Chapter 14, Problem 24E

(a)

Interpretation Introduction

Interpretation:

The hybrid orbitals should be predicted which is used by sulfur atom(s) in ${\text{SO}}_{\text{2}}$ along with its molecular structure and bond angle.

Concept Introduction:

When two atomic orbitals combine with each other to produce hybrid orbitals, redistribution of energy of orbitals of distinct atoms to form orbitals with equal energy occurs. This process is known as hybridization and the formed new orbitals are known as hybrid orbitals.

When the atomic orbitals overlap with each other in a region of high electron density, then molecular orbitals are formed. Overlapping of atomic orbitals determines the efficiency of interaction between atomic orbitals. Energy of bond molecular orbitals is less than the nonbonding molecular orbitals.

Explanation of Solution

On the basis of types of orbitals involved in mixing, different hybridization is classified as sp, sp², sp³, sp³d, sp³d², sp³d³.

sp-hybridization: It is formed when one s and one p orbital mix with each other in same shell of an tom to produce two new equal orbitals. This hybridization takes place in linear molecules.

  

sp²-hybridization: It is formed when one s and two p orbital mix with each other in same shell of an tom to produce three new equal orbitals. This hybridization takes place in molecules exhibits trigonal planar geometry.

  

sp³-hybridization: It is formed when one s and three p orbital mix with each other in same shell of an tom to produce four new equal orbitals. This hybridization takes place in molecules exhibits tetrahedral geometry. In this hybridization, no p-unhybridized orbital is present as all are hybridized and form four sigma bonds.

The given molecule is ${\text{SO}}_{\text{2}}$ .

Number of valence electrons in sulfur = 6

Number of valence electrons in oxygen = 6

Total number of valence electrons = $\text{6+2}\times \text{6 =18}$

The bonds present between sulfur atom and oxygen atom is sigma and pi bonds and also one lone pair of electrons are present on sulfur atom which pushes the oxygen atom down. Thus, geometry of ${\text{SO}}_{\text{2}}$ is bent and the bond angle is less than 120⁰.

Electronic configuration of sulfur is $1s^{2}2s^{2}2p^{6}3s^{2}3p^4$

Electronic configuration of oxygen is $1s^{2}2s^{2}2p^4$

The sulfur atom uses one $s$ orbital and two $p$ orbitals to form sp² hybridization.

Lewis structure of ${\text{SO}}_{\text{2}}$ is:

  

(b)

Interpretation Introduction

Interpretation:

The hybrid orbitals should be predicted which is used by sulfur atom(s) in ${\text{SO}}_3$ along with its molecular structure and bond angle.

Concept Introduction:

When two atomic orbitals combine with each other to produce hybrid orbitals, redistribution of energy of orbitals of distinct atoms to form orbitals with equal energy occurs. This process is known as hybridization and the formed new orbitals are known as hybrid orbitals.

When the atomic orbitals overlap with each other in a region of high electron density, then molecular orbitals are formed. Overlapping of atomic orbitals determines the efficiency of interaction between atomic orbitals. Energy of bond molecular orbitals is less than the nonbonding molecular orbitals.

Explanation of Solution

On the basis of types of orbitals involved in mixing, different hybridization is classified as sp, sp², sp³, sp³d, sp³d², sp³d³.

sp-hybridization: It is formed when one s and one p orbital mix with each other in same shell of an tom to produce two new equal orbitals. This hybridization takes place in linear molecules.

  

sp²-hybridization: It is formed when one s and two p orbital mix with each other in same shell of an tom to produce three new equal orbitals. This hybridization takes place in molecules exhibits trigonal planar geometry.

  

sp³-hybridization: It is formed when one s and three p orbital mix with each other in same shell of an tom to produce four new equal orbitals. This hybridization takes place in molecules exhibits tetrahedral geometry. In this hybridization, no p-unhybridized orbital is present as all are hybridized and form four sigma bonds.

The given molecule is ${\text{SO}}_3$ .

Number of valence electrons in sulfur = 6

Number of valence electrons in oxygen = 6

Total number of valence electrons = $\text{6+3}\times \text{6 =24}$

The bonds present between sulfur atom and oxygen atom is sigma and pi bonds. There are three bond pairs of electrons surrounding the sulfur atom. The oxygen atom which forms double bond with sulfur atom has two lone pairs and remaining two oxygen atoms has three lone pair of electrons.

