Final answer:
Ionic forces lead to the highest melting points among various intermolecular forces because they are stronger than hydrogen bonding, dipole-dipole, and London dispersion forces.
Step-by-step explanation:
The intermolecular forces that are likely to lead to the highest melting point are ionic forces. These are typically much stronger than the other types of intermolecular forces, such as London dispersion forces, dipole-dipole forces, or hydrogen bonding.
Ionic bonds are the result of the electrostatic forces between positively and negatively charged ions, and these forces are generally much stronger than the other types of van der Waals forces including London dispersion forces (which increase with the number of electrons but are still weaker),
dipole-dipole interactions (which are stronger than dispersion forces but weaker than hydrogen bonding), and even hydrogen bonding (which is a type of strong dipole-dipole interaction occurring when hydrogen is bonded to a highly electronegative atom like fluorine, oxygen, or nitrogen).
The hierarchy of strength from weakest to strongest intermolecular forces typically follows: London dispersion forces < dipole-dipole forces < hydrogen bonding < ionic bonding.