is `[Nicl_4]^(2-)` having tetrahedral shape

Explanation

To determine whether the complex ion \([NiCl_4]^{2-}\) has a tetrahedral shape, we can follow these steps:

### Step 1: Identify the oxidation state of Nickel
Nickel (Ni) in the complex \([NiCl_4]^{2-}\) is in the +2 oxidation state. This is because each chloride ion (Cl) has a -1 charge, and there are four chloride ions contributing a total charge of -4. To balance this to achieve the overall charge of -2 for the complex, Nickel must be +2.

**Hint:** Remember that the overall charge of the complex is the sum of the charges of the central metal ion and the ligands.

### Step 2: Determine the electronic configuration of Ni²⁺
The electronic configuration of neutral Nickel (Ni) is \([Ar] 3d^8 4s^2\). When Nickel loses two electrons to become Ni²⁺, the configuration becomes \([Ar] 3d^8\).

**Hint:** Pay attention to how electrons are removed from the orbitals; typically, the 4s electrons are removed before the 3d electrons.

### Step 3: Analyze the coordination number and geometry
In \([NiCl_4]^{2-}\), Nickel is coordinated to four chloride ions (Cl⁻). The coordination number is 4, which can lead to either a tetrahedral or square planar geometry depending on the d-electron count and hybridization.

**Hint:** Coordination number indicates how many ligands surround the central metal ion, which influences the geometry.

### Step 4: Determine the hybridization
For a coordination number of 4, if the metal ion has a d⁸ configuration, it typically adopts a tetrahedral geometry when the ligands are weak field ligands like Cl⁻. In this case, the hybridization involves one s and three p orbitals, leading to sp³ hybridization.

**Hint:** Consider the nature of the ligands; strong field ligands tend to lead to square planar geometries, while weak field ligands can lead to tetrahedral geometries.

### Step 5: Conclusion on the shape
Since \([NiCl_4]^{2-}\) has a coordination number of 4 and is composed of weak field ligands (Cl⁻), it adopts a tetrahedral shape due to sp³ hybridization.

**Final Answer:** Yes, \([NiCl_4]^{2-}\) has a tetrahedral shape.