Nitronium perchlorate

Not to be confused with Nitrosyl perchlorate.

Nitronium perchlorate

Ball-and-stick model of the unit cell.[1][2]

Names
Other names

nitronium perchlorate, nitroxyl perchlorate, nitryl perchlorate

Identifiers

CAS Number

* 17495-81-7 Y

3D model (JSmol)

* Interactive image

PubChem CID

* 139089036

InChI

* InChI=1S/ClHO4.NO2/c2-1(3,4)5;2-1-3/h(H,2,3,4,5);/q;+1/p-1

Key: YGZIDGORJKNFDL-UHFFFAOYSA-M

SMILES

* [N+](=O)=O.[O-]Cl(=O)(=O)=O

Properties

Chemical formula

| NO6Cl
Molar mass | 145.5
Appearance  | Colorless monoclinic crystals
Melting point |  135 °C (275 °F; 408 K) (decomposition)
Boiling point | decomposition

Solubility in water

| decomposes
Hazards
Main hazards | Explosive, Oxidizing Agent
Related compounds

Other anions

| Nitronium tetrafluoroborate

Other cations

| Ammonium perchlorate
Nitrosyl perchlorate
Sodium perchlorate
Potassium perchlorate

Related compounds

| Nitryl chloride

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Y verify (what is YN ?)
Infobox references

Nitronium perchlorate, NO2ClO4, also known as nitryl perchlorate and nitroxyl perchlorate, is an inorganic chemical, the salt of the perchlorate anion and the 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.

Nitronium perchlorate was investigated as an oxidizer in solid rocket propellants. Thomas N. Scortia filed for patent on such propellant in 1963,[3] however, 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.[4]

The decomposition rate of nitronium perchlorate can be altered by doping with multivalent cations.[5]

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 aerosols of their particles. Of all the perchlorates, nitronium perchlorate is the most powerful oxidizer. It can be easily detonated.[6]

## References

1. ↑ Wilson, C. J. G.; Wood, P. A.; Parsons, S. (2018). ICSD Entry: 25817. Cambridge Crystallographic Data Centre. doi:10.5517/ccdc.csd.cc2dmhvd. https://doi.org/10.5517/ccdc.csd.cc2dmhvd. Retrieved 2023-11-06.
2. ↑ Truter, M. R.; Cruickshank, D. W. J.; Jeffrey, G. A. (1960). "The crystal structure of nitronium perchlorate". Acta Crystallographica 13 (11): 855–862. doi:10.1107/S0365110X60002120. Bibcode: 1960AcCry..13..855T.
3. ↑ Thomas N. Scortia. NITRONIUM PERCHLORATE PROPELLANT COMPOSITION, USPTO patent number 3575744, filed Mar 27, 1963; issued Apr 20, 1971; assignee: United Aircraft 5 Corporation.
4. ↑ Diebold, James P. (17 April 1973). Encapsulation of Nitronium Perchlorate Employing Ammonia to Form Ammonium Perchlorate. (Patent) Department of the Navy, Washington DC. Accession Number: AD0164909.
5. ↑ NITRANIUM PERCHLORATE REACTION RATE ALTERATION. USPTO patent number 3770527.
6. ↑ Thiokol Propulsion: Rockets Basics - A Guide to Solid Propellant Rocketry . Checked 2009-06-18. Dead link 15 April 2018.

## Further reading

* Schmidt, Eckart W. (2022). "Perchlorate Oxidizers". Encyclopedia of Oxidizers. De Gruyter. pp. 3767–3776. doi:10.1515/9783110750294-028. ISBN 978-3-11-075029-4.

## External links

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Compounds containing perchlorate group

HClO4 |  |  |  | He
LiClO4 | Be(ClO4)2 | B(ClO4)−4
B(ClO4)3 | ROClO3 | N(ClO4)3
NH4ClO4
NOClO4 | O  | FClO4 | Ne
NaClO4 | Mg(ClO4)2 | Al(ClO4)3 | Si  | P  | S  | ClO−4
ClOClO3
Cl2O7 | Ar
KClO4 | Ca(ClO4)2 | Sc(ClO4)3 | Ti(ClO4)4 | VO(ClO4)3
VO2(ClO4)  | Cr(ClO4)3 | Mn(ClO4)2 | Fe(ClO4)3 | Co(ClO4)2,
Co(ClO4)3 | Ni(ClO4)2 | Cu(ClO4)2 | Zn(ClO4)2 | Ga(ClO4)3 | Ge  | As  | Se  | Br  | Kr
RbClO4 | Sr(ClO4)2 | Y(ClO4)3 | Zr(ClO4)4 | Nb(ClO5)4 | Mo  | Tc  | Ru  | Rh(ClO4)3 | Pd(ClO4)2 | AgClO4 | Cd(ClO4)2 | In(ClO4)3 | Sn(ClO4)4 | Sb  | TeO(ClO4)2 | I  | Xe
CsClO4 | Ba(ClO4)2 |  | Hf(ClO4)4 | Ta(ClO5)5 | W  | Re  | Os  | Ir  | Pt  | Au  | Hg2(ClO4)2,
Hg(ClO4)2 | Tl(ClO4)3 | Pb(ClO4)2 | Bi(ClO4)3 | Po  | At  | Rn
FrClO4 | Ra  |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
La  | Ce(ClO4)x | Pr  | Nd  | Pm  | Sm(ClO4)3 | Eu(ClO4)3 | Gd(ClO4)3 | Tb(ClO4)3 | Dy(ClO4)3 | Ho(ClO4)3 | Er(ClO4)3 | Tm(ClO4)3 | Yb(ClO4)3 | Lu(ClO4)3
Ac  | Th(ClO4)4 | Pa  | UO2(ClO4)2 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | Es  | Fm  | Md  | No  | Lr

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