Compare ionic compounds, polar molecules, acids and a non-polar hydrocarbon. Water is polar: its oxygen end is δ− and its hydrogen ends are δ+. Dissolving is favourable when water–solute attractions are strong enough to replace disrupted water–water or solute–solute attractions.
Compare ionic, polar and non-polar substances and observe how water molecules interact with each type of particle. The simulation helps students connect solubility to charge, molecular polarity and intermolecular forces rather than relying only on the phrase “like dissolves like”. Use it to support secondary chemistry discussions about dissolving, hydration and why some substances remain separate from water.
Key concepts: Solubility, Polarity, Intermolecular forces, Ionic substances.