Thus, geometry of ${\text{SO}}_3$ is trigonal planar and the bond angle is 120⁰.

Electronic configuration of sulfur is $1s^{2}2s^{2}2p^{6}3s^{2}3p^4$

Electronic configuration of oxygen is $1s^{2}2s^{2}2p^4$

The sulfur atom form double bond which each oxygen atom implies one s and two p orbitals are mix with each other to form sp² hybridization.

Lewis structure of ${\text{SO}}_3$ is:

  

(c)

Interpretation Introduction

Interpretation:

The hybrid orbitals should be predicted which is used by sulfur atom(s) in ${\text{S}}_{\text{2}}{\text{O}}_3^{2-}$ along with its molecular structure and bond angle.

  

Concept Introduction:

When two atomic orbitals combine with each other to produce hybrid orbitals, redistribution of energy of orbitals of distinct atoms to form orbitals with equal energy occurs. This process is known as hybridization and the formed new orbitals are known as hybrid orbitals.

When the atomic orbitals overlap with each other in a region of high electron density, then molecular orbitals are formed. Overlapping of atomic orbitals determines the efficiency of interaction between atomic orbitals. Energy of bond molecular orbitals is less than the nonbonding molecular orbitals.

Explanation of Solution

On the basis of types of orbitals involved in mixing, different hybridization is classified as sp, sp², sp³, sp³d, sp³d², sp³d³.

sp-hybridization: It is formed when one s and one p orbital mix with each other in same shell of an tom to produce two new equal orbitals. This hybridization takes place in linear molecules.

  

sp²-hybridization: It is formed when one s and two p orbital mix with each other in same shell of an tom to produce three new equal orbitals. This hybridization takes place in molecules exhibits trigonal planar geometry.

  

sp³-hybridization: It is formed when one s and three p orbital mix with each other in same shell of an tom to produce four new equal orbitals. This hybridization takes place in molecules exhibits tetrahedral geometry. In this hybridization, no p-unhybridized orbital is present as all are hybridized and form four sigma bonds.

The given molecule is ${\text{S}}_{\text{2}}{\text{O}}_3^{2-}$ .

Number of valence electrons in sulfur = 6

Number of valence electrons in oxygen = 6

According to structure of ${\text{S}}_{\text{2}}{\text{O}}_3^{2-}$ , three oxygen atoms and one sulfur atom is linked with central sulfur atom. Also, charge on molecule is -2.

Total number of valence electrons = $\text{2}\times \text{6+3}\times \text{6 +2=32}$

The bonds present between sulfur atom and sulfur atom and one oxygen atom is pi bond and remaining two oxygen atoms are linked by sigma bond.

Thus, geometry of ${\text{S}}_{\text{2}}{\text{O}}_3^{2-}$ is tetrahedral and the bond angle is $109.5°$ .

Electronic configuration of sulfur is $1s^{2}2s^{2}2p^{6}3s^{2}3p^4$

Electronic configuration of oxygen is $1s^{2}2s^{2}2p^4$

The central sulfur atom uses one s-orbital and three p orbitals and thus hybridization of central sulfur atom is sp³

Lewis structure of ${\text{S}}_{\text{2}}{\text{O}}_3^{2-}$ is:

  

(d)

Interpretation Introduction

Interpretation:

The hybrid orbitals should be predicted which is used by sulfur atom(s) in ${\text{S}}_{\text{2}}{\text{O}}_8^{2-}$ along with its molecular structure and bond angle.

  

Concept Introduction:

When two atomic orbitals combine with each other to produce hybrid orbitals, redistribution of energy of orbitals of distinct atoms to form orbitals with equal energy occurs. This process is known as hybridization and the formed new orbitals are known as hybrid orbitals.

When the atomic orbitals overlap with each other in a region of high electron density, then molecular orbitals are formed. Overlapping of atomic orbitals determines the efficiency of interaction between atomic orbitals. Energy of bond molecular orbitals is less than the nonbonding molecular orbitals.

Explanation of Solution

On the basis of types of orbitals involved in mixing, different hybridization is classified as sp, sp², sp³, sp³d, sp³d², sp³d³.

sp-hybridization: It is formed when one s and one p orbital mix with each other in same shell of an tom to produce two new equal orbitals. This hybridization takes place in linear molecules.

