Classify the strongest type of intermolecular force in the follow- ing interactions: solvent–solvent, solvent–solute, and solute– solute when solid iodine 1I22 is placed in the water. Based on these interactions, predict whether I2 is soluble in water.

Verified step by step guidance

1. Identify the types of molecules involved: Iodine (I2) is a nonpolar molecule, while water (H2O) is a polar molecule.
2. Determine the strongest intermolecular force for solvent-solvent interactions: Water molecules interact with each other primarily through hydrogen bonding, which is a strong type of dipole-dipole interaction.
3. Determine the strongest intermolecular force for solute-solute interactions: Iodine molecules interact with each other through London dispersion forces, which are the weakest type of intermolecular forces.
4. Determine the strongest intermolecular force for solvent-solute interactions: When iodine is placed in water, the interaction between iodine and water is primarily through dipole-induced dipole forces, which are weaker than hydrogen bonds.
5. Predict the solubility of I2 in water: Since the interactions between iodine and water are weaker than the interactions within water itself, iodine is not very soluble in water.

Key Concepts

Intermolecular Forces

Intermolecular forces are the forces of attraction or repulsion between molecules. They include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Understanding these forces is crucial for predicting the behavior of substances in different environments, such as solubility in solvents.

Solubility Principles

Solubility refers to the ability of a solute to dissolve in a solvent, which is influenced by the nature of both the solute and solvent. The principle 'like dissolves like' indicates that polar solvents tend to dissolve polar solutes, while nonpolar solvents dissolve nonpolar solutes. This concept is essential for predicting the solubility of iodine in water.

Iodine and Water Interactions

Iodine (I2) is a nonpolar molecule, while water (H2O) is a polar solvent. The interactions between iodine and water involve weaker London dispersion forces, which are not strong enough to overcome the hydrogen bonding present in water. This difference in polarity explains why iodine is not soluble in water.