Nitrous oxide
Structural formula | ||||||||||||||||
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General | ||||||||||||||||
Surname | Nitrous oxide | |||||||||||||||
other names |
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Molecular formula | N 2 O 5 | |||||||||||||||
Brief description |
colorless solid |
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properties | ||||||||||||||||
Molar mass | 108.01 g · mol -1 | |||||||||||||||
Physical state |
firmly |
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density |
1.64 g cm −3 |
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Melting point |
30-35 ° C |
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solubility |
reacts with water |
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safety instructions | ||||||||||||||||
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As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . |
Dinitrogen pentoxide is the anhydride of nitric acid and belongs to the group of nitrogen oxides .
presentation
Dinitrogen pentoxide can be obtained from nitric acid by dewatering with phosphorus pentoxide .
- Nitric acid reacts with diphosphorus pentoxide to form phosphoric acid and nitrous oxide .
Other possibilities for production consist in the reaction of salt-like nitrates or concentrated nitric acid with nitryl fluoride (NO 2 F) or of the latter with hydrogen fluoride or by oxidation of the NO 2, which is dimer in the gas phase as N 2 O 4, with ozone.
From 1983 onwards, technical synthesis was mostly carried out by electrolysis of nitric acid in the presence of nitrous oxide .
properties
Dinitrogen pentoxide forms colorless crystals which violently decompose with water to nitric acid.
- Dinitrogen pentoxide reacts with water to form nitric acid.
The compound is soluble in chloroform , carbon tetrachloride , trichlorofluoromethane and sulfolane , but the solutions must be cooled to at least 0 ° C. It decomposes to NO 2 and O 2 at room temperature . The half-life is about 10 days at 0 ° C and about 10 hours at 20 ° C. If heated rapidly, the decomposition is often explosive.
In the solid state, nitrous oxide has the ionic structure [NO 2 + ] [NO 3 - ] and has a hexagonal crystal structure with the space group P 6 3 / mmc (space group no. 194) . It has very strong oxidizing properties.
use
Solutions of pure nitrous oxide in organic solvents (e.g. dichloromethane or trichlorofluoromethane ) are mild nitrating agents that have found wide application.
literature
- Erwin Riedel : Inorganic Chemistry. 5th edition. De Gruyter, Berlin 2002, ISBN 3-11-017439-1 .
Individual evidence
- ↑ a b c d e f g h G. Brauer (Ed.): Handbook of Preparative Inorganic Chemistry , 2nd ed., Vol. 1, Academic Press 1963, pp. 489-490.
- ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
- ↑ a b Thomas M. Klapötke : Chemistry of high-energy materials . Walter de Gruyter, 2009, ISBN 978-3-11-021487-1 , p. 142 ( limited preview in Google Book search).
- ↑ Bruce M. McClelland, Alan D. Richardson, Kenneth Hedberg: A Reinvestigation of the Structure and Torsional Potential of N 2 O 5 by Gas-Phase Electron Diffraction Augmented by Ab Initio Theoretical Calculations . In: Helvetica Chimica Acta . tape 84 , no. 6 , 2001, p. 1612-1624 , doi : 10.1002 / 1522-2675 (20010613) 84: 6 <1612 :: AID-HLCA1612> 3.0.CO; 2-K .
- ↑ Ralf Steudel : Chemistry of Non-Metals: From Structure and Bond to Application . Walter de Gruyter, 2008, ISBN 978-3-11-021128-3 , p. 347 ( limited preview in Google Book search).
- ^ Jean d'Ans, Ellen Lax, Roger Blachnik: Pocket book for chemists and physicists . Springer DE, 1998, ISBN 3-642-58842-5 , pp. 586 ( limited preview in Google Book search).