The kekule structure should be drawn for the given molecule Concept introduction: Lone-pair electrons are valence electrons that are not used in bonding. A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion. When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond. A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron. kekule structure: Without lone pairs of electros in Lewis structures is known as kekule structure.

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Answer 1

Question

Chapter 1.4, Problem 22P

(a)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(b)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(c)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(d)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

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Answer 2

Question

Chapter 1.4, Problem 22P

(a)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(b)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(c)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(d)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

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Answer 3

Question

Chapter 1.4, Problem 22P

(a)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(b)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(c)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(d)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

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Answer 4

Question

Chapter 1.4, Problem 22P

(a)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(b)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(c)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(d)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

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Answer 5

Chapter 1.4, Problem 22P

(a)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(b)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(c)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

(d)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

Answer 6

Chapter 1.4, Problem 22P

(a)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

Answer 7

Chapter 1.4, Problem 22P

(a)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

Answer 8

(b)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

Answer 9

(b)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

Answer 10

(c)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

Answer 11

(c)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

Answer 12

(d)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

Answer 13

(d)

Interpretation Introduction

Interpretation:

The kekule structure should be drawn for the given molecule

Concept introduction:

Lone-pair electrons are valence electrons that are not used in bonding.

A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.

Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).

Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.

When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.

A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

kekule structure:

Without lone pairs of electros in Lewis structures is known as kekule structure.

Answer 14

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Answer 15

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Answer 16

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Answer 17

Ch. 1.1 - Oxygen has three isotopes, 16O, 17O, and 18O. The...Ch. 1.1 - a. How many protons do the following species...Ch. 1.1 - Chlorine has two isotopes, 35Cl and 37Cl; 75.77%...Ch. 1.2 - Prob. 4P Ch. 1.2 - a. Write the ground-state electronic configuration...Ch. 1.2 - Look at the relative positions of each pair of...Ch. 1.3 - a. Find potassium (K) in the periodic table and...Ch. 1.3 - Which bond is more polar? a. b. c. d.Ch. 1.3 - Which of the following has a. the most polar bond?...Ch. 1.3 - Use the symbols + and to show the direction of...

Solution Summary: The author explains that lone-pair electrons are not used in bonding. A proton is positively charged hydrogen ion.

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