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Nitronium perchlorate: Difference between revisions

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{{Distinguish|Nitrosyl perchlorate}}
{{chembox
| Watchedfields = changed
| verifiedrevid = 428779915
| ImageFileL1ImageFile = Nitronium-perchlorate-unit-cell-3D-ballsbs-17.png
| ImageCaption = [[Ball-and-stick model]] of the [[unit cell]].<ref name="ICSD_25817">{{ cite journal | url = https://doi.org/10.5517/ccdc.csd.cc2dmhvd | title = ICSD Entry: 25817 | website = [[Cambridge Structural Database]]: Access Structures | year = 2018 | publisher = [[Cambridge Crystallographic Data Centre]] | access-date = 2023-11-06 }}</ref><ref>{{ cite journal | first1 = M. R. | last1 = Truter | first2 = D. W. J. | last2 = Cruickshank | first3 = G. A. | last3 = Jeffrey | title = The crystal structure of nitronium perchlorate | journal = [[Acta Crystallographica|Acta Crystallogr.]] | year = 1960 | volume = 13 | pages = 855–862 | doi = 10.1039/D2CE01616H | doi-access = free | hdl = 20.500.11820/e81bbc4f-a6d1-4e16-a288-6eb9ff626485 | hdl-access = free }}</ref>
| ImageNameL1 = Ball-and-stick model of the nitronium cation
| ImageFileR1 = Perchlorate-3D-balls.png
| ImageNameR1 = Ball-and-stick model of the perchlorate anion
| OtherNames = nitronium perchlorate, nitroxyl perchlorate, nitryl perchlorate
|Section1={{Chembox Identifiers
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| MeltingPt_notes = (decomposition)
| BoilingPt = decomposition
| Appearance = Colorless monoclinic crystals
| Solubility = decomposes
}}
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'''Nitronium perchlorate''', NO<sub>2</sub>ClO<sub>4</sub>, also known as '''nitryl perchlorate''' and '''nitroxyl perchlorate''', is an [[inorganic chemical]], the [[Salt (chemistry)|salt]] of the [[perchlorate]] anion and the [[nitronium ion|nitronium]] cation. It forms colorless [[monoclinic]] crystals. It is [[hygroscopic]], and is a strong [[oxidizing]] and [[nitrating]] agent. It may become [[hypergolic]] in contact with organic materials. <!-- Encyclopedia of explosives and related items, vol. 8, 1978 -->
 
Nitronium perchlorate was investigated as an [[oxidizer]] in [[solid rocket propellant]]s. [[Thomas N. Scortia]] filed for patent on such propellant in 1963.,<ref>Thomas N. Scortia. [httphttps://wwwpatents.google.com/patents?id=eoh1AAAAEBAJpatent/US3575744 NITRONIUM PERCHLORATE PROPELLANT COMPOSITION], USPTO patent number 3575744, filed Mar 27, 1963; issued Apr 20, 1971; assignee: United Aircraft 5 Corporation.</ref> Howeverhowever, its reactivity and incompatibility with many materials hindered such use. Coating of nitronium perchlorate particles with [[ammonium nitrate]], prepared in situ by passing of dry [[ammonia]] gas over the particles, was investigated, and a patent was awarded.<ref>Diebold, James P. (17 April 1973). [https://web.archive.org/web/20110717061845/http://oai.dtic.mil/oai/oai?verb=getRecord&metadataPrefix=html&identifier=AD0164909 Encapsulation of Nitronium Perchlorate Employing Ammonia to Form Ammonium Perchlorate.] (Patent) Department of the Navy, Washington DC. Accession Number: AD0164909.</ref>
 
DecompositionThe decomposition rate of nitronium perchlorate can be altered by doping with [[Polyvalency (chemistry)|multivalent]] cations.<ref>[http://www.freepatentsonline.com/3770527.html NITRANIUM PERCHLORATE REACTION RATE ALTERATION]. USPTO patent number 3770527.</ref>
 
Nitronium perchlorate and ammonium perchlorate do not produce smoke when stoichiometrically burned with non-metallic fuels. Potassium perchlorate and other metal perchlorates generate smoke, as the metal chlorides are solid materials creating [[Aerosol|aerosols]] of their particles. Of all the perchlorates, nitronium perchlorate is the most powerful oxidizer. It can be easily [[detonation|detonated]], however.<ref>[http://rocketsciencebooks.home.att.net/basics.html Thiokol Propulsion: Rockets Basics - A Guide to Solid Propellant Rocketry]. Checked 2009-06-18. Dead link 15 April 2018.</ref>
 
==References==
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