Nitrosonium
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| Names | |
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Systematic IUPAC name
Oxidonitrogen(1+)
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| Other names
Nitrosonium
Iminooxidanium |
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| Identifiers | |
| 14452-93-8 | |
| 3D model (Jmol) | Interactive image |
| Abbreviations | NO(+) |
| ChEBI | CHEBI:29120 |
| ChemSpider | 76569 |
| 456 | |
| PubChem | 84878 |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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| Infobox references | |
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. This ion is usually obtained as the following salts: NOClO4, NOSO4H (nitrosylsulfuric acid, more descriptively written ONSO3OH), and NOBF4. The ClO−
4 and BF−
4 salts are slightly soluble in CH3CN. NOBF4 can be purified by sublimation at 200–250 °C and 0.01 mmHg (1.3 Pa).
NO+ is isoelectronic with CO, CN− and N2. It arises via protonation of nitrous acid:
NO+ reacts readily with water to form nitrous acid:
For this reason, NOBF4 must be protected from water or even moist air. With base, the reaction generates nitrite:
NO+ reacts with aryl amines, ArNH2, to give diazonium salts, ArN+
2. The resulting diazonium group is easily displaced (unlike the amino group) by a variety of nucleophiles.
NO+, e.g. as NOBF4, is a strong oxidizing agent:
NOBF4 is a convenient oxidant because the byproduct NO is a gas, which can be swept from the reaction using a stream of N2. Upon contact with air, NO forms NO2, which can cause secondary reactions if it is not removed. NO2 is readily detectable by its characteristic orange color.
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