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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.

Decide which intermolecular forces act between the molecules of each compound in the table: I₂, CH₂Cl₂, OF₂, HClO.

Analyze the intermolecular forces (dispersion, dipole, hydrogen-bonding) in compounds like iodine, dichloromethane, oxygen difluoride, and hypochlorous acid. Learn about how molecular structure determines these forces in high school chemistry.

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