PbF4, PbCl4 exist but PbBr4 and PbI4 do not exist because of

F and Cl are more oxidising in nature and can achieve Pb in (IV) O.S. but Br2 and I2 can not achieve Pb in (IV) O.S. secondly Pb4+ is strong in oxidising nature and in its presence, Br- and I- can not exist.

PbF4, PbCl4 exist but PbBr4 and PbI4 do not exist because of

F and Cl are more oxidising in nature and can achieve Pb in (IV) O.S. but Br2 and I2 can not achieve Pb in (IV) O.S. secondly Pb4+ is strong in oxidising nature and in its presence, Br- and I- can not exist.

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PbF₄, PbCl₄ exist but PbBr₄ and PbI₄ do not exist because of

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large size of Br^- and I^-

strong oxidising character of Pb⁴⁺

strong reducing character of Pb⁴⁺

low electronegativity of Br and I

answer is B.

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Detailed Solution

F and Cl are more oxidising in nature and can achieve Pb in (IV) O.S. but Br₂ and I₂ can not achieve Pb in (IV) O.S. secondly ${Pb}^{4 +}$ is strong in oxidising nature and in its presence, Br^- and I^- can not exist.

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