`[Fe(CN)_6]^(4-)` and `[Fe(H_2O)_6]^(2+)` are of different colours in solutions. Why?

[Fe(CN)_6)]^(4-) and [Fe(H_2O)_6)]^(2+) are of different colours in dilute solutions. Why ?

[Sc(H_2O_6)_6]^(3+) and [Ti(H_2O)_6]^(3+) ions are coloured why ?

True of False : Both [Fe(CN)_6]^(4-) and [FeF_6]^(3-) are outer orbital complexes.

Consider the following complex ions, P, Q and R. P = [FeF_6]^(3-), Q = [V(H_2O)_6]^(2+) and R = [Fe(H_2O)_6]^(2+) . The correct order of the complex ions, according to their spin-only magnetic moment values (in B.M.) is

Explain [Fe(H_2O)_6]^(3+) is paramagnetic.

Iron forms a many complexes in its +2 and +3 oxidation states such as [Fe(H_2O)_6]^(2+) (A), [Fe(CN)_6]^(4-) (B), [Fe(H_2O)_6]^(3+) (C), [Fe(CN)_6]^(3-)(D) , etc. They exhibit different magnetic properties and undergo different hybridisation of iron. Which of the following statements is wrong ?

Explain magnetic Behaviour of [Fe(CN)_6]^(4-) and [Fe(CN)_6]^(3-) anions.

K_4[Fe(CN)_6] is a

[Ti (H_2O)_6]^(3+) is coloured while [Sc(H_2O)_6]^(3+) is colourless. Explain.