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Is pb2o4 basic oxide or amphoteric oxide?
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Luka Babic
Is pb2o4 basic oxide or amphoteric oxide?
I am not sure about your 1st question but can sure give you a method to identify I'd an oxide is acidic or basic. Check the oxidation number of the central atom. Higher the oxidation number more acidic oxide it is. For ex. P2O5 is more acidic than P2O3 where the oxidation states are +5 and +3 respectively.
I am not sure about your 1st question but can sure give you a method to identify I'd an oxide is acidic or basic. Check the oxidation number of the central atom. Higher the oxidation number more acidic oxide it is. For ex. P2O5 is more acidic than P2O3 where the oxidation states are +5 and +3 respectively.
If, as I suspect, you are referring to a mixed valence oxide[1], in the case of Pb this could very well be Pb₃O₄. This oxide can actually be considered as a mixture of Pb(II) and Pb(IV).
Pb₃O₄ is a typical amphoteric oxide, in that it reacts with either acids or bases: in the first case, it forms Pb(II) compounds and PbO₂ (with oxidising acids such as HNO₃) or Pb(II) compounds (with non-oxidising acids such as HCl); in the second case, Pb₃O₄ dissolves in alkali to form plumbates (II) and (IV): if the alkali is, say, NaOH, such plumbates will be [Pb(OH)₃]¯ and [Pb(OH)₆]²¯.
If, as I suspect, you are referring to a mixed valence oxide[1], in the case of Pb this could very well be Pb₃O₄. This oxide can actually be considered as a mixture of Pb(II) and Pb(IV).
Pb₃O₄ is a typical amphoteric oxide, in that it reacts with either acids or bases: in the first case, it forms Pb(II) compounds and PbO₂ (with oxidising acids such as HNO₃) or Pb(II) compounds (with non-oxidising acids such as HCl); in the second case, Pb₃O₄ dissolves in alkali to form plumbates (II) and (IV): if the alkali is, say, NaOH, such plumbates will be [Pb(OH)₃]¯ and [Pb(OH)₆]²¯.
“pb2O4”??? Do you mean lead(IV) oxide, PbO2? PbO2 is an amphoteric oxide which has both the properties of an acid and a base.
With a base or a basic oxide it will form the metal hydroxyplumbate or the metal orthoplumbate. With an acid, lead(IV) is reduced to lead(II) to produce a salt.
“pb2O4”??? Do you mean lead(IV) oxide, PbO2? PbO2 is an amphoteric oxide which has both the properties of an acid and a base.
With a base or a basic oxide it will form the metal hydroxyplumbate or the metal orthoplumbate. With an acid, lead(IV) is reduced to lead(II) to produce a salt.
I am not sure about your 1st question but can sure give you a method to identify I'd an oxide is acidic or basic. Check the oxidation number of the central atom. Higher the oxidation number more acidic oxide it is. For ex. P2O5 is more acidic than P2O3 where the oxidation states are +5 and +3 respectively.
I am not sure about your 1st question but can sure give you a method to identify I'd an oxide is acidic or basic. Check the oxidation number of the central atom. Higher the oxidation number more acidic oxide it is. For ex. P2O5 is more acidic than P2O3 where the oxidation states are +5 and +3 respectively.
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Let us say, the oxide has the formula MxOy, where M is the metal; It should react with acids and give compounds in which the cation is formed by M;
It should also react with alkalies in which the anion has M as one of the components;
eg Boron trichloride - derived from reaction with HCl;
Sodium metaborate - derived from reaction with NaOH.
Let us say, the oxide has the formula MxOy, where M is the metal; It should react with acids and give compounds in which the cation is formed by M;
It should also react with alkalies in which the anion has M as one of the components;
eg Boron trichloride - derived from reaction with HCl;
Sodium metaborate - derived from reaction with NaOH.
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Uhm…”Pb₂O₄” is unknown, as far as I know.
The commonest oxides of lead are
If, as I suspect, you are referring to a mixed valence oxide[1], in the case of Pb this could very well be Pb₃O₄. This oxide can actually be considered as a mixture of Pb(II) and Pb(IV).
Pb₃O₄ is a typical amphoteric oxide, in that it reacts with either acids or bases: in the first case, it forms Pb(II) compounds and PbO₂ (with oxidising acids such as HNO₃) or Pb(II) compounds (with non-oxidising acids such as HCl); in the second case, Pb₃O₄ dissolves in alkali to form plumbates (II) and (IV): if the alkali is, say, NaOH, such plumbates will be [Pb(OH)₃]¯ and [Pb(OH)₆]²¯.
Footnotes
[1] Category:Mixed valence compounds - WikipediaUhm…”Pb₂O₄” is unknown, as far as I know.
The commonest oxides of lead are
If, as I suspect, you are referring to a mixed valence oxide[1], in the case of Pb this could very well be Pb₃O₄. This oxide can actually be considered as a mixture of Pb(II) and Pb(IV).
Pb₃O₄ is a typical amphoteric oxide, in that it reacts with either acids or bases: in the first case, it forms Pb(II) compounds and PbO₂ (with oxidising acids such as HNO₃) or Pb(II) compounds (with non-oxidising acids such as HCl); in the second case, Pb₃O₄ dissolves in alkali to form plumbates (II) and (IV): if the alkali is, say, NaOH, such plumbates will be [Pb(OH)₃]¯ and [Pb(OH)₆]²¯.
Footnotes
[1] Category:Mixed valence compounds - WikipediaMore
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Metals that can react with both acid and base. Example - Sb, Zn, As, Sn, Pb, Al
These could be remembered by SAB Jan ki aas suno prabhu allah
Metals that can react with both acid and base. Example - Sb, Zn, As, Sn, Pb, Al
These could be remembered by SAB Jan ki aas suno prabhu allah
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“pb2O4”??? Do you mean lead(IV) oxide, PbO2? PbO2 is an amphoteric oxide which has both the properties of an acid and a base.
With a base or a basic oxide it will form the metal hydroxyplumbate or the metal orthoplumbate. With an acid, lead(IV) is reduced to lead(II) to produce a salt.
A quick look at Wikipedia, indicates ….
“pb2O4”??? Do you mean lead(IV) oxide, PbO2? PbO2 is an amphoteric oxide which has both the properties of an acid and a base.
With a base or a basic oxide it will form the metal hydroxyplumbate or the metal orthoplumbate. With an acid, lead(IV) is reduced to lead(II) to produce a salt.
A quick look at Wikipedia, indicates ….
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