`Ni^(+2)` ion can be estimated by using dimethyl glyoxime and forms a cherry-red precipitate. The complex is stablized by:

Options

A. Ioinc bonds
B. Coordinate covalent bonds
C. Dative `pi`-bonds
D. Hydrogenn bonds

Answer

To determine how the cherry-red precipitate formed by the reaction of Ni²⁺ ions with dimethylglyoxime (DMG) is stabilized, we can analyze the nature of the bonding involved in the complex.

### Step-by-Step Solution:

1. **Understanding Dimethylglyoxime (DMG)**:
- Dimethylglyoxime is a bidentate ligand, meaning it can attach to a metal ion at two sites. It has two nitrogen atoms that can donate lone pairs to the metal ion.

2. **Formation of the Complex**:
- When Ni²⁺ ions react with dimethylglyoxime, the nitrogen atoms from DMG coordinate to the nickel ion. Each DMG molecule donates two lone pairs of electrons to the nickel ion, forming coordinate covalent bonds.

3. **Electronic Configuration of Nickel**:
- The electronic configuration of Ni²⁺ (nickel in the +2 oxidation state) is [Ar] 3d⁸. The presence of DMG allows nickel to achieve a more stable electronic configuration through coordination.

4. **Stabilization of the Complex**:
- The complex is stabilized by the formation of multiple chelate rings. Each DMG molecule can form a ring with the nickel ion, and the more rings that are formed, the more stable the complex becomes.

5. **Role of Hydrogen Bonds**:
- In addition to coordinate covalent bonds, hydrogen bonds can also play a role in stabilizing the complex. The oxygen atom in one DMG can form a hydrogen bond with a hydrogen atom from another DMG molecule, further stabilizing the structure.

6. **Conclusion**:
- The stabilization of the Ni²⁺-DMG complex is primarily due to coordination covalent bonds formed by the donation of lone pairs from the nitrogen atoms of DMG and the additional stabilization provided by hydrogen bonds between DMG molecules.

### Final Answer:
The complex is stabilized by **coordination covalent bonds** and **hydrogen bonds**.