Silver hyponitrite is sparingly soluble in concentrated
alkali hyponitrite solutions, but quite soluble in aqueous
ammonia due to the formation of the complex cation [(NH 3)2Ag]+.[6] The compound is slowly decomposed by light.[5]
The anhydrous compound decomposes in vacuum at 158 °C. The primary decomposition products are
silver(I) oxideAg 2O and
nitrous oxideN 2O. However, these then react to form a variable mixture of
nitrogen, metallic
silver, and various
oxides of the two elements and silver salts.[1]
^
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abcdG. David Mendenhall (1974), "Convenient synthesis of silver hyponitrite". Journal of the American Chemical society, volume 96, issue 15, page 5000.
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abMasatsugu Sekiguchi, Michio Kobayashi, Hiroshi Minato (1974), "Reactions between Acyl Halides and Silver Hyponitrite". Bulletin of the Chemical Society of Japan, volume 45, issue 9, pages 2932-2934.
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^C.N. Polydoropoulos, Th. Yannakopoulos (1961), "Silver hyponitrite: Solubility product and complexes in aqueous ammonia". Journal of Inorganic and Nuclear Chemistry, volume 19, issues 1–2, pages 107–114.
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^J. R. Partington and C. C. Shah (1932), J. Chem. Soc., page 2589.
^Ho, S. K.; de Sousa, J. B. (1961). "347. Alkoxy-radicals. Part I. The kinetics of thermal decomposition of dibenzyl hyponitrite in solution". Journal of the Chemical Society (Resumed): 1788.
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^J. B. Sousa and S. K. Ho (1960), Nature, volume 186, page 776.
^Ray, N. H. (1 January 1960). "794. The rates of decomposition of free-radical polymerisation-catalysts: measurements of short half-lives by a thermal method". Journal of the Chemical Society (Resumed): 4023–4028.
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^H. Kiefer and T. G. Traylor (1966), Tetrahedron Lett., page 6163.
^Huang, R. L.; Lee, Tong-Wai; Ong, S. H. (1 January 1969). "Reactions of the α-methoxybenzyl radical in carbon tetrachloride and in other solvents. Carbon tetrachloride as a chlorinating agent". Journal of the Chemical Society C: Organic (1): 40–44.
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^R. C. Neuman and R. J. Bussey (1970), J. Am. Chem. Soc., volume 92, page 2440.