Chapter 20, Problem 20.99SP

(a)

Interpretation Introduction

Interpretation:

Valence bond description of the bonding in the given compound has to be given along with its orbital diagram for the free metal ion and metal ion in the complex. The hybrid orbitals which are used by the metal ion for bonding should be indicated and the number of unpaired electron should be specified.

Concept introduction:

Coordination compounds are a special class of compounds in which the metal atoms or ions are bounded to a number of anions or neutral molecules.

A coordination compound can be simply represented as follows,

Coordination number of a complex is defined as the number of ligand donor atoms to which the metal is directly bonded.

According to valence bond theory, the metal atom or ion under the influence of ligands can use its $\left(n-1\right)d,ns,nporns,np,nd$ orbitals for hybridization to yield a set of equivalent orbitals of definite geometry such as octahedral, tetrahedral and square planar.

These hybridized orbitals are allowed to overlap with ligand orbitals that can donate electron pairs for bonding.

$\begin{array}{ccc}\text{Coordination}\text{number}& \text{Hybridisation}& \text{Structure}\\ \text{4}& {\text{sp}}^{\text{3}}& \text{Tetrahedral}\\ \text{4}& {\text{dsp}}^{\text{2}}& \text{Square}\text{planar}\\ \text{5}& {\text{sp}}^{\text{3}}\text{d}& \text{Trigonal}\text{bipyramidal}\\ \text{6}& {\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}& \text{Octahedral}\\ \text{6}& {\text{d}}^{\text{2}}{\text{sp}}^{\text{3}}& \text{Octahedral}\end{array}$

Inner orbital complex are coordination compounds having a central metal atom that undergoes hybridization of atomic orbital including the inner d ($\left(\text{n-1}\right)\text{d}$) orbitals.

Outer orbital complex are coordination compounds having a central metal atom that undergoes hybridization of atomic orbital including the outer most d ($\text{nd}$) orbitals.

(b)

Interpretation Introduction

Interpretation:

Valence bond description of the bonding in the given compound has to be given along with its orbital diagram for the free metal ion and metal ion in the complex. The hybrid orbitals which are used by the metal ion for bonding should be indicated and the number of unpaired electron should be specified.

Concept introduction:

Coordination compounds are a special class of compounds in which the metal atoms or ions are bounded to a number of anions or neutral molecules.

A coordination compound can be simply represented as follows,

Coordination number of a complex is defined as the number of ligand donor atoms to which the metal is directly bonded.

According to valence bond theory, the metal atom or ion under the influence of ligands can use its $\left(n-1\right)d,ns,nporns,np,nd$ orbitals for hybridization to yield a set of equivalent orbitals of definite geometry such as octahedral, tetrahedral and square planar.

These hybridized orbitals are allowed to overlap with ligand orbitals that can donate electron pairs for bonding.

$\begin{array}{ccc}\text{Coordination}\text{number}& \text{Hybridisation}& \text{Structure}\\ \text{4}& {\text{sp}}^{\text{3}}& \text{Tetrahedral}\\ \text{4}& {\text{dsp}}^{\text{2}}& \text{Square}\text{planar}\\ \text{5}& {\text{sp}}^{\text{3}}\text{d}& \text{Trigonal}\text{bipyramidal}\\ \text{6}& {\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}& \text{Octahedral}\\ \text{6}& {\text{d}}^{\text{2}}{\text{sp}}^{\text{3}}& \text{Octahedral}\end{array}$

Inner orbital complex are coordination compounds having a central metal atom that undergoes hybridization of atomic orbital including the inner d ($\left(\text{n-1}\right)\text{d}$) orbitals.

Outer orbital complex are coordination compounds having a central metal atom that undergoes hybridization of atomic orbital including the outer most d ($\text{nd}$) orbitals.

(c)

Interpretation Introduction

Interpretation:

Valence bond description of the bonding in the given compound has to be given along with its orbital diagram for the free metal ion and metal ion in the complex. The hybrid orbitals which are used by the metal ion for bonding should be indicated and the number of unpaired electron should be specified.

Concept introduction:

Coordination compounds are a special class of compounds in which the metal atoms or ions are bounded to a number of anions or neutral molecules.

A coordination compound can be simply represented as follows,

Coordination number of a complex is defined as the number of ligand donor atoms to which the metal is directly bonded.

According to valence bond theory, the metal atom or ion under the influence of ligands can use its $\left(n-1\right)d,ns,nporns,np,nd$ orbitals for hybridization to yield a set of equivalent orbitals of definite geometry such as octahedral, tetrahedral and square planar.

These hybridized orbitals are allowed to overlap with ligand orbitals that can donate electron pairs for bonding.

$\begin{array}{ccc}\text{Coordination}\text{number}& \text{Hybridisation}& \text{Structure}\\ \text{4}& {\text{sp}}^{\text{3}}& \text{Tetrahedral}\\ \text{4}& {\text{dsp}}^{\text{2}}& \text{Square}\text{planar}\\ \text{5}& {\text{sp}}^{\text{3}}\text{d}& \text{Trigonal}\text{bipyramidal}\\ \text{6}& {\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}& \text{Octahedral}\\ \text{6}& {\text{d}}^{\text{2}}{\text{sp}}^{\text{3}}& \text{Octahedral}\end{array}$

Inner orbital complex are coordination compounds having a central metal atom that undergoes hybridization of atomic orbital including the inner d ($\left(\text{n-1}\right)\text{d}$) orbitals.

Outer orbital complex are coordination compounds having a central metal atom that undergoes hybridization of atomic orbital including the outer most d ($\text{nd}$) orbitals.

(d)

Interpretation Introduction

Interpretation:

Valence bond description of the bonding in the given compound has to be given along with its orbital diagram for the free metal ion and metal ion in the complex. The hybrid orbitals which are used by the metal ion for bonding should be indicated and the number of unpaired electron should be specified.

Concept introduction:

Coordination compounds are a special class of compounds in which the metal atoms or ions are bounded to a number of anions or neutral molecules.

A coordination compound can be simply represented as follows,

Coordination number of a complex is defined as the number of ligand donor atoms to which the metal is directly bonded.

According to valence bond theory, the metal atom or ion under the influence of ligands can use its $\left(n-1\right)d,ns,nporns,np,nd$ orbitals for hybridization to yield a set of equivalent orbitals of definite geometry such as octahedral, tetrahedral and square planar.

These hybridized orbitals are allowed to overlap with ligand orbitals that can donate electron pairs for bonding.

$\begin{array}{ccc}\text{Coordination}\text{number}& \text{Hybridisation}& \text{Structure}\\ \text{4}& {\text{sp}}^{\text{3}}& \text{Tetrahedral}\\ \text{4}& {\text{dsp}}^{\text{2}}& \text{Square}\text{planar}\\ \text{5}& {\text{sp}}^{\text{3}}\text{d}& \text{Trigonal}\text{bipyramidal}\\ \text{6}& {\text{sp}}^{\text{3}}{\text{d}}^{\text{2}}& \text{Octahedral}\\ \text{6}& {\text{d}}^{\text{2}}{\text{sp}}^{\text{3}}& \text{Octahedral}\end{array}$

Inner orbital complex are coordination compounds having a central metal atom that undergoes hybridization of atomic orbital including the inner d ($\left(\text{n-1}\right)\text{d}$) orbitals.

Outer orbital complex are coordination compounds having a central metal atom that undergoes hybridization of atomic orbital including the outer most d ($\text{nd}$) orbitals.