  

sp²-hybridization: It is formed when one s and two p orbital mix with each other in same shell of an tom to produce three new equal orbitals. This hybridization takes place in molecules exhibits trigonal planar geometry.

  

sp³-hybridization: It is formed when one s and three p orbital mix with each other in same shell of an tom to produce four new equal orbitals. This hybridization takes place in molecules exhibits tetrahedral geometry. In this hybridization, no p-unhybridized orbital is present as all are hybridized and form four sigma bonds.

The given molecule is ${\text{S}}_{\text{2}}{\text{O}}_8^{2-}$ .

Number of valence electrons in sulfur = 6

Number of valence electrons in oxygen = 6

There are eight oxygen atoms and two sulfur atoms are present in the molecule and charge on the molecule is equal to -2.

Total number of valence electrons = $\text{2}\times \text{6+8}\times \text{6 +2=62}$

Here, each sulfur atom is linked with four oxygen atoms, two oxygen atoms are double bonded and two oxygen atoms are single bonded.

The two oxygen atoms present in the center of the structure are bonded by single bond. By bonding in this way, each atom completes its octet.

Thus, geometry of ${\text{S}}_{\text{2}}{\text{O}}_8^{2-}$ is tetrahedral and the bond angle is $109.5°$ .

Electronic configuration of sulfur is $1s^{2}2s^{2}2p^{6}3s^{2}3p^4$

Electronic configuration of oxygen is $1s^{2}2s^{2}2p^4$

Both sulfur atoms uses one s-orbital and three p orbitals and thus hybridization of both sulfur atoms is sp³

Lewis structure of ${\text{S}}_{\text{2}}{\text{O}}_8^{2-}$ is:

  

(e)

Interpretation Introduction

Interpretation:

The hybrid orbitals should be predicted which is used by sulfur atom(s) in ${\text{SO}}_3^{2-}$ along with its molecular structure and bond angle.

Concept Introduction:

When two atomic orbitals combine with each other to produce hybrid orbitals, redistribution of energy of orbitals of distinct atoms to form orbitals with equal energy occurs. This process is known as hybridization and the formed new orbitals are known as hybrid orbitals.

When the atomic orbitals overlap with each other in a region of high electron density, then molecular orbitals are formed. Overlapping of atomic orbitals determines the efficiency of interaction between atomic orbitals. Energy of bond molecular orbitals is less than the nonbonding molecular orbitals.

Explanation of Solution

On the basis of types of orbitals involved in mixing, different hybridization is classified as sp, sp², sp³, sp³d, sp³d², sp³d³.

sp-hybridization: It is formed when one s and one p orbital mix with each other in same shell of an tom to produce two new equal orbitals. This hybridization takes place in linear molecules.

  

sp²-hybridization: It is formed when one s and two p orbital mix with each other in same shell of an tom to produce three new equal orbitals. This hybridization takes place in molecules exhibits trigonal planar geometry.

  

sp³-hybridization: It is formed when one s and three p orbital mix with each other in same shell of an tom to produce four new equal orbitals. This hybridization takes place in molecules exhibits tetrahedral geometry. In this hybridization, no p-unhybridized orbital is present as all are hybridized and form four sigma bonds.

The given molecule is ${\text{SO}}_3^{2-}$ .

Number of valence electrons in sulfur = 6

Number of valence electrons in oxygen = 6

There are three oxygen atoms and one sulfur atom present in the molecule and charge on the molecule is equal to -2.

Total number of valence electrons = $\text{1}\times \text{6+3}\times \text{6 +2=26}$

Here, sulfur atom is linked with three oxygen atoms where two oxygen atoms are single bonded with sulfur and one oxygen atom is double bonded with sulfur. By bonding in this way, each atom completes its octet.

Thus, geometry of ${\text{SO}}_3^{2-}$ is trigonal pyramidal and the bond angle is $109.5°$ .

