What is the Oxidation Number of Pb in Pb(O)2?

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The oxidation number of lead (Pb) in Pb(O)2 is +4, while oxygen (O) has an oxidation number of -2, as PbO2 is not a peroxide. The confusion arises from the incorrect classification of PbO2 as a peroxide, which would imply O has an oxidation number of -1. In contrast, BaO2 is a true peroxide where O is -1 and Ba is +2. The discussion clarifies that PbO2 should be treated with standard oxidation rules, leading to the conclusion that Pb's oxidation state is +4. Understanding the correct nomenclature is essential to avoid such misunderstandings.
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Homework Statement


The problem is:

Find the oxidation number of each element in the compound: Pb(O)2

I said oxidation number of Pb = x, O = -1 since this is a peroxide, therefore oxidation number of Pb is plus 2. However, the solution manual says O is -2 and thus Pb is 2.

But elsewhere, for the problem BaO2, they say the oxidation number of O is -1 and Ba is +2.

I'm confused.

Homework Equations

The Attempt at a Solution

 
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PbO2 is not a peroxide.
 
Not clear whether it is the manual or you who is saying Pb in PbO2 is +2 but now hopefully not.

I have a vague recollection that lead dioxide did sometimes get improperly and misleadingly called "lead peroxide",
probably before chemical nomenclature was formalised and the name still hangs around.
 
Borek is 100% right, it ain't a peroxide ... Hint: Oxy = -2, Calculate oxidation state of Pb.
 
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