The possible resonance structures for the following skeleton structure have to be determined. Also, the resonance structure that is the most important has to be identified. Concept Introduction: The 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 that has the lowest group number or lowest electronegativity considered as the central atom. Step 2: Estimate 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. The formula to calculate formal charge of the atom is as follows: Formal charge = ( number of valence electrons ) − ( ( number of lone pairs of electrons ) + ( 1 2 ) ( number of shared electrons ) ) (1) Some molecules and ions do not have one unique Lewis structure. The Lewis structures that differ only in the placement of multiple bonds are called resonance structures. Resonance structures are defined as a set of two or more Lewis structures that collectively describe the electronic bonding. The actual bonding is an average of the bonding in the resonance structures. Also, not all resonance structures contribute equally in every case. Resonance structures that have high formal charges or that place charges of the same sign on adjacent atoms do not contribute to the bonding.

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Answer 1

Question

Chapter 9, Problem 9.67QE

(a)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following skeleton structure have to be determined. Also, the resonance structure that is the most important has to be identified.

Concept Introduction:

The 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 that has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Estimate 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.

The formula to calculate formal charge of the atom is as follows:

Formal charge=(number ofvalenceelectrons)−((number of lone pairs of electrons )+(12) (number of shared electrons)) (1)

Some molecules and ions do not have one unique Lewis structure. The Lewis structures that differ only in the placement of multiple bonds are called resonance structures.

Resonance structures are defined as a set of two or more Lewis structures that collectively describe the electronic bonding. The actual bonding is an average of the bonding in the resonance structures. Also, not all resonance structures contribute equally in every case. Resonance structures that have high formal charges or that place charges of the same sign on adjacent atoms do not contribute to the bonding.

(b)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following structure have to be determined. Also, the resonance structure that is the most important has to be determined.

Concept introduction:

Refer to part (a)

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Draw the Fischer projection from the skeletal structure shown below. HO OH OH OH OH H Q Drawing Atoms, Bonds and Rings Charges I ☐ T HO H H OH HO I CH2OH H OH Drag H OH -CH2OH CHO -COOH Undo Reset Remove Done

please provide the structure for this problem, thank you

Answer 2

Question

Chapter 9, Problem 9.67QE

(a)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following skeleton structure have to be determined. Also, the resonance structure that is the most important has to be identified.

Concept Introduction:

The 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 that has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Estimate 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.

The formula to calculate formal charge of the atom is as follows:

Formal charge=(number ofvalenceelectrons)−((number of lone pairs of electrons )+(12) (number of shared electrons)) (1)

Some molecules and ions do not have one unique Lewis structure. The Lewis structures that differ only in the placement of multiple bonds are called resonance structures.

Resonance structures are defined as a set of two or more Lewis structures that collectively describe the electronic bonding. The actual bonding is an average of the bonding in the resonance structures. Also, not all resonance structures contribute equally in every case. Resonance structures that have high formal charges or that place charges of the same sign on adjacent atoms do not contribute to the bonding.

(b)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following structure have to be determined. Also, the resonance structure that is the most important has to be determined.

Concept introduction:

Refer to part (a)

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Answer 3

Question

Chapter 9, Problem 9.67QE

(a)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following skeleton structure have to be determined. Also, the resonance structure that is the most important has to be identified.

Concept Introduction:

The 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 that has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Estimate 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.

The formula to calculate formal charge of the atom is as follows:

Formal charge=(number ofvalenceelectrons)−((number of lone pairs of electrons )+(12) (number of shared electrons)) (1)

Some molecules and ions do not have one unique Lewis structure. The Lewis structures that differ only in the placement of multiple bonds are called resonance structures.

Resonance structures are defined as a set of two or more Lewis structures that collectively describe the electronic bonding. The actual bonding is an average of the bonding in the resonance structures. Also, not all resonance structures contribute equally in every case. Resonance structures that have high formal charges or that place charges of the same sign on adjacent atoms do not contribute to the bonding.

(b)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following structure have to be determined. Also, the resonance structure that is the most important has to be determined.

Concept introduction:

Refer to part (a)

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Answer 4

Question

Chapter 9, Problem 9.67QE

(a)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following skeleton structure have to be determined. Also, the resonance structure that is the most important has to be identified.

Concept Introduction:

The 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 that has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Estimate 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.

