Chapter 6, Problem 51P

a)

Interpretation Introduction

Interpretation: The hybridization on central atom in ${\text{CCl}}_4$ should be determined. Also, geometry of ${\text{CCl}}_4$ should be determined.

Concept introduction: Bonding between atoms in covalent molecule is shown by diagrams known as Lewis structures. These also show lone pairs in molecule.

Steps to determine Lewis dot diagram is as follows:

1. Count total valence electrons of central atom to add valence electrons from all atoms present. If species is negative ion, add electrons to achieve the total charge. If it is positive ion, subtract electrons to result in total charge.

2. Calculate total electrons that each atom has noble gas configuration of electrons around it.

3. Calculate the difference of electron. This determines the number of shared electrons.

4. Then assign two electrons to each bond in molecule or ion.

5. If electrons are left place them as double or triple bonds.

6. Place remaining electrons as lone pairs to atom, to satisfy octet of atom except hydrogen.

7. Determine formal charge of each atom.

Hybridization is mixing of two atomic orbitals with same energy level to give new orbital. This is based on quantum mechanics. The atomic orbitals of equal energy level only are part of hybridization.

The hybridization can be determined by number of hybrid orbitals or steric number formed by the atom. The formula to calculate steric number is as follows:

  $\text{Steric number }\left(\text{SN}\right)=\left[\begin{array}{l}\left(\text{number of atoms bonded to central atom}\right)+\\ \left(\text{number of lone pairs on central atom}\right)\end{array}\right]$

The hybridization is predicted as follows:

1. If value of SN is 2, two hybrid orbitals are formed and hybridization will be sp.

2. If value of SN is 3, three hybrid orbitals are formed and hybridization will be $s{p}^2$ .

3. If value of SN is 4, four hybrid orbitals are formed and hybridization will be $s{p}^3$ .

4. If value of SN is 5, five hybrid orbitals are formed and hybridization will be $s{p}^{3}d$ .

5. If value of SN is 6, six hybrid orbitals are formed and hybridization will be $s{p}^3{d}^2$ .

b)

Interpretation Introduction

Interpretation: The hybridization on carbon atom in ${\text{CO}}_2$ should be determined. Also, geometry of ${\text{CO}}_2$ should be determined.

Concept introduction: Bonding between atoms in covalent molecule is shown by diagrams known as Lewis structures. These also show lone pairs in molecule.

Steps to determine Lewis dot diagram is as follows:

1. Count total valence electrons of central atom to add valence electrons from all atoms present. If species is negative ion, add electrons to achieve the total charge. If it is positive ion, subtract electrons to result in total charge.

2. Calculate total electrons that each atom has noble gas configuration of electrons around it.

3. Calculate the difference of electron. This determines the number of shared electrons.

4. Then assign two electrons to each bond in molecule or ion.

5. If electrons are left place them as double or triple bonds.

6. Place remaining electrons as lone pairs to atom, to satisfy octet of atom except hydrogen.

7. Determine formal charge of each atom.

Hybridization is mixing of two atomic orbitals with same energy level to give new orbital. This is based on quantum mechanics. The atomic orbitals of equal energy level only are part of hybridization.

The hybridization can be determined by number of hybrid orbitals or steric number formed by the atom. The formula to calculate steric number is as follows:

  $\text{Steric number }\left(\text{SN}\right)=\left[\begin{array}{l}\left(\text{number of atoms bonded to central atom}\right)+\\ \left(\text{number of lone pairs on central atom}\right)\end{array}\right]$

The hybridization is predicted as follows:

1. If value of SN is 2, two hybrid orbitals are formed and hybridization will be sp.

2. If value of SN is 3, three hybrid orbitals are formed and hybridization will be $s{p}^2$ .

3. If value of SN is 4, four hybrid orbitals are formed and hybridization will be $s{p}^3$ .

4. If value of SN is 5, five hybrid orbitals are formed and hybridization will be $s{p}^{3}d$ .

5. If value of SN is 6, six hybrid orbitals are formed and hybridization will be $s{p}^3{d}^2$ .

c)

Interpretation Introduction

Interpretation: The hybridization on central atom in ${\text{OF}}_2$ should be determined. Also, geometry of ${\text{OF}}_2$ should be determined.

Concept introduction: Bonding between atoms in covalent molecule is shown by diagrams known as Lewis structures. These also show lone pairs in molecule.

Steps to determine Lewis dot diagram is as follows:

1. Count total valence electrons of central atom to add valence electrons from all atoms present. If species is negative ion, add electrons to achieve the total charge. If it is positive ion, subtract electrons to result in total charge.

2. Calculate total electrons that each atom has noble gas configuration of electrons around it.

3. Calculate the difference of electron. This determines the number of shared electrons.

4. Then assign two electrons to each bond in molecule or ion.

5. If electrons are left place them as double or triple bonds.

6. Place remaining electrons as lone pairs to atom, to satisfy octet of atom except hydrogen.

7. Determine formal charge of each atom.

Hybridization is mixing of two atomic orbitals with same energy level to give new orbital. This is based on quantum mechanics. The atomic orbitals of equal energy level only are part of hybridization.

