A molecule is square planar with no lone pair. What type of hybridisation is associated with it?

Options

A. `sp^(3)d`
B. `sp^(3)d^(2)`
C. `dsp^(3)`
D. `dsp^(2)`

Explanation

To determine the type of hybridization associated with a square planar molecule that has no lone pairs, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Molecular Geometry**:
- The question states that the molecule is square planar. This geometry typically involves a central atom surrounded by four bonded atoms arranged at the corners of a square.

2. **Count the Bond Pairs**:
- In a square planar molecule, there are four bond pairs and no lone pairs on the central atom.

3. **Determine the Hybridization**:
- For a square planar geometry, we need to consider the electron pair geometry. The presence of four bond pairs suggests that we have a total of five orbitals involved in hybridization (one s orbital and three p orbitals from the central atom, along with one d orbital).
- The hybridization that corresponds to a square planar arrangement is typically denoted as dsp². This means:
- One d orbital, one s orbital, and two p orbitals combine to form four equivalent hybrid orbitals.

4. **Conclusion**:
- Therefore, the type of hybridization associated with a square planar molecule with no lone pairs is **dsp²**.

### Final Answer:
The hybridization associated with a square planar molecule with no lone pairs is **dsp²**.