Silver subfluoride
Crystal structure | |||||||
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__ F - __ Ag 1/2 + | |||||||
General | |||||||
Surname | Silver subfluoride | ||||||
other names |
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Ratio formula | Ag 2 F | ||||||
Brief description |
bronze-colored to yellow-green crystals |
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properties | |||||||
Molar mass | 234.735 g mol −1 | ||||||
Physical state |
firmly |
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Melting point |
Decomposition> 100 ° C |
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solubility |
Decomposes on contact 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 . |
Silver subfluoride (Ag 2 F) is a bronze-colored, electrically conductive solid, in which silver formally has the oxidation state +0.5.
Appearance and properties
Silver subfluoride can be produced by electrolysis of AgF on a silver cathode at low current densities or from finely divided silver with AgF in hydrogen fluoride (HF):
Ag 2 F forms bronze-colored trigonal crystals that conduct electricity well, but disintegrate into Ag and AgF above 100 ° C. The enthalpy of formation ∆H f is −212 kJ. The structure can be viewed as an anti-CdI 2 type ( polytype 2H), with Ag forming double layers in a hexagonal close packing of spheres (layer sequence ABAB). The F - ions are located in the octahedral gaps every second layer . The Ag-Ag distances at 2.996 Å are very close to the distances in metallic silver (2.89 Å), while the Ag-F distances of 2.814 Å correspond to an ionic bond.
See also
Individual evidence
- ^ NN Greenwood, A. Earnshaw. Chemistry of the elements . 1. corr. Edition. VCH, Weinheim, 1990, p. 1516, ISBN 3-527-26169-9 .
- ^ 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 , pp. 1343-1344.
- ↑ a b Lee Poyer et al .: Disilver fluoride (Silver "subfluoride") . In: Therald Moeller (Ed.): Inorganic Syntheses . tape 5 . McGraw-Hill, Inc., 1957, pp. 18-21 (English).
- ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
- ↑ G. Brauer (Ed.), Handbook of Preparative Inorganic Chemistry 2nd ed., Vol. 1, Academic Press 1963, pp. 239-240.