What principle explains that polar solvents dissolve polar solutes while nonpolar solvents dissolve nonpolar solutes?

The principle that explains why polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes is known as "Like Dissolves Like." This concept is grounded in the molecular interactions between solutes and solvents. Polar substances, having distinct regions of partial positive and negative charges, interact favorably with other polar substances through dipole-dipole interactions or hydrogen bonding. Conversely, nonpolar substances, which do not have charged regions, tend to interact with other nonpolar substances through dispersive forces or van der Waals forces.

This compatibility is crucial because it determines solubility: polar solutes will easily mix and dissolve in polar solvents due to their similar chemical characteristics, whereas nonpolar solutes will not dissolve well in polar solvents because there is little to no interaction. This principle is fundamental in understanding various chemical processes, including biological reactions and solutions in everyday life.

The other options, while relevant in other contexts, do not encapsulate this solubility behavior accurately. The Solubility Principle is vague and does not specifically address the affinity between solutes and solvents. Molecular Compatibility might suggest a relationship but lacks the clarity and established recognition of "Like Dissolves Like." Hydration Theory primarily deals with the interaction of water molecules with sol