Questions: Which of the following statements about intermolecular forces is true? Dispersion forces is the only attractive force between a molecule of HCl with a molecule of HBr in the liquid phase. Dispersion forces is the only attractive force between a molecule of Cl2 with a molecule of Br2 in the liquid phase. Dispersion forces is the only attractive force between a molecule of HF with another molecule of HF in the liquid phase. Dispersion forces is the only attractive force between a molecule of HCl with a molecule of H2O in the liquid phase. Dispersion forces is the only attractive force between a molecule of I-Cl with a molecule of I-F in the liquid phase.

Solution Steps

Intermolecular forces are the forces of attraction or repulsion between molecules. The main types include:

• Dispersion Forces (London Forces): Present in all molecules, especially nonpolar ones.
• Dipole-Dipole Interactions: Occur between polar molecules.
• Hydrogen Bonding: A strong type of dipole-dipole interaction, occurring when hydrogen is bonded to highly electronegative atoms like N, O, or F.

1. HCl and HBr: Both are polar molecules, so they experience dipole-dipole interactions in addition to dispersion forces.
2. Cl\(_2\) and Br\(_2\): Both are nonpolar molecules, so they only experience dispersion forces.
3. HF and HF: HF is a polar molecule capable of hydrogen bonding, so it experiences hydrogen bonding in addition to dispersion forces.
4. HCl and H\(_2\)O: Both are polar, and H\(_2\)O can form hydrogen bonds, so they experience dipole-dipole interactions and possibly hydrogen bonding.
5. I-Cl and I-F: Both are polar molecules, so they experience dipole-dipole interactions in addition to dispersion forces.

The only statement where dispersion forces are the only attractive forces is between nonpolar molecules. Therefore, the true statement is:

• Dispersion forces is the only attractive force between a molecule of Cl\(_2\) with a molecule of Br\(_2\) in the liquid phase.

Final Answer