Indicate the principal type of solute–solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute–solvent interaction: (b) CH₂Cl₂ in benzene (C₆H₆)

Verified step by step guidance

1. Identify the types of molecules involved in the solution: CH₂Cl₂ (dichloromethane) and C₆H₆ (benzene).
2. Determine the polarity of each molecule: CH₂Cl₂ is a polar molecule due to the electronegativity difference between carbon and chlorine, while benzene is a nonpolar molecule.
3. Analyze the type of interaction between the solute (CH₂Cl₂) and the solvent (benzene): The primary interaction is likely to be dipole-induced dipole interaction, where the permanent dipole of CH₂Cl₂ induces a temporary dipole in the nonpolar benzene molecules.
4. Consider the strength of the interaction: Dipole-induced dipole interactions are generally weaker than hydrogen bonding but stronger than London dispersion forces.
5. Rank the interaction strength: Since this solution involves dipole-induced dipole interactions, it would be ranked as having a moderate strength of solute-solvent interaction compared to other types of interactions like ion-dipole or hydrogen bonding.

Key Concepts

Solute-Solvent Interactions

Solute-solvent interactions refer to the forces that occur between solute particles and solvent molecules when a solution is formed. These interactions can include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. The strength and type of these interactions significantly influence the solubility of a solute in a solvent.

Polarity

Polarity is a key concept in chemistry that describes the distribution of electrical charge over the atoms in a molecule. Polar molecules have a significant difference in electronegativity between their atoms, leading to partial positive and negative charges. In the context of solute-solvent interactions, polar solutes tend to dissolve well in polar solvents, while nonpolar solutes dissolve better in nonpolar solvents.

Ranking of Interactions

Ranking solute-solvent interactions involves comparing the strength of different types of intermolecular forces present in a solution. Generally, hydrogen bonds are the strongest, followed by dipole-dipole interactions, and then London dispersion forces. Understanding this hierarchy helps in predicting the behavior of solutions and their properties, such as boiling and melting points.