Plumbite

In chemistry, plumbite is the PbO2−
2 oxyanion or hydrated forms, or any salt containing this anion. In these salts, lead is in the oxidation state +2. It is the traditional term for the IUPAC name plumbate(II). For example, lead(II) oxide (PbO) dissolves in alkali to form salts containing the HPbO−
2 anion (hydrogen plumbite):[1]

PbO + OH−
→ HPbO−

Lead(II) hydroxide also dissolves in excess alkali to form the [Pb(OH)
6]4− anion (hexahydroxyplumbate(II)):[2]

Pb(OH)
2 \+ 4 OH−
→ [Pb(OH)
6]4−

The plumbite ion is a weak reducing agent. When it functions as one, it is oxidized to the plumbate ion.

## See also

* Plumbate
* Lead
* Lead(II) oxide

## References

1. ↑ Amit Arora (2005). Text Book Of Inorganic Chemistry. Discovery Publishing House. pp. 450–452. ISBN 81-8356-013-X.
2. ↑ E. N. Ramsden (2000). A-level chemistry. A-Level Chemistry Series (4th ed.). Nelson Thornes. p. 434. ISBN 0-7487-5299-4. https://archive.org/details/alevelchemistry0004rams/page/434.

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Lead compounds

Pb(II)|

* PbBr2
* Pb(C5H5)2
* Pb(C2H3O2)2
* PbCl2
* PbCO3
* PbCrO4
* PbF2
* PbHAsO4
* PbI2
* Pb(NO3)2
* Pb(N3)2
* PbO
* Pb(OH)2
* Pb3(PO4)2
* PbS
* Pb(SCN)2
* PbSe
* PbSO4
* PbTe
* PbTiO3
* plumbite
* PbC2 (hypothetical)

Pb(II,IV)|

* Pb3O4

Pb(IV)|

* Pb(C2H3O2)4
* PbCl4
* PbF4
* PbH4
* PbO2
* PbS2
* plumbate
* Pb(OH)4 (hypothetical)

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