Chapter 21, Problem 21.121QP

(a)

Interpretation Introduction

Interpretation:

The bonding of group 4A atoms in the given compound should be described.

Concept introduction:

Valence bond theory:

The valence bond theory was proposed by Linus Pauling and it deals with bonding of atomic hybrid orbitals in the molecules.

Postulates of valence bond theory:

• The central metal makes a vacant orbitals by losing of electrons from it, which is equal to the coordination number.
• The ligands are make a covalent bond with central metal atom it is equal to the vacant orbital of central metal atom
• The filled orbital of ligand and vacant orbital of central metal atom are overlap to make a $\text{σ}$ bond.
• The formation of $\text{σ}$ bond by overlapping of orbitals is called hybridisation.
• The hybridised orbital are have a directional characteristics but it is not in un hybridised orbitals.
• Based on the direction of the hybridised orbitals, the shape of the molecule and bonding was explained.

Explanation of Solution

Given:

The given molecule is ethylene and carbon is group 4A element.

Carbon atom has 4 valence electrons and these are present in the tetrahedral direction and carbon atom have 1 $\text{C-C}$ bond and 3 $\text{C-H}$ bonds, these bonds are formed by the ${\text{sp}}^{\text{3}}$ hybridization.

Each $\text{C-H}$ binds are formed by the hybridization of ${\text{sp}}^{\text{3}}$ hybrid orbitals of carbon atom with $\text{s}$ orbital of Hydrogen atom.

Conclusion

The bonding of group 4A atoms in the given compound was described.

(b)

Interpretation Introduction

Interpretation:

The bonding of group 4A atoms in the given compound should be described.

Concept introduction:

Valence bond theory:

The valence bond theory was proposed by Linus Pauling and it deals with bonding of atomic hybrid orbitals in the molecules.

Postulates of valence bond theory:

• The central metal makes a vacant orbitals by losing of electrons from it, which is equal to the coordination number.
• The ligands are make a covalent bond with central metal atom it is equal to the vacant orbital of central metal atom
• The filled orbital of ligand and vacant orbital of central metal atom are overlap to make a $\text{σ}$ bond.
• The formation of $\text{σ}$ bond by overlapping of orbitals is called hybridisation.
• The hybridised orbital are have a directional characteristics but it is not in un hybridised orbitals.
• Based on the direction of the hybridised orbitals, the shape of the molecule and bonding was explained.

Explanation of Solution

Given:

The given molecule is ${\text{AsF}}_3$ and Arsenic is a group 4A element.

Arsenic atom has 5 valence electrons and one lone pair of electrons and it has tetrahedral directed 3 single electrons.

${\text{AsF}}_3$ has 3 $\text{As-F}$ bonds, these bonds are formed by the ${\text{sp}}^{\text{3}}$ hybridization.

Each $\text{As-F}$ binds are formed by the hybridization of ${\text{sp}}^{\text{3}}$ hybrid orbitals of Arsenic atom with $\text{2p}$ orbital of Fluorine atom.

Conclusion

The bonding of group 4A atoms in the given compound was described.

(c)

Interpretation Introduction

Interpretation:

The bonding of group 4A atoms in the given compound should be described.

Concept introduction:

Valence bond theory:

The valence bond theory was proposed by Linus Pauling and it deals with bonding of atomic hybrid orbitals in the molecules.

Postulates of valence bond theory:

• The central metal makes a vacant orbitals by losing of electrons from it, which is equal to the coordination number.
• The ligands are make a covalent bond with central metal atom it is equal to the vacant orbital of central metal atom
• The filled orbital of ligand and vacant orbital of central metal atom are overlap to make a $\text{σ}$ bond.
• The formation of $\text{σ}$ bond by overlapping of orbitals is called hybridisation.
• The hybridised orbital are have a directional characteristics but it is not in un hybridised orbitals.
• Based on the direction of the hybridised orbitals, the shape of the molecule and bonding was explained.

Explanation of Solution

Given:

The given molecule is ${\text{CH}}_{\text{3}}{\text{CH=CH}}_{\text{2}}$ and Carbon is a group 4A element.

Carbon atom has 4 valence electrons and it has three type of bonds

$\begin{array}{l}\text{C-H}\\ \text{C-C}\\ \text{C=C}\end{array}$

Here, $\text{C-H}$ and $\text{C-C}$ bonds are formed ${\text{sp}}^{\text{3}}$ hybridisation and $\text{C=C}$ formed by ${\text{sp}}^2$ hybridisation.

In the ${\text{sp}}^{\text{3}}$ hybridisation overlapping of one $s$ orbital with three $p$ orbitals in perpendicularly so it will make a $\text{σ}$ bond.

In ${\text{sp}}^2$ hybridisation overlapping of one $s$ orbital with two $p$ orbitals involving in sidewise overlapping so it will make a $\text{π}$ bond.

${\text{CH}}_{\text{3}}{\text{CH=CH}}_{\text{2}}$ has 6 $\text{C-H}$ bonds and 1 $\text{C-C}$ bond and 1 $\text{C=C}$ bond.

Conclusion

The bonding of group 4A atoms in the given compound was described.

(d)

Interpretation Introduction

Interpretation:

The bonding of group 4A atoms in the given compound should be described.

Concept introduction:

Valence bond theory:

The valence bond theory was proposed by Linus Pauling and it deals with bonding of atomic hybrid orbitals in the molecules.

Postulates of valence bond theory:

• The central metal makes a vacant orbitals by losing of electrons from it, which is equal to the coordination number.
• The ligands are make a covalent bond with central metal atom it is equal to the vacant orbital of central metal atom
• The filled orbital of ligand and vacant orbital of central metal atom are overlap to make a $\text{σ}$ bond.
• The formation of $\text{σ}$ bond by overlapping of orbitals is called hybridisation.
• The hybridised orbital are have a directional characteristics but it is not in un hybridised orbitals.
• Based on the direction of the hybridised orbitals, the shape of the molecule and bonding was explained.

Explanation of Solution

Given:

The given molecule is ${\text{SiH}}_4$ and Silicon is a group 4A element.

Silicon atom has 4 valence electrons and these are present in the tetrahedral direction and Silicon atom have 3 $\text{Si-H}$ bonds, these bonds are formed by the ${\text{sp}}^{\text{3}}$ hybridization.

Each $\text{Si-H}$ binds are formed by the hybridization of ${\text{sp}}^{\text{3}}$ hybrid orbitals of Silicon atom with $s$ orbital of Hydrogen atom.

Conclusion

The bonding of group 4A atoms in the given compound was described.