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)

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Identify the types of molecules involved in the solution: CH₂Cl₂ (dichloromethane) and C₆H₆ (benzene).

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.

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.

Consider the strength of the interaction: Dipole-induced dipole interactions are generally weaker than hydrogen bonding but stronger than London dispersion forces.

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.

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주요 개념

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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.

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)