Subjective Type

$$[Fe(CN)_{6}]^{4-}$$ and $$[Fe(H_{2}O)_{6}]^{2+}$$ are of different colours in dilute solutions. Why?

Solution

In both complexes, iron has +2 oxidation state with outer electronic configuration of $$\displaystyle 3d^6$$ and four unpaired electrons.
In presence of weak filed water ligand, these unpaired electrons do not pair up. However, in presence of strong field cyanide ligand, the unpaired electrons pair up and there are no unpaired electrons.
In two complexes, there is difference in the number of unpaured electrons. This gives rise to different colours.

SIMILAR QUESTIONS

Chemical Bonding

The correct molecular geometry of $$Fe\left ( CO \right )_{5}$$ is: (Z=26 for Fe)

Chemical Bonding

Cuprous ion is colourless while cupric ion is coloured because

Chemical Bonding

Atomic number of Mn, Fe, and Co are $$25, 26$$, and $$27$$ respectively. Which of the following inner orbital octahedral complex ions are diamagnetic?

Chemical Bonding

The difference in the number of unpaired electrons of a metal ion in its high-spin and low-spin octahedral complexes is two. The metal ion is :

Chemical Bonding

A solution of $$[Ni(H_{2}O)_{6}]^{2+}$$ is green but a solution of $$[Ni(CN)_{4}]^{2-}$$ is colourless, Explain.

Chemical Bonding

Atomic number of Mn, Fe, and Co are $$25, 26$$, and $$27$$ respectively. Which of the following inner orbital octahedral complex ions are diamagnetic?

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