Question

The molecule(s) with non-zero dipole moment is/are:

• A. (N_2)
• B. (CO_2)
• C. (NO)
• D. (SO_2)

Hint:

To determine if a molecule has a non-zero dipole moment, evaluate its geometry and the symmetry of its electron distribution. Asymmetrical geometries with polar bonds often lead to non-zero dipole moments.

Answer 1

The Correct Option is C

Step 1: Understanding dipole moment. Dipole moment arises when there is an unequal distribution of electron density in a molecule, resulting in a separation of charges. A molecule with a symmetrical geometry and equal bond dipoles cancels the dipole moments, leading to a net dipole moment of zero. Conversely, an asymmetrical geometry or unequal bond dipoles results in a non-zero dipole moment.
Step 2: Analyzing the given options. - Option (A): (N_2): Nitrogen ((N_2)) is a diatomic molecule with a homonuclear bond. The electron distribution is symmetric, and there is no charge separation. Therefore, (N_2) has a dipole moment of zero. 
- Option (B): (CO_2): Carbon dioxide ((CO_2)) has a linear geometry with two bond dipoles that are equal in magnitude but opposite in direction. The dipoles cancel each other out, resulting in a net dipole moment of zero. 
- Option (C): (NO): Nitric oxide ((NO)) is a diatomic molecule with an unequal distribution of electrons due to the difference in electronegativity between nitrogen and oxygen. This asymmetry results in a non-zero dipole moment. 
- Option (D): (SO_2): Sulfur dioxide ((SO_2)) has a bent molecular geometry due to the lone pair on sulfur. The bond dipoles do not cancel out, resulting in a net dipole moment.
Step 3: Conclusion. The molecules with non-zero dipole moment are (NO) and (SO_2), corresponding to options (C) and (D).