Lewis structures of all the important resonance forms of N 3 − are to be drawn. Concept introduction: Steps to draw the Lewis structure of the molecule are as follows: Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom. Step 2: Calculate the total number of valence electrons. Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond. Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons. When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

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Answer 1

Question

Chapter 10, Problem 10.11P

(a)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of N3− are to be drawn.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

(b)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of NO2− are to be determined.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

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Answer 2

Question

Chapter 10, Problem 10.11P

(a)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of N3− are to be drawn.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

(b)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of NO2− are to be determined.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

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Answer 3

Question

Chapter 10, Problem 10.11P

(a)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of N3− are to be drawn.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

(b)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of NO2− are to be determined.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

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Answer 4

Question

Chapter 10, Problem 10.11P

(a)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of N3− are to be drawn.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

(b)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of NO2− are to be determined.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

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Answer 5

Chapter 10, Problem 10.11P

(a)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of N3− are to be drawn.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

(b)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of NO2− are to be determined.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

Answer 6

Chapter 10, Problem 10.11P

(a)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of N3− are to be drawn.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

Answer 7

Chapter 10, Problem 10.11P

(a)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of N3− are to be drawn.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

Answer 8

(b)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of NO2− are to be determined.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

Answer 9

(b)

Interpretation Introduction

Interpretation:

Lewis structures of all the important resonance forms of NO2− are to be determined.

Concept introduction:

Steps to draw the Lewis structure of the molecule are as follows:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

When bonds in a molecule can be expressed by different Lewis structures then resonance structures are used to depict the bonding in that molecule. These resonance structures have the same placement of atoms but different locations of bonding and lone pairs of electrons also one resonance form can be converted intoanother by moving lone pairs to bonding positions, and vice versa.

Answer 10

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Ch. 10.1 - Write a Lewis structure for H2S; ; SOCl2. Ch. 10.1 - Prob. 10.1BFP Ch. 10.1 - Prob. 10.2AFP Ch. 10.1 - Prob. 10.2BFP Ch. 10.1 - Prob. 10.3AFP Ch. 10.1 - Prob. 10.3BFP Ch. 10.1 - Prob. 10.4AFP Ch. 10.1 - Prob. 10.4BFP Ch. 10.1 - Write a Lewis structure with minimal formal...Ch. 10.1 - Prob. 10.5BFP

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