`PbCl_(4)` exists but `PbBr_(4)` and `PbI_(4)` do not because ofA. bromine and iodine are more electronegative these chlorine.B. iodine and bromine are smaller in size.C. larger iodine and bromine are able to reduce `Pb^(4+)` to `Pb^(2+)` or `Pb`.D. the statement is incorrect

`PbCl_(4)` exists but `PbBr_(4)` and `PbI_(4)` do not because ofA. bro

1.	`PbCl_(4)` exists but `PbBr_(4)` and `PbI_(4)` do not because ofA. bromine and iodine are more electronegative these chlorine.B. iodine and bromine are smaller in size.C. larger iodine and bromine are able to reduce `Pb^(4+)` to `Pb^(2+)` or `Pb`.D. the statement is incorrect
Answer» Correct Answer - C `Pb^(4+)` has higher polarising power and `Br^(-)` and `I^(-)` being larger in size can easily give the electrons to `Pb^(4+)`, i.e. as compared to `Cl^(-),Br^(-)` and `I^(-)` are good reducing agents.

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`PbCl_(4)` exists but `PbBr_(4)` and `PbI_(4)` do not because ofA. bromine and iodine are more electronegative these chlorine.B. iodine and bromine are smaller in size.C. larger iodine and bromine are able to reduce `Pb^(4+)` to `Pb^(2+)` or `Pb`.D. the statement is incorrect

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