To analyse whether the given molecules follows octet rule or not. 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 3.73P

Interpretation Introduction

Interpretation:

To analyse whether the given molecules follows octet rule or not.

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 3.73P

Interpretation Introduction

Interpretation:

To analyse whether the given molecules follows octet rule or not.

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 3.73P

Interpretation Introduction

Interpretation:

To analyse whether the given molecules follows octet rule or not.

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 3.73P

Interpretation Introduction

Interpretation:

To analyse whether the given molecules follows octet rule or not.

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 3.73P

Interpretation Introduction

Interpretation:

To analyse whether the given molecules follows octet rule or not.

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 3.73P

Interpretation Introduction

Interpretation:

To analyse whether the given molecules follows octet rule or not.

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 3.73P

Interpretation Introduction

Interpretation:

To analyse whether the given molecules follows octet rule or not.

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

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Answer 11

Ch. 3.2 - Problem 3-1 Show how the following chemical...Ch. 3.4 - Problem 3-2 Judging from their relative positions...Ch. 3.5 - Problem 3-3 Write the formulas for the ionic...Ch. 3.6 - Problem 3-4 Name these binary ionic compounds: (a)...Ch. 3.6 - Prob. 3.5P Ch. 3.6 - Problem 3-6 Give each binary compound a systematic...Ch. 3.6 - Problem 3-7 Name these ionic compounds, each of...Ch. 3.7 - Prob. 3.8P Ch. 3.7 - Prob. 3.9P Ch. 3.7 - Prob. 3.10P

Solution Summary: The author analyzes whether the given molecules follow the octet rule or not.

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