Final answer:
Yes, a larger dipole moment results in stronger dipole-dipole interactions. These are substantially weaker than ionic interactions but predominant in small polar molecules over dispersion forces.
Step-by-step explanation:
A larger dipole moment correlates with stronger dipole-dipole interactions. These interactions involve an attraction between the positive end of one dipole and the negative end of another. Notably, dipole-dipole forces are weaker than ionic bonds due to only partial charges being involved. However, within molecules of similar molar mass, as the dipole moment increases, so does the strength of the intermolecular attractions.
It's important to note that the force of attraction between dipoles decreases rapidly as their distance increases. For dipole interactions, the energy is proportional to 1/r³, meaning that at double the distance, the interaction strength decreases by a factor of eight. Contrarily, ion-ion interactions decline at a lesser rate of 1/r, so at double the distance, the strength only reduces by half.
Although dipole-induced dipole and London dispersion forces also contribute to molecular attractions, dipole-dipole interactions are predominant in small polar molecules, where these are significantly stronger than dispersion forces.