Which of the following does not exist ?

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SiCl62–

SiF62–

GeF62–

PbF62–

answer is A.

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Detailed Solution

→ Si+4 is smaller size cation and hence it can't accomadate the six larger size Cl¯ ion,→ Interaction between lone pair of chloride and Si+4 is not strongHence the "[SiCl6]-2" can't exist in nature [SiF6]-2, [GeF6]-2, [PbF6]-2 Can exist in nature due to the presence of empty d-orbitals in their valency shell [PbBr6]-2 ,[PbI6]-2 can't exist in natureReason:Due to low electronegativity of Br, I ; they can't activate the inert pair electrons hence can't from [PbBr6]-2 and [PbI6]-2Where as [PbF6]-2 can exist in natureBecause of high electronegativity of fluorine, it can activate the inert pair electrons and form [PbF6]-2

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