Which is the strongest intermolecular force present in a sample of BrF?

• A. London dispersion forces
• B. Dipole-dipole interactions
• C. Hydrogen bonding
• D. Ion-dipole interactions

Answer: (B)

Verified step by step guidance

1. Identify the type of molecule BrF is: it is a diatomic molecule composed of bromine (Br) and fluorine (F).
2. Determine the electronegativity difference between Br and F to assess if the molecule is polar. Since fluorine is much more electronegative than bromine, BrF is a polar molecule.
3. Recall the types of intermolecular forces: London dispersion forces (present in all molecules), dipole-dipole interactions (present in polar molecules), hydrogen bonding (requires H bonded to N, O, or F), and ion-dipole interactions (involving ions and polar molecules).
4. Since BrF is polar but does not have hydrogen bonded to N, O, or F, hydrogen bonding is not possible. Also, there are no ions present, so ion-dipole interactions are excluded.
5. Conclude that the strongest intermolecular force in BrF is dipole-dipole interactions, which occur between polar molecules.