Electronic configuration of sulfur is $1s^{2}2s^{2}2p^{6}3s^{2}3p^4$

Electronic configuration of oxygen is $1s^{2}2s^{2}2p^4$

Sulfur atom uses one s-orbital and three p orbitals and thus hybridization of sulfur atom is sp³

Lewis structure of ${\text{SO}}_3^{2-}$ is:

  

(f)

Interpretation Introduction

Interpretation:

The hybrid orbitals should be predicted which is used by sulfur atom(s) in ${\text{SO}}_4^{2-}$ along with its molecular structure and bond angle.

Concept Introduction:

When two atomic orbitals combine with each other to produce hybrid orbitals, redistribution of energy of orbitals of distinct atoms to form orbitals with equal energy occurs. This process is known as hybridization and the formed new orbitals are known as hybrid orbitals.

When the atomic orbitals overlap with each other in a region of high electron density, then molecular orbitals are formed. Overlapping of atomic orbitals determines the efficiency of interaction between atomic orbitals. Energy of bond molecular orbitals is less than the nonbonding molecular orbitals.

Explanation of Solution

On the basis of types of orbitals involved in mixing, different hybridization is classified as sp, sp², sp³, sp³d, sp³d², sp³d³.

sp-hybridization: It is formed when one s and one p orbital mix with each other in same shell of an tom to produce two new equal orbitals. This hybridization takes place in linear molecules.

  

sp²-hybridization: It is formed when one s and two p orbital mix with each other in same shell of an tom to produce three new equal orbitals. This hybridization takes place in molecules exhibits trigonal planar geometry.

  

sp³-hybridization: It is formed when one s and three p orbital mix with each other in same shell of an tom to produce four new equal orbitals. This hybridization takes place in molecules exhibits tetrahedral geometry. In this hybridization, no p-unhybridized orbital is present as all are hybridized and form four sigma bonds.

The given molecule is ${\text{SO}}_4^{2-}$ .

Number of valence electrons in sulfur = 6

Number of valence electrons in oxygen = 6

There are four oxygen atoms and one sulfur atom present in the molecule and charge on the molecule is equal to -2.

Total number of valence electrons = $\text{1}\times \text{6+4}\times \text{6 +2=32}$

Here, sulfur atom is linked with four oxygen atoms where two oxygen atoms are single bonded with sulfur and two oxygen atoms are double bonded with sulfur. By bonding in this way, each atom completes its octet.

Thus, geometry of ${\text{SO}}_4^{2-}$ is tetrahedral and the bond angle is $109.5°$ . The sulfur atom is linked with four oxygen atoms and has no lone pairs.

Electronic configuration of sulfur is $1s^{2}2s^{2}2p^{6}3s^{2}3p^4$

Electronic configuration of oxygen is $1s^{2}2s^{2}2p^4$

Sulfur atom uses one s-orbital and three p orbitals and thus hybridization of sulfur atom is sp³

Lewis structure of ${\text{SO}}_4^{2-}$ is:

  

(g)

Interpretation Introduction

Interpretation:

The hybrid orbitals should be predicted which is used by sulfur atom(s) in ${\text{SF}}_{\text{2}}$ along with its molecular structure and bond angle.

Concept Introduction:

When two atomic orbitals combine with each other to produce hybrid orbitals, redistribution of energy of orbitals of distinct atoms to form orbitals with equal energy occurs. This process is known as hybridization and the formed new orbitals are known as hybrid orbitals.

When the atomic orbitals overlap with each other in a region of high electron density, then molecular orbitals are formed. Overlapping of atomic orbitals determines the efficiency of interaction between atomic orbitals. Energy of bond molecular orbitals is less than the nonbonding molecular orbitals.

Explanation of Solution

On the basis of types of orbitals involved in mixing, different hybridization is classified as sp, sp², sp³, sp³d, sp³d², sp³d³.

sp-hybridization: It is formed when one s and one p orbital mix with each other in same shell of an tom to produce two new equal orbitals. This hybridization takes place in linear molecules.

  

sp²-hybridization: It is formed when one s and two p orbital mix with each other in same shell of an tom to produce three new equal orbitals. This hybridization takes place in molecules exhibits trigonal planar geometry.

  

sp³-hybridization: It is formed when one s and three p orbital mix with each other in same shell of an tom to produce four new equal orbitals. This hybridization takes place in molecules exhibits tetrahedral geometry. In this hybridization, no p-unhybridized orbital is present as all are hybridized and form four sigma bonds.

The given molecule is ${\text{SF}}_{\text{2}}$ .

