(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.

Question

Want to see the full answer?

Answer 1

Question

Chapter 3, Problem 3.72P

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Consider this step in a radical reaction: Br N O hv What type of step is this? Check all that apply. Draw the products of the step on the right-hand side of the drawing area below. If more than one set of products is possible, draw any set. Also, draw the mechanism arrows on the left-hand side of the drawing area to show how this happens. O primary Otermination O initialization O electrophilic O none of the above × ☑

None

Can I get a drawing of what is happening with the orbitals (particularly the p orbital) on the O in the OH group? Is the p orbital on the O involved in the ring resonance? Why or why not?

Answer 2

Question

Chapter 3, Problem 3.72P

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 3, Problem 3.72P

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 3, Problem 3.72P

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 3, Problem 3.72P

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 3.72P

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 3.72P

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

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 15

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 explains how to draw the Lewis structure of a molecule in which carbon atom is bonded to an oxygen.

Concept explainers

Videos

Want to see the full answer?

Chapter 3 Solutions