Peroxynitrite

Ion
Peroxynitrite

Chemical structure of the peroxynitrite anion
Names
IUPAC name
Oxido nitrite
Identifiers
CAS Number
  • 19059-14-4
3D model (JSmol)
  • Interactive image
ChEBI
  • CHEBI:25941
KEGG
  • C16845
PubChem CID
  • 104806
UNII
  • UR67NH4U77 checkY
CompTox Dashboard (EPA)
  • DTXSID10172540 Edit this at Wikidata
InChI
  • InChI=1S/HNO3/c2-1-4-3/h3H/p-1
    Key: CMFNMSMUKZHDEY-UHFFFAOYSA-M
  • N(=O)O[O-]
Properties
Chemical formula
 NO3−
Molar mass 62.005 g·mol−1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
Chemical compound
Reactions of peroxynitrite leading to either apoptotic or necrotic cell death

Peroxynitrite (sometimes called peroxonitrite) is an ion with the formula ONOO−. It is a structural isomer of nitrate, NO−
3

Preparation

Peroxynitrite can be prepared by the reaction of superoxide with nitric oxide:[1][2][3]

NO + O−2 → NO(O2)−

It is prepared by the reaction of hydrogen peroxide with nitrite:[4]

H2O2 + NO−
2 → ONOO− + H2O

Its presence is indicated by the absorbance at 302 nm (pH 12, ε302 = 1670 M−1 cm−1).

Reactions

Peroxynitrite is weakly basic with a pKa of ~6.8.

It is reactive toward DNA and proteins.

ONOO− reacts nucleophilically with carbon dioxide. In vivo, the concentration of carbon dioxide is about 1 mM, and its reaction with ONOO− occurs quickly. Thus, under physiological conditions, the reaction of ONOO− with carbon dioxide to form nitrosoperoxycarbonate (ONOOCO−
2) is by far the predominant pathway for ONOO−. ONOOCO−
2 homolyzes to form carbonate radical and nitrogen dioxide, again as a pair of caged radicals. Approximately 66% of the time, these two radicals recombine to form carbon dioxide and nitrate. The other 33% of the time, these two radicals escape the solvent cage and become free radicals. It is these radicals (carbonate radical and nitrogen dioxide) that are believed to cause peroxynitrite-related cellular damage.

Peroxynitrous acid

Its conjugate acid peroxynitrous acid is highly reactive, although peroxynitrite is stable in basic solutions.[5][6]

See also

References

  1. ^ Bohle, D. Scott; Sagan, Elisabeth S. (2004). "Tetramethylammonium Salts of Superoxide and Peroxynitrite". Inorganic Syntheses: 36. doi:10.1002/0471653683.ch1.
  2. ^ Pacher, P; Beckman, J. S; Liaudet, L (2007). "Nitric oxide and peroxynitrite in health and disease". Physiological Reviews. 87 (1): 315–424. doi:10.1152/physrev.00029.2006. PMC 2248324. PMID 17237348.
  3. ^ Szabó, C; Ischiropoulos, H; Radi, R (2007). "Peroxynitrite: Biochemistry, pathophysiology and development of therapeutics". Nature Reviews Drug Discovery. 6 (8): 662–80. doi:10.1038/nrd2222. PMID 17667957.
  4. ^ Beckman, J. S; Koppenol, W. H (1996). "Nitric oxide, superoxide, and peroxynitrite: The good, the bad, and ugly". American Journal of Physiology. Cell Physiology. 271 (5 Pt 1): C1424–37. doi:10.1152/ajpcell.1996.271.5.C1424. PMID 8944624.
  5. ^ Holleman, A. F.; Wiberg, E. Inorganic Chemistry Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  6. ^ Koppenol, W. H (1998). "The chemistry of peroxynitrite, a biological toxin". Química Nova. 21 (3): 326–331. doi:10.1590/S0100-40421998000300014.
  • v
  • t
  • e
Nitrogen species
Hydrides
  • NH3
  • NH4+
  • NH2−
  • N3−
  • NH2OH
  • N2H4
  • HN3
  • N3−
  • NH5 (?)
Organic
Oxides
  • NO / (NO)2
  • N2O3
  • HNO2 / NO−
    2     / NO+
  • NO2 / (NO2)2
  • N2O5
  • HNO3 / NO−
    3     / NO+
    2
  • NO3
  • HNO / (HON)2 / N2O2−
    2     / N2O
  • H2NNO2
  • HO2NO / ONOO−
  • HO2NO2 / O2NOO−
  • NO3−
    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)