Why pbx2 is more stable than pbx4
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Answered by
115
in pbx2 , oxidation state of pb =+2
and pbx4 , oxidation state of pb =+4
we know ,
oxidation state of +2 is more stable than +4 . due to inert pair effect .
this is due to poor screening effect of d and f electrons that restrict ns electron to take part in the bond formation .
so, PbX2 is more stable than PbX4
and pbx4 , oxidation state of pb =+4
we know ,
oxidation state of +2 is more stable than +4 . due to inert pair effect .
this is due to poor screening effect of d and f electrons that restrict ns electron to take part in the bond formation .
so, PbX2 is more stable than PbX4
Answered by
39
The oxidation state of Pb in Pbx2 is +2 and oxidation state of Pb in Pbx4 is +4.
As we know Lead belongs to group 14 (carbon family) , where elements exhibit a unique property of variable valency due to inert pair effect. This inert pair effect is due to the shielding of s electrons by intervening d and f electrons. Hence number of electrons in d and f orbital increases as we go down in a group, thus by making inert pair effect more prominent and so
+4 oxidation state becomes less stable.
Hence ,
pbx2 is more stable than pbx4
As we know Lead belongs to group 14 (carbon family) , where elements exhibit a unique property of variable valency due to inert pair effect. This inert pair effect is due to the shielding of s electrons by intervening d and f electrons. Hence number of electrons in d and f orbital increases as we go down in a group, thus by making inert pair effect more prominent and so
+4 oxidation state becomes less stable.
Hence ,
pbx2 is more stable than pbx4
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