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.

  $\text{Formal}\text{charge}\left(\text{F}\text{C}\right)\text{=}\left(\begin{array}{l}\text{number}\text{of}\text{valence}\\ \text{electron}\text{in}\text{atom}\end{array}\right)-\frac{\text{1}}{\text{2}}\left(\begin{array}{l}\text{number}\text{of}\text{bonding}\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{number}\text{of}\text{non-bonding}\\ \text{electrons}\end{array}\right)$

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Explanation of Solution

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

$\text{Formal}\text{charge}\left(\text{F}\text{C}\right)\text{=}\left(\begin{array}{l}\text{no}\text{.of}\text{valence}\\ \text{electron}\text{in}\text{atom}\end{array}\right)-\frac{\text{1}}{\text{2}}\left(\begin{array}{l}\text{no}\text{.of}\text{bonding}\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{no}\text{.of}\text{non-bonding}\\ \text{electrons}\end{array}\right)$

$\begin{array}{c}\text{Number}\text{of}\text{valenceelectrons}\text{=}5\\ \text{Number}\text{of}\text{bonding}\text{electrons}\text{=}8\\ \text{Number}\text{of}\text{non-bonding}\text{electrons}\text{=}\text{0}\end{array}$

$\begin{array}{c}\text{FC}\text{=}5-\frac{\text{1}}{\text{2}}\left(8\right)\\ \text{=}+1\end{array}$

Formal charge on oxygen atom

$\text{Formal}\text{charge}\left(\text{F}\text{C}\right)\text{=}\left(\begin{array}{l}\text{no}\text{.of}\text{valence}\\ \text{electron}\text{in}\text{atom}\end{array}\right)-\frac{\text{1}}{\text{2}}\left(\begin{array}{l}\text{no}\text{.of}\text{bonding}\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{no}\text{.of}\text{non-bonding}\\ \text{electrons}\end{array}\right)$

$\begin{array}{c}\text{Number}\text{of}\text{valenceelectrons}\text{=}6\\ \text{Number}\text{of}\text{bonding}\text{electrons}\text{=}4\\ \text{Number}\text{of}\text{non-bonding}\text{electrons}\text{=}4\end{array}$

$\begin{array}{c}\text{FC}\text{=}6-\frac{\text{1}}{\text{2}}\left(4\right)-4\\ \text{=}0\end{array}$

(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.

  $\text{Formal}\text{charge}\left(\text{F}\text{C}\right)\text{=}\left(\begin{array}{l}\text{number}\text{of}\text{valence}\\ \text{electron}\text{in}\text{atom}\end{array}\right)-\frac{\text{1}}{\text{2}}\left(\begin{array}{l}\text{number}\text{of}\text{bonding}\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{number}\text{of}\text{non-bonding}\\ \text{electrons}\end{array}\right)$

To draw: Lewis structure of the ions.

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Explanation of Solution

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

$\text{Formal}\text{charge}\left(\text{F}\text{C}\right)\text{=}\left(\begin{array}{l}\text{no}\text{.of}\text{valence}\\ \text{electron}\text{in}\text{atom}\end{array}\right)-\frac{\text{1}}{\text{2}}\left(\begin{array}{l}\text{no}\text{.of}\text{bonding}\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{no}\text{.of}\text{non-bonding}\\ \text{electrons}\end{array}\right)$

$\begin{array}{c}\text{Number}\text{of}\text{valenceelectrons}\text{=}4\\ \text{Number}\text{of}\text{bonding}\text{electrons}\text{=}8\\ \end{array}$

$\begin{array}{c}\text{FC}\text{=}4-\frac{\text{1}}{\text{2}}\left(8\right)\\ \text{=}0\end{array}$

Formal charge on sulfur atom

$\text{Formal}\text{charge}\left(\text{F}\text{C}\right)\text{=}\left(\begin{array}{l}\text{no}\text{.of}\text{valence}\\ \text{electron}\text{in}\text{atom}\end{array}\right)-\frac{\text{1}}{\text{2}}\left(\begin{array}{l}\text{no}\text{.of}\text{bonding}\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{no}\text{.of}\text{non-bonding}\\ \text{electrons}\end{array}\right)$

$\begin{array}{c}\text{Number}\text{of}\text{valenceelectrons}\text{=}6\\ \text{Number}\text{of}\text{bonding}\text{electrons}\text{=}2\\ \text{Number}\text{of}\text{non-bonding}\text{electrons}\text{=}6\end{array}$

$\begin{array}{c}\text{FC}\text{=}6-\frac{\text{1}}{\text{2}}\left(2\right)-6\\ \text{=}-1\end{array}$

(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.

