Chapter 14, Problem 19E

(a)

Interpretation Introduction

Interpretation: The hybridization for HCN molecule 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 on each bonded atoms. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

The sum of valence electrons must be arranged in such a way that all atoms have complete octet.

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

• 
• sp hybridization

Explanation of Solution

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 HCN:

  $(1\times 1)+(4\times 1)+(5\times 1)=10$

Hence the best Lewis structure for HCN must be:

  

Hybridization of a molecule can be checked with the help of below formula:

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ \text{Hybridization = }2\text{ + 0 = 2 = sp}\end{array}$

(b)

Interpretation Introduction

Interpretation: The hybridization of ${\text{PH}}_{\text{3}}$ 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 on each bonded atoms. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

The sum of valence electrons must be arranged in such a way that all atoms have complete octet.

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  

  ${\text{sp}}^{\text{3}}$ hybridization

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 ${\text{PH}}_{\text{3}}$ :

  $(3\times 1)+(5\times 1)=8$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ \text{Hybridization = }3{\text{ + 1 = 4 = sp}}^{\text{3}}\end{array}$

(c)

Interpretation Introduction

Interpretation: The hybridization of ${\text{CHCl}}_{\text{3}}$ 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 on each bonded atoms. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

The sum of valence electrons must be arranged in such a way that all atoms have complete octet.

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  

  ${\text{sp}}^{\text{3}}$ hybridization

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 ${\text{CHCl}}_{\text{3}}$ :

  $(1\times 4)+(3\times 1)+(7\times 1)=14$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ \text{Hybridization = }4{\text{ + 0 = 4 = sp}}^{\text{3}}\end{array}$

(d)

Interpretation Introduction

Interpretation: The hybridization of ${\text{NH}}_4^{+}$ 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.

The sum of valence electrons must be arranged in such a way that all atoms must get octet configuration (8 electrons).

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  

  ${\text{sp}}^{\text{3}}$ hybridization

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 ${\text{NH}}_4^{+}$ :

  $(1\times 5)+(4\times 1)-1=8$

Hence the best Lewis structure for ${\text{NH}}_4^{+}$ must be:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ \text{Hybridization = }4{\text{ + 0 = 4 = sp}}^{\text{3}}\end{array}$

(e)

Interpretation Introduction

Interpretation: The hybridization of ${\text{H}}_{\text{2}}\text{CO}$ 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 on each bonded atoms. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

The sum of valence electrons must be arranged in such a way that all atoms have complete octet.

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  

  ${\text{sp}}^{\text{2}}$ hybridization

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 ${\text{H}}_{\text{2}}\text{CO}$ :

  $(2\times 1)+(1\times 4)+(1\times 6)=12$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ \text{Hybridization =}3{\text{ + 0 = 3 = sp}}^{\text{2}}\end{array}$

(f)

Interpretation Introduction

Interpretation: The hybridization of ${\text{SeF}}_{\text{2}}$ 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.

The sum of valence electrons must be arranged in such a way that all atoms must get octet configuration (8 electrons).

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  

  ${\text{sp}}^{\text{3}}$ hybridization

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 ${\text{SeF}}_{\text{2}}$ :

  $(1\times 6)+(2\times 7)=20$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =2 + 2 = 4 = sp}}^{\text{3}}\end{array}$

(g)

Interpretation Introduction

Interpretation: The hybridization of ${\text{CO}}_{\text{2}}$ 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.

The sum of valence electrons must be arranged in such a way that all atoms must get octet configuration (8 electrons).

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  

sp- hybridization

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 ${\text{CO}}_{\text{2}}$ :

  $(1\times 4)+(2\times 6)=16$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ \text{Hybridization =2 +0 = 2 = sp}\end{array}$

(h)

Interpretation Introduction

Interpretation: The hybridization of ${\text{O}}_{\text{2}}$ 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.

The sum of valence electrons must be arranged in such a way that all atoms must get octet configuration (8 electrons).

