Chapter 4, Problem 4.60E

Interpretation Introduction

(a)

Interpretation:

Whether the molecule $\text{HI}$ is polar or nonpolar is to be stated.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are the result of the electronegativity difference between bonding atoms. If the electronegativity difference is $0$, the bond is known as nonpolar covalent bond, if electronegativity difference is between $0$ to $2.1$, then the bond is known as polar covalent bond and if it is more than $2.1$, then the bond is known as ionic bond.

Interpretation Introduction

(b)

Interpretation:

Whether the molecule ${\text{SO}}_{\text{2}}$ is polar or nonpolar is to be stated.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are the result of the electronegativity difference between bonding atoms. If the electronegativity difference is $0$, the bond is known as nonpolar covalent bond, if electronegativity difference is between $0$ to $2.1$, then the bond is known as polar covalent bond and if it is more than $2.1$, then the bond is known as ionic bond.

Interpretation Introduction

(c)

Interpretation:

Whether the molecule ${\text{O}}_{\text{3}}$ is polar or nonpolar is to be stated.

Concept introduction:

Electronegativity is defined as the tendency of an atom to attract electrons towards it. Polarized bonds are the result of the electronegativity difference between bonding atoms. If the electronegativity difference is $0$, the bond is known as nonpolar covalent bond, if electronegativity difference is between $0$ to $2.1$, then the bond is known as polar covalent bond and if it is more than $2.1$, then the bond is known as ionic bond.