Which of the following represents the intermolecular forces present in CO₂?

• A. Dipole-dipole forces only
• B. London dispersion forces only
• C. London dispersion and dipole-dipole forces
• D. Hydrogen bonding only

Answer: (B)

Verified step by step guidance

1. Step 1: Identify the molecular structure and polarity of CO₂. Carbon dioxide (CO₂) is a linear molecule with two polar C=O bonds arranged symmetrically.
2. Step 2: Determine the overall molecular polarity. Because the molecule is linear and symmetrical, the dipole moments of the two C=O bonds cancel each other out, making CO₂ a nonpolar molecule.
3. Step 3: Understand the types of intermolecular forces. Dipole-dipole forces occur between polar molecules, hydrogen bonding occurs when H is bonded to N, O, or F, and London dispersion forces (also called induced dipole-induced dipole forces) occur in all molecules but are the only forces in nonpolar molecules.
4. Step 4: Since CO₂ is nonpolar, it does not exhibit dipole-dipole forces or hydrogen bonding. Therefore, the only intermolecular forces present are London dispersion forces.
5. Step 5: Conclude that the correct representation of intermolecular forces in CO₂ is 'London dispersion forces only.'