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Question: Which of the given complexes is most paramagnetic in nature?...

Which of the given complexes is most paramagnetic in nature?

A

[Fe(CN)6]4−[\text{Fe(CN)}_6]^{4-}

B

[Co(NH3)6]3+[\text{Co(NH}_3)_6]^{3+}

C

[Mn(H2O)6]2+[\text{Mn(H}_2\text{O)}_6]^{2+}

D

[Ni(H2O)6]2+[\text{Ni(H}_2\text{O)}_6]^{2+}

Answer

[Mn(H2O)6]2+[\text{Mn(H}_2\text{O)}_6]^{2+}

Explanation

Solution

To determine which complex is most paramagnetic, we need to find the number of unpaired electrons in each complex. Paramagnetism increases with the number of unpaired electrons.

  1. [Fe(CN)6]4−[\text{Fe(CN)}_6]^{4-}: Has 0 unpaired electrons because CN−\text{CN}^- is a strong field ligand, causing pairing.

  2. [Co(NH3)6]3+[\text{Co(NH}_3)_6]^{3+}: Has 0 unpaired electrons because NH3\text{NH}_3 is a strong field ligand for Co3+\text{Co}^{3+}, causing pairing.

  3. [Mn(H2O)6]2+[\text{Mn(H}_2\text{O)}_6]^{2+}: Has 5 unpaired electrons because H2O\text{H}_2\text{O} is a weak field ligand and Mn2+\text{Mn}^{2+} has a d5d^5 configuration.

  4. [Ni(H2O)6]2+[\text{Ni(H}_2\text{O)}_6]^{2+}: Has 2 unpaired electrons because H2O\text{H}_2\text{O} is a weak field ligand and Ni2+\text{Ni}^{2+} has a d8d^8 configuration.

Therefore, [Mn(H2O)6]2+[\text{Mn(H}_2\text{O)}_6]^{2+} is the most paramagnetic.