The central atom in a molecule is in `sp^2` hybrid state. The shape of molecule will be

Options

A. Pyramidal
B. Tetrahedral
C. Octahedral
D. Trigonal planar

Explanation

To determine the shape of a molecule with a central atom in the `sp^2` hybrid state, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Hybridization**:
The question states that the central atom is in an `sp^2` hybrid state. This means that one s orbital and two p orbitals are mixed to form three equivalent hybrid orbitals.

2. **Determine the Number of Sigma Bonds**:
In an `sp^2` hybridization, the central atom can form three sigma bonds. This is because there are three hybrid orbitals available for bonding.

3. **Consider Lone Pairs**:
The shape of the molecule also depends on the presence of lone pairs on the central atom. If there are no lone pairs, the shape will be determined solely by the sigma bonds. If there are lone pairs, they will also influence the molecular geometry.

4. **Identify the Molecular Geometry**:
For a central atom with three sigma bonds and no lone pairs, the molecular geometry is trigonal planar. This is because the three bonding pairs will arrange themselves in a plane to minimize repulsion, forming a 120-degree angle between them.

5. **Conclusion**:
Therefore, if the central atom is in an `sp^2` hybrid state and has three sigma bonds with no lone pairs, the shape of the molecule will be trigonal planar.

### Final Answer:
The shape of the molecule with a central atom in `sp^2` hybrid state is **trigonal planar**.

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