The magnetic moment (in `mu_B`) of [Ni(dimethylglyxoimate)`""_2`] complex is closest to:

Options

A. `5 :37`
B. `0.00`
C. `1.73`
D. `2.25`

Explanation

To determine the magnetic moment of the [Ni(dimethylglyoximate)₂] complex, we will follow these steps:

### Step 1: Identify the oxidation state of nickel in the complex.
Nickel typically has an oxidation state of +2 in coordination complexes, especially when coordinated with strong field ligands like dimethylglyoximate.

**Hint:** The oxidation state can often be inferred from the charge of the complex and the ligands involved.

### Step 2: Determine the electronic configuration of Ni²⁺.
Nickel (Ni) has an atomic number of 28, and its electronic configuration is:
- Ni: [Ar] 3d⁸ 4s²

For Ni²⁺, we remove two electrons from the 4s orbital:
- Ni²⁺: [Ar] 3d⁸ 4s⁰

**Hint:** Remember that when forming cations, electrons are removed from the outermost shell first.

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

**Hint:** Strong field ligands tend to lead to low-spin complexes, which means that electrons will pair up rather than remain unpaired.

### Step 4: Determine the electron configuration in the presence of the ligand.
In the presence of the strong field ligand DMG, the 3d electrons will pair up:
- For 3d⁸, the configuration will be: ↑↓ ↑↓ ↑↓ ↑↓ ↑ (total of 8 electrons, all paired)

**Hint:** Visualize the d-orbitals and how electrons fill them according to Hund's rule and the Pauli exclusion principle.

### Step 5: Count the number of unpaired electrons.
Since all 8 electrons in the 3d orbitals are paired, there are no unpaired electrons in the complex.

**Hint:** Unpaired electrons are crucial for determining magnetic properties.

### Step 6: Calculate the magnetic moment.
The formula for calculating the magnetic moment (μ) is:
\[ \mu = \sqrt{n(n + 2)} \]
where \( n \) is the number of unpaired electrons.

In this case, since \( n = 0 \):
\[ \mu = \sqrt{0(0 + 2)} = \sqrt{0} = 0 \]

**Hint:** The magnetic moment is directly related to the number of unpaired electrons.

### Conclusion:
The magnetic moment of the [Ni(dimethylglyoximate)₂] complex is 0 Bohr magnetons (μ_B).

**Final Answer:** The closest value for the magnetic moment of the complex is **0.00** (Option B).