The strongest may be only 5-10% as strong as a covalent bond. The weakest of these is much weaker. The strength of intermolecular forces varies, with the strongest being significantly weaker (about 5-10%) than covalent bonds, and the weakest, such as London dispersion forces, being much weaker than the stronger intermolecular forces.
The strongest intermolecular forces, such as hydrogen bonding, dipole-dipole interactions, and ion-dipole interactions, may be only 5-10% as strong as a covalent bond. These intermolecular forces involve attractions between molecules rather than the sharing or transferring of electrons within a single molecule. Hydrogen bonding, for example, is a type of intermolecular force where a hydrogen atom bonded to a highly electronegative atom (such as oxygen, nitrogen, or fluorine) experiences a strong attraction to another electronegative atom in a neighboring molecule.
In contrast, the weakest intermolecular force is van der Waals forces, specifically London dispersion forces. These forces arise due to temporary fluctuations in electron distribution, creating instantaneous dipoles. London dispersion forces are considerably weaker than covalent bonds or the stronger intermolecular forces mentioned earlier.