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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

A

large size of `Br^(Θ)` and `I^((Θ)`

B

strong oxidising character of `Pb^(4+)`

C

strong reducing character of `Pb^(4+)`

D

low electronegativity of `Br^(Θ)` and `I^(Θ)`

Text Solution

AI Generated Solution

To explain why \( \text{PbCl}_4 \) exists while \( \text{PbBr}_4 \) and \( \text{PbI}_4 \) do not, we can break down the reasoning into several steps: ### Step-by-Step Solution: 1. **Understanding the Compounds**: - \( \text{PbCl}_4 \) is a compound where lead (Pb) is in the +4 oxidation state, bonded to four chlorine (Cl) atoms. - \( \text{PbBr}_4 \) and \( \text{PbI}_4 \) would similarly involve lead in the +4 oxidation state, bonded to bromine (Br) and iodine (I) respectively. ...
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