Chapter 13, Problem 86E

(a)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{POCl}}_{\text{3}}$ with minimum formal charge for the given compound 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 existing 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 86E

  

Explanation of Solution

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:

  

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{ on P = 5 - 0 - 5 = 0}\\ \text{FC}\text{}\text{ on Cl = 7 - 6 - 1 = 0}\\ \text{FC}\text{}\text{ on O = 6 - 4 - 2 = 0}\end{array}$

Here all bonded atoms have minimum formal charge therefore it must be the best Lewis structure.

(b)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{SO}}_{\text{4}}{}^{\text{2-}}$ with minimum formal charge for the given ion 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 existing 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 86E

  

Explanation of Solution

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:

  

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

Here all bonded atoms have minimum formal charge therefore it must be the best Lewis structure.

(c)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{ClO}}_{\text{4}}{}^{\text{-}}$ with minimum formal charge for the given ion 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 existing 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 86E

  

Explanation of Solution

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:

  

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

Here all bonded atoms have minimum formal charge therefore it must be the best Lewis structure.

(d)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{PO}}_{\text{4}}{}^{\text{3-}}$ with minimum formal charge for the given ion 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 existing 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 86E

  

Explanation of Solution

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:

  

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

Here all bonded atoms have minimum formal charge therefore it must be the best Lewis structure.

(e)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{SO}}_{\text{2}}{\text{Cl}}_{\text{2}}$ with minimum formal charge for the given compound 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 existing 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 86E

  

Explanation of Solution

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:

  

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

Here all bonded atoms have minimum formal charge therefore it must be the best Lewis structure.

(f)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{XeO}}_{\text{4}}$ with minimum formal charge for the given compound 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 existing 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 86E

  

Explanation of Solution

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:

  

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{ on Xe = 8 - 0 - 8 = 0}\\ \text{FC}\text{}\text{ on O (=O) = 6 - 4 - 2 = 0}\end{array}$

Here all bonded atoms have minimum formal charge therefore it must be the best Lewis structure.

(g)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{ ClO}}_3{}^{\text{-}}$ with minimum formal charge for the given ion 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 existing 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 86E

  

Explanation of Solution

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:

  

  $\begin{array}{l}\text{FC = VE – LE – bond pair}\\ \text{FC}\text{}\text{ on Cl = 7 - 2 - 5 = 0}\\ \text{FC}\text{}\text{ on O( -O) = 6 - 6 - 1 = -1}\\ \text{FC}\text{}\text{ on O (=O) = 6 - 4 - 2 = 0}\end{array}$

Here all bonded atoms have minimum formal charge therefore it must be the best Lewis structure.

(h)

Interpretation Introduction

Interpretation: The Lewis structure for ${\text{NO}}_4{}^{\text{3-}}$ with minimum formal charge for the given ion 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 existing 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 86E

  

Explanation of Solution

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:

  

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

Here all bonded atoms have minimum formal charge therefore it must be the best Lewis structure.