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Peroxynitrate
Identifiers

CAS Number	125239-87-4^N[EPA]
3D model (JSmol)	Interactive image
ChEBI	CHEBI:29270
ChemSpider	4574117
PubChem CID	5460620
CompTox Dashboard (EPA)	DTXSID301032974
InChI InChI=1S/HNO4/c2-1(3)5-4/h4H/p-1 Key: UUZZMWZGAZGXSF-UHFFFAOYSA-M
SMILES [N+](=O)([O-])O[O-]
Properties
Chemical formula	NO₄⁻
Molar mass	78.004 g·mol⁻¹
Related compounds
Related compounds	peroxycarbonate; peroxysulfate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

Peroxynitrate (or peroxonitrate) refers to salts of the unstable peroxynitric acid, HNO₄. Peroxynitrate is unstable and decomposes to nitrate and dioxygen.^[1]

No solid peroxynitrate salts are known.^[2] However, there is a report that the chemist Sebastian Moiseevich Tanatar produced sodium peroxynitrate octahydrate (NaNO₃·H₂O₂·8H₂O) by evaporating a solution of sodium nitrate and hydrogen peroxide until crystallisation begins and then mixing with alcohol to form crystals of the octahydrate.^[3]

References

^ Miyamoto, Sayuri; Ronsein, Graziella E.; Corrêa, Thaís C.; Martinez, Glaucia R.; Medeiros, Marisa H. G.; Di Mascio, Paolo (2009). "Direct evidence of singlet molecular oxygen generation from peroxynitrate, a decomposition product of peroxynitrite". Dalton Transactions (29): 5720–5729. doi:10.1039/b905560f. ISSN 1477-9226. PMID 20449086.
^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
^ Mellor, Joseph William (1922). A Comprehensive Treatise on Inorganic and Theoretical Chemistry, Volume 2. New York: Longmans, Green and Co. p. 816.

v t e Nitrogen species
Hydrides	NH₃ NH+4 NH−2 N³⁻ NH₂OH N₂H₄ HN₃ N−3 NH₅ (?)
Organic	NR₃ >C=NR −CONR₂ −CN HCN CN⁻ (CN)₂ H₂NCN HOCN HNCO HNCS CH₂N₂ −NO −NO₂
Oxides	NO / (NO)₂ N₂O₃ HNO₂ / NO−2 / NO⁺ NO₂ / (NO₂)₂ N₂O₅ HNO₃ / NO−3 / NO+2 NO₃ HNO / (HON)₂ / N₂O−2 / N₂O H₂NNO₂ HO₂NO / ONOO⁻ HO₂NO₂ / O₂NOO⁻ NO−4 H₄N₂O₄ / N₂O2−3
Halides	NF NF₂ NF₃ NF₅ (?) NCl₃ NBr₃ NI₃ FN₃ ClN₃ BrN₃ IN₃ NH₂F N₂F₂ NH₂Cl NHF₂ NHCl₂ NHBr₂ NHI₂
Oxidation states	−3, −2, −1, 0, +1, +2, +3, +4, +5 (a strongly acidic oxide)

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