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  

  ${\text{sp}}^{\text{2}}$ hybridization

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 ${\text{O}}_{\text{2}}$ :

  $(2\times 6)=12$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =1 + 2 = 3 = sp}}^{\text{2}}\end{array}$

(i)

Interpretation Introduction

Interpretation: The hybridization of HBr 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 on each bonded atoms. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

The sum of valence electrons must be arranged in such a way that all atoms have complete octet.

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  

  ${\text{sp}}^{\text{3}}$ hybridization

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 $\text{HBr}$ :

  $(1\times 1)+(1\times 7)=8$

Hence the best Lewis structure for $\text{HBr}$ must be:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =1 + 3 =4 = sp}}^{\text{3}}\end{array}$

(j)

Interpretation Introduction

Interpretation: The hybridization of ${\text{POCl}}_{\text{3}}{\text{, SO}}_{\text{4}}{}^{\text{2-}}{\text{, XeO}}_{\text{4}}{\text{, PO}}_{\text{4}}{}^{\text{3-}}{\text{, ClO}}_{\text{4}}{}^{\text{-}}$ 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.

The sum of valence electrons must be arranged in such a way that all atoms must get octet configuration (8 electrons).

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  ${\text{POCl}}_{\text{3}}{\text{, SO}}_{\text{4}}{}^{\text{2-}}{\text{, XeO}}_{\text{4}}{\text{, PO}}_{\text{4}}{}^{\text{3-}}{\text{, ClO}}_{\text{4}}{}^{\text{-}}$ = ${\text{sp}}^{\text{3}}$ hybridize

Explanation of Solution

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:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =4 + 0 =4 = sp}}^{\text{3}}\end{array}$

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:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =4 + 0 =4 = sp}}^{\text{3}}\end{array}$

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:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =4 + 0 =4 = sp}}^{\text{3}}\end{array}$

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:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =4 + 0 =4 = sp}}^{\text{3}}\end{array}$

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:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =4 + 0 =4 = sp}}^{\text{3}}\end{array}$

(k)

Interpretation Introduction

Interpretation: The hybridization of ${\text{NF}}_{\text{3}}{\text{, SO}}_3{}^{\text{2-}}{\text{, PO}}_3{}^{\text{3-}}{\text{, ClO}}_{\text{3}}{}^{\text{-}}$ 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.

The sum of valence electrons must be arranged in such a way that all atoms must get octet configuration (8 electrons).

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  ${\text{NF}}_{\text{3}}{\text{, SO}}_3{}^{\text{2-}}{\text{, PO}}_3{}^{\text{3-}}{\text{, ClO}}_{\text{3}}{}^{\text{-}}$ = ${\text{sp}}^{\text{3}}$ hybridization

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 ${\text{NF}}_{\text{3}}$ :

  $(1\times 5)+(3\times 7)=26$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =3 + 1 =4 = sp}}^{\text{3}}\end{array}$

Total number of valence electrons in ${\text{SO}}_3{}^{\text{2-}}$ :

  $(1\times 6)+(3\times 6)+2=26$

Hence the best Lewis structure for ${\text{SO}}_3{}^{\text{2-}}$ must be:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =3 + 1 =4 = sp}}^{\text{3}}\end{array}$

Total number of valence electrons in ${\text{PO}}_3{}^{\text{3-}}$ :

  $(1\times 5)+(3\times 6)+3=26$

Hence the best Lewis structure for ${\text{PO}}_3{}^{\text{3-}}$ must be:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =3 + 1 =4 = sp}}^{\text{3}}\end{array}$

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:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =3 + 1 =4 = sp}}^{\text{3}}\end{array}$

(l)

Interpretation Introduction

Interpretation: The hybridization of ${\text{ClO}}_{\text{2}}^{\text{-}}{\text{, SCl}}_{\text{2}}{\text{, PCl}}_{\text{2}}{}^{\text{-}}$ 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.

The sum of valence electrons must be arranged in such a way that all atoms must get octet configuration (8 electrons).

