Chapter 10, Problem 10.28QP

(a)

Interpretation Introduction

Interpretation: The angle between $\text{sp}$ and $\text{sp}$ hybrid orbitals have to be found.

Concept Introduction:

Bond angle:

Bond angle is the angle between two bonds in a molecule and it is determined based on the geometry a molecule.

Molecular geometry

Molecular geometry is based on the arrangement of electron pairs around the central atom. In VSEPR theory, the geometry of a molecule is explained based on the electrostatic repulsion between the lone pairs and bond pairs of electrons surrounding the central atom of the molecule.

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of a new set of hybrid orbitals which have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are $\text{sp,}{\text{sp}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}\text{,}{\text{sp}}^{\text{3}}\text{d,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{3}}.$

The following table is the tabulation of important hybridizations and the bond angles:

Hybridization	Molecular geometry	Bond angle
$\text{sp}$	Linear	${\text{180}}^{\text{o}}$
${\text{sp}}^2$	Trigonal planar	${120}^{\circ }$
${\text{sp}}^3$	Tetrahedral	${109.5}^{\circ }$

(b)

Interpretation Introduction

Interpretation: The angle between ${\text{sp}}^2$ and ${\text{sp}}^2$ hybrid orbitals have to be found.

Concept Introduction:

Bond angle:

Bond angle is the angle between two bonds in a molecule and it is determined based on the geometry a molecule.

Molecular geometry

Molecular geometry is based on the arrangement of electron pairs around the central atom. In VSEPR theory, the geometry of a molecule is explained based on the electrostatic repulsion between the lone pairs and bond pairs of electrons surrounding the central atom of the molecule.

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of a new set of hybrid orbitals which have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are $\text{sp,}{\text{sp}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}\text{,}{\text{sp}}^{\text{3}}\text{d,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{3}}.$

‘

The following table is the tabulation of important hybridizations and the bond angles:

Hybridization	Molecular geometry	Bond angle
$\text{sp}$	Linear	${\text{180}}^{\text{o}}$
${\text{sp}}^2$	Trigonal planar	${120}^{\circ }$
${\text{sp}}^3$	Tetrahedral	${109.5}^{\circ }$

(c)

Interpretation Introduction

Interpretation: The angle between ${\text{sp}}^3$ and ${\text{sp}}^3$ hybrid orbitals have to be found.

Concept Introduction:

Bond angle:

Bond angle is the angle between two bonds in a molecule and it is determined based on the geometry a molecule.

Molecular geometry

Molecular geometry is based on the arrangement of electron pairs around the central atom. In VSEPR theory, the geometry of a molecule is explained based on the electrostatic repulsion between the lone pairs and bond pairs of electrons surrounding the central atom of the molecule.

Hybridization is the phenomenon of intermixing of the atomic orbitals of different energy that results in the formation of a new set of hybrid orbitals which have equivalent energies. The various types of atomic orbitals are: s, p, and d orbitals. Types of hybridization that involves s, p and d orbitals are $\text{sp,}{\text{sp}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}\text{,}{\text{sp}}^{\text{3}}\text{d,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}\text{,}{\text{sp}}^{\text{3}}{\text{d}}^{\text{3}}.$

The following table is the tabulation of important hybridizations and the bond angles:

Hybridization	Molecular geometry	Bond angle
$\text{sp}$	Linear	${\text{180}}^{\text{o}}$
${\text{sp}}^2$	Trigonal planar	${120}^{\circ }$
${\text{sp}}^3$	Tetrahedral	${109.5}^{\circ }$