Which statement best describes the ion-dipole interaction occurring when KI is dissolved in water?

• A. The dissolution of KI in water is driven primarily by covalent bonding between KI and H_2O.
• B. KI molecules form hydrogen bonds with water molecules, resulting in dissolution.
• C. Water molecules induce dipoles in KI, leading to dispersion forces as the main interaction.
• D. The K^+ and I^- ions are attracted to the partial charges on the water molecules, with K^+ interacting with the oxygen atom and I^- interacting with the hydrogen atoms.

Answer: (D)

Verified step by step guidance

1. Understand that KI (potassium iodide) is an ionic compound composed of K^+ (potassium ions) and I^- (iodide ions). When KI dissolves in water, it dissociates into these ions.
2. Recognize that water is a polar molecule with a partial negative charge on the oxygen atom and partial positive charges on the hydrogen atoms due to its bent molecular shape and polar O-H bonds.
3. Identify that ion-dipole interactions occur between charged ions and polar molecules. Specifically, positive ions (cations) are attracted to the negative end of the dipole, and negative ions (anions) are attracted to the positive end of the dipole.
4. Apply this concept to KI in water: K^+ ions are attracted to the oxygen atoms of water molecules (which have partial negative charges), and I^- ions are attracted to the hydrogen atoms of water molecules (which have partial positive charges).
5. Conclude that this ion-dipole attraction is the primary interaction responsible for the dissolution of KI in water, rather than covalent bonding, hydrogen bonding, or induced dipole interactions.