Chapter 12.2, Problem 12.2CC

Interpretation Introduction

Interpretation:

Given that compound X has stronger intermolecular force and has no dipole-dipole forces, compound Y has Hydrogen bonding, the relative solubility of the compounds X and Y in water and non-polar solvent has to be predicted and the same has to be explained.

Concept Introduction:

• The intermolecular forces are the attractive forces between the molecules of a compound.
• The three types of intermolecular forces are – London dispersion force, dipole-dipole force and Hydrogen bonding. Among these London dispersion force is the weakest one and dipole-dipole force is the strongest one.
• London dispersion forces exist in non-polar covalent compounds. Dipole-dipole forces present in polar covalent compounds. This is the force responsible for the condensation of non-polar compounds into liquids or solids under low temperature.
• Hydrogen bonding is formed in polar covalent compounds containing direct bond between Hydrogen and other high electronegativity like Fluorine, Oxygen or Nitrogen.
• The order of strength of intermolecular force is,

London dispersion force < Dipole-dipole force < Hydrogen bonding.

However London dispersion forces become stronger in case of larger molecules.