Nitric oxide

Nitric oxide (nitrogen oxide or nitrogen monoxide[1]) is a colorless gas with the formula NO. It is one of the principal oxides of nitrogen. Nitric oxide is a free radical: it has an unpaired electron, which is sometimes denoted by a dot in its chemical formula (•N=O or •NO). Nitric oxide is also a heteronuclear diatomic molecule, a class of molecules whose study spawned early modern theories of chemical bonding.[6]

Not to be confused with nitrogen oxide or nitrous oxide.
Nitric oxide
Skeletal formula showing two lone pairs and one three-electron bond
Space-filling model of nitric oxide
Names
IUPAC name
Nitrogen monoxide[1]
Systematic IUPAC name
Oxidonitrogen(•)[2] (additive)
Other names
Nitrogen oxide
Nitrogen(II) oxide
Oxonitrogen
Identifiers
3D model (JSmol)
3DMet
ChEBI
ChEMBL
ChemSpider
DrugBank
ECHA InfoCard 100.030.233
EC Number
  • 233-271-0
Gmelin Reference
 451
IUPHAR/BPS
KEGG
RTECS number
  • QX0525000
UNII
UN number 1660
CompTox Dashboard (EPA)
  • InChI=1S/NO/c1-2 Y
    Key: MWUXSHHQAYIFBG-UHFFFAOYSA-N Y
  • InChI=1/NO/c1-2
    Key: MWUXSHHQAYIFBG-UHFFFAOYAI
  • [N]=O
Properties
NO
Molar mass 30.006 g·mol−1
Appearance Colourless gas
Density 1.3402 g/L
Melting point −164 °C (−263 °F; 109 K)
Boiling point −152 °C (−242 °F; 121 K)
0.0098 g / 100 ml (0 °C)
0.0056 g / 100 ml (20 °C)
1.0002697
Structure
Molecular shape
 linear (point group C∞v)
Thermochemistry
Std molar
entropy (S⦵298)
 210.76 J/(K·mol)
90.29 kJ/mol
Pharmacology
R07AX01 (WHO)
License data
Inhalation
Pharmacokinetics:
Bioavailability
 good
via pulmonary capillary bed
2–6 seconds
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
  • Fatal if inhaled
  • Causes severe burns
  • Causes eye damage
  • Corrosive to the respiratory tract
[3]
GHS labelling:
[4][3]
Danger
Hazard statements
 H270, H280, H314, H330[4][3]
Precautionary statements
 P220, P244, P260, P280, P303+P361+P353+P315, P304+P340+P315, P305+P351+P338+P315, P370+P376, P403, P405[4][3]
NFPA 704 (fire diamond)
Lethal dose or concentration (LD, LC):
315 ppm (rabbit, 15 min)
854 ppm (rat, 4 h)
2500 ppm (mouse, 12 min)[5]
320 ppm (mouse)[5]
Safety data sheet (SDS) External SDS
Related compounds
Related nitrogen oxides
 Dinitrogen pentoxide

Dinitrogen tetroxide
Dinitrogen trioxide
Nitrogen dioxide
Nitrous oxide
Nitroxyl (reduced form)
Hydroxylamine (hydrogenated form)

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

An important intermediate in industrial chemistry, nitric oxide forms in combustion systems and can be generated by lightning in thunderstorms. In mammals, including humans, nitric oxide is a signaling molecule in many physiological and pathological processes.[7] It was proclaimed the "Molecule of the Year" in 1992.[8] The 1998 Nobel Prize in Physiology or Medicine was awarded for discovering nitric oxide's role as a cardiovascular signalling molecule.[9]

Nitric oxide should not be confused with nitrogen dioxide (NO2), a brown gas and major air pollutant, nor with nitrous oxide (N2O), an anesthetic.[6]

Reactions

With di- and triatomic molecules

Upon condensing to a liquid, nitric oxide dimerizes to dinitrogen dioxide, but the association is weak and reversible. The N–N distance in crystalline NO is 218 pm, nearly twice the N–O distance.[6]

Since the heat of formation of •NO is endothermic, NO can be decomposed to the elements. Catalytic converters in cars exploit this reaction:

2 NO → O2 + N2

When exposed to oxygen, nitric oxide converts into nitrogen dioxide:

2 NO + O2 → 2 NO2

This reaction is thought to occur via the intermediates ONOO• and the red compound ONOONO.[10]

In water, nitric oxide reacts with oxygen to form nitrous acid (HNO2). The reaction is thought to proceed via the following stoichiometry:

4 NO + O2 + 2 H2O → 4 HNO2

Nitric oxide reacts with fluorine, chlorine, and bromine to form the nitrosyl halides, such as nitrosyl chloride:

2 NO + Cl2 → 2 NOCl

With NO2, also a radical, NO combines to form the intensely blue dinitrogen trioxide:[6]

