Let's analyze the table and determine the intermolecular forces present for each compound.

1. Iodine (I₂):

   • Dispersion forces: Since I₂ is a nonpolar molecule made up of two identical atoms, it only exhibits London dispersion forces.
   • Dipole: No, because I₂ is nonpolar.
   • Hydrogen bonding: No, hydrogen bonding requires hydrogen atoms bonded to highly electronegative atoms (N, O, F).

2. Dichloromethane (CH₂Cl₂):

   • Dispersion forces: Yes, all molecules experience dispersion forces.
   • Dipole: Yes, CH₂Cl₂ is a polar molecule due to the asymmetrical distribution of polar C-Cl bonds.
   • Hydrogen bonding: No, hydrogen bonding requires hydrogen directly bonded to N, O, or F, which CH₂Cl₂ does not have.

3. Oxygen difluoride (OF₂):

   • Dispersion forces: Yes, all molecules have dispersion forces.
   • Dipole: Yes, OF₂ is polar due to the difference in electronegativity between oxygen and fluorine.
   • Hydrogen bonding: No, because there are no hydrogen atoms directly bonded to highly electronegative atoms (N, O, F).

4. Hypochlorous acid (HClO):

   • Dispersion forces: Yes, all molecules experience dispersion forces.
   • Dipole: Yes, HClO is a polar molecule.
   • Hydrogen bonding: Yes, it can form hydrogen bonds due to the presence of the O-H group.

Summary for each compound:

• Iodine (I₂): Dispersion forces only.
• Dichloromethane (CH₂Cl₂): Dispersion forces, Dipole.
• Oxygen difluoride (OF₂): Dispersion forces, Dipole.
• Hypochlorous acid (HClO): Dispersion forces, Dipole, Hydrogen bonding.

Would you like more details on any of these interactions or further clarifications? Here are some additional questions to consider:

1. How does molecular geometry affect dipole moments?
2. What causes London dispersion forces to increase in strength?
3. Can a molecule with only dispersion forces ever have strong intermolecular attractions?
4. What other molecules can exhibit hydrogen bonding?
5. How does the electronegativity of atoms influence dipole interactions?

Tip: Polar molecules tend to have stronger intermolecular forces compared to nonpolar molecules due to dipole interactions.