A) \[{{[Fe{{(CN)}_{6}}]}^{3-}}\]
B) \[{{[Co{{(ox)}_{3}}]}^{3-}}\]
C) \[{{\left[ Fe{{F}_{6}} \right]}^{3-}}\]
D) \[{{[Co{{F}_{6}}]}^{3-}}\]
Correct Answer: B
Solution :
[b] \[{{[Fe{{(CN)}_{6}}]}^{3-}}\] has magnetic moment of a single unpaired electron whereas \[{{[Fe{{F}_{6}}]}^{3-}}\]has a magnetic moment of five unpaired electrons. \[{{[Co{{F}_{6}}]}^{3-}}\] is paramagnetic with four unpaired electrons while \[{{[Co{{({{C}_{2}}{{O}_{4}})}_{3}}]}^{3}}\] is diamagnetic. This anomaly is explained by valence bond theory in terms of formation of inner and outer orbital coordination entities. \[{{[Co{{({{C}_{2}}{{O}_{4}})}_{3}}]}^{3-}}\] is an inner orbital complexes having \[{{d}^{2}}s{{p}^{3}}\] hybridization.
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