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  ${\text{ClO}}_{\text{2}}^{\text{-}}{\text{, SCl}}_{\text{2}}{\text{, PCl}}_{\text{2}}{}^{\text{-}}$ = ${\text{sp}}^{\text{3}}$

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 ${\text{ClO}}_{\text{2}}^{\text{-}}$ :

  $(1\times 7)+(2\times 6)+1=20$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =2+ 2 =4 = sp}}^{\text{3}}\end{array}$

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

  $(1\times 6)+(2\times 7)=20$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =2+ 2 =4 = sp}}^{\text{3}}\end{array}$

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

  $(1\times 5)+(2\times 7)+1=20$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization =2+ 2 =4 = sp}}^{\text{3}}\end{array}$

(m)

Interpretation Introduction

Interpretation: The hybridization of ${\text{N}}_{\text{2}}{\text{O}}_4{\text{,NO}}_{\text{2}}{}^{\text{-}}{\text{,NO}}_{\text{3}}{}^{\text{-}}$ 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 present on bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

The sum of valence electrons must be arranged in such a way that all atoms must get octet configuration (8 electrons).

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  ${\text{N}}_{\text{2}}{\text{O}}_4{\text{,NO}}_{\text{2}}{}^{\text{-}}{\text{,NO}}_{\text{3}}{}^{\text{-}}$ = ${\text{sp}}^2$ hybridization

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.

According to the given molecular formula, the structure of ${\text{NO}}_{\text{2}}{}^{\text{-}}$ must be:

  $(1\times 5)+(2\times 6)+1=18$

Hence the best Lewis structure for ${\text{NO}}_{\text{2}}{}^{\text{-}}$ must be:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization = 2+ 1 =3 = sp}}^2\end{array}$

According to the given molecular formula, the structure of ${\text{NO}}_{\text{3}}{}^{\text{-}}$ must be:

  $(1\times 5)+(3\times 6)+1=24$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization = 3+ 0 =3 = sp}}^2\end{array}$

According to the given molecular formula, the structure of ${\text{N}}_{\text{2}}{\text{O}}_4$ must be:

  $(2\times 5)+(4\times 6)=34$

Hence the best Lewis structure for ${\text{N}}_{\text{2}}{\text{O}}_4$ must be:

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ {\text{Hybridization = 3+ 0 =3 = sp}}^2\end{array}$

(n)

Interpretation Introduction

Interpretation: The hybridization of ${\text{OCN}}^{\text{-}}{\text{,SCN}}^{\text{-}}{\text{,N}}_{\text{3}}{}^{\text{-}}$ 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 present on each bonded atom. Lewis dot structure is also known as Lewis dot formula or electron dot structure.

The sum of valence electrons must be arranged in such a way that all atoms must get octet configuration (8 electrons).

Hybridization of a molecule can be checked with the help of below formula:

  $\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}$

Answer to Problem 19E

  ${\text{OCN}}^{\text{-}}{\text{,SCN}}^{\text{-}}{\text{,N}}_{\text{3}}{}^{\text{-}}$ = sp hybridization

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.

According to the given molecular formula, the structure of ${\text{OCN}}^{\text{-}}$ must be:

  $(1\times 6)+(1\times 4)+(1\times 5)+1=16$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ \text{Hybridization = 2 + 0 =2 = sp}\end{array}$

According to the given molecular formula, the structure of ${\text{SCN}}^{\text{-}}$ must be:

  $(1\times 6)+(1\times 4)+(1\times 5)+1=16$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ \text{Hybridization = 2 + 0 =2 = sp}\end{array}$

According to the given molecular formula, the structure of ${\text{N}}_{\text{3}}{}^{\text{-}}$ must be:

  $(3\times 5)+1=16$

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

  

  $\begin{array}{l}\text{Hybridization = Number of }\sigma \text{bond + number of lone pair}\\ \text{Hybridization = 2 + 0 =2 = sp}\end{array}$