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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).
In atmospheric chemistry: NO x (or NOx) refers to the sum of NO and NO 2. [1] [2] NO y (or NOy) refers to the sum of NO x and all oxidized atmospheric odd-nitrogen species (e.g. the sum of NO x, HNO 3, HNO 2, etc.) NO z (or NOz) = NO y − NO x; Mixed Oxides of Nitrogen ("MON"): solutions of nitric oxide in dinitrogen tetroxide/nitrogen dioxide.
Nitrogen oxides are released during manufacturing of nitrogen fertilizers. Though nitrous oxide is emitted during its application, it is then reacted in atmosphere to form nitrogen oxides. This third source is attributed to the reaction of atmospheric nitrogen, N 2, with radicals such as C, CH, and CH 2 fragments derived from fuel, [26] rather ...
Nitrous oxide (N 2 O), better known as laughing gas, is made by thermal decomposition of molten ammonium nitrate at 250 °C. This is a redox reaction and thus nitric oxide and nitrogen are also produced as byproducts. It is mostly used as a propellant and aerating agent for sprayed canned whipped cream, and was formerly commonly used as an ...
Since nitrogen is more electronegative than carbon, metal-nitrosyl complexes tend to be more electrophilic than related metal carbonyl complexes. Nucleophiles often add to the nitrogen. [2] The nitrogen atom in bent metal nitrosyls is basic, thus can be oxidized, alkylated, and protonated, e.g.: (Ph 3 P) 2 (CO)ClOsNO + HCl → (Ph 3 P) 2 (CO ...
In general, nitric oxide is a poor nitrosant, Traube-type reactions notwithstanding. But atmospheric oxygen can oxidize nitric oxide to nitrogen dioxide, which does nitrosate. Alternatively cupric ions catalyze disproportionation into NO + and NO −. [5]
The nitrosonium ion is NO +, in which the nitrogen atom is bonded to an oxygen atom with a bond order of 3, and the overall diatomic species bears a positive charge. It can be viewed as nitric oxide with one electron removed.
The lighter isotope of nitrogen, 14 N, is preferred during denitrification, leaving the heavier nitrogen isotope, 15 N, in the residual matter. This selectivity leads to the enrichment of 14 N in the biomass compared to 15 N. [ 27 ] Moreover, the relative abundance of 14 N can be analyzed to distinguish denitrification apart from other ...