Nitrylamide
Structural formula | ||||||||||
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General | ||||||||||
Surname | Nitrylamide | |||||||||
other names |
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Molecular formula | H 2 N 2 O 2 | |||||||||
Brief description |
white solid |
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properties | ||||||||||
Molar mass | 62.03 g mol −1 | |||||||||
Physical state |
firmly |
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Melting point |
72-75 ° C |
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safety instructions | ||||||||||
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Thermodynamic properties | ||||||||||
ΔH f 0 |
−89.5 kJ / mol |
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As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . |
Nitrylamide is an inorganic chemical compound and the simplest member of the nitramine group . It is a structural isomer to hypositrous acid .
Extraction and presentation
Nitrylamide can be obtained through a multi-stage reaction starting from potassium cyanate with ethanolic hydrochloric acid , ethyl nitrate , ammonia , potassium hydroxide and sulfuric acid, the last step being the hydrolysis of dipotassium nitrocarbamate. It was first portrayed by J. Thiele and A. Lachman at the beginning of the 20th century.
It is also possible to display it by reacting nitrous oxide with ammonia
or sodium sulfamate with nitric acid .
properties
Nitrylamide is a very decomposable solid that is in the form of shiny, white flakes. It is a very weak acid and soluble in ether, alcohol, water and acetone , sparingly soluble in benzene and hardly soluble in ligroin . It has a monoclinic crystal structure with the C 2 / c (No. 15) . It melts with partial decomposition, the solution being weakly acidic and decomposing at increasing speed into nitrous oxide and water. For example, the hydrolysis of nitramide is only catalyzed by bases but not by acids and is an example of general base catalysis. Johannes Nicolaus Brønsted formulated his acid-base concept based on investigations into the catalytic decomposition of nitramide . The compound decomposes explosively in the presence of caustic soda and on contact with concentrated sulfuric acid.
Individual evidence
- ↑ a b c d e f g Georg Brauer (Ed.), With the collaboration of Marianne Baudler u. a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume I, Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , p. 484.
- ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
- ↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. (Internet version: 2010), CRC Press / Taylor and Francis, Boca Raton, FL, Standard Thermodynamic Properties of Chemical Substances, pp. 5-13.
- ^ A b A. F. Holleman , E. Wiberg , N. Wiberg : Textbook of Inorganic Chemistry . 101st edition. Walter de Gruyter, Berlin 1995, ISBN 3-11-012641-9 , p. 721.
- ↑ a b Häussler, A .; Klapötke, TM ; Piotrowski, H .: Experimental and Theoretical Study on the Structure of Nitramide H 2 NNO 2 . In: Journal of Nature Research B . 55, 2000, pp. 151-156 ( online ).
- ↑ Walter J. Moore: Fundamentals of physical chemistry . Walter de Gruyter, 1990, ISBN 3-11-009941-1 , p. 354 ( limited preview in Google Book search).
- ↑ “The catalytic decomposition of nitramide and its physico-chemical significance,” in Zeitschrift fur physical chemistry, 108 (1924), 185–235
- ↑ Lutz Roth, Ursula Weller-Schäferbarthold: Hazardous chemical reactions. 81. Supplementary delivery, ecomed-Verlag 2017.