Question

The correct statement(s) about the octahedral Mn-complex with spin only magnetic moment of approximately 6.0 \( \mu_B \) is(are)

• A. Possible oxidation state of Mn in the complex is +4
• B. Possible oxidation state of Mn in the complex is +2
• C. Ligands associated with the complex is strong field ligand
• D. Ligands associated with the complex is weak field ligand

Hint:

The magnetic moment and electron configuration can be used to deduce the oxidation state and the field strength of ligands. A \( \mu_s \) of 6.0 \( \mu_B \) corresponds to a Mn(II) complex with weak field ligands.

Answer 1

The Correct Option is B

Step 1: Understanding spin-only magnetic moment.
The spin-only magnetic moment \( \mu_s \) is calculated using the formula: \[ \mu_s = \sqrt{n(n+2)} \, \mu_B \] where \( n \) is the number of unpaired electrons. Given that the magnetic moment is approximately 6.0 \( \mu_B \), solving for \( n \) gives approximately 4 unpaired electrons, suggesting a \( d^5 \) configuration.
Step 2: Oxidation state of Mn.
- Mn(II): The \( d^5 \) configuration corresponds to Mn(II) with 4 unpaired electrons in a weak field octahedral complex.
- Mn(IV): Would have a \( d^3 \) configuration, which would not give 4 unpaired electrons.
Step 3: Conclusion.
The possible oxidation state of Mn in this complex is +2, with weak field ligands.
Final Answer: \[ \boxed{\text{Possible oxidation state of Mn in the complex is +2.}} \]