|Jmol-3D images||Image 1|
|Molar mass||122.42 g/mol|
|Melting point||750 ºC decomp.|
|Solubility in water||insoluble|
|Solubility||insoluble in acid
slightly soluble in aqua regia
|EU Index||Not listed|
|Other anions||Palladium sulfide|
|Other cations||Nickel(II) oxide|
| (what is: / ?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Palladium(II) oxide is the inorganic compound of formula PdO. It is the only well characterised oxide of palladium. It is prepared by treating the metal with oxygen. Above about 900 °C, the oxide reverts to palladium metal and oxygen gas. It is not attacked by acids. As palladium is an unreactive metal, palladium oxide is difficult to produce and decomposes relatively easily.
PdO is often obtained as a poorly defined material that is generated for applications as a catalyst (see Adams catalyst). Palladium oxide is prepared by heating palladium sponge in oxygen at 350 °C.
- 2 Pd + O2 → 2 PdO
- 2 PdCl2 + 4 KNO3 → 2 PdO + 4 KCl + 2 NO2 + O2 (possible reaction)
or the product of dissolving palladium in aqua regia, followed by the addition of sodium nitrate at 600 °C. A hydrated form of the oxide (which dissolves in acid) can be prepared by precipitation from solution, for example, by hydrolysis of palladium nitrate or reaction of a soluble palladium compound with a strong base. The brown hydrated oxide converts to black anhydrous oxide on heating. Its susceptibility to attack by acids decreases at lower water content.
- Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. pp. 1336–37. ISBN 0-08-022057-6.
- Donald Starr and R. M. Hixon (1943), "Tetrahydrofuran", Org. Synth.; Coll. Vol. 2: 566
- Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1965, NY. Vol. 2. p. 1583.
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