-1669.
  5. ^ 张青莲 (1991). 《无机化学丛书》第六卷：卤素、铜分族、锌分族. 北京: 科学出版社. pp. P338-341. ISBN 7-03-002238-6.