Nitroxyl

Nitroxyl (common name) or azanone (IUPAC name)[1] is the chemical compound HNO. It is well known in the gas phase.[2][3] Nitroxyl can be formed as a short-lived intermediate in the solution phase. The conjugate base, NO⁻, nitroxide anion, is the reduced form of nitric oxide (NO) and is isoelectronic with dioxygen. The bond dissociation energy of H–NO is 49.5 kcal/mol, which is unusually weak for a bond to the hydrogen atom.

Nitroxyl

Names
IUPAC name Azanone
Systematic IUPAC name Oxidanimine
Other names Hydrogen oxonitrate(I) Nitronous oxide Nitrosyl hydride Hyponitrous acid monomer
Identifiers
CAS Number	14332-28-6^Y
3D model (JSmol)	Interactive image
ChEMBL	ChEMBL1200689^Y
ChemSpider	920^Y
MeSH	Nitroxyl
PubChem CID	945
UNII	GFQ4MMS07W^Y
InChI InChI=1S/HNO/c1-2/h1H^Y Key: ODUCDPQEXGNKDN-UHFFFAOYSA-N^Y
SMILES N=O
Properties
Chemical formula	HNO
Molar mass	31.014 g·mol^−1
log P	0.74
Structure
Coordination geometry	Digonal
Molecular shape	Dihedral
Thermochemistry
Heat capacity (C)	33.88 J K^−1 mol^−1
Std molar entropy (S^o298)	220.91 J K^−1 mol^−1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Generation

Nitroxyl is produced from the reagents Angeli's salt (Na₂N₂O₃) and Piloty's acid (PhSO₂NHOH).[4] Other notable studies on the production of HNO exploit cycloadducts of acyl nitroso species, which are known to decompose via hydrolysis to HNO and acyl acid. Upon photolysis these compounds release the acyl nitroso species which then further decompose.[5] HNO is generated via organic oxidation of cyclohexanone oxime with lead tetraacetate to form 1-nitrosocyclohexyl acetate:[6]

This compound can be hydrolyzed under basic conditions in a phosphate buffer to HNO, acetic acid, and cyclohexanone.

Dichloramine reacts with hydroxyl ion, which can be present in water or comes from water, to yield nitroxyl radical and the chloride ion.[7]

Reactions

Nitroxyl is a weak acid, with pK_a of about 11, the conjugate base being the triplet state of NO⁻. Nitroxyl itself, however, is a singlet ground state. Thus, deprotonation of nitroxyl uniquely involves the forbidden spin crossing from the singlet state starting material to triplet state product (¹HNO + B^– → ³NO^– +BH. Due to the spin-forbidden nature of deprotonation, proton abstraction is many orders of magnitude slower (k = 4.9 × 10⁴ M⁻¹⋅s⁻¹ for deprotonation by OH^–) than what one would expect for a heteroatom proton-transfer process (processes that are so fast that they are sometimes diffusion-controlled).

The K_a of starting from or ending with the electronic excited states has also been determined. When process of deprotonating singlet state HNO to obtain singlet state NO^– has a pK_a is about 23. On the other hand, when deprotonating triplet HNO to obtain triplet NO^–, the pK_a is about –1.8. [8][9]

Nitroxyl rapidly decomposes by a bimolecular pathway to nitrous oxide (k at 298 K = 8×10⁶ M s):[8]

2 HNO → N₂O + H₂O

The reaction proceeds via dimerization to hyponitrous acid, H₂N₂O₂, which subsequently undergoes dehydration. Therefore, HNO is generally prepared in situ as described above.

Nitroxyl is very reactive towards nucleophiles, including thiols. The initial adduct rearranges to a sulfinamide:[9]

HNO + RSH → RS(O)NH₂

Detection

In biological samples, nitroxyl can be detected using fluorescent sensors, many of which are based on the reduction of Cu(II) to Cu(I) with concomitant increase in fluorescence.[10]

Medicinal chemistry

Nitroxyl donors, known as nitroso compounds, show potential in the treatment of heart failure and ongoing research is focused on finding new molecules for this task.

See also

• Nitroxyl radicals (also called aminoxyl radicals) — chemical species containing the R₂N–O^• functional group

References

1. Doctorovich, F.; Bikiel, D.; Pellegrino, J.; Suárez, S. A.; Larsen, A.; Martí, M. A. (2011). "Nitroxyl (azanone) trapping by metalloporphyrins". Coordination Chemistry Reviews. 255 (23–24): 2764–2784. doi:10.1016/j.ccr.2011.04.012.
2. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
3. Wiberg, Egon; Holleman, Arnold Frederick (2001). Inorganic Chemistry. Elsevier. ISBN 978-0-12-352651-9.
4. Nagasawa, H. T.; Kawle, S. P.; Elberling, J. A.; DeMaster, E. G.; Fukuto, J. M. (1995). "Prodrugs of Nitroxyl as Potential Aldehyde Dehydrogenase Inhibitors vis-a-vis Vascular Smooth Muscle Relaxants". J. Med. Chem. 38 (11): 1865–1871. doi:10.1021/jm00011a005. PMID 7783118.
5. Cohen, A. D.; Zeng, B.-B.; King, S. B.; Toscano, J. P. (2003). "Direct observation of an acyl nitroso species in solution by time-resolved IR spectrocopy". J. Am. Chem. Soc. 125 (6): 1444–1445. doi:10.1021/ja028978e. PMID 12568581.
6. Sha, Xin; Isbell, T. Scott; Patel, Rakesh P.; Day, Cynthia S.; King, S. Bruce (2006). "Hydrolysis of Acyloxy Nitroso Compounds Yields Nitroxyl (HNO)". J. Am. Chem. Soc. 128 (30): 9687–9692. doi:10.1021/ja062365a. PMID 16866522.
7. White, George Clifford (1986). The handbook of chlorination (2nd ed.). New York: Van Nostrand Reinhold. p. 169. ISBN 978-0-442-29285-0.
8. Shafirovich, V.; Lymar, S. V. (2002). "Nitroxyl and its anion in aqueous solutions: Spin states, protic equilibria, and reactivities toward oxygen and nitric oxide". Proceedings of the National Academy of Sciences of the United States of America. 99, 7340 (11): 7340–7345. doi:10.1073/pnas.112202099. PMC 124232. PMID 12032284.CS1 maint: uses authors parameter (link)
9. Bianco, C. L.; Toscano, J. P.; Bartberger, M. D.; Fukuto, J. M. (2017). "The chemical biology of HNO signaling". Archives of Biochemistry and Biophysics. 617: 129–136. doi:10.1016/j.abb.2016.08.014. PMC 5318259. PMID 27555493.CS1 maint: uses authors parameter (link)
10. Rivera-Fuentes, Pablo; Lippard, Stephen J. (2015). "Metal-Based Optical Probes for Live Cell Imaging of Nitroxyl (HNO)". Acc. Chem. Res. 38 (11): 2427–2434. doi:10.1021/acs.accounts.5b00388. hdl:1721.1/107934. PMID 26550842.