While Ti3+,V3+,Fe3+ and Co2+ can afford a large number of tetrahedral complexes, Cr3+ can never have. What is the reason behind this?
A
Cr3+ forces high crystal field splitting with a varieties of ligands.
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B
Crystal field stabilisation energy in octrahedral vis-a-vis tetrahedral Cr3+ system plays the deciding role.
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C
The ionic radius of Cr3+ is the largest among other M3+ ions mentioned.
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D
Electronegativity of Cr3+ is the largest among these trivalent 3d-metals and so chromium prefers to be associated with a many ligands as its ionic radius permits.
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Solution
The correct option is B Crystal field stabilisation energy in octrahedral vis-a-vis tetrahedral Cr3+ system plays the deciding role. While Ti3+,V3+,Fe3+ and Co2+ afford a large number of tetrahedral complexes, Cr3+ never have. Crystal field stabilisation energy in octrahedral vis-a-vis tetrahedral, Cr3+ system plays the deciding role. Cr3+ has 3 electrons in 3d sub-shell. In octahedral field, the valence shell electronic configuration becomes t32ge0g.
CFSE=3×4Dq=12Dq.
In tetrahedral field, the outer electronic configuration becomes e2gt12g.
CFSE=2×6Dq−4Dq=8Dq.
Since, the CFSE in octahedral complexes is more, the octahedral complexes are formed for Cr3+.