The structure of NOClO4 has not been elucidated by X-ray crystallography. However, the Raman spectroscopy of NOClO4 suggests that nitrosyl perchlorate consists of distinct NO+ and ClO4– ions.[4]
Properties
Nitrosyl perchlorate decomposes at 100 °C to nitronium perchlorate, which then subsequently decomposes into chlorine and nitrogen oxides.[5][6]
This compound hydrolyzes in water to form nitrous acid and perchloric acid:[5]
Nitrosyl perchlorate is used in the laboratory as a perchlorating agent.[7][8] Although it has been investigated as a potential rocket propellant, it has not been commercialized.[1]
^ abK. A. Hofmann; Graf Armin Zedtwitz (1909). "Nitrosyl-perchlorat: das Anhydrid der salpetrigen Säure mit der Überchlorsäure" [Nitrosyl perchlorate: the anhydride of nitrous acid with perchloric acid]. Berichte der deutschen chemischen Gesellschaft (in German). 42 (2): 2031–2034. doi:10.1002/cber.19090420285.
^M. Schmeisser (1963). "Nitrosyl perchlorate". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=320. NY,NY: Academic Press.
^William Rogie Angus; Alan H. Leckie (1935). "Investigations of raman spectra II—The raman spectra of perchloric acid and nitrosyl perchlorate". Proceedings of the Royal Society of London. Series A - Mathematical and Physical Sciences. 150 (871): 615–618. doi:10.1098/rspa.1935.0125.
^Thomas J. Wierenga; J. Ivan Legg (1982). "Synthesis and characterization of cobalt(III) nicotinic acid complexes". Inorganic Chemistry. 21 (7): 2881–2885. doi:10.1021/ic00137a071.
^M.M. Markowitz; J.E. Ricci; R.J. Goldman; P.F. Winternitz (1960). "A new method for the conversion of inorganic salts to the corresponding perchlorates". Journal of Inorganic and Nuclear Chemistry. 16 (1–2): 159–161. doi:10.1016/0022-1902(60)80104-2.