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Many atoms have nuclei consisting of several protons packed into an extremely small volume. Each proton has a positive charge, and since positive charges repel each other, the theory of electromagnetism says that these nuclei must not exist in a stable state. The fact that they do indeed exist leads us to believe that there is a force holding the protons together which must be stronger than the electromagnetic force. We call this force the strong nuclear force.

In summary, the fact that protons are held together in nuclei despite their electric repulsion is evidence that there is a force (called the strong nuclear force) which is stronger than their electric repulsion.

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Which intermolecular force is the weakest?

If you are asking about bonds of attraction between separate molecules, there are two kinds: dipole-dipole attraction and London dispersion force attraction. Dipole-dipole attraction is the stronger of the two, because the molecules in this case are polar, meaning that electrons are more often clustered at certain spots on the molecule and rarified at the opposite end, resulting in a greater charge on both ends (London dispersion forces are the weak forces of attraction between nonpolar molecules during random, fleeting moments of polarization). These forces are not to be confused with ionic attraction (which is attraction between ions, not molecules) and covalent bonds (which are the forces holding the individual atoms in a molecule together), both of which are stronger than any intermolecular force of attraction (with covalent bonding being the strongest of all bonds at the chemical as opposed to the nuclear level). Keep in mind, though, that the exact strength of attraction varies depending on the electronegativities of the different atoms in the molecule (but the weakest polar molecular bonds are, by definition, stronger than the strongest nonpolar molecular bonds).


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