Palladium(II) oxide: Difference between revisions

| verifiedrevid = 402517651

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| OtherNames = Palladium monoxide

| Section1 = {{Chembox Identifiers

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| CASNo_Ref = {{cascite|correct|CAS}}

| Section2 = {{Chembox Properties

| Formula = PdO

| MolarMass = 122.42 g/mol

| Appearance = greenish-black powder

| Density = 8.3 g/cm³

| Solubility = insoluble

| SolubleOther = insoluble in [[acid]] <br> slightly soluble in [[aqua regia]]

| MeltingPt = 750 ºC decomp.

| BoilingPt =

| Section7 = {{Chembox Hazards

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| EUIndex = Not listed

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| FlashPt = Non-flammable

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| Section8 = {{Chembox Related

| OtherAnions = [[Palladium sulfide]]

| OtherCations = [[Nickel(II) oxide]]

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| Function =

| OtherCpds =

'''Palladium(II) oxide''' is the [[inorganic compound]] of formula [[Palladium|Pd]][[Oxygen|O]]. It is the only well characterised oxide of palladium.<ref name = "Greenwood">{{Greenwood&Earnshaw1st|pages=1336–37}}</ref> It is prepared by treating the metal with oxygen. Above about 900&nbsp;°C, the oxide reverts to Pd metal. It is not attacked by acids.<ref name = "Greenwood" /> As palladium is an unreactive metal, palladium oxide is difficult to produce and decomposes relatively easily.

<!--==Structure==

Probably sq planar with bent O, like PtS motif-->

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

The oxide is obtained as a black powder. The oxide also may be prepared specially for catalytic use by heating variously a mixture of [[palladium(II) chloride]] and [[potassium nitrate]],

: 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.<ref name=OS>{{OrgSynth | title = Tetrahydrofuran | author = Donald Starr and R. M. Hixon | prep = cv2p0566 | collvol = 2 | collvolpages = 566 | year = 1943}}</ref><ref>Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1965, NY. Vol. 2. p. 1583.</ref> 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.

The hydrated oxide (hydroxide), PdO^.''n''H₂O can be produced as a dark-yellow precipitate by adding alkali to a solution of [[palladium nitrate]], Pd(NO₃)₂.<ref name = "Greenwood"/>

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[[cs:Oxid palladnatý]]

[[de:Palladium(II)-oxid]]

[[nl:Palladium(II)oxide]]

[[pt:Óxido de paládio (II)]]

[[zh:氧化钯]]