Number of valence electrons in sulfur = 6

Number of valence electrons in fluorine = 7

There are twofluorine atoms and one sulfur atom present in the molecule and charge on the molecule is equal to 0.

Total number of valence electrons = $\text{1}\times \text{6+2}\times \text{7 = 20}$

Here, sulfur atom is linked with two fluorine atoms by sigma bond. By bonding in this way, each atom completes its octet.

Thus, geometry of ${\text{SF}}_{\text{2}}$ is bent because of the presence of lone pair of electrons on sulfur atom and the bond angle is less than $109.5°$ .

Electronic configuration of sulfur is $1s^{2}2s^{2}2p^{6}3s^{2}3p^4$

Electronic configuration of fluorine is $1s^{2}2s^{2}2p^5$

Sulfur atom uses one s-orbital and three p orbitals and thus hybridization of sulfur atom is sp³ implies hybrid orbitals are present.

Lewis structure of ${\text{SF}}_{\text{2}}$ is:

  

(h)

Interpretation Introduction

Interpretation:

The hybrid orbitals should be predicted which is used by sulfur atom(s) in ${\text{SF}}_4$ along with its molecular structure and bond angle.

Concept Introduction:

When two atomic orbitals combine with each other to produce hybrid orbitals, redistribution of energy of orbitals of distinct atoms to form orbitals with equal energy occurs. This process is known as hybridization and the formed new orbitals are known as hybrid orbitals.

When the atomic orbitals overlap with each other in a region of high electron density, then molecular orbitals are formed. Overlapping of atomic orbitals determines the efficiency of interaction between atomic orbitals. Energy of bond molecular orbitals is less than the nonbonding molecular orbitals.

Explanation of Solution

On the basis of types of orbitals involved in mixing, different hybridization is classified as sp, sp², sp³, sp³d, sp³d², sp³d³.

sp-hybridization: It is formed when one s and one p orbital mix with each other in same shell of an tom to produce two new equal orbitals. This hybridization takes place in linear molecules.

  

sp²-hybridization: It is formed when one s and two p orbital mix with each other in same shell of an tom to produce three new equal orbitals. This hybridization takes place in molecules exhibits trigonal planar geometry.

  

sp³-hybridization: It is formed when one s and three p orbital mix with each other in same shell of an tom to produce four new equal orbitals. This hybridization takes place in molecules exhibits tetrahedral geometry. In this hybridization, no p-unhybridized orbital is present as all are hybridized and form four sigma bonds.

The given molecule is ${\text{SF}}_4$ .

Number of valence electrons in sulfur = 6

Number of valence electrons in fluorine = 7

There are four fluorine atoms and one sulfur atom present in the molecule and charge on the molecule is equal to 0.

Total number of valence electrons = $\text{1}\times \text{6+4}\times \text{7 = 34}$

Here, sulfur atom is linked with four fluorine atoms by sigma bond. By bonding in this way, each atom completes its octet. Also, one lone pair of electrons is present on sulfur atom.

Thus, geometry of ${\text{SF}}_4$ is sea saw because of the presence of lone pair of electrons on sulfur atom and the equatorial bond angles are $120°$ whereas axial bond angle is $90°$ and, four hybrid orbitals are needed for the accommodation of four bond pair and one lone pair on sulfur atom. Thus, hybridization of sulfur atom is sp³d.

Lewis structure of ${\text{SF}}_4$ is:

  

(i)

Interpretation Introduction

Interpretation:

The hybrid orbitals should be predicted which is used by sulfur atom(s) in ${\text{SF}}_6$ along with its molecular structure and bond angle.

Concept Introduction:

When two atomic orbitals combine with each other to produce hybrid orbitals, redistribution of energy of orbitals of distinct atoms to form orbitals with equal energy occurs. This process is known as hybridization and the formed new orbitals are known as hybrid orbitals.

When the atomic orbitals overlap with each other in a region of high electron density, then molecular orbitals are formed. Overlapping of atomic orbitals determines the efficiency of interaction between atomic orbitals. Energy of bond molecular orbitals is less than the nonbonding molecular orbitals.

Explanation of Solution

On the basis of types of orbitals involved in mixing, different hybridization is classified as sp, sp², sp³, sp³d, sp³d², sp³d³.

sp-hybridization: It is formed when one s and one p orbital mix with each other in same shell of an tom to produce two new equal orbitals. This hybridization takes place in linear molecules.

