For the given ions, Lewis structure should be drawn and formal charges should be shown Concept introduction: Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule. Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms. Formal charge of an atom can be determined by the given formula. Formal charge ( F C ) = ( number of valence electron in atom ) − 1 2 ( number of bonding electrons ) − ( number of non-bonding electrons )

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Answer 1

Question

Chapter 6, Problem 6.29QP

(a)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(a)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 1

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 2

The given molecule contains one nitrogen atom and two oxygen atom with it.

The Nitrogen has totally 7 electrons with 4 valence electrons due to the presence of positive charges and the number of electrons present in the oxygen is 8 with 6 valence electrons with it. The number of bonds present in primary structure of given molecule is two single bonds which forms in expense of eight electrons.

Hence, eight have to be subtracted with the total electrons present in the structure that results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge can be shown as

Formal charge on nitrogen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 5Number of bonding electrons = 8Number of non-bonding electrons = 0$

$FC = 5− 12(8)= +1$

Formal charge on oxygen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 6− 12(4)−4= 0$

(b)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

To draw: Lewis structure of the ions.

(b)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 3

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 4

The given molecule contains one carbon atom one sulfur atoms and one nitrogen atom with it.

The S atom has totally 16 electrons with 6 valence electrons. And the number of electrons present in C atom is 6 with 4 valence electrons with it number of electrons present in the nitrogen atom is 7 with five valence electrons. The number of bonds present in the primary structure of the given molecule is one single bond and one triple bond which form in the expense of 8 electrons.

Hence, 8have to subtract with the total electrons present in the structure those results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge on carbon atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 4Number of bonding electrons = 8$

$FC = 4− 12(8)= 0$

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

(c)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(c)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 5

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 6

The given molecule contains 2 sulfur atoms,

The S atom has totally 16 electrons with 6 valence electrons. The number of bonds present in the primary structure of the given molecule is 1 single bond which form in the expense of 2 electrons

Hence, 2 have to subtracted with the total electrons present in the structure that results in 12 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

(d)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(d)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 7

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 8

The given molecule contains two fluorine atom and one chlorine atom n atom with it.

The number of electrons present in the Chlorine is 17 with 7 valence electrons with it. The number of electrons present in the fluorine atom is 9 with 7 valence electrons. The number of bonds present in the primary structure of the given molecule is two single bond expenses of 4 electrons.

Hence, 4 have to subtracted with the total electrons present in the structure that results in 16 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on fluorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 7− 12(2)−6= 0$

Formal charge on chlorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 7− 12(4)−4= +1$

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Students have asked these similar questions

Instructions: Complete the questions in the space provided. Show all your work 1. You are trying to determine the rate law expression for a reaction that you are completing at 25°C. You measure the initial reaction rate and the starting concentrations of the reactions for 4 trials. BrO³¯ (aq) + 5Br¯ (aq) + 6H* (aq) → 3Br₂ (l) + 3H2O (l) Initial rate Trial [BrO3] [H*] [Br] (mol/L) (mol/L) | (mol/L) (mol/L.s) 1 0.10 0.10 0.10 8.0 2 0.20 0.10 0.10 16 3 0.10 0.20 0.10 16 4 0.10 0.10 0.20 32 a. Based on the above data what is the rate law expression? b. Solve for the value of k (make sure to include proper units) 2. The proposed reaction mechanism is as follows: i. ii. BrО¸¯ (aq) + H+ (aq) → HBrO3 (aq) HBrO³ (aq) + H* (aq) → H₂BrO3* (aq) iii. H₂BrO³* (aq) + Br¯ (aq) → Br₂O₂ (aq) + H2O (l) [Fast] [Medium] [Slow] iv. Br₂O₂ (aq) + 4H*(aq) + 4Br‍(aq) → 3Br₂ (l) + H2O (l) [Fast] Evaluate the validity of this proposed reaction. Justify your answer.

е. Д CH3 D*, D20

C. NaOMe, Br Br

Answer 2

Question

Chapter 6, Problem 6.29QP

(a)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(a)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 1

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 2

The given molecule contains one nitrogen atom and two oxygen atom with it.

The Nitrogen has totally 7 electrons with 4 valence electrons due to the presence of positive charges and the number of electrons present in the oxygen is 8 with 6 valence electrons with it. The number of bonds present in primary structure of given molecule is two single bonds which forms in expense of eight electrons.

Hence, eight have to be subtracted with the total electrons present in the structure that results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge can be shown as

Formal charge on nitrogen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 5Number of bonding electrons = 8Number of non-bonding electrons = 0$

$FC = 5− 12(8)= +1$

Formal charge on oxygen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 6− 12(4)−4= 0$

(b)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

To draw: Lewis structure of the ions.

