(a) Interpretation: To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an other carbon atom. Concept Introduction: A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively. Lewis structure of a molecule can be determined as- 1.Calculate the total number of valence electrons.(T.V.E. = a). Sum up all the electrons of all atoms present in the molecule. If the molecule is an anion, add the same number of electrons as the charge present on the ion. If it is a cation, subtract the same number of electrons as the charge present on the ion. 2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for hydrogen (b). 3. Therefore number of bonds formed = b − a 2 4.Remaining electrons are called as lone pairs. 5.Assign formal charges to atoms.

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Answer 1

Question

Chapter 3, Problem 56P

Interpretation Introduction

(a)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an other carbon atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1.Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for hydrogen (b).

3. Therefore number of bonds formed = b−a2

4.Remaining electrons are called as lone pairs.

5.Assign formal charges to atoms.

Interpretation Introduction

(b)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an oxygen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

Interpretation Introduction

(c)

Interpretation:

To draw the Lewis structure for a molecule in which carbon atom is bonded by a double bond to a nitrogen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

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Answer 2

Question

Chapter 3, Problem 56P

Interpretation Introduction

(a)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an other carbon atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1.Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for hydrogen (b).

3. Therefore number of bonds formed = b−a2

4.Remaining electrons are called as lone pairs.

5.Assign formal charges to atoms.

Interpretation Introduction

(b)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an oxygen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

Interpretation Introduction

(c)

Interpretation:

To draw the Lewis structure for a molecule in which carbon atom is bonded by a double bond to a nitrogen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

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Answer 3

Question

Chapter 3, Problem 56P

Interpretation Introduction

(a)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an other carbon atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1.Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for hydrogen (b).

3. Therefore number of bonds formed = b−a2

4.Remaining electrons are called as lone pairs.

5.Assign formal charges to atoms.

Interpretation Introduction

(b)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an oxygen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

Interpretation Introduction

(c)

Interpretation:

To draw the Lewis structure for a molecule in which carbon atom is bonded by a double bond to a nitrogen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

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Answer 4

Question

Chapter 3, Problem 56P

Interpretation Introduction

(a)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an other carbon atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1.Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for hydrogen (b).

3. Therefore number of bonds formed = b−a2

4.Remaining electrons are called as lone pairs.

5.Assign formal charges to atoms.

Interpretation Introduction

(b)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an oxygen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

Interpretation Introduction

(c)

Interpretation:

To draw the Lewis structure for a molecule in which carbon atom is bonded by a double bond to a nitrogen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

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Answer 5

Chapter 3, Problem 56P

Interpretation Introduction

(a)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an other carbon atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1.Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for hydrogen (b).

3. Therefore number of bonds formed = b−a2

4.Remaining electrons are called as lone pairs.

5.Assign formal charges to atoms.

Interpretation Introduction

(b)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an oxygen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

Interpretation Introduction

(c)

Interpretation:

To draw the Lewis structure for a molecule in which carbon atom is bonded by a double bond to a nitrogen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

Answer 6

Chapter 3, Problem 56P

Interpretation Introduction

(a)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an other carbon atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1.Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for hydrogen (b).

3. Therefore number of bonds formed = b−a2

4.Remaining electrons are called as lone pairs.

5.Assign formal charges to atoms.

Answer 7

Chapter 3, Problem 56P

Interpretation Introduction

(a)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an other carbon atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1.Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for hydrogen (b).

3. Therefore number of bonds formed = b−a2

4.Remaining electrons are called as lone pairs.

5.Assign formal charges to atoms.

Answer 8

Interpretation Introduction

(b)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an oxygen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

Answer 9

Interpretation Introduction

(b)

Interpretation:

To draw the Lewis structure of a molecule in which carbon atom is bonded by a double bond to an oxygen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

Answer 10

Interpretation Introduction

(c)

Interpretation:

To draw the Lewis structure for a molecule in which carbon atom is bonded by a double bond to a nitrogen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

Answer 11

Interpretation Introduction

(c)

Interpretation:

To draw the Lewis structure for a molecule in which carbon atom is bonded by a double bond to a nitrogen atom.

Concept Introduction:

A covalent bond is formed by sharing of same number of electrons between two atoms to complete their octet. Atoms taking part in covalent bond formation may share one, two or three electron pairs thus forming single, double and triple bond respectively.

Lewis structure of a molecule can be determined as-

1. Calculate the total number of valence electrons.(T.V.E. = a).
Sum up all the electrons of all atoms present in the molecule.

If the molecule is an anion, add the same number of electrons as the charge present on the ion.

If it is a cation, subtract the same number of electrons as the charge present on the ion.

2. Calculate the total number of electrons required for each atom to have a complete octet or doublet for Hydrogen.(b).

3. Therefore number of bonds formed = b−a2

4. Remaining electrons are called as lone pairs.

5. Assign formal charges to atoms.

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 3.1 - Problem 3-1 Show how the following chemical...Ch. 3.3 - Problem 3-2 Judging from their relative positions...Ch. 3.4 - Problem 3-3 Write the formulas for the ionic...Ch. 3.5 - Problem 3-4 Name these binary ionic compounds: (a)...Ch. 3.5 - Prob. 3.5QC Ch. 3.5 - Problem 3-6 Give each binary compound a systematic...Ch. 3.5 - Problem 3-7 Name these ionic compounds, each of...Ch. 3.6 - Prob. 3.8QC Ch. 3.6 - Prob. 3.9QC Ch. 3.6 - Prob. 3.10QC

Solution Summary: The author explains how to draw the Lewis structure of a molecule in which carbon atom is bonded to an oxygen.

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