A European Informational Website
learn more
|- | align="center" colspan="2" bgcolor="#ffffff" | |- | Density and phase | 1.3 × 10<sup>3</sup> kg m<sup>−3</sup> (liquid)<br>1.34 g dm<sup>−3</sup> (vapour) |- | NFPA 704 |
|- | R-phrases | , , , , |- | S-phrases | , , , |-
The chemical compound nitric oxide is a gas with chemical formula NO. It is an important signaling molecule in the body of mammals including humans, one of the few gaseous signaling molecules known. It is also a toxic air pollutant produced by automobile engines and power plants.
Nitric oxide (NO) should not be confused with nitrous oxide (N<sub>2</sub>O), a general anaesthetic, or with nitrogen dioxide (NO<sub>2</sub>) which is another poisonous air pollutant.
The nitric oxide molecule is a free radical, which is relevant to understanding its high reactivity. It reacts with the oxygen in air to form nitrogen dioxide, signalled by the appearance of the reddish-brown color.
From a thermodynamic perspective, NO is unstable with respect to O<sub>2</sub> and N<sub>2</sub>, although this conversion is very slow at ambient temperatures in the absence of a catalyst. Because the heat of formation of NO is endothermic, its synthesis from molecular nitrogen and oxygen requires elevated temperatures, >1000 °C. A major natural source is lightning. The use of internal combustion engines has drastically increased the presence of nitric oxide in the environment. One purpose of catalytic converters in cars is to minimize NO formation by catalytic reversion to O<sub>2</sub> and N<sub>2</sub>.
Nitric oxide in the air may convert to nitric acid, which has been implicated in acid rain. Furthermore, both NO and NO<sub>2</sub> participate in ozone layer depletion. Nitric oxide (NO) is a small highly diffusible gas and a ubiquitous bioactive molecule.
Although NO has relatively few direct uses, it is produced on a massive scale as an intermediate in the Ostwald process for the synthesis of nitric acid from ammonia. In 2005, the US alone produced 6M metric tonnes of nitric acid.[1] It finds use in the semiconductor industry for various processes. In one of its applications it is used along with nitrous oxide to form oxynitride gates in CMOS devices.
Nitric oxide can be used for detecting surface radicals on polymers. Quenching of surface radicals with nitric oxide results in incorporation of nitrogen, which can be quantified by means of X-ray photoelectron spectroscopy.
Nitric oxide is a key biological messenger, playing a role in a variety of biological process. Nitric oxide, known as the 'endothelium-derived relaxing factor', or 'EDRF', is biosynthesised from arginine and oxygen by various nitric oxide synthase (NOS) enzymes and by reduction of inorganic nitrate. The endothelium (inner lining) of blood vessels use nitric oxide to signal the surrounding smooth muscle to relax, thus dilating the artery and increasing blood flow. The production of nitric oxide is elevated in populations living at high-altitudes, which helps these people avoid hypoxia. Effects include blood vessel dilatation, neurotransmission, modulation of the hair cycle, and penile erections. Nitroglycerin and amyl nitrite serve as vasodilators because they are converted to nitric oxide in the body.
Nitric oxide is also generated by macrophages and neutrophils as part of the human immune response. Nitric oxide is toxic to bacteria and other human pathogens. Many bacterial pathogens have evolved mechanisms for nitric oxide resistance.[2]
Nitric oxide can contribute to reperfusion injury when excessive amount produced during reperfusion (following a period of ischemia) reacts with superoxide to produce the damaging free radical peroxynitrite. Inhaled nitric oxide has been shown to help survival and recovery from paraquat poisoning, which produces lung tissue damaging superoxide and hinders NOS metabolism.