NO + NO2 ⇌ ON−NO2

Organic chemistry

The addition of a nitric oxide moiety to another molecule is often referred to as nitrosylation. The Traube reaction[11] is the addition of a two equivalents of nitric oxide onto an enolate, giving a diazeniumdiolate (also called a nitrosohydroxylamine).[12] The product can undergo a subsequent retro-aldol reaction, giving an overall process similar to the haloform reaction. For example, nitric oxide reacts with acetone and an alkoxide to form a diazeniumdiolate on each α position, with subsequent loss of methyl acetate as a by-product:[13]

This reaction, which was discovered around 1898, remains of interest in nitric oxide prodrug research. Nitric oxide can also react directly with sodium methoxide, ultimately forming sodium formate and nitrous oxide by way of an N-methoxydiazeniumdiolate.[14]

Coordination complexes

Nitric oxide reacts with transition metals to give complexes called metal nitrosyls. The most common bonding mode of nitric oxide is the terminal linear type (M−NO).[6] Alternatively, nitric oxide can serve as a one-electron pseudohalide. In such complexes, the M−N−O group is characterized by an angle between 120° and 140°. The NO group can also bridge between metal centers through the nitrogen atom in a variety of geometries.

Production and preparation

In commercial settings, nitric oxide is produced by the oxidation of ammonia at 750–900 °C (normally at 850 °C) with platinum as catalyst in the Ostwald process:

4 NH3 + 5 O2 → 4 NO + 6 H2O

The uncatalyzed endothermic reaction of oxygen (O2) and nitrogen (N2), which is effected at high temperature (>2000 °C) by lightning has not been developed into a practical commercial synthesis (see Birkeland–Eyde process):

N2 + O2 → 2 NO

Laboratory methods

In the laboratory, nitric oxide is conveniently generated by reduction of dilute nitric acid with copper:

8 HNO3 + 3 Cu → 3 Cu(NO3)2 + 4 H2O + 2 NO

An alternative route involves the reduction of nitrous acid in the form of sodium nitrite or potassium nitrite:

2 NaNO2 + 2 NaI + 2 H2SO4 → I2 + 2 Na2SO4 + 2 H2O + 2 NO
2 NaNO2 + 2 FeSO4 + 3 H2SO4 → Fe2(SO4)3 + 2 NaHSO4 + 2 H2O + 2 NO
3 KNO2 + KNO3 + Cr2O3 → 2 K2CrO4 + 4 NO

The iron(II) sulfate route is simple and has been used in undergraduate laboratory experiments. So-called NONOate compounds are also used for nitric oxide generation.

Detection and assay
Nitric oxide (white) in conifer cells, visualized using DAF-2 DA (diaminofluorescein diacetate)

Nitric oxide concentration can be determined using a chemiluminescent reaction involving ozone.[15] A sample containing nitric oxide is mixed with a large quantity of ozone. The nitric oxide reacts with the ozone to produce oxygen and nitrogen dioxide, accompanied with emission of light (chemiluminescence):

NO + O3 → NO2 + O2 + hν

which can be measured with a photodetector. The amount of light produced is proportional to the amount of nitric oxide in the sample.

Other methods of testing include electroanalysis (amperometric approach), where ·NO reacts with an electrode to induce a current or voltage change. The detection of NO radicals in biological tissues is particularly difficult due to the short lifetime and concentration of these radicals in tissues. One of the few practical methods is spin trapping of nitric oxide with iron-dithiocarbamate complexes and subsequent detection of the mono-nitrosyl-iron complex with electron paramagnetic resonance (EPR).[16][17]

A group of fluorescent dye indicators that are also available in acetylated form for intracellular measurements exist. The most common compound is 4,5-diaminofluorescein (DAF-2).[18]

Environmental effects

Acid rain deposition

Nitric oxide reacts with the hydroperoxyl radical (HO•
2) to form nitrogen dioxide (NO2), which then can react with a hydroxyl radical (•OH) to produce nitric acid (HNO3):

•NO + HO•
2 → •NO2 + •OH
•NO2 + •OH → HNO3

Nitric acid, along with sulfuric acid, contributes to acid rain deposition.

Ozone depletion

•NO participates in ozone layer depletion. Nitric oxide reacts with stratospheric ozone to form O2 and nitrogen dioxide:

•NO + O3 → NO2 + O2

This reaction is also utilized to measure concentrations of •NO in control volumes.

Precursor to NO2

As seen in the acid deposition section, nitric oxide can transform into nitrogen dioxide (this can happen with the hydroperoxy radical, HO•
2, or diatomic oxygen, O2). Symptoms of short-term nitrogen dioxide exposure include nausea, dyspnea and headache. Long-term effects could include impaired immune and respiratory function.[19]

Biological functions

NO is a gaseous signaling molecule.[20] It is a key vertebrate biological messenger, playing a role in a variety of biological processes.[21] It is a bioproduct in almost all types of organisms, including bacteria, plants, fungi, and animal cells.[22]

