Which substance below exhibits dipole-dipole intermolecular forces?

• A. CO2
• B. CCl4
• C. N2
• D. CH3Cl

Answer: (D)

Verified step by step guidance

1. Identify the molecular geometry and polarity of each substance listed: CO2, CCl4, N2, and CH3Cl.
2. Recall that dipole-dipole intermolecular forces occur between polar molecules, which have a permanent dipole moment due to uneven distribution of electron density.
3. Analyze CO2: It is a linear molecule with two polar C=O bonds arranged symmetrically, resulting in a nonpolar molecule overall, so it does not exhibit dipole-dipole forces.
4. Analyze CCl4: It has a tetrahedral geometry with four identical C-Cl bonds symmetrically arranged, making the molecule nonpolar and thus lacking dipole-dipole forces.
5. Analyze N2: It is a diatomic molecule with identical atoms, making it nonpolar and only subject to London dispersion forces, not dipole-dipole forces.
6. Analyze CH3Cl: It has a tetrahedral shape but with different atoms (three H and one Cl), creating an uneven charge distribution and a permanent dipole moment, so it exhibits dipole-dipole intermolecular forces.