Dimethyl glyoxime forms a square planar complex with `Ni^(2+)` . This complex should be `:`

Options

A. diamagnetic
B. paramagnetic having 1 unpaired electron
C. paramagnetic having 2 unpaired electrons
D. ferromagnetic

Explanation

To determine the nature of the complex formed by dimethylglyoxime (DMG) with nickel ion (Ni²⁺), we will follow these steps:

### Step 1: Identify the oxidation state of nickel
Nickel in the complex is in the +2 oxidation state (Ni²⁺).

**Hint:** Remember that the oxidation state of the metal ion is crucial for determining its electron configuration.

### Step 2: Write the electron configuration of Ni²⁺
The electron configuration of neutral nickel (Ni) is [Ar] 3d⁸ 4s². When it loses two electrons to form Ni²⁺, the configuration becomes [Ar] 3d⁸.

**Hint:** The removal of electrons occurs first from the 4s orbital before the 3d orbital.

### Step 3: Determine the nature of the ligand
Dimethylglyoxime (DMG) is a strong field ligand. Strong field ligands cause the pairing of electrons in the d-orbitals.

**Hint:** Strong field ligands are associated with low spin complexes, leading to paired electrons.

### Step 4: Analyze the d-orbital splitting
In the presence of a strong field ligand like DMG, the d-orbitals split into two sets: lower energy (t₂g) and higher energy (e_g). For Ni²⁺ with a 3d⁸ configuration, the electrons will fill the lower energy orbitals first, resulting in paired electrons.

**Hint:** Visualize the d-orbital splitting to understand how electrons are arranged in the presence of ligands.

### Step 5: Determine the hybridization
For a square planar complex, the hybridization of Ni²⁺ with DMG will be dsp². This is because the complex geometry requires the involvement of one d-orbital, one s-orbital, and two p-orbitals.

**Hint:** Remember that square planar complexes typically involve dsp² hybridization.

### Step 6: Determine if the complex is diamagnetic or paramagnetic
Since all the electrons in the 3d orbitals are paired due to the strong field ligand, the complex is diamagnetic.

**Hint:** A complex is diamagnetic if all electrons are paired; it is paramagnetic if there are unpaired electrons.

### Final Answer
The complex formed by dimethylglyoxime with Ni²⁺ is **diamagnetic**.

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