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PbCl4 exists , but PbBr4 and Pbl4 do no...

` PbCl_4` exists , but `PbBr_4` and `Pbl_4` do not exist because of

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`Pb^(4+)` is an oxidizing agent and readily changes into `Pb^(2+)` The Br’ and I ions are reducing agents. The redox reaction occurs indicating that `PbBr_(4)` and `Pbl_(4)` are unstable compounds
`Pb^(4+)+4BrtoPbBr_(2)Br_(2)`
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