nitric oxide

Chem.

a colorless, slightly water-soluble gas, NO, formed by the action of dilute nitric acid on copper, and by the direct combination of atmospheric oxygen and nitrogen at the high temperatures of an electric arc: an intermediate in the manufacture of nitric acid.

[1800-10]

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Colourless, toxic gas (NO), formed from nitrogen and oxygen by the action of electric sparks or high temperatures or, more conveniently, by the action of dilute nitric acid on copper or mercury.

First prepared с 1620 by Jan B. Helmont, it was first studied in 1772 by Joseph Priestley, who called it "nitrous air." An industrial procedure for the manufacture of hydroxylamine is based on the reaction of nitric oxide with hydrogen in the presence of a catalyst. The formation of nitric oxide from nitric acid and mercury is applied in a volumetric method of analysis for nitric acid or its salts. The gas is synthesized via enzyme-catalyzed reactions in humans and other animals, where it serves as a signaling molecule. Among its numerous biological roles, it causes dilation of blood vessels and as such is an important regulator of blood pressure. Nitric oxide is one of the components of air pollution generated by internal-combustion engines.

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▪ chemical compound

      colourless, toxic gas that is formed by the oxidation of nitrogen. Though it has few industrial applications, nitric oxide performs important chemical signaling functions in humans and other animals and has various applications in medicine. It is also a serious air pollutant generated by automotive engines and thermal power plants.

      Nitric oxide is formed from nitrogen and oxygen by the action of electric sparks or high temperatures or, more conveniently, by the action of dilute nitric acid upon copper or mercury. It was first prepared about 1620 by the Belgian scientist Jan Baptist van Helmont (Helmont, Jan Baptista van), and it was first studied in 1772 by the English chemist Joseph Priestley (Priestley, Joseph), who called it “nitrous air.”

      Nitric oxide liquefies at −151.8 °C (−241.2 °F) and solidifies at −163.6 °C (−262.5 °F); both the liquid and the solid are blue in colour. The gas is almost insoluble in water, but it dissolves rapidly in a slightly alkaline solution of sodium sulfite, forming the compound sodium dinitrososulfite, Na₂(NO)₂SO₃. It reacts rapidly with oxygen to form nitrogen dioxide, NO₂. Nitric oxide is a relatively unstable, diatomic molecule that possesses a free radical (i.e., an unpaired electron). The molecule can gain or lose one electron to form the ions NO⁻ or NO⁺.

      In the chemical industry, nitric oxide is an intermediate compound formed during the oxidation of ammonia to nitric acid. An industrial procedure for the manufacture of hydroxylamine is based on the reaction of nitric oxide with hydrogen in the presence of a catalyst. The formation of nitric oxide from nitric acid and mercury is applied in a volumetric method (volumetric analysis) of analysis for nitric acid or its salts.

      Though it is a toxic gas at high concentrations, nitric oxide functions as an important signaling molecule in animals. It acts as a messenger molecule, transmitting signals to cells in the cardiovascular, nervous, and immune systems. It is the only gas that is known to act as a messenger molecule within the human body. The nitric oxide molecule's possession of a free radical makes it much more reactive than other signaling molecules, and its small size enables it to diffuse through cell membranes and walls to perform a range of signaling functions in various bodily systems. The body synthesizes nitric oxide from the amino acid L-arginine by means of the enzyme nitric oxide synthase.

      The main site of the molecule's synthesis is the inner layer of blood vessels, the endothelium, though the molecule is also produced by other types of cells. From the endothelium, nitric oxide diffuses to underlying smooth muscle cells and causes them to relax. This relaxation causes the walls of blood vessels to dilate, or widen, which in turn increases blood flow through the vessels and decreases blood pressure. Nitric oxide's role in dilating blood vessels makes it an important controller of blood pressure. Nitric oxide is also produced by neurons (nerve cells) and is used by the nervous system as a neurotransmitter to regulate functions ranging from digestion to blood flow to memory and vision. In the immune system, nitric oxide is produced by macrophages, which are a type of leukocyte (white blood cell) that engulf bacteria and other foreign particles that have invaded the body. The nitric oxide released by macrophages kills bacteria, other parasites, and tumour cells by disrupting their metabolism.

      Nitric oxide's role in regulating blood flow and pressure is utilized by modern medicine in several ways. The drug nitroglycerin has been used since the late 19th century to relieve the condition known as angina pectoris, which is caused by an insufficient supply of blood to the heart muscle. Nitroglycerin was long known to achieve its therapeutic effect by dilating the coronary arteries (thereby increasing the flow of blood to the heart), but why it did so remained unknown until the late 1980s, when researchers realized that the drug serves to replenish the body's supply of nitric oxide, more of which is then available to relax, and thereby widen, the coronary blood vessels.

      Another medical use of nitric oxide is in the treatment of impotence, or erectile dysfunction, in men. Nitric oxide is essential to the achievement of an erection. During sexual stimulation, nitric oxide released within the penis relaxes the smooth muscle cells of the corpus cavernosa, making it easier for blood to flow into those spongy tissues, the expansion of which hardens and elevates the penis. The drug sildenafil citrate (trade name Viagra) treats impotence by enhancing nitric oxide's relaxant effects on smooth muscle cells in the corpus cavernosa, resulting in the increased blood flow that causes an erection.

      Nitric oxide is an important component of the air pollution generated by automotive engines and thermal power-generating plants. When a mixture of air and hydrocarbon fuel is burned in an internal-combustion engine and a power plant, the ordinarily inert nitrogen in the air combines with oxygen at very high temperatures to form nitric oxide. The nitric oxide and hydrocarbon vapours emitted by automotive exhausts and power-plant smokestacks undergo complex photochemical reactions in the lower atmosphere to form various secondary pollutants called photochemical oxidants, which make up the photochemical smog that hovers over many large cities. Nitric oxide combines with water vapour in the atmosphere to form nitric acid, which is one of the components of acid rain. Heightened levels of atmospheric nitric oxide resulting from industrial activity may also be one of the causes of the gradual depletion of the ozone layer (ozonosphere) in the upper atmosphere. Sunlight causes nitric oxide to react chemically with ozone (O₃), thereby converting the ozone to molecular oxygen (O₂).

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