Question

Which of the following has highest liability?with reason_________
(a)SF6
(b)[PF6]-
(c)[siF6]2+
(d)[AlF6]2-

Answer 1

what is your question

Answer 2

Answer:

$[AlF_{6}]^{2-}$

Explanation:

Given: Here we have different structures of compound which I have to arrange in order of liability.

To find: We have to determine which compound has more liability.

Concept: The ability or simplicity with which the bonds in the metal-ligand can be broken determines a complex's lability.

Thus, it is how easily the ligand can be replaced by the entering nucleophile.Following is a summary of Henry Taube's research on the features and rates of the ion exchange reaction.The ligands function as Lewis bases, and the metal atoms as Lewis acids.

Strong Lewis acids, or metals with greater charges, will interact with ligands more strongly and be more difficult to break.The CRYSTAL FIELD THEORY is the most significant factor influencing a complex's lability.

Because the second and third-row elements have much greater CFSE, it has been found that the second and third-row metals are significantly more inert than the first row metals.

Higher d orbital splitting energy is the result of substantially stronger interactions between the extensively scattered d orbitals and the ligands.

More labile than metals with the final electron in the "t2g" set are those whose valence electrons are in the "eg" set.

This is so because the "eg" set is thought to be sigma antibonding and has higher energy while being less stable.The metal ions in the complexes  are  $Al^{3+} , Si^{4+} , P^{5+}.$

Since none of the metals have "d" electrons, their splitting is almost identical. The nature of the ions is also isoelectronic.

The metals are outer orbital octahedral complexes because the ligand Fluoro is a weak field ligand and the outer d orbitals are unoccupied.

The charge of the metal ion determines how the ions interact with the metal; the higher the charge, the more powerful the interaction with the ligand.

More stability and decreased reactivity result from stronger contact.

$Al^{3+} , Si^{4+}, P^{5+}$ and the strength of the metal with the ligand are the order of the metal ion's charge and strength.

As a result, the complexes' order of lability is$[AlF_{6} ^{3-} > [SiF_{6} ^{2+} > [PF_{6}]^{-} > SF_{6}$.

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