Chapter 8, Problem 8.91SP

Interpretation Introduction

Interpretation:

The intermolecular forces that predominate in the given substances needs to be determined. Also, the given substances need to be arranged in order of normal boiling points.

Given information:

The given substances are: Al₂O₃, F₂, H₂O, Br₂, ICl, NaCl.

Concept introduction:

Usually four different types of intermolecular forces are present in the substances.

• Ion-dipole forces: Molecules which have polar bonds and an overall dipole moment are known as dipoles. One side of the molecule has a slight positive or negative charge and the other has the opposite charge. When an ion attracts one end of a dipole towards itself, the intermolecular force of attraction is known as ion-dipole force.
• Dipole-dipole forces: When two dipoles are attracted to/repelled each other, the intermolecular forces are called as dipole-dipole forces.
• Hydrogen bonding: When a hydrogen atom is attached to a highly electronegative atom. This type of O, N or F, this hydrogen atom can form a bond with another electronegative atom. This type of intermolecular force is known as a hydrogen bonding.
• London-dispersion forces: London dispersion forces are seen in all types of molecules. They are caused by the formation of instantaneous, temporary dipoles in non-polar molecules.