PbCl4 exist, but PbBr4 and PbI4 do not because of

Inability of bromine and iodine to oxidise Pb 2+ to Pb 4+

More electropisitive character of Br 2 and I 2

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PbCl₄ exist, but PbBr₄ and PbI₄ do not because of

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Chlorine is a gas

Br^- and I^- are bigger in size

Inability of bromine and iodine to oxidise Pb²⁺ to Pb⁴⁺

More electropisitive character of Br₂ and I₂

answer is A.

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(1) PbBr₄ , PbI₄ is unstable compounds and can't exist in nature

Reason: Iodine, Bromine are less Electronegative hence. they can't activate (excite) the 'S' electrons present in the valence sell

(i.e Inert pair effect) and they can't oxidize the Pb⁺² to Pb⁺⁴

(2) PbF₄ , PbCl₄ are exist in nature

Reason : Fluorine , Chlorine are more Electronegative hence They can activate (excite) the 'S' electrons present in the valence sell

and oxidize the Pb⁺² to Pb⁺⁴

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