Nitric oxide, an endothelium-derived relaxing factor (EDRF), is biosynthesized endogenously from L-arginine, oxygen, and NADPH by various nitric oxide synthase (NOS) enzymes.[23] Reduction of inorganic nitrate may also make nitric oxide.[24] One of the main enzymatic targets of nitric oxide is guanylyl cyclase.[25] The binding of nitric oxide to the heme region of the enzyme leads to activation, in the presence of iron.[25] Nitric oxide is highly reactive (having a lifetime of a few seconds), yet diffuses freely across membranes. These attributes make nitric oxide ideal for a transient paracrine (between adjacent cells) and autocrine (within a single cell) signaling molecule.[24] Once nitric oxide is converted to nitrates and nitrites by oxygen and water, cell signaling is deactivated.[25]

The endothelium (inner lining) of blood vessels uses nitric oxide to signal the surrounding smooth muscle to relax, resulting in vasodilation and increasing blood flow.[24] Sildenafil (Viagra) is a drug that uses the nitric oxide pathway. Sildenafil does not produce nitric oxide, but enhances the signals that are downstream of the nitric oxide pathway by protecting cyclic guanosine monophosphate (cGMP) from degradation by cGMP-specific phosphodiesterase type 5 (PDE5) in the corpus cavernosum, allowing for the signal to be enhanced, and thus vasodilation.[23] Another endogenous gaseous transmitter, hydrogen sulfide (H2S) works with NO to induce vasodilation and angiogenesis in a cooperative manner.[26][27]

Nasal breathing produces nitric oxide within the body, while oral breathing does not.[28]

Occupational safety and health

In the U.S., the Occupational Safety and Health Administration (OSHA) has set the legal limit (permissible exposure limit) for nitric oxide exposure in the workplace as 25 ppm (30 mg/m3) over an 8-hour workday. The National Institute for Occupational Safety and Health (NIOSH) has set a recommended exposure limit (REL) of 25 ppm (30 mg/m3) over an 8-hour workday. At levels of 100 ppm, nitric oxide is immediately dangerous to life and health.[29]

Explosion hazard

Liquid nitrogen oxide is very sensitive to detonation even in the absence of fuel, and can be initiated as readily as nitroglycerin. Detonation of the endothermic liquid oxide close to its b.p. (-152°C) generated a 100 kbar pulse and fragmented the test equipment. It is the simplest molecule that is capable of detonation in all three phases. The liquid oxide is sensitive and may explode during distillation, and this has been the cause of industrial accidents.[30] Gaseous nitric oxide detonates at about 2300 m/s, but as a solid it can reach a detonation velocity of 6100 m/s.[31]

References
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  4. "Nitrogen monoxide - Registration Dossier - ECHA". Retrieved 2020-11-02.
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  6. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  7. Hou, Y. C.; Janczuk, A.; Wang, P. G. (1999). "Current trends in the development of nitric oxide donors". Current Pharmaceutical Design. 5 (6): 417–441. PMID 10390607.
  8. Culotta, Elizabeth; Koshland, Daniel E. Jr. (1992). "NO news is good news". Science. 258 (5090): 1862–1864. Bibcode:1992Sci...258.1862C. doi:10.1126/science.1361684. PMID 1361684.
  9. "The Nobel Prize in Physiology or Medicine 1998". NobelPrize.org. Retrieved 2022-06-17.
  10. Galliker, Benedikt; et al. (2009). "Intermediates in the Autoxidation of Nitrogen Monoxide". Chemistry - A European Journal. 15 (25): 6161–6168. doi:10.1002/chem.200801819. ISSN 0947-6539. PMID 19437472.
  11. Not to be confused with Traube purine synthesis.
  12. Arulsamy, Navamoney; Bohle, D. Scott (2006). "Synthesis of Diazeniumdiolates from the Reactions of Nitric Oxide with Enolates". J. Org. Chem. 71 (2): 572–581. doi:10.1021/jo051998p. PMID 16408967.
  13. Traube, Wilhelm (1898). "Ueber Synthesen stickstoffhaltiger Verbindungen mit Hülfe des Stickoxyds". Justus Liebig's Annalen der Chemie (in German). 300: 81–128. doi:10.1002/jlac.18983000108.
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  17. Nagano, T; Yoshimura, T (2002). "Bioimaging of nitric oxide". Chemical Reviews. 102 (4): 1235–1270. doi:10.1021/cr010152s. PMID 11942795.
  18. Kojima H, Nakatsubo N, Kikuchi K, Kawahara S, Kirino Y, Nagoshi H, Hirata Y, Nagano T (1998). "Detection and imaging of nitric oxide with novel fluorescent indicators: diaminofluoresceins". Anal. Chem. 70 (13): 2446–2453. doi:10.1021/ac9801723. PMID 9666719.
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  20. Liu, Hongying; Weng, Lingyan; Yang, Chi (2017-03-28). "A review on nanomaterial-based electrochemical sensors for H2O2, H2S and NO inside cells or released by cells". Microchimica Acta. 184 (5): 1267–1283. doi:10.1007/s00604-017-2179-2. ISSN 0026-3672. S2CID 21308802.
  21. Weller, Richard, Could the sun be good for your heart? TedxGlasgow. Filmed March 2012, posted January 2013
  22. Roszer, T (2012) The Biology of Subcellular Nitric Oxide. ISBN 978-94-007-2818-9
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