(b)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 3

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 4

The given molecule contains one carbon atom one sulfur atoms and one nitrogen atom with it.

The S atom has totally 16 electrons with 6 valence electrons. And the number of electrons present in C atom is 6 with 4 valence electrons with it number of electrons present in the nitrogen atom is 7 with five valence electrons. The number of bonds present in the primary structure of the given molecule is one single bond and one triple bond which form in the expense of 8 electrons.

Hence, 8have to subtract with the total electrons present in the structure those results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge on carbon atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 4Number of bonding electrons = 8$

$FC = 4− 12(8)= 0$

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

(c)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(c)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 5

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 6

The given molecule contains 2 sulfur atoms,

The S atom has totally 16 electrons with 6 valence electrons. The number of bonds present in the primary structure of the given molecule is 1 single bond which form in the expense of 2 electrons

Hence, 2 have to subtracted with the total electrons present in the structure that results in 12 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

(d)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(d)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 7

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 8

The given molecule contains two fluorine atom and one chlorine atom n atom with it.

The number of electrons present in the Chlorine is 17 with 7 valence electrons with it. The number of electrons present in the fluorine atom is 9 with 7 valence electrons. The number of bonds present in the primary structure of the given molecule is two single bond expenses of 4 electrons.

Hence, 4 have to subtracted with the total electrons present in the structure that results in 16 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on fluorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 7− 12(2)−6= 0$

Formal charge on chlorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 7− 12(4)−4= +1$

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Answer 3

Question

Chapter 6, Problem 6.29QP

(a)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(a)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 1

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 2

The given molecule contains one nitrogen atom and two oxygen atom with it.

The Nitrogen has totally 7 electrons with 4 valence electrons due to the presence of positive charges and the number of electrons present in the oxygen is 8 with 6 valence electrons with it. The number of bonds present in primary structure of given molecule is two single bonds which forms in expense of eight electrons.

Hence, eight have to be subtracted with the total electrons present in the structure that results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge can be shown as

Formal charge on nitrogen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 5Number of bonding electrons = 8Number of non-bonding electrons = 0$

$FC = 5− 12(8)= +1$

Formal charge on oxygen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 6− 12(4)−4= 0$

(b)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

To draw: Lewis structure of the ions.

(b)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 3

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 4

The given molecule contains one carbon atom one sulfur atoms and one nitrogen atom with it.

The S atom has totally 16 electrons with 6 valence electrons. And the number of electrons present in C atom is 6 with 4 valence electrons with it number of electrons present in the nitrogen atom is 7 with five valence electrons. The number of bonds present in the primary structure of the given molecule is one single bond and one triple bond which form in the expense of 8 electrons.

Hence, 8have to subtract with the total electrons present in the structure those results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge on carbon atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 4Number of bonding electrons = 8$

$FC = 4− 12(8)= 0$

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

(c)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(c)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 5

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 6

The given molecule contains 2 sulfur atoms,

The S atom has totally 16 electrons with 6 valence electrons. The number of bonds present in the primary structure of the given molecule is 1 single bond which form in the expense of 2 electrons

Hence, 2 have to subtracted with the total electrons present in the structure that results in 12 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

(d)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(d)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 7

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 8

The given molecule contains two fluorine atom and one chlorine atom n atom with it.

The number of electrons present in the Chlorine is 17 with 7 valence electrons with it. The number of electrons present in the fluorine atom is 9 with 7 valence electrons. The number of bonds present in the primary structure of the given molecule is two single bond expenses of 4 electrons.

Hence, 4 have to subtracted with the total electrons present in the structure that results in 16 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on fluorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 7− 12(2)−6= 0$

Formal charge on chlorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 7− 12(4)−4= +1$

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Answer 4

Question

Chapter 6, Problem 6.29QP

(a)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(a)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 1

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 2

The given molecule contains one nitrogen atom and two oxygen atom with it.

The Nitrogen has totally 7 electrons with 4 valence electrons due to the presence of positive charges and the number of electrons present in the oxygen is 8 with 6 valence electrons with it. The number of bonds present in primary structure of given molecule is two single bonds which forms in expense of eight electrons.

Hence, eight have to be subtracted with the total electrons present in the structure that results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge can be shown as

Formal charge on nitrogen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 5Number of bonding electrons = 8Number of non-bonding electrons = 0$

$FC = 5− 12(8)= +1$

Formal charge on oxygen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 6− 12(4)−4= 0$

(b)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

To draw: Lewis structure of the ions.

(b)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 3

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 4

The given molecule contains one carbon atom one sulfur atoms and one nitrogen atom with it.

