Chapter 3, Problem 3.51PP

a.

Summary Introduction

To determine:

The Lewis structure of $\text{HCl}$ the molecule.

Introduction:

The Lewis structures are also called electron dot structures. In the Lewis structure, electrons are denoted by dots. These dots represent the number of electrons present in the outer most shell of an element.

Summary Introduction

To determine:

The labeled polar covalent bond of $\text{HCl}$ with dipole moment arrow.

Introduction:

The dipole moment in the molecule arises due to the electronegativity difference between the atoms. The dipole moment of the symmetric molecule is zero because the electron withdrawing molecules cancel each other’s dipole moments. However, the dipole moment of unsymmetrical molecules is not zero. There is always a net dipole moment.

Summary Introduction

To determine:

The molecule is polar or non-polar and the dipole moment arrow of the molecule.

Introduction:

The polarity of a bond is directly related to the electronegativity difference. A polar bond corresponds to a non-uniform distribution of the electron cloud between two nonmetals. Thus, the bond formed between them is a covalent bond. This corresponds to the fact that an atom with higher electronegativity value will show a higher affinity for electrons.

A non-polar bond is formed by a mononuclear diatomic molecule that corresponds to a uniform distribution of the electron cloud. These molecules do not possess a dipole moment.

b.

Summary Introduction

To determine:

The Lewis structure of $\text{COS}$ the molecule.

Introduction:

The Lewis structures are also called electron dot structures. In the Lewis structure, electrons are denoted by dots. These dots represent the number of electrons present in the outer most shell of an element.

Summary Introduction

To determine:

The labeled polar covalent bond of $\text{COS}$ with dipole moment arrow.

Introduction:

The dipole moment in the molecule arises due to the electronegativity difference between the atoms. The dipole moment of the symmetric molecule is zero because the electron withdrawing molecules cancel out each other’s dipole moments. However, the dipole moment of unsymmetrical molecules is not zero. There is always a net dipole moment.

Summary Introduction

To determine:

The molecule is polar or non-polar and the dipole moment arrow of the molecule.

Introduction:

The polarity of a bond is directly related to the electronegativity difference. A polar bond corresponds to a non-uniform distribution of the electron cloud between two nonmetals. Thus, the bond formed between them is a covalent bond. This corresponds to the fact that an atom with higher electronegativity value will show a higher affinity for electrons.

A non-polar bond is formed by a mononuclear diatomic molecule that corresponds to a uniform distribution of the electron cloud. These molecules do not possess a dipole moment.

c.

Summary Introduction

To determine:

The Lewis structure of ${\text{H}}_2\text{S}$ the molecule.

Introduction:

The Lewis structures are also called electron dot structures. In the Lewis structure, electrons are denoted by dots. These dots represent the number of electrons present in the outer most shell of an element.

Summary Introduction

To determine:

The labeled polar covalent bond of ${\text{H}}_2\text{S}$ with dipole moment arrow.

Introduction:

The dipole moment in the molecule arises due to the electronegativity difference between the atoms. The dipole moment of the symmetric molecule is zero because the electron withdrawing molecules cancel out each other’s dipole moments. However, the dipole moment of unsymmetrical molecules is not zero. There is always a net dipole moment.

Summary Introduction

To determine:

If the molecule is polar or non-polar and the dipole moment arrow of the molecule.

Introduction:

The polarity of a bond is directly related to the electronegativity difference. A polar bond corresponds to a non-uniform distribution of the electron cloud between two nonmetals. Thus, the bond formed between them is a covalent bond. This corresponds to the fact that an atom with higher electronegativity value will show a higher affinity for electrons.

A non-polar bond is formed by a mononuclear diatomic molecule that corresponds to a uniform distribution of the electron cloud. These molecules do not possess a dipole moment.

d.

Summary Introduction

To determine:

The Lewis structure of ${\text{CH}}_2{\text{Br}}_2$ the molecule.

Introduction:

The Lewis structures are also called electron dot structures. In the Lewis structure, electrons are denoted by dots. These dots represent the number of electrons present in the outer most shell of an element.

Summary Introduction

To determine:

The labeled polar covalent bond of ${\text{CH}}_2{\text{Br}}_2$ with dipole moment arrow.

Introduction:

The dipole moment in the molecule arises due to the electronegativity difference between the atoms. The dipole moment of the symmetric molecule is zero because the electron withdrawing molecules cancel out each other’s dipole moments. However, the dipole moment of unsymmetrical molecules is not zero. There is always a net dipole moment.

Summary Introduction

To determine:

The molecule is polar or non-polar and the dipole moment arrow of the molecule.

Introduction:

The polarity of a bond is directly related to the electronegativity difference. A polar bond corresponds to a non-uniform distribution of the electron cloud between two nonmetals. Thus, the bond formed between them is a covalent bond. This corresponds to the fact that an atom with higher electronegativity value will show a higher affinity for electrons.

A non-polar bond is formed by a mononuclear diatomic molecule that corresponds to a uniform distribution of the electron cloud. These molecules do not possess a dipole moment.