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 and Ni²⁺, we can follow these steps:

### Step 1: Identify the Coordination Complex
Dimethylglyoxime (DMG) is a bidentate ligand that coordinates with Ni²⁺ to form a complex. The formula for the complex can be written as Ni(DMG)₂, indicating that two dimethylglyoxime molecules coordinate with one nickel ion.

**Hint:** Remember that bidentate ligands can attach to the metal ion at two different sites.

### Step 2: Determine the Hybridization
Nickel in the +2 oxidation state has the electronic configuration of Argon (Ar) 3d⁸. When forming a square planar complex, the hybridization involved is dsp². This hybridization occurs because the Ni²⁺ ion uses one s orbital, one p orbital, and two d orbitals to form four equivalent hybrid orbitals.

**Hint:** Square planar complexes typically involve dsp² hybridization, which is common for d⁸ metal ions.

### Step 3: Analyze the Electron Configuration
In the case of Ni²⁺ (3d⁸), the filling of the d orbitals occurs as follows:
1. The 3d orbitals fill according to Hund's rule and the Pauli exclusion principle.
2. In the presence of a strong field ligand like dimethylglyoxime, the electrons in the 3d orbitals pair up, leading to a fully filled set of orbitals.

**Hint:** Strong field ligands cause pairing of electrons, which is crucial for determining the magnetic properties of the complex.

### Step 4: Determine the Magnetic Properties
Since all the d electrons in the Ni²⁺ ion are paired in the square planar complex formed with dimethylglyoxime, the complex will have no unpaired electrons. Therefore, it is diamagnetic.

**Hint:** A complex is diamagnetic if all electrons are paired, which can be checked by looking at the electron configuration.

### Conclusion
The complex formed by dimethylglyoxime with Ni²⁺ is diamagnetic in nature.

### Final Answer
The complex should be **diamagnetic**.