The S atom has totally 16 electrons with 6 valence electrons. And the number of electrons present in C atom is 6 with 4 valence electrons with it number of electrons present in the nitrogen atom is 7 with five valence electrons. The number of bonds present in the primary structure of the given molecule is one single bond and one triple bond which form in the expense of 8 electrons.

Hence, 8have to subtract with the total electrons present in the structure those results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge on carbon atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 4Number of bonding electrons = 8$

$FC = 4− 12(8)= 0$

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

(c)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(c)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 5

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 6

The given molecule contains 2 sulfur atoms,

The S atom has totally 16 electrons with 6 valence electrons. The number of bonds present in the primary structure of the given molecule is 1 single bond which form in the expense of 2 electrons

Hence, 2 have to subtracted with the total electrons present in the structure that results in 12 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

(d)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(d)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 7

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 8

The given molecule contains two fluorine atom and one chlorine atom n atom with it.

The number of electrons present in the Chlorine is 17 with 7 valence electrons with it. The number of electrons present in the fluorine atom is 9 with 7 valence electrons. The number of bonds present in the primary structure of the given molecule is two single bond expenses of 4 electrons.

Hence, 4 have to subtracted with the total electrons present in the structure that results in 16 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on fluorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 7− 12(2)−6= 0$

Formal charge on chlorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 7− 12(4)−4= +1$

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Answer 5

Chapter 6, Problem 6.29QP

(a)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(a)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 1

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 2

The given molecule contains one nitrogen atom and two oxygen atom with it.

The Nitrogen has totally 7 electrons with 4 valence electrons due to the presence of positive charges and the number of electrons present in the oxygen is 8 with 6 valence electrons with it. The number of bonds present in primary structure of given molecule is two single bonds which forms in expense of eight electrons.

Hence, eight have to be subtracted with the total electrons present in the structure that results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge can be shown as

Formal charge on nitrogen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 5Number of bonding electrons = 8Number of non-bonding electrons = 0$

$FC = 5− 12(8)= +1$

Formal charge on oxygen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 6− 12(4)−4= 0$

(b)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

To draw: Lewis structure of the ions.

(b)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 3

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 4

The given molecule contains one carbon atom one sulfur atoms and one nitrogen atom with it.

The S atom has totally 16 electrons with 6 valence electrons. And the number of electrons present in C atom is 6 with 4 valence electrons with it number of electrons present in the nitrogen atom is 7 with five valence electrons. The number of bonds present in the primary structure of the given molecule is one single bond and one triple bond which form in the expense of 8 electrons.

Hence, 8have to subtract with the total electrons present in the structure those results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge on carbon atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 4Number of bonding electrons = 8$

$FC = 4− 12(8)= 0$

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

(c)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(c)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 5

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 6

The given molecule contains 2 sulfur atoms,

The S atom has totally 16 electrons with 6 valence electrons. The number of bonds present in the primary structure of the given molecule is 1 single bond which form in the expense of 2 electrons

Hence, 2 have to subtracted with the total electrons present in the structure that results in 12 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

(d)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(d)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 7

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 8

The given molecule contains two fluorine atom and one chlorine atom n atom with it.

The number of electrons present in the Chlorine is 17 with 7 valence electrons with it. The number of electrons present in the fluorine atom is 9 with 7 valence electrons. The number of bonds present in the primary structure of the given molecule is two single bond expenses of 4 electrons.

Hence, 4 have to subtracted with the total electrons present in the structure that results in 16 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on fluorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 7− 12(2)−6= 0$

Formal charge on chlorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 7− 12(4)−4= +1$

Answer 6

Chapter 6, Problem 6.29QP

(a)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(a)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 1

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 2

The given molecule contains one nitrogen atom and two oxygen atom with it.

The Nitrogen has totally 7 electrons with 4 valence electrons due to the presence of positive charges and the number of electrons present in the oxygen is 8 with 6 valence electrons with it. The number of bonds present in primary structure of given molecule is two single bonds which forms in expense of eight electrons.

Hence, eight have to be subtracted with the total electrons present in the structure that results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge can be shown as

Formal charge on nitrogen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 5Number of bonding electrons = 8Number of non-bonding electrons = 0$

$FC = 5− 12(8)= +1$

Formal charge on oxygen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 6− 12(4)−4= 0$

Answer 7

Chapter 6, Problem 6.29QP

(a)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

Answer 8

(a)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 1

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 2

The given molecule contains one nitrogen atom and two oxygen atom with it.

The Nitrogen has totally 7 electrons with 4 valence electrons due to the presence of positive charges and the number of electrons present in the oxygen is 8 with 6 valence electrons with it. The number of bonds present in primary structure of given molecule is two single bonds which forms in expense of eight electrons.

