Plumbite: Difference between revisions
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In [[chemistry]], '''plumbite''' is the {{Chem2|PbO2(2-)}} [[oxyanion]] or hydrated forms, or any [[salt (chemistry)|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)'''. |
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The '''plumbite''' [[ion]] is Pb(OH)<sub>3</sub><sup>-</sup>, or similar. |
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For example, [[lead(II) oxide]] (PbO) dissolves in [[alkali]] to form salts containing the {{Chem2|HPbO2-}} anion (hydrogen plumbite):<ref name="arora2005">{{Cite book |title= Text Book Of Inorganic Chemistry |author= Amit Arora |publisher= Discovery Publishing House |year= 2005 |isbn= 81-8356-013-X |pages= 450–452}}</ref> |
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There are '''plumbite''' compounds, for example, [[sodium plumbite]], Na<sub>2</sub>PbO<sub>2</sub>. |
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:{{chem2|PbO + OH- → HPbO2-}} |
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[[Lead(II) hydroxide]] also dissolves in excess alkali to form the {{Chem2|[Pb(OH)6](4-)}} anion (hexahydroxyplumbate(II)):<ref name="ramsden2000">{{Cite book |title= A-level chemistry |series= A-Level Chemistry Series |author= E. N. Ramsden |edition= 4th |publisher= Nelson Thornes |year= 2000 |isbn= 0-7487-5299-4 |page= [https://archive.org/details/alevelchemistry0004rams/page/434 434] |url= https://archive.org/details/alevelchemistry0004rams/page/434}}</ref> |
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See [[:Category:Plumbites|category]] for a list. |
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:{{Chem2|Pb(OH)2 + 4 OH- → [Pb(OH)6](4-)}} |
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The plumbite ion is a weak [[reducing agent]]. When it functions as one, it is oxidized to the [[plumbate]] ion. |
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Plumbite ion may be formed by adding strong base to [[plumbous hydroxide]]. |
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==See also== |
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Plumbite ion is a weak [[reducing agent]]. |
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*[[Plumbate]] |
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*[[Lead#Chemistry|Lead]] |
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*[[Lead(II) oxide]] |
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==References== |
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{{Reflist}} |
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{{lead compounds}} |
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[[Category:Transition metal oxyanions]] |
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Latest revision as of 18:01, 2 November 2023
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−2
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
[edit]References
[edit]- ^ Amit Arora (2005). Text Book Of Inorganic Chemistry. Discovery Publishing House. pp. 450–452. ISBN 81-8356-013-X.
- ^ E. N. Ramsden (2000). A-level chemistry. A-Level Chemistry Series (4th ed.). Nelson Thornes. p. 434. ISBN 0-7487-5299-4.
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