The Lewis structure of H 2 S has to be determined. Also, the bonding and lone pairs in the structure have to be labeled. Concept Introduction: The bond result from the electrostatic force of attraction between oppositely charged ions is called ionic bond and the bond result from the mutual sharing of electrons between atoms is called covalent bond. The Lewis electron-dot symbol can be used to describe the covalent bonds in molecules. Two types of pairs of electrons are as follows: 1. Bonding pairs of electrons are shared between two atoms. 2. Lone or nonbonding, pairs of electrons are on one atom and are not shared. Lewis structures are representations of the covalent bond. In this Lewis symbols show how the valence electrons are present in the molecule. Steps to write Lewis structures are as follows: 1. The skeleton structure with single bonds between all bonded atoms has to be written 2. Sum the valence electrons of the atoms in the molecule. (a) For cations, one electron is subtracted for each positive charge. (b) For anions, one electron is added for each negative charge. 3. Subtract two electrons for each bond in the skeleton structure. 4. Count the number of electrons needed to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet. 5 The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

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Answer 1

Question

Chapter 9, Problem 9.35QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of H2S has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

The bond result from the electrostatic force of attraction between oppositely charged ions is called ionic bond and the bond result from the mutual sharing of electrons between atoms is called covalent bond. The Lewis electron-dot symbol can be used to describe the covalent bonds in molecules.

Two types of pairs of electrons are as follows:

1. Bonding pairs of electrons are shared between two atoms.

2. Lone or nonbonding, pairs of electrons are on one atom and are not shared.

Lewis structures are representations of the covalent bond. In this Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons for each bond in the skeleton structure.

4. Count the number of electrons needed to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5 The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of H2CO has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of PF3 has to be determined. Also, the bonding and lone pairs in the structure have to be labelled.

Concept Introduction:

Refer to part (a)

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Answer 2

Question

Chapter 9, Problem 9.35QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of H2S has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

The bond result from the electrostatic force of attraction between oppositely charged ions is called ionic bond and the bond result from the mutual sharing of electrons between atoms is called covalent bond. The Lewis electron-dot symbol can be used to describe the covalent bonds in molecules.

Two types of pairs of electrons are as follows:

1. Bonding pairs of electrons are shared between two atoms.

2. Lone or nonbonding, pairs of electrons are on one atom and are not shared.

Lewis structures are representations of the covalent bond. In this Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons for each bond in the skeleton structure.

4. Count the number of electrons needed to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5 The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of H2CO has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of PF3 has to be determined. Also, the bonding and lone pairs in the structure have to be labelled.

Concept Introduction:

Refer to part (a)

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Answer 3

Question

Chapter 9, Problem 9.35QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of H2S has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

The bond result from the electrostatic force of attraction between oppositely charged ions is called ionic bond and the bond result from the mutual sharing of electrons between atoms is called covalent bond. The Lewis electron-dot symbol can be used to describe the covalent bonds in molecules.

Two types of pairs of electrons are as follows:

1. Bonding pairs of electrons are shared between two atoms.

2. Lone or nonbonding, pairs of electrons are on one atom and are not shared.

Lewis structures are representations of the covalent bond. In this Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons for each bond in the skeleton structure.

4. Count the number of electrons needed to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5 The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of H2CO has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of PF3 has to be determined. Also, the bonding and lone pairs in the structure have to be labelled.

Concept Introduction:

Refer to part (a)

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Answer 4

Question

Chapter 9, Problem 9.35QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of H2S has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

The bond result from the electrostatic force of attraction between oppositely charged ions is called ionic bond and the bond result from the mutual sharing of electrons between atoms is called covalent bond. The Lewis electron-dot symbol can be used to describe the covalent bonds in molecules.

Two types of pairs of electrons are as follows:

1. Bonding pairs of electrons are shared between two atoms.

2. Lone or nonbonding, pairs of electrons are on one atom and are not shared.

Lewis structures are representations of the covalent bond. In this Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons for each bond in the skeleton structure.

4. Count the number of electrons needed to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5 The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of H2CO has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of PF3 has to be determined. Also, the bonding and lone pairs in the structure have to be labelled.

Concept Introduction:

Refer to part (a)

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Answer 5

Chapter 9, Problem 9.35QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of H2S has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

The bond result from the electrostatic force of attraction between oppositely charged ions is called ionic bond and the bond result from the mutual sharing of electrons between atoms is called covalent bond. The Lewis electron-dot symbol can be used to describe the covalent bonds in molecules.

