Chapter 13, Problem 85E

(a)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{POCl}}_{\text{3}}$ that obeys the octet rule needs to be drawn.

Concept Introduction:

Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

Formal charge on each atom can be determined with the help of number of valence shell electrons, number of lone pair electrons and bond pair electrons. The formula for the formal charge can be written as:

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{= formal charge}\\ \text{VE = Valence electrons }\\ \text{LE}\text{}\text{= number of lone pair electrons }\\ \text{Bond pair = Number of bond pairs}\end{array}$

Answer to Problem 85E

  

Explanation of Solution

The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.

Total number of valence electrons in ${\text{POCl}}_{\text{3}}$ :

  $(1\times 5)+(1\times 6)+(3\times 7)=32$

Hence the best Lewis structure for ${\text{POCl}}_{\text{3}}$ must be:

  

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{ on P = 5 - 0 -4 = +1}\\ \text{FC}\text{}\text{ on Cl = 7 - 6 - 1 = 0}\\ \text{FC}\text{}\text{ on O = 6 - 6 - 1 = -1}\end{array}$

(b)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{SO}}_{\text{4}}{}^{\text{2-}}$ that obeys the octet rule needs to be determined.

Concept Introduction:

Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

Formal charge on each atom can be determined with the help of number of valence shell electrons, number of lone pair electrons and bond pair electrons. The formula for the formal charge can be written as:

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{= formal charge}\\ \text{VE = Valence electrons }\\ \text{LE}\text{}\text{= number of lone pair electrons }\\ \text{Bond pair = Number of bond pairs}\end{array}$

Answer to Problem 85E

  

Explanation of Solution

The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.

Total number of valence electrons in ${\text{SO}}_{\text{4}}{}^{\text{2-}}$ :

  $(1\times 6)+(4\times 6)+2=32$

Hence the best Lewis structure for ${\text{SO}}_{\text{4}}{}^{\text{2-}}$ must be:

  

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{ on S = 6 - 0 - 4 = +2}\\ \text{FC}\text{}\text{ on O( -O) = 6 - 6 - 1 = -1}\end{array}$

(c)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{ClO}}_{\text{4}}{}^{\text{-}}$ that obeys the octet rule needs to be determined.

Concept Introduction:

Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

Formal charge on each atom can be determined with the help of number of valence shell electrons, number of lone pair electrons and bond pair electrons. The formula for the formal charge can be written as:

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{= formal charge}\\ \text{VE = Valence electrons }\\ \text{LE}\text{}\text{= number of lone pair electrons }\\ \text{Bond pair = Number of bond pairs}\end{array}$

Answer to Problem 85E

  

Explanation of Solution

The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.

Total number of valence electrons in ${\text{ClO}}_{\text{4}}{}^{\text{-}}$ :

  $(1\times 7)+(4\times 6)+1=32$

Hence the best Lewis structure for ${\text{ClO}}_{\text{4}}{}^{\text{-}}$ must be:

  

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{ on Cl = 7 - 0 - 4 = +3}\\ \text{FC}\text{}\text{ on O( -O) = 6 - 6 - 1 = -1}\end{array}$

(d)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{PO}}_{\text{4}}{}^{\text{3-}}$ that obey the octet rule needs to be determined.

Concept Introduction:

Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

Formal charge on each atom can be determined with the help of number of valence shell electrons, number of lone pair electrons and bond pair electrons. The formula for the formal charge can be written as:

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{= formal charge}\\ \text{VE = Valence electrons }\\ \text{LE}\text{}\text{= number of lone pair electrons }\\ \text{Bond pair = Number of bond pairs}\end{array}$

Answer to Problem 85E

  

Explanation of Solution

The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.

Total number of valence electrons in ${\text{PO}}_{\text{4}}{}^{\text{3-}}$ :

  $(1\times 5)+(4\times 6)+3=32$

Hence the best Lewis structure for ${\text{PO}}_{\text{4}}{}^{\text{3-}}$ must be:

  

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{ on P = 5 - 0 - 4 = +1}\\ \text{FC}\text{}\text{ on O( -O) = 6 - 6 - 1 = -1}\end{array}$

(e)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{SO}}_{\text{2}}{\text{Cl}}_{\text{2}}$ that obeys the octet rule needs to be determined.

