Chapter 10, Problem 10A.2E

(a)

Interpretation Introduction

Interpretation:

The dipole moment of $\text{HF}$ molecule has to be determined from the electronegativities of the elements and the answer should be expressed in Debye and coulomb meters.

Concept introduction:

Polar covalent bond involves an unequal sharing of electrons between two bonded atoms; it creates a partial separation of charge and a dipole moment.

Covalent bonds are polar, if there is a difference in electronegativity between the bonded atoms.

Direction of dipole moment in a molecule is can be represented as follows,

  $\text{Positive }\underset{}{\to }\text{ Negative}$

(b)

Interpretation Introduction

Interpretation:

The dipole moment of $\text{HCl}$ molecule has to be determined from the electronegativities of the elements and the answer should be expressed in Debye and coulomb meters.

Concept introduction:

Polar covalent bond involves an unequal sharing of electrons between two bonded atoms; it creates a partial separation of charge and a dipole moment.

Covalent bonds are polar, if there is a difference in electronegativity between the bonded atoms.

Direction of dipole moment in a molecule is can be represented as follows,

  $\text{Positive }\underset{}{\to }\text{ Negative}$

(c)

Interpretation Introduction

Interpretation:

The dipole moment of $\text{HBr}$ molecule has to be determined from the electronegativities of the elements and the answer should be expressed in Debye and coulomb meters.

Concept introduction:

Polar covalent bond involves an unequal sharing of electrons between two bonded atoms; it creates a partial separation of charge and a dipole moment.

Covalent bonds are polar, if there is a difference in electronegativity between the bonded atoms.

Direction of dipole moment in a molecule is can be represented as follows,

  $\text{Positive }\underset{}{\to }\text{ Negative}$