The Lewis structure of 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.

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Answer 1

Question

Chapter 3, Problem 3.51PP

a.

Summary Introduction

To determine:

The Lewis structure of 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 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 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 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 H2S 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 H2S 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 CH2Br2 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 CH2Br2 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.

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Answer 2

Question

Chapter 3, Problem 3.51PP

a.

Summary Introduction

To determine:

The Lewis structure of 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 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 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 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 H2S 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 H2S 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 CH2Br2 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 CH2Br2 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.

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Answer 3

Question

Chapter 3, Problem 3.51PP

a.

Summary Introduction

To determine:

The Lewis structure of 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 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 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 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 H2S 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 H2S 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 CH2Br2 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 CH2Br2 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.

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Answer 4

Question

Chapter 3, Problem 3.51PP

a.

Summary Introduction

To determine:

The Lewis structure of 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 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 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 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 H2S 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 H2S 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 CH2Br2 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 CH2Br2 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.

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Answer 5

Chapter 3, Problem 3.51PP

a.

Summary Introduction

To determine:

The Lewis structure of 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 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 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 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 H2S 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 H2S 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 CH2Br2 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 CH2Br2 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.

Answer 6

Chapter 3, Problem 3.51PP

a.

Summary Introduction

To determine:

The Lewis structure of 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.

Answer 7

Chapter 3, Problem 3.51PP

a.

Summary Introduction

To determine:

The Lewis structure of 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.

Answer 8

Summary Introduction

To determine:

The labeled polar covalent bond of 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.

Answer 9

Summary Introduction

To determine:

The labeled polar covalent bond of 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.

Answer 10

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.

Answer 11

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.

Answer 12

b.

Summary Introduction

To determine:

The Lewis structure of 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.

Answer 13

b.

Summary Introduction

To determine:

The Lewis structure of 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.

Answer 14

Summary Introduction

To determine:

The labeled polar covalent bond of 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.

Answer 15

Summary Introduction

To determine:

The labeled polar covalent bond of 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.

Answer 16

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.

Answer 17

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.

Answer 18

c.

Summary Introduction

To determine:

The Lewis structure of H2S 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.

Answer 19

c.

Summary Introduction

To determine:

The Lewis structure of H2S 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.

Answer 20

Summary Introduction

To determine:

The labeled polar covalent bond of H2S 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.

Answer 21

Summary Introduction

To determine:

The labeled polar covalent bond of H2S 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.

Answer 22

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.

Answer 23

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.

Answer 24

d.

Summary Introduction

To determine:

The Lewis structure of CH2Br2 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.

Answer 25

d.

Summary Introduction

To determine:

The Lewis structure of CH2Br2 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.

Answer 26

Summary Introduction

To determine:

The labeled polar covalent bond of CH2Br2 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.

Answer 27

Summary Introduction

To determine:

The labeled polar covalent bond of CH2Br2 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.

Answer 28

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.

Answer 29

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.

Answer 30

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Answer 31

Expert Solution & Answer

Answer 32

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Answer 33

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The Lewis structure of 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.

Solution Summary: The author explains the Lewis structure of HCl and the labeled polar covalent bond with the dipole moment arrow.

To determine:

The Lewis structure of 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.

To determine:

The Lewis structure of 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.

To determine:

The Lewis structure of H2S 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.

To determine:

The Lewis structure of CH2Br2 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.

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Chapter 3 Solutions

The Lewis structure of 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.

Solution Summary: The author explains the Lewis structure of HCl and the labeled polar covalent bond with the dipole moment arrow.

To determine: The Lewis structure of 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.

To determine: The Lewis structure of 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.

To determine: The Lewis structure of H2S 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.

To determine: The Lewis structure of CH2Br2 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.

Want to see the full answer?

Chapter 3 Solutions

To determine:

The Lewis structure of 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.

To determine:

The Lewis structure of 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.

To determine:

The Lewis structure of H2S 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.

To determine:

The Lewis structure of CH2Br2 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.