Two types of pairs of electrons are as follows:

1. Bonding pairs of electrons are shared between two atoms.

2. Lone or nonbonding, pairs of electrons are on one atom and are not shared.

Lewis structures are representations of the covalent bond. In this Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons for each bond in the skeleton structure.

4. Count the number of electrons needed to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5 The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of H2CO has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

Refer to part (a)

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of PF3 has to be determined. Also, the bonding and lone pairs in the structure have to be labelled.

Concept Introduction:

Refer to part (a)

Answer 6

Chapter 9, Problem 9.35QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of H2S has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

The bond result from the electrostatic force of attraction between oppositely charged ions is called ionic bond and the bond result from the mutual sharing of electrons between atoms is called covalent bond. The Lewis electron-dot symbol can be used to describe the covalent bonds in molecules.

Two types of pairs of electrons are as follows:

1. Bonding pairs of electrons are shared between two atoms.

2. Lone or nonbonding, pairs of electrons are on one atom and are not shared.

Lewis structures are representations of the covalent bond. In this Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons for each bond in the skeleton structure.

4. Count the number of electrons needed to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5 The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

Answer 7

Chapter 9, Problem 9.35QE

(a)

Interpretation Introduction

Interpretation:

The Lewis structure of H2S has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

The bond result from the electrostatic force of attraction between oppositely charged ions is called ionic bond and the bond result from the mutual sharing of electrons between atoms is called covalent bond. The Lewis electron-dot symbol can be used to describe the covalent bonds in molecules.

Two types of pairs of electrons are as follows:

1. Bonding pairs of electrons are shared between two atoms.

2. Lone or nonbonding, pairs of electrons are on one atom and are not shared.

Lewis structures are representations of the covalent bond. In this Lewis symbols show how the valence electrons are present in the molecule.

Steps to write Lewis structures are as follows:

1. The skeleton structure with single bonds between all bonded atoms has to be written

2. Sum the valence electrons of the atoms in the molecule.

(a) For cations, one electron is subtracted for each positive charge.

(b) For anions, one electron is added for each negative charge.

3. Subtract two electrons for each bond in the skeleton structure.

4. Count the number of electrons needed to satisfy the octet rule for each atom in the structure. If the number of electrons needed is less than the number remaining, add one bond for every two electrons needed between atoms to attain an octet.

5 The remaining electrons are placed as lone pairs on atoms that need them to satisfy the octet rule.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of H2CO has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

Refer to part (a)

Answer 9

(b)

Interpretation Introduction

Interpretation:

The Lewis structure of H2CO has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

Refer to part (a)

Answer 10

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of PF3 has to be determined. Also, the bonding and lone pairs in the structure have to be labelled.

Concept Introduction:

Refer to part (a)

Answer 11

(c)

Interpretation Introduction

Interpretation:

The Lewis structure of PF3 has to be determined. Also, the bonding and lone pairs in the structure have to be labelled.

Concept Introduction:

Refer to part (a)

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 9 - Prob. 9.1QE Ch. 9 - Prob. 9.2QE Ch. 9 - Prob. 9.3QE Ch. 9 - What main factors control the magnitude of lattice...Ch. 9 - Prob. 9.5QE Ch. 9 - Prob. 9.6QE Ch. 9 - Prob. 9.7QE Ch. 9 - Prob. 9.8QE Ch. 9 - Prob. 9.9QE Ch. 9 - Prob. 9.10QE

Solution Summary: The author explains how the Lewis structure is determined, and the bonding and lone pairs in the structure have to be labeled.

Concept explainers

Videos

Interpretation:

The Lewis structure of H2CO has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

Refer to part (a)

Interpretation:

The Lewis structure of PF3 has to be determined. Also, the bonding and lone pairs in the structure have to be labelled.

Concept Introduction:

Refer to part (a)

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Chapter 9 Solutions

Solution Summary: The author explains how the Lewis structure is determined, and the bonding and lone pairs in the structure have to be labeled.

Concept explainers

Videos

Interpretation: The Lewis structure of H2CO has to be determined. Also, the bonding and lone pairs in the structure have to be labeled. Concept Introduction: Refer to part (a)

Interpretation: The Lewis structure of PF3 has to be determined. Also, the bonding and lone pairs in the structure have to be labelled. Concept Introduction: Refer to part (a)

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Chapter 9 Solutions

Interpretation:

The Lewis structure of H2CO has to be determined. Also, the bonding and lone pairs in the structure have to be labeled.

Concept Introduction:

Refer to part (a)

Interpretation:

The Lewis structure of PF3 has to be determined. Also, the bonding and lone pairs in the structure have to be labelled.

Concept Introduction:

Refer to part (a)