  $\text{Formal}\text{charge}\left(\text{F}\text{C}\right)\text{=}\left(\begin{array}{l}\text{number}\text{of}\text{valence}\\ \text{electron}\text{in}\text{atom}\end{array}\right)-\frac{\text{1}}{\text{2}}\left(\begin{array}{l}\text{number}\text{of}\text{bonding}\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{number}\text{of}\text{non-bonding}\\ \text{electrons}\end{array}\right)$

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Explanation of Solution

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

$\text{Formal}\text{charge}\left(\text{F}\text{C}\right)\text{=}\left(\begin{array}{l}\text{no}\text{.of}\text{valence}\\ \text{electron}\text{in}\text{atom}\end{array}\right)-\frac{\text{1}}{\text{2}}\left(\begin{array}{l}\text{no}\text{.of}\text{bonding}\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{no}\text{.of}\text{non-bonding}\\ \text{electrons}\end{array}\right)$

$\begin{array}{c}\text{Number}\text{of}\text{valenceelectrons}\text{=}6\\ \text{Number}\text{of}\text{bonding}\text{electrons}\text{=}2\\ \text{Number}\text{of}\text{non-bonding}\text{electrons}\text{=}6\end{array}$

$\begin{array}{c}\text{FC}\text{=}6-\frac{\text{1}}{\text{2}}\left(2\right)-6\\ \text{=}-1\end{array}$

(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.

  $\text{Formal}\text{charge}\left(\text{F}\text{C}\right)\text{=}\left(\begin{array}{l}\text{number}\text{of}\text{valence}\\ \text{electron}\text{in}\text{atom}\end{array}\right)-\frac{\text{1}}{\text{2}}\left(\begin{array}{l}\text{number}\text{of}\text{bonding}\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{number}\text{of}\text{non-bonding}\\ \text{electrons}\end{array}\right)$

Answer to Problem 6.29QP

Lewis structure and formal charges for the given molecule is,

Explanation of Solution

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

$\text{Formal}\text{charge}\left(\text{F}\text{C}\right)\text{=}\left(\begin{array}{l}\text{no}\text{.of}\text{valence}\\ \text{electron}\text{in}\text{atom}\end{array}\right)-\frac{\text{1}}{\text{2}}\left(\begin{array}{l}\text{no}\text{.of}\text{bonding}\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{no}\text{.of}\text{non-bonding}\\ \text{electrons}\end{array}\right)$

$\begin{array}{c}\text{Number}\text{of}\text{valenceelectrons}\text{=}7\\ \text{Number}\text{of}\text{bonding}\text{electrons}\text{=}2\\ \text{Number}\text{of}\text{non-bonding}\text{electrons}\text{=}6\end{array}$

$\begin{array}{c}\text{FC}\text{=}7-\frac{\text{1}}{\text{2}}\left(2\right)-6\\ \text{=}0\end{array}$

Formal charge on chlorine atom

$\text{Formal}\text{charge}\left(\text{F}\text{C}\right)\text{=}\left(\begin{array}{l}\text{no}\text{.of}\text{valence}\\ \text{electron}\text{in}\text{atom}\end{array}\right)-\frac{\text{1}}{\text{2}}\left(\begin{array}{l}\text{no}\text{.of}\text{bonding}\\ \text{electrons}\end{array}\right)-\left(\begin{array}{l}\text{no}\text{.of}\text{non-bonding}\\ \text{electrons}\end{array}\right)$

$\begin{array}{c}\text{Number}\text{of}\text{valenceelectrons}\text{=}7\\ \text{Number}\text{of}\text{bonding}\text{electrons}\text{=}4\\ \text{Number}\text{of}\text{non-bonding}\text{electrons}\text{=}4\end{array}$

$\begin{array}{c}\text{FC}\text{=}7-\frac{\text{1}}{\text{2}}\left(4\right)-4\\ \text{=}+1\end{array}$