Final answer:
All the molecules listed, including methane, carbon tetrachloride, and bromine trifluoride, exhibit London dispersion forces. This is because all molecules have these forces, in addition to any other type of intermolecular forces they might possess.
Step-by-step explanation:
London dispersion forces are a type of intermolecular force present in all molecules, whether polar or nonpolar. These forces are temporary and depend on the instantaneous distribution of electrons in a molecule. Looking at the examples provided:
- Methane (CH4) is a nonpolar molecule with London dispersion forces.
- Carbon tetrachloride (CCl4) is also nonpolar and exhibits London dispersion forces.
- Even though bromine trifluoride (BrF3) is polar with a net dipole moment, it still possesses London dispersion forces, in addition to dipole-dipole interactions.
Therefore, the answer to the question is d. all of the above.