The appropriate formal charge of each atoms in given species should be given. Concept introduction: 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. Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms. Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below: Formal charge calculation of molecule or ion =NVE-{LPE+ 1 2 ( BE )

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Answer 1

Question

Chapter 1.4, Problem 12P

(a)

Interpretation Introduction

Interpretation:

The appropriate formal charge of each atoms in given species should be given.

Concept introduction:

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.

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

(b)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

(c)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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

(d)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

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Answer 2

Question

Chapter 1.4, Problem 12P

(a)

Interpretation Introduction

Interpretation:

The appropriate formal charge of each atoms in given species should be given.

Concept introduction:

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.

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

(b)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

(c)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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

(d)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

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Answer 3

Question

Chapter 1.4, Problem 12P

(a)

Interpretation Introduction

Interpretation:

The appropriate formal charge of each atoms in given species should be given.

Concept introduction:

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.

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

(b)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

(c)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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

(d)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

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Answer 4

Question

Chapter 1.4, Problem 12P

(a)

Interpretation Introduction

Interpretation:

The appropriate formal charge of each atoms in given species should be given.

Concept introduction:

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.

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

(b)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

(c)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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

(d)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

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Answer 5

Chapter 1.4, Problem 12P

(a)

Interpretation Introduction

Interpretation:

The appropriate formal charge of each atoms in given species should be given.

Concept introduction:

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.

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

(b)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

(c)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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

(d)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

Answer 6

Chapter 1.4, Problem 12P

(a)

Interpretation Introduction

Interpretation:

The appropriate formal charge of each atoms in given species should be given.

Concept introduction:

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.

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

Answer 7

Chapter 1.4, Problem 12P

(a)

Interpretation Introduction

Interpretation:

The appropriate formal charge of each atoms in given species should be given.

Concept introduction:

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.

Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.

Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:

Formal charge calculation of molecule or ion =NVE-{LPE+12(BE)

Answer 8

(b)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

Answer 9

(b)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

Answer 10

(c)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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

Answer 11

(c)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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

Answer 12

(d)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

Answer 13

(d)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

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.

Answer 14

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Answer 15

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Answer 16

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Answer 17

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