The Question is from neet-chemistry coordination-compounds valence-bond-theory, and it was created by the author Mr. S M HUSSAIN

Question

Which of the following is diamagnetic in nature?

Mr. S M HUSSAIN · Accepted Answer

## CORE INFORMATION
✓ **Answer**: C
## CONCEPT FRAMEWORK
 **Primary Concept**: Diamagnetism and Paramagnetism
 **Related Topics**: Coordination complexes, Crystal field theory, Ligand field theory, Magnetic properties of complexes
 **Prerequisites**: Understanding of electronic configurations, d-orbital splitting in complexes, and the relationship between electronic configuration and magnetic properties.
## SOLUTION PATHWAY
**Given Information**:
    Four coordination complexes: ${\left[ {{m{Fe}}{{\left( {{m{CN}}} ight)}_6}} ight]^{3 - }}$, ${\left[ {{m{NiC}}{{m{l}}_4}} ight]^{2 - }}$, $\left[ {{m{Ni}}{{\left( {{m{CO}}} ight)}_4}} ight]$, ${\left[ {{m{MnC}}{{m{l}}_4}} ight]^{2 - }$
**Method & Steps**:
1. Determine the oxidation state of the central metal ion in each complex.
2. Determine the electronic configuration of the central metal ion.
3. Consider the ligand field splitting and determine the number of unpaired electrons.
4.  A complex is diamagnetic if it has no unpaired electrons; otherwise, it is paramagnetic.

* ${\left[ {{m{Fe}}{{\left( {{m{CN}}} ight)}_6}} ight]^{3 - }}$: Fe is in +3 oxidation state ($Fe^{3+}$), $d^5$ configuration. CN- is a strong field ligand, causing significant pairing of electrons.  It will likely have unpaired electrons, making it paramagnetic.
    * ${\left[ {{m{NiC}}{{m{l}}_4}} ight]^{2 - }}$: Ni is in +2 oxidation state ($Ni^{2+}$), $d^8$ configuration. Cl- is a weak field ligand, resulting in high-spin complex with unpaired electrons, making it paramagnetic.
    * $\left[ {{m{Ni}}{{\left( {{m{CO}}} ight)}_4}} ight]$: Ni is in 0 oxidation state ($Ni^{0}$), $d^{10}$ configuration. CO is a strong field ligand.  All electrons are paired, making it diamagnetic.
    * ${\left[ {{m{MnC}}{{m{l}}_4}} ight]^{2 - }}$: Mn is in +2 oxidation state ($Mn^{2+}$), $d^5$ configuration. Cl- is a weak field ligand, resulting in a high-spin complex with unpaired electrons, making it paramagnetic.

3. Identify the diamagnetic complex.
    Result: $\left[ {{m{Ni}}{{\left( {{m{CO}}} ight)}_4}} ight]$ is diamagnetic.
    Verification: The $d^{10}$ configuration with all electrons paired confirms diamagnetism.
## OPTION ANALYSIS
A :x: Paramagnetic
B :x: Paramagnetic
C ✓: Diamagnetic
D :x: Paramagnetic
## LEARNING AIDS
 **Common Mistakes**:
  1. Incorrectly assigning oxidation states: Carefully balance charges to determine the oxidation state of the central metal ion.
  2. Ignoring ligand field strength: The strength of the ligand significantly impacts the electron pairing and magnetic properties.
 **Quick Tips**:
  1. Strong field ligands (like CN-) favor low-spin complexes (more electron pairing).
  2. Weak field ligands (like Cl-) favor high-spin complexes (less electron pairing).

Mr. S M HUSSAIN · Answer

${\left[ {{\rm{Fe}}{{\left( {{\rm{CN}}} \right)}_6}} \right]^{3 - }}$

Mr. S M HUSSAIN · Answer

${\left[ {{\rm{NiC}}{{\rm{l}}_4}} \right]^{2 - }}$

Mr. S M HUSSAIN · Answer

The correct Option is "$\left[ {{\rm{Ni}}{{\left( {{\rm{CO}}} \right)}_4}} \right]$"

Mr. S M HUSSAIN · Answer

${\left[ {{\rm{MnC}}{{\rm{l}}_4}} \right]^{2 - }}$

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