In plants, nitric oxide can be produced by any of four routes: (i) nitric oxide synthase (as in animals), (ii) by plasma membrane-bound nitrate reductase, (iii) by mitochondrial electron transport chain, or (iv) by non-enzymatic reactions. It is a signaling molecule, acts mainly against oxidative stress and also plays a role in plant pathogen interactions. Treating cut flowers and other plants with nitric oxide has been shown to lengthen the time before wilting.[3]
A biologically important reaction of nitric oxide is S-nitrosation (or S-nitrosylation), the covalent attachment of a nitric oxide to the thiol group of cysteine within proteins. S-Nitrosylation has been described by some of its proponents as a mechanism for dynamic, post-translational regulation of most or all main classes of protein. Firm evidence to support this claim is limited.
When exposed to oxygen, NO is converted into NO<sub>2</sub>. 2NO + O<sub>2</sub> → 2NO<sub>2</sub> This conversion has been speculated as occurring via the ONOONO intermediate. In water, NO react with oxygen and water to form HNO<sub>2</sub> or nitrous acid. The reaction is thought to proceed via the following stoichiometry: 4 NO + O<sub>2</sub> + 2 H<sub>2</sub>O → 4 HNO<sub>2</sub>
NO will react with fluorine, chlorine, and bromine to from the XNO species, known as the nitrosyl halides, such as nitrosyl chloride. Nitrosyl iodide can form but is an extremely short lived species and tends to reform I<sub>2</sub>. 2NO + Cl<sub>2</sub> → 2NOCl
Nitroxyl (HNO) is the reduced form of nitric oxide.
As stated above, nitric oxide is produced industrially by the direct reaction of O<sub>2</sub> and N<sub>2</sub> at high temperatures. In the laboratory, it is conveniently generated by reduction of nitric acid: 8HNO3 + 3Cu → 3Cu(NO<sub>3</sub>)<sub>2</sub> + 4H<sub>2</sub>O + 2NO or by the reduction of nitrous acid: 2 NaNO2 + 2 NaI + 2 H<sub>2</sub>SO<sub>4</sub> → I<sub>2</sub> + 4 NaHSO4 + 2 NO 2 NaNO<sub>2</sub> + 2 FeSO<sub>4</sub> + 3 H<sub>2</sub>SO<sub>4</sub> → Fe<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub> + 2 NaHSO<sub>4</sub> + 2 H<sub>2</sub>O + 2 NO 3 KNO<sub>2</sub>(l) + KNO3 (l) + Cr<sub>2</sub>O<sub>3</sub>(s) → 2 K<sub>2</sub>CrO<sub>4</sub>(s) + 4 NO (g)
The iron(II) sulfate route is simple and has been used in undergraduate laboratory experiments.
Commercially, NO is produced by the oxidation of ammonia at 750 to 900 °C (normally at 850 °C) in the presence of platinum as catalyst: 4NH<sub>3</sub> + 5O<sub>2</sub> → 4NO + 6H<sub>2</sub>O
The uncatalyzed endothermic reaction of O2 and N2 which is performed at high temperature (>2000°C) with lightning has not been developed into a practical commercial synthesis: N<sub>2</sub> + O<sub>2</sub> → 2NO
NO forms complexes with all transition metals to give complexes called metal nitrosyls. The most common bonding mode of NO is the terminal linear type (M-NO). The angle of the M-N-O group can vary from 160-180° but are still termed as "linear". In this case the NO group is formally considered a 3-electron donor. Alternatively, one can view such complexes as derived from NO<sup>+</sup>, which is isoelectronic with CO.
Nitric oxide can serve as a one-electron pseudohalide. In such complexes, the M-N-O group is characterized by an angle between 120-140°.
The NO group can also bridge between metal centers through the nitrogen atom in a variety of geometries.
The concentration of nitric oxide can be determined using a simple chemiluminescent reaction involving ozone: 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. This reaction also produces light (chemiluminescence), which can be measured with a photodetector. The amount of light produced is proportional to the amount of nitric oxide in the sample. NO + O<sub>3</sub> → NO<sub>2</sub> + O<sub>2</sub> + light
Other methods of testing include electroanalysis, where NO reacts with an electrode to induce a current or voltage change. The detection of NO radicals in biological tissues is particulary 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). [4] [5]