Chapter 7, Problem 7.52QP

(a)

Interpretation Introduction

Interpretation:

The hybridization of the central atom of the molecules with the following molecular geometries has to be predicted.

1. (a) Tetrahedral (b) trigonal planar (c) trigonal bipyramidal (d) linear (e) octahedral

Concept Introduction:

Hybridization is a hypothetical concept.  It refers to overlapping of atomic orbitals and the resultant orbitals formed are known as hybrid orbitals. An orbital that doesn’t involve in hybridization is termed as unhybridized orbital. After hybridization, the orbitals cannot be distinguished individually.  The orientation of the orbitals while overlapping impacts the nature of the bond forms. By knowing the hybridization of central atom in the molecule its geometry can be predicted and vice-versa.

Answer to Problem 7.52QP

	Molecular Geometry	Hybridization of the central atom
(a)	Tetrahedral	${\text{sp}}^{\text{3}}$

Explanation of Solution

Tetrahedral

A molecule having tetrahedral geometry has the empirical formula ${\text{AB}}_{\text{4}}$ which can be represented as –

Figure 1

The bond angle between two atoms in a tetrahedral molecule is $109.5^{°}.$ The geometry represented above is similar to the shape of ${\text{sp}}^{\text{3}}$ hybrid orbitals which are formed by combination of one s-orbital and three p-orbitals.

Figure 2

Thus a molecule having tetrahedral geometry has central atom with $s{p}^3$hybridization.

(b)

Interpretation Introduction

Interpretation:

The hybridization of the central atom of the molecules with the following molecular geometries has to be predicted.

1. (a) Tetrahedral (b) trigonal planar (c) trigonal bipyramidal (d) linear (e) octahedral

Concept Introduction:

Hybridization is a hypothetical concept.  It refers to overlapping of atomic orbitals and the resultant orbitals formed are known as hybrid orbitals. An orbital that doesn’t involve in hybridization is termed as unhybridized orbital. After hybridization, the orbitals cannot be distinguished individually.  The orientation of the orbitals while overlapping impacts the nature of the bond forms. By knowing the hybridization of central atom in the molecule its geometry can be predicted and vice-versa.

Answer to Problem 7.52QP

	Molecular Geometry	Hybridization of the central atom
(b)	Trigonal planar	${\text{sp}}^{\text{2}}$

Explanation of Solution

Trigonal planar

A molecule having trigonal planar geometry has the empirical formula $A{B}_3$ which can be represented as –

Figure 3

The bond angle between two atoms in a trigonal planar molecule is $120^{°}.$ The geometry represented above is similar to the shape of ${\text{sp}}^2$ hybrid orbitals which are formed by combination of one s-orbital and two p-orbitals.

Figure 4

Thus a molecule having trigonal planar geometry has central atom with $s{p}^2$hybridization.

(c)

Interpretation Introduction

Interpretation:

The hybridization of the central atom of the molecules with the following molecular geometries has to be predicted.

1. (a) Tetrahedral (b) trigonal planar (c) trigonal bipyramidal (d) linear (e) octahedral

Concept Introduction:

Hybridization is a hypothetical concept.  It refers to overlapping of atomic orbitals and the resultant orbitals formed are known as hybrid orbitals. An orbital that doesn’t involve in hybridization is termed as unhybridized orbital. After hybridization, the orbitals cannot be distinguished individually.  The orientation of the orbitals while overlapping impacts the nature of the bond forms. By knowing the hybridization of central atom in the molecule its geometry can be predicted and vice-versa.

Answer to Problem 7.52QP

S.No	Molecular Geometry	Hybridization of the central atom
(c)	Trigonal bipyramidal	${\text{sp}}^{\text{3}}{\text{d or dsp}}^{\text{3}}$

Explanation of Solution

Trigonal bipyramidal

A molecule having trigonal bipyramidal geometry has the empirical formula $A{B}_5$ which can be represented as –

Figure 5

Trigonal bipyramidal molecule has two set of bonds – two axial bonds and three equatorial bonds. The two axial bonds are $180^{°}$ apart. The bond angle between axial and equatorial atoms is $90^{°}$. The geometry represented above is similar to the shape of $ds{p}^3\text{ or }s{p}^{3}d$ hybrid orbitals which are formed by combination of one s-orbital and three p-orbitals and one d-orbital.

