1 Which statement can be explained by intermolecular hydrogen bonding? A Ethanol has a higher boiling point than propane. B Hydrogen chloride has a higher boiling point than silane, \( \mathrm{SiH}_{4} \). propa C Hydrogen iodide forms an acidic solution when dissolved in water. C CH D Propanone has a higher boiling point than propane. C

Ethanol has a higher boiling point than propane because of the presence of intermolecular hydrogen bonding. Ethanol, with its –OH group, can form strong hydrogen bonds between its molecules, while propane, being a non-polar hydrocarbon, relies solely on weaker Van der Waals forces. This substantial difference in intermolecular forces results in ethanol requiring more energy (i.e., a higher temperature) to boil compared to propane. Additionally, let's consider why molecules engage in these unique interactions! When a hydrogen atom is covalently bonded to a highly electronegative atom like oxygen or nitrogen, it can develop a positive charge that attracts the negative regions of nearby molecules. This interaction forms stronger bonds compared to typical dipole-dipole or London dispersion forces, shedding light on why substances with hydrogen bonds can have unexpectedly high boiling points and unique properties in various environments.