Which one of the following complex ions has the highest magnetic moment?

[C r (N H_{3})_{6}]^{3 +}

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[F e (C N)_{6}]^{3 -}

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[F e (C N)_{6}]^{4 -}

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[Z n (N H_{3})_{6}]^{2 +}

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Solution

The correct option is A $[C r (N H_{3})_{6}]^{3 +}$
Higher the number of unpaired electrons, the higher is the magnetic moment.
In $[C r (N H_{3})_{6}]^{3 +}, C r$ is present as $C r^{3 +}$ . Thus, $C r$ in $[C r (N H_{3})_{6}]^{3 +} = [A r] 3 d^{3} 4 s^{0} 4 p^{0}$ . So, it will have 3 unpaired electrons.
In $[F e (C N)_{6}]^{3 -}$ , one unpaired electron is present and in $[F e (C N)_{6}]^{4 -}$ and $[Z n (N H_{3})_{6}]^{2 +}$ , both, unpaired electrons are absent. $C N^{-}$ is a strong field ligand, thus causes pairing.

Hence, $[C r (N H_{3})_{6}]^{3 +}$ has the highest magnetic moment among the given complex ions. $[μ = \sqrt{3 (3 + 2)} = 3.87 B M]$

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