Concept Introduction:

Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

Formal charge on each atom can be determined with the help of number of valence shell electrons, number of lone pair electrons and bond pair electrons. The formula for the formal charge can be written as:

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{= formal charge}\\ \text{VE = Valence electrons }\\ \text{LE}\text{}\text{= number of lone pair electrons }\\ \text{Bond pair = Number of bond pairs}\end{array}$

Answer to Problem 85E

  

Explanation of Solution

The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.

Total number of valence electrons in ${\text{SO}}_{\text{2}}{\text{Cl}}_{\text{2}}$ :

  $(1\times 6)+(2\times 6)+(2\times 7)=32$

Hence the best Lewis structure for ${\text{SO}}_{\text{2}}{\text{Cl}}_{\text{2}}$ must be:

  

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{ on S = 6 - 0 - 4 = +2}\\ \text{FC}\text{}\text{ on Cl = 7 - 6 - 1 = 0}\\ \text{FC}\text{}\text{ on O = 6 - 6 - 1 = -1}\end{array}$

(f)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{XeO}}_{\text{4}}$ that obeys the octet rule needs to be determined.

Concept Introduction:

Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

Formal charge on each atom can be determined with the help of number of valence shell electrons, number of lone pair electrons and bond pair electrons. The formula for the formal charge can be written as:

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{= formal charge}\\ \text{VE = Valence electrons }\\ \text{LE}\text{}\text{= number of lone pair electrons }\\ \text{Bond pair = Number of bond pairs}\end{array}$

Answer to Problem 85E

  

Explanation of Solution

The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.

Total number of valence electrons in ${\text{XeO}}_{\text{4}}$ :

  $(1\times 8)+(4\times 6)=32$

Hence the best Lewis structure for ${\text{XeO}}_{\text{4}}$ must be:

  

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{ on Xe = 8 - 0 - 4 = +4}\\ \text{FC}\text{}\text{ on O = 6 - 6 -1 =-1}\end{array}$

(g)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{ ClO}}_3{}^{\text{-}}$ that obeys the octet rule needs to be determined.

Concept Introduction:

Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

Formal charge on each atom can be determined with the help of number of valence shell electrons, number of lone pair electrons and bond pair electrons. The formula for the formal charge can be written as:

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{= formal charge}\\ \text{VE = Valence electrons }\\ \text{LE}\text{}\text{= number of lone pair electrons }\\ \text{Bond pair = Number of bond pairs}\end{array}$

Answer to Problem 85E

  

Explanation of Solution

The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.

Total number of valence electrons in ${\text{ClO}}_{\text{3}}{}^{\text{-}}$ :

  $(1\times 7)+(3\times 6)+1=26$

Hence the best Lewis structure for ${\text{ClO}}_{\text{3}}{}^{\text{-}}$ must be:

  

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{ on Cl = 7 - 2 - 4 = +1}\\ \text{FC}\text{}\text{ on O( -O) = 6 - 6 - 1 = -1}\\ \text{FC}\text{}\text{ on O (=O) = 6 - 4 - 2 = 0}\end{array}$

(h)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{NO}}_4{}^{\text{3-}}$ that obeys the octet rule needs to be determined.

Concept Introduction:

Lewis dot structure is the representation which shows the bonding between atoms present in a molecule. It shows lone pairs and bond pairs that exist on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

Formal charge on each atom can be determined with the help of number of valence shell electrons, number of lone pair electrons and bond pair electrons. The formula for the formal charge can be written as:

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{= formal charge}\\ \text{VE = Valence electrons }\\ \text{LE}\text{}\text{= number of lone pair electrons }\\ \text{Bond pair = Number of bond pairs}\end{array}$

Answer to Problem 85E

  

Explanation of Solution

The bond formation between the atoms takes place due to the sharing of valence electrons of bonded atoms while the remaining electrons present in outer shell represented as lone pair of electrons. To draw the Lewis structure, calculate the total number of valence electrons in each atom and draw the structure in such a way that each atom gets its octet configuration.

Total number of valence electrons in ${\text{NO}}_4{}^{\text{3-}}$ :

  $(1\times 5)+(4\times 6)+1=30$

Hence the best Lewis structure for ${\text{NO}}_4{}^{\text{3-}}$ must be:

  

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{ on N = 5 - 2 - 3 = 0}\\ \text{FC}\text{}\text{ on O( -O) = 6 - 6 - 1 = -1}\\ \text{FC}\text{}\text{ on O (=O) = 6 - 4 - 2 = 0}\end{array}$