Dipole-dipole interactions occur in polar molecules where the difference in electronegativity between the combining atoms creates positive and negative dipoles. These opposite poles align and result in electrostatic attraction throughout the polar medium. So, naturally, the strength of the interaction would depend on Coulomb’s law - the higher the magnitude of the charges and the lesser the distance between those charges, the stronger the dipole-dipole attractive interaction.

Amongst the various types of solids - metallic, ionic, covalent - the molecular solid is a type that is differentiated from the rest based on its intermolecular attractive strength.

A molecular solid is composed of distinct, unconnected molecules that are held together by weak van der Waals forces or Hydrogen bonds rather than stronger ionic or covalent bonds. 

Following the footsteps of Gilbert N. Lewis in understanding the nature of the covalent bond, Linus N. Pauling stumbled upon an interesting observation. 

Pauling noticed that the nature of the chemical bond could be explained using a scale or continuum. 

Atom, the omnipresent component that builds up all the stuff the universe is made of, has its identity tied to the tiny, sub-atomic particle- the proton(s). The proton number decides the type of atom; however, the atom’s reactivity is determined by an outer-nuclear component- the electrons.

In nuclear reactions, the proton number can change so that an atom's identity also changes. However, only the electron count changes in organic chemical reactions without affecting an atom's identity.