Figure 6

If the d-orbital of the $n^{th}$ shell participates in the formation of hybrid orbitals then hybridization is $s{p}^{3}d$ also known as outer orbital hybridization. In $ds{p}^3$ hybridization the d-orbital of ${(n-1)}^{th}$ shell participates in hybridization.  It is also known as inner orbital hybridization.  Thus a molecule having trigonal bipyramidal geometry has central atom with $s{p}^{3}d\text{ or }ds{p}^3$hybridization.

(d)

Interpretation Introduction

Interpretation:

The hybridization of the central atom of the molecules with the following molecular geometries has to be predicted.

1. (a) Tetrahedral (b) trigonal planar (c) trigonal bipyramidal (d) linear (e) octahedral

Concept Introduction:

Hybridization is a hypothetical concept.  It refers to overlapping of atomic orbitals and the resultant orbitals formed are known as hybrid orbitals. An orbital that doesn’t involve in hybridization is termed as unhybridized orbital. After hybridization, the orbitals cannot be distinguished individually.  The orientation of the orbitals while overlapping impacts the nature of the bond forms. By knowing the hybridization of central atom in the molecule its geometry can be predicted and vice-versa.

Answer to Problem 7.52QP

S.No	Molecular Geometry	Hybridization of the central atom
(d)	Linear	$\text{sp}$

Explanation of Solution

Linear

A molecule having linear geometry has the empirical formula $A{B}_2$ which can be represented as –

Figure 7

The bond angle between two atoms in linear molecule is $180^{°}.$ The geometry represented above is similar to the shape of $sp$ hybrid orbitals which are formed by combination of one s-orbital and one p-orbital.

Figure 8

Thus a molecule having linear geometry has central atom with $sp$hybridization.

(e)

Interpretation Introduction

Interpretation:

The hybridization of the central atom of the molecules with the following molecular geometries has to be predicted.

1. (a) Tetrahedral (b) trigonal planar (c) trigonal bipyramidal (d) linear (e) octahedral

Concept Introduction:

Hybridization is a hypothetical concept.  It refers to overlapping of atomic orbitals and the resultant orbitals formed are known as hybrid orbitals. An orbital that doesn’t involve in hybridization is termed as unhybridized orbital. After hybridization, the orbitals cannot be distinguished individually.  The orientation of the orbitals while overlapping impacts the nature of the bond forms. By knowing the hybridization of central atom in the molecule its geometry can be predicted and vice-versa.

Answer to Problem 7.52QP

S.No	Molecular Geometry	Hybridization of the central atom
(e)	Octahedral	${\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}{\text{or d}}^{\text{2}}{\text{sp}}^{\text{3}}$

Explanation of Solution

Octahedral

A molecule having octahedral geometry has the empirical formula $A{B}_6$ which can be represented as –

Figure 9

The bond angle between two atoms in octahedral molecule is $90^{°}.$ The geometry represented above is similar to the shape of $s{p}^3{d}^2\text{ or }{d}^{2}s{p}^3$ hybrid orbitals which are formed by combination of one s-orbital and three p-orbitals and two d-orbitals.

Figure 10

If the d-orbital of the $n^{th}$ shell participates in the formation of hybrid orbitals then hybridization is $s{p}^3{d}^2$ also known as outer orbital hybridization. In $d^{2}s{p}^3$ hybridization the d-orbital of ${(n-1)}^{th}$ shell participates in hybridization.  It is also known as inner orbital hybridization.  Thus a molecule having octahedral geometry has central atom with $s{p}^3{d}^2\text{ or }{d}^{2}s{p}^3$hybridization.

Conclusion

The hybridization of the central atom of the molecules with the given molecular geometries has been predicted.