The hybridization can be determined by number of hybrid orbitals or steric number formed by the atom. The formula to calculate steric number is as follows:

  $\text{Steric number }\left(\text{SN}\right)=\left[\begin{array}{l}\left(\text{number of atoms bonded to central atom}\right)+\\ \left(\text{number of lone pairs on central atom}\right)\end{array}\right]$

The hybridization is predicted as follows:

1. If value of SN is 2, two hybrid orbitals are formed and hybridization will be sp.

2. If value of SN is 3, three hybrid orbitals are formed and hybridization will be $s{p}^2$ .

3. If value of SN is 4, four hybrid orbitals are formed and hybridization will be $s{p}^3$ .

4. If value of SN is 5, five hybrid orbitals are formed and hybridization will be $s{p}^{3}d$ .

5. If value of SN is 6, six hybrid orbitals are formed and hybridization will be $s{p}^3{d}^2$ .

d)

Interpretation Introduction

Interpretation: The hybridization on central carbon atom in ${\text{CH}}_3{}^{-}$ should be determined. Also, geometry of ${\text{CH}}_3{}^{-}$ should be determined.

Concept introduction: Bonding between atoms in covalent molecule is shown by diagrams known as Lewis structures. These also show lone pairs in molecule.

Steps to determine Lewis dot diagram is as follows:

1. Count total valence electrons of central atom to add valence electrons from all atoms present. If species is negative ion, add electrons to achieve the total charge. If it is positive ion, subtract electrons to result in total charge.

2. Calculate total electrons that each atom has noble gas configuration of electrons around it.

3. Calculate the difference of electron. This determines the number of shared electrons.

4. Then assign two electrons to each bond in molecule or ion.

5. If electrons are left place them as double or triple bonds.

6. Place remaining electrons as lone pairs to atom, to satisfy octet of atom except hydrogen.

7. Determine formal charge of each atom.

Hybridization is mixing of two atomic orbitals with same energy level to give new orbital. This is based on quantum mechanics. The atomic orbitals of equal energy level only are part of hybridization.

The hybridization can be determined by number of hybrid orbitals or steric number formed by the atom. The formula to calculate steric number is as follows:

  $\text{Steric number }\left(\text{SN}\right)=\left[\begin{array}{l}\left(\text{number of atoms bonded to central atom}\right)+\\ \left(\text{number of lone pairs on central atom}\right)\end{array}\right]$

The hybridization is predicted as follows:

1. If value of SN is 2, two hybrid orbitals are formed and hybridization will be sp.

2. If value of SN is 3, three hybrid orbitals are formed and hybridization will be $s{p}^2$ .

3. If value of SN is 4, four hybrid orbitals are formed and hybridization will be $s{p}^3$ .

4. If value of SN is 5, five hybrid orbitals are formed and hybridization will be $s{p}^{3}d$ .

5. If value of SN is 6, six hybrid orbitals are formed and hybridization will be $s{p}^3{d}^2$ .

e)

Interpretation Introduction

Interpretation: The hybridization on central atom in ${\text{BeH}}_2$ should be determined. Also, geometry of ${\text{BeH}}_2$ should be determined.

Concept introduction: Bonding between atoms in covalent molecule is shown by diagrams known as Lewis structures. These also show lone pairs in molecule.

Steps to determine Lewis dot diagram is as follows:

1. Count total valence electrons of central atom to add valence electrons from all atoms present. If species is negative ion, add electrons to achieve the total charge. If it is positive ion, subtract electrons to result in total charge.

2. Calculate total electrons that each atom has noble gas configuration of electrons around it.

3. Calculate the difference of electron. This determines the number of shared electrons.

4. Then assign two electrons to each bond in molecule or ion.

5. If electrons are left place them as double or triple bonds.

6. Place remaining electrons as lone pairs to atom, to satisfy octet of atom except hydrogen.

7. Determine formal charge of each atom.

Hybridization is mixing of two atomic orbitals with same energy level to give new orbital. This is based on quantum mechanics. The atomic orbitals of equal energy level only are part of hybridization.

The hybridization can be determined by number of hybrid orbitals or steric number formed by the atom. The formula to calculate steric number is as follows:

  $\text{Steric number }\left(\text{SN}\right)=\left[\begin{array}{l}\left(\text{number of atoms bonded to central atom}\right)+\\ \left(\text{number of lone pairs on central atom}\right)\end{array}\right]$

The hybridization is predicted as follows:

1. If value of SN is 2, two hybrid orbitals are formed and hybridization will be sp.

2. If value of SN is 3, three hybrid orbitals are formed and hybridization will be $s{p}^2$ .

3. If value of SN is 4, four hybrid orbitals are formed and hybridization will be $s{p}^3$ .

4. If value of SN is 5, five hybrid orbitals are formed and hybridization will be $s{p}^{3}d$ .

5. If value of SN is 6, six hybrid orbitals are formed and hybridization will be $s{p}^3{d}^2$ .