Silver(I,III) oxide
| Silver(I,III) oxide | ||
|---|---|---|
| IUPAC name silver(I,III) oxide | ||
| Other names silver peroxide, argentic oxide, silver suboxide, divasil | ||
| Identifiers | ||
| CAS number | 1301-96-8  | |
| Properties | ||
| Molecular formula | AgO Ag2O.Ag2O3 | |
| Molar mass | 123.87 g/mol | |
| Appearance | grey-black powder diamagnetic | |
| Density | 7.48 g/cm3 | |
| Melting point | >100 °C, decomposition | |
| Solubility in water | .0027 g/100 mL | |
| Solubility | soluble in alkalis | |
(verify) (what is: / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | ||
| Infobox references | ||
Silver(I,III) oxide is the inorganic compound with the formula Ag4O4. It is a component of silver oxide-zinc alkaline batteries. It can be prepared by the slow addition of a silver(I) salt to a persulfate solution e.g. AgNO3 to a Na2S2O8 solution.[1] It adopts an unusual structure, being a mixed-valence compound.[2]
Structure
The empirical formula AgO might suggest that silver is in the +2 oxidation state, however, AgO is diamagnetic. X-ray diffraction studies show that silver atoms adopt two different coordination environments, one having two collinear oxide neighbours and the other four coplanar oxide neighbours.[1] AgO is therefore formulated as AgIAgIIIO2[3] or Ag2O·Ag2O3. It is also known as silver peroxide, although it does not have peroxide (O22−) anions, being a 1:1 molar mixture of silver(I) oxide, Ag2O, and silver(III) oxide, Ag2O3.
References
- ↑ 1.0 1.1 Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
- ↑ David Tudela "Silver(II) Oxide or Silver(I,III) Oxide?" J. Chem. Educ., 2008, volume 85, p 863. doi: 10.1021/ed085p863
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419. p. 1181.
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