Which of the following statement is/are false for $[{TiCl}_{4}] and {[{FeCl}_{4}]}^{-}$ ?

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Square planar and tetrahedral respectively and both are paramagnetic.

Solutions of both complexes are colored.

Both tetrahedral and diamagnetic.

Both tetrahedral but the former is diamagnetic and the latter is paramagnetic.

answer is A, C, D.

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Detailed Solution

TiCl₂ is paramagnetic, whereas TiO₂ is diamagnetic, because TiCl₄ has 54 electrons and unpaired electrons, making it paramagnetic in nature. TiO₂ is diamagnetic because there are no unpaired electrons.

Because Fe³⁺ ions have five unpaired electrons when the Cl^- ligand arrives, the five unpaired electrons are rearranged, and one electron remains unpaired.

The correct answer is a, c, and d.

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