How does solubility relate to bonding?

"Like dissolves in like" is a useful generalization concerning the strengths of the intermolecular forces between particles.

Solutes whose particles are likewise held together by strong intermolecular forces, such as sodium chloride particles, which are held together by strong coulombic forces, will be soluble in water and dissolve in it, for instance, because water molecules are held together by strong hydrogen bonds.

Conversely, carbon tetrachloride will not dissolve in water because its particles are held together by weak van der Waals forces; however, it will dissolve in a solvent that also contains weak intermolecular forces, such as bromine.

Newton's Law of Universal Gravitational Attraction between Particles states that for longer chain alkanes, the solubility in water will increase as the chain length increases due to stronger intermolecular forces.

Solubility relates to bonding through the interactions between solute and solvent molecules. For example, polar solutes tend to dissolve in polar solvents due to similar intermolecular forces, while nonpolar solutes dissolve in nonpolar solvents. This relates to the types of bonds present in the solute and solvent molecules, such as hydrogen bonding, dipole-dipole interactions, or London dispersion forces.