Hence, eight have to be subtracted with the total electrons present in the structure that results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge can be shown as

Formal charge on nitrogen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 5Number of bonding electrons = 8Number of non-bonding electrons = 0$

$FC = 5− 12(8)= +1$

Formal charge on oxygen atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 6− 12(4)−4= 0$

Answer 13

(b)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

To draw: Lewis structure of the ions.

(b)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 3

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 4

The given molecule contains one carbon atom one sulfur atoms and one nitrogen atom with it.

The S atom has totally 16 electrons with 6 valence electrons. And the number of electrons present in C atom is 6 with 4 valence electrons with it number of electrons present in the nitrogen atom is 7 with five valence electrons. The number of bonds present in the primary structure of the given molecule is one single bond and one triple bond which form in the expense of 8 electrons.

Hence, 8have to subtract with the total electrons present in the structure those results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge on carbon atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 4Number of bonding electrons = 8$

$FC = 4− 12(8)= 0$

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

Answer 14

(b)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

To draw: Lewis structure of the ions.

Answer 15

(b)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 3

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 4

The given molecule contains one carbon atom one sulfur atoms and one nitrogen atom with it.

The S atom has totally 16 electrons with 6 valence electrons. And the number of electrons present in C atom is 6 with 4 valence electrons with it number of electrons present in the nitrogen atom is 7 with five valence electrons. The number of bonds present in the primary structure of the given molecule is one single bond and one triple bond which form in the expense of 8 electrons.

Hence, 8have to subtract with the total electrons present in the structure those results in 8 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration.

Formal charge on carbon atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 4Number of bonding electrons = 8$

$FC = 4− 12(8)= 0$

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

Answer 20

(c)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(c)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 5

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 6

The given molecule contains 2 sulfur atoms,

The S atom has totally 16 electrons with 6 valence electrons. The number of bonds present in the primary structure of the given molecule is 1 single bond which form in the expense of 2 electrons

Hence, 2 have to subtracted with the total electrons present in the structure that results in 12 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

Answer 21

(c)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

Answer 22

(c)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 5

Answer 23

(c)

Expert Solution

Answer 24

(c)

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 6

The given molecule contains 2 sulfur atoms,

The S atom has totally 16 electrons with 6 valence electrons. The number of bonds present in the primary structure of the given molecule is 1 single bond which form in the expense of 2 electrons

Hence, 2 have to subtracted with the total electrons present in the structure that results in 12 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on sulfur atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 6Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 6− 12(2)−6= −1$

Answer 27

(d)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

(d)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 7

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 8

The given molecule contains two fluorine atom and one chlorine atom n atom with it.

The number of electrons present in the Chlorine is 17 with 7 valence electrons with it. The number of electrons present in the fluorine atom is 9 with 7 valence electrons. The number of bonds present in the primary structure of the given molecule is two single bond expenses of 4 electrons.

Hence, 4 have to subtracted with the total electrons present in the structure that results in 16 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on fluorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 2Number of non-bonding electrons = 6$

$FC = 7− 12(2)−6= 0$

Formal charge on chlorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$

$Number of valenceelectrons = 7Number of bonding electrons = 4Number of non-bonding electrons = 4$

$FC = 7− 12(4)−4= +1$

Answer 28

(d)

Interpretation Introduction

Interpretation:

For the given ions, Lewis structure should be drawn and formal charges should be shown

Concept introduction:

Lewis structures is also known as Lewis dot structures which represents the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

Formal charge (FC) is the charge assigned to an atom in a molecule, irrespective of relative electronegativity by thinking that electrons in all chemical bonds are shared equally among atoms.

Formal charge of an atom can be determined by the given formula.
$Formal charge (F C) = (number of valence electron in atom)−12(number of bonding electrons)−(number of non-bonding electrons)$

Answer 29

(d)

Expert Solution

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 7

Answer 30

(d)

Expert Solution

Answer 31

(d)

Expert Solution

Answer 32

Expert Solution

Answer 33

Explanation of Solution

Chemistry Atoms First, Second Edition, Chapter 6, Problem 6.29QP , additional homework tip 8

The given molecule contains two fluorine atom and one chlorine atom n atom with it.

The number of electrons present in the Chlorine is 17 with 7 valence electrons with it. The number of electrons present in the fluorine atom is 9 with 7 valence electrons. The number of bonds present in the primary structure of the given molecule is two single bond expenses of 4 electrons.

Hence, 4 have to subtracted with the total electrons present in the structure that results in 16 electrons which finally has to be distributed over the atoms present in the given molecule such that each atom fulfills its octet configuration

Formal charge on fluorine atom

$Formal charge (F C) = (no.of valence electron in atom)−12(no.of bonding electrons)−(no.of non-bonding electrons)$