Chapter 8.4, Problem 32LC

Interpretation Introduction

Interpretation: The comparison between the strengths of intermolecular attractions with ionic bonds and covalent bonds needs to be done.

Concept Introduction: Intermolecular attraction is the force of attraction between molecules. These interactions include forces of attraction as well as repulsion between atoms and other particles like atoms or ions. A covalent bond is formed by sharing of valence electrons between two atoms. On the other hand, an ionic bond is formed by the complete transfer of electrons from a metal to a non-metal.

Explanation of Solution

The three types of intermolecular forces are London dispersion forces, dipole-dipole interactions, and hydrogen bonding.

A covalent bond is formed by sharing of valence electrons between two atoms. Here, atoms involved in bonding, share electron pairs to form a bond. The number of electron pairs shared decides the number of bonds that is single, double, or triple. Also, the covalent bond can be polar and non-polar depending on the relative electronegativity between two atoms involved in bonding.

An ionic bond is formed between positive and negatively charged ions. Here, positive charge ions are formed when atoms lose electron/s. Similarly, negative charge ions are formed when an atom gain electron/s. The number of electrons gained or lost by an atom is equal to the charge on the ion formed. Here, the complete transfer of electron/s from positively charged ion to negatively charged ion takes place.

The relative strength is such that intermolecular forces are the weakest among all and an ionic bond is the strongest.

The order of strength is as follows:

  $\text{Intermolecular forces}<\text{ Covalent bond}<\text{Ionic bond}$