Which of the following molecules will exhibit dipole-dipole forces between like molecules?

• A. CCl4
• B. CH3Cl
• C. N2
• D. CO2

Answer: (B)

Verified step by step guidance

1. Identify the molecular geometry and polarity of each molecule. Dipole-dipole forces occur between polar molecules, so we need to determine which molecules are polar.
2. For CCl\_4 (carbon tetrachloride), note that it has a tetrahedral geometry with four identical C-Cl bonds symmetrically arranged. This symmetry causes the bond dipoles to cancel out, making CCl\_4 nonpolar.
3. For CH\_3Cl (chloromethane), the molecule has a tetrahedral shape but with three C-H bonds and one C-Cl bond. Since chlorine is more electronegative than hydrogen and carbon, the C-Cl bond creates a net dipole moment, making CH\_3Cl polar.
4. For N\_2 (nitrogen gas), it is a diatomic molecule with two identical atoms sharing electrons equally, so it is nonpolar and does not exhibit dipole-dipole forces.
5. For CO\_2 (carbon dioxide), the molecule is linear with two polar C=O bonds pointing in opposite directions. The bond dipoles cancel out, making CO\_2 nonpolar overall.