Азот оксидінің сипаттамасы

Colorless gas with the formula NO

a molecule of one nitrogen atom and one oxygen atom
Chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 477001381
| Name =
| ImageFile = Nitric oxide 2D. svg
| ImageFile Ref =
| ImageSize = 121
| ImageName = Skeletal formula of nitric oxide with bond length
| ImageFileL1 = Nitric oxide. svg
| ImageNameL1 = Skeletal formula showing two lone pairs and one three electron bond
| ImageFileR1 = Nitric oxide 3D vdW. png
| ImageFileR1 Ref =
| ImageNameR1 = Space filling model of nitric oxide
| IUPACName = Nitrogen monoxide (additive)
| OtherNames = Nitrogen oxideNitrogen(II) oxideOxonitrogenNitrogen monoxide
| Section1 =
| Section2 =
| Section3 =
| Section4 =
| Section5 =
| Section6 =
| Section7 = Chembox Hazards
| ExternalSDS = External SDS
| MainHazards =
| GHSPictograms =
| LCLo = 320 ppm (mouse)) is a colorless gas with the formula 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. It was proclaimed the "Molecule of the Year" in 1992. The 1998 Nobel Prize in Physiology or Medicine was awarded for discovering nitric oxide's role as a cardiovascular signalling molecule. Nitric oxide should not be confused with nitrogen dioxide (NO2), a brown gas and major air pollutant, or with nitrous oxide (N2O), an anesthetic gas. The first two orbitals are actually pure atomic 1sO and 1sN from oxygen and nitrogen respectively and therefore are usually not noted in the united atom notation. Orbitals noted with an asterisk are antibonding. The ordering of 5σ and 1π according to their binding energies is subject to discussion. Removal of a 1π electron leads to 6 states whose energies span over a range starting at a lower level than a 5σ electron an extending to a higher level. This is due to the different orbital momentum couplings between a 1π and a 2π electron. The lone electron in the 2π orbital makes NO a doublet (X ²Π) in its ground state whose degeneracy is split in the fine structure from spin orbit coupling with a total momentum J=3/2 or J=1/2.

The dipole of NO has been measured experimentally to 0.15740 D and is oriented from O to N (⁻NO⁺) due to the transfer of negative electronic charge from oxygen to nitrogen.

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). 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.

As seen in the acid deposition section, nitric oxide can transform into nitrogen dioxide (this can happen with the hydroperoxy radical, HO2•, 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.

NO is a gaseous signaling molecule. It is a key vertebrate biological messenger, playing a role in a variety of biological processes. It is a bioproduct in almost all types of organisms, including bacteria, plants, fungi, and animal cells. Nitric oxide, an endothelium derived relaxing factor (EDRF), is biosynthesized endogenously from L arginine, oxygen, and NADPH by various nitric oxide synthase (NOS) enzymes. Reduction of inorganic nitrate may also make nitric oxide. The binding of nitric oxide to the heme region of the enzyme leads to activation, in the presence of iron. Once nitric oxide is converted to nitrates and nitrites by oxygen and water, cell signaling is deactivated. Nasal breathing produces nitric oxide within the body, while oral breathing does not.

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.

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. Gaseous nitric oxide detonates at about 2300 m/s, but as a solid it can reach a detonation velocity of 6100 m/s.