The context provides key insights: (i) n-hexane and n-heptane form ideal solutions where A-A, B-B, and A-B intermolecular attractive forces are nearly equal—this applies to n-hexane and n-octane as well, both being non-polar hydrocarbons with London dispersion forces. (ii) I₂ and CCl₄ are both non-polar molecules, so London dispersion forces dominate. (iii) The context mentions ionic compounds like KCl dissociate in aqueous solution (i close to 2), indicating ion-dipole interactions between NaClO₄ ions and water. (iv) The context explicitly states that chloroform forms hydrogen bonds with acetone—similarly, methanol (with -OH group) forms hydrogen bonds with acetone's carbonyl oxygen. (v) Acetonitrile and acetone are both polar molecules with permanent dipoles, so dipole-dipole interactions are most significant.