The formula to calculate formal charge of the atom is as follows:

Formal charge=(number ofvalenceelectrons)−((number of lone pairs of electrons )+(12) (number of shared electrons)) (1)

Some molecules and ions do not have one unique Lewis structure. The Lewis structures that differ only in the placement of multiple bonds are called resonance structures.

Resonance structures are defined as a set of two or more Lewis structures that collectively describe the electronic bonding. The actual bonding is an average of the bonding in the resonance structures. Also, not all resonance structures contribute equally in every case. Resonance structures that have high formal charges or that place charges of the same sign on adjacent atoms do not contribute to the bonding.

(b)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following structure have to be determined. Also, the resonance structure that is the most important has to be determined.

Concept introduction:

Refer to part (a)

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Answer 5

Chapter 9, Problem 9.67QE

(a)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following skeleton structure have to be determined. Also, the resonance structure that is the most important has to be identified.

Concept Introduction:

The 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 that has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Estimate 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.

The formula to calculate formal charge of the atom is as follows:

Formal charge=(number ofvalenceelectrons)−((number of lone pairs of electrons )+(12) (number of shared electrons)) (1)

Some molecules and ions do not have one unique Lewis structure. The Lewis structures that differ only in the placement of multiple bonds are called resonance structures.

Resonance structures are defined as a set of two or more Lewis structures that collectively describe the electronic bonding. The actual bonding is an average of the bonding in the resonance structures. Also, not all resonance structures contribute equally in every case. Resonance structures that have high formal charges or that place charges of the same sign on adjacent atoms do not contribute to the bonding.

(b)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following structure have to be determined. Also, the resonance structure that is the most important has to be determined.

Concept introduction:

Refer to part (a)

Answer 6

Chapter 9, Problem 9.67QE

(a)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following skeleton structure have to be determined. Also, the resonance structure that is the most important has to be identified.

Concept Introduction:

The 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 that has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Estimate 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.

The formula to calculate formal charge of the atom is as follows:

Formal charge=(number ofvalenceelectrons)−((number of lone pairs of electrons )+(12) (number of shared electrons)) (1)

Some molecules and ions do not have one unique Lewis structure. The Lewis structures that differ only in the placement of multiple bonds are called resonance structures.

Resonance structures are defined as a set of two or more Lewis structures that collectively describe the electronic bonding. The actual bonding is an average of the bonding in the resonance structures. Also, not all resonance structures contribute equally in every case. Resonance structures that have high formal charges or that place charges of the same sign on adjacent atoms do not contribute to the bonding.

Answer 7

Chapter 9, Problem 9.67QE

(a)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following skeleton structure have to be determined. Also, the resonance structure that is the most important has to be identified.

Concept Introduction:

The 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 that has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Estimate 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.

The formula to calculate formal charge of the atom is as follows:

Formal charge=(number ofvalenceelectrons)−((number of lone pairs of electrons )+(12) (number of shared electrons)) (1)

Some molecules and ions do not have one unique Lewis structure. The Lewis structures that differ only in the placement of multiple bonds are called resonance structures.

Resonance structures are defined as a set of two or more Lewis structures that collectively describe the electronic bonding. The actual bonding is an average of the bonding in the resonance structures. Also, not all resonance structures contribute equally in every case. Resonance structures that have high formal charges or that place charges of the same sign on adjacent atoms do not contribute to the bonding.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following structure have to be determined. Also, the resonance structure that is the most important has to be determined.

Concept introduction:

Refer to part (a)

Answer 9

(b)

Interpretation Introduction

Interpretation:

The possible resonance structures for the following structure have to be determined. Also, the resonance structure that is the most important has to be determined.

Concept introduction:

Refer to part (a)

Answer 10

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Answer 11

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Answer 12

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Answer 13

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 the steps to draw the Lewis structure of the molecule.

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Interpretation:

The possible resonance structures for the following structure have to be determined. Also, the resonance structure that is the most important has to be determined.

Concept introduction:

Refer to part (a)

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Chapter 9 Solutions

Solution Summary: The author explains the steps to draw the Lewis structure of the molecule.

Concept explainers

Videos

Interpretation: The possible resonance structures for the following structure have to be determined. Also, the resonance structure that is the most important has to be determined. Concept introduction: Refer to part (a)

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Chapter 9 Solutions

Interpretation:

The possible resonance structures for the following structure have to be determined. Also, the resonance structure that is the most important has to be determined.

Concept introduction:

Refer to part (a)