  

sp²-hybridization: It is formed when one s and two p orbital mix with each other in same shell of an tom to produce three new equal orbitals. This hybridization takes place in molecules exhibits trigonal planar geometry.

  

sp³-hybridization: It is formed when one s and three p orbital mix with each other in same shell of an tom to produce four new equal orbitals. This hybridization takes place in molecules exhibits tetrahedral geometry. In this hybridization, no p-unhybridized orbital is present as all are hybridized and form four sigma bonds.

The given molecule is ${\text{SF}}_6$ .

Number of valence electrons in sulfur = 6

Number of valence electrons in fluorine = 7

There are six fluorine atoms and one sulfur atom present in the molecule and charge on the molecule is equal to 0.

Total number of valence electrons = $\text{1}\times \text{6+6}\times \text{7 = 48}$

Here, sulfur atom is linked with six fluorine atoms by sigma bond. By bonding in this way, each atom completes its octet. No lone pair of electrons is present on sulfur atom.

Thus, geometry of ${\text{SF}}_6$ is octahedral and bond angle is $90°$ and, electrons from 3s and 3p orbitals of sulfur atom are promoted to 3d orbitals for the formation of six sigma bonds with fluorine atoms. Thus, the hybridization of sulfur atom is sp³d².

Lewis structure of ${\text{SF}}_6$ is:

  

(j)

Interpretation Introduction

Interpretation:

The hybrid orbitals should be predicted which is used by sulfur atom(s) in ${\text{F}}_{\text{3}}\text{S-SF}$ along with its molecular structure and bond angle.

Concept Introduction:

When two atomic orbitals combine with each other to produce hybrid orbitals, redistribution of energy of orbitals of distinct atoms to form orbitals with equal energy occurs. This process is known as hybridization and the formed new orbitals are known as hybrid orbitals.

When the atomic orbitals overlap with each other in a region of high electron density, then molecular orbitals are formed. Overlapping of atomic orbitals determines the efficiency of interaction between atomic orbitals. Energy of bond molecular orbitals is less than the nonbonding molecular orbitals.

Explanation of Solution

On the basis of types of orbitals involved in mixing, different hybridization is classified as sp, sp², sp³, sp³d, sp³d², sp³d³.

sp-hybridization: It is formed when one s and one p orbital mix with each other in same shell of an tom to produce two new equal orbitals. This hybridization takes place in linear molecules.

  

sp²-hybridization: It is formed when one s and two p orbital mix with each other in same shell of an tom to produce three new equal orbitals. This hybridization takes place in molecules exhibits trigonal planar geometry.

  

sp³-hybridization: It is formed when one s and three p orbital mix with each other in same shell of an tom to produce four new equal orbitals. This hybridization takes place in molecules exhibits tetrahedral geometry. In this hybridization, no p-unhybridized orbital is present as all are hybridized and form four sigma bonds.

The given molecule is ${\text{F}}_{\text{3}}\text{S-SF}$ .

Number of valence electrons in sulfur = 6

Number of valence electrons in fluorine = 7

There are four fluorine atoms and two sulfur atoms present in the molecule and charge on the molecule is equal to 0.

Total number of valence electrons = $\text{2}\times \text{6+6}\times \text{4 = 40}$

Here, two sulfur atoms are linked by sigma bond. The three fluorine atoms are linked by one sulfur atom and one fluorine atom is linked with another sulfur atom. By bonding in this way, each atom completes its octet. Also, one lone pair of electrons is present on one sulfur atom and two lone pairs of electrons are present on another sulfur atom.

Thus, geometry of ${\text{F}}_{\text{3}}\text{S-SF}$ is sea-saw because of presence of lone pair of electrons present on sulfur atom and equatorial bond angles is $120°$ whereas axial bond angles is $90°$ . Here, four hybrid orbitals are needed to acquire four bonding pairs and one lone pair; therefore, the hybridization of sulfur atom which is linked with three fluorine atoms is sp³d whereas the hybridization of sulfur atom which is linked with one oxygen atom is sp³.

Lewis structure of ${\text{F}}_{\text{3}}\text{S-SF}$ is: