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Liquid nitrogen (N 2 at below −196 °C) is a colorless, odorless and nonflammable liquid that is used for cooling, freezing and preservation. Learn about the history, production, physical and chemical properties, and applications of liquid nitrogen from this comprehensive Wikipedia article.
Nitrogen is a chemical element that can form many compounds with different oxidation states and structures. Learn about dinitrogen complexes, nitrides, azides, nitrido complexes, and other nitrogen compounds with examples and properties.
Liquid nitrogen is nitrogen in a liquid state at low temperature, produced by fractional distillation of liquid air. It is widely used as a coolant, in cryotherapy, food preparation, astronomy and other applications, but also requires thermal insulation and careful handling due to its low boiling point and expansion ratio.
Learn how to draw Lewis structures, also called Lewis dot formulas, to show the bonding and lone pairs of electrons in molecules and ions. Find methods, examples, exceptions, and a table for calculating bonds and lone pairs.
Phosphorus mononitride is an inorganic compound with the formula PN, a binary nitride of phosphorus and nitrogen. It is highly unstable and reactive, and has been detected in the interstellar medium and in some comets.
Nitrogen dioxide is a reddish-brown gas with the formula NO2. It is a paramagnetic, bent molecule with C2v point group symmetry and a free radical. It is poisonous, an intermediate in nitric acid production, and an atmospheric pollutant.
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).
A carbon–nitrogen bond is a covalent bond between carbon and nitrogen and is one of the most abundant bonds in organic chemistry and biochemistry. [ 1 ] Nitrogen has five valence electrons and in simple amines it is trivalent , with the two remaining electrons forming a lone pair .
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