Among the following which is polar ? .

Options

A. `CO_(2)`
B. `SO_(2)`
C. `BeCl_(2)`
D.

Explanation

To determine which of the given molecules is polar, we need to analyze the molecular geometry and the dipole moments of each molecule. A molecule is considered polar if it has a net dipole moment that is not equal to zero.

### Step-by-Step Solution:

1. **Identify the Molecules**: We have four molecules to consider: CO2, SO2, BeCl2, and another unspecified molecule (let's assume it's also linear, like Cl2).

2. **Analyze CO2 (Carbon Dioxide)**:
- Structure: CO2 has a linear structure (O=C=O).
- Dipole Moments: The dipole moments of the two C=O bonds are equal in magnitude but opposite in direction. Therefore, they cancel each other out.
- Conclusion: The dipole moment of CO2 is zero, making it nonpolar.

3. **Analyze SO2 (Sulfur Dioxide)**:
- Structure: SO2 has a bent (angular) structure due to the presence of a lone pair on the sulfur atom.
- Dipole Moments: The dipole moments of the S=O bonds do not cancel out because of the bent shape. The molecule has a net dipole moment.
- Conclusion: The dipole moment of SO2 is not zero, making it polar.

4. **Analyze BeCl2 (Beryllium Chloride)**:
- Structure: BeCl2 has a linear structure (Cl-Be-Cl).
- Dipole Moments: Similar to CO2, the dipole moments of the two Be-Cl bonds are equal and opposite, leading to cancellation.
- Conclusion: The dipole moment of BeCl2 is zero, making it nonpolar.

5. **Analyze the Fourth Molecule (assumed to be Cl2)**:
- Structure: Cl2 is a diatomic molecule with a linear structure.
- Dipole Moments: There are no dipole moments since both atoms are identical.
- Conclusion: The dipole moment of Cl2 is zero, making it nonpolar.

### Final Conclusion:
Among the given molecules, only SO2 has a dipole moment that is not equal to zero, which makes it polar. Therefore, the correct answer is SO2.