Indicate the wrong statement :-

Options

A. Generally a sigma bond has free rotation along the axis
B. p-orbitals always have only sideway overlapping
C. s-orbital never form `pi`-bond
D. There can not be more than one sigma bond between two atoms

Answer

To solve the question of indicating the wrong statement regarding sigma and pi bonds, we will analyze each statement one by one.

### Step-by-step Solution:

1. **Understanding Sigma Bonds**:
- A sigma bond is formed by the head-on overlapping of atomic orbitals. This can occur between two s orbitals, an s and a p orbital, or between two p orbitals aligned along the same axis.
- **Conclusion**: Sigma bonds allow for free rotation around the bond axis.

2. **Analyzing Statement A**:
- Statement A claims that "generally, sigma bond has free rotation along the axis."
- This statement is correct because sigma bonds do allow for rotation due to their head-on overlapping nature.

3. **Analyzing Statement B**:
- Statement B states that "p orbitals have only sideways overlapping."
- This statement is incorrect. While p orbitals can form pi bonds through sideways overlapping, they can also form sigma bonds through head-on overlapping (e.g., p_x with p_x).
- **Conclusion**: This is the wrong statement.

4. **Analyzing Statement C**:
- Statement C claims that "s orbitals never form pi bonds."
- This statement is correct. S orbitals can only form sigma bonds due to their spherical symmetry and cannot overlap sideways to form pi bonds.

5. **Analyzing Statement D**:
- Statement D states that "there cannot be more than one sigma bond between two atoms."
- This statement is also correct. When two atoms bond, they can form one sigma bond and possibly multiple pi bonds, but only one sigma bond can exist between any two atoms.

6. **Final Conclusion**:
- After analyzing all statements, the only incorrect statement is **Statement B**: "p orbitals have only sideways overlapping."

### Final Answer:
The wrong statement is **B**: p orbitals have only sideways overlapping.