Classify the strongest type of intermolecular force in the following interactions: solvent–solvent, solvent–solute, and solute–solute when solid glucose (C6H12O6) is placed in water. Based on these interactions, predict whether glucose is soluble in water.

Intermolecular forces are the forces of attraction or repulsion between neighboring particles (atoms, molecules, or ions). They are weaker than covalent or ionic bonds and include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Understanding these forces is crucial for predicting the behavior of substances in different states and their solubility in solvents.

Hydrogen bonding is a specific type of strong dipole-dipole interaction that occurs when hydrogen is covalently bonded to highly electronegative atoms like oxygen, nitrogen, or fluorine. In the case of glucose and water, the hydroxyl (-OH) groups in glucose can form hydrogen bonds with water molecules, significantly influencing its solubility in water.

Solubility refers to the ability of a solute to dissolve in a solvent, which is influenced by the nature of the solute and solvent, as well as temperature and pressure. The principle 'like dissolves like' suggests that polar solutes, such as glucose, are more soluble in polar solvents like water due to favorable interactions, including hydrogen bonding and dipole interactions.