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Due to relatively weak N–O bonding, all nitrogen oxides are unstable with respect to N 2 and O 2, which is the principle behind the catalytic converter, and prevents the oxygen and nitrogen in the atmosphere from combusting.
Three candidate gasotransmitters, nitric oxide, carbon monoxide, and hydrogen sulfide, have ironically been discarded as useless toxic gases throughout history. These molecules are a classic example of dose-dependent hormesis such that low-dose is beneficial whereas absence or excessive dosing is toxic.
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]
Although most metal oxides are crystalline solids, many non-metal oxides are molecules. Examples of molecular oxides are carbon dioxide and carbon monoxide. All simple oxides of nitrogen are molecular, e.g., NO, N 2 O, NO 2 and N 2 O 4. Phosphorus pentoxide is a more complex molecular oxide with a deceptive name, the real formula being P 4 O 10.
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).
For example: H 2 N 2 O 2 + 2 H + + 2 e − ⇌ N 2 + 2 H 2 O; E 0 = +2.65 V. Oxidation reactions usually result in the formation of the nitrate ion, with nitrogen in oxidation state +5. For example, oxidation with permanganate ion can be used for quantitative analysis of nitrite (by titration): 5 NO − 2 + 2 MnO − 4 + 6 H + → 5 NO − 3 ...