Chapter 20, Problem 20.27CP

(a)

Interpretation Introduction

Interpretation: The structure of the given coordination complex has to be drawn. The oxidation state, coordination number and the coordination geometry of the metal should be determined.

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,

Oxidation number is the charge of the central atom of a coordination complex and it is represented by roman numerals.

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

The geometry of a transition metal complex depends on the coordination number and nature of the metal ion.

Coordination number of complexes, shape with example are listed below,

$\begin{array}{ccc}\text{Coordination}\text{number}& \text{Shape}& \text{Examples}\\ \text{2}& \text{Linear}& {\left[{\text{CuCl}}_{\text{2}}\right]}^{\text{-}}\text{,}{\left[\text{Ag}{\left({\text{NH}}_{\text{3}}\right)}_{\text{2}}\right]}^{\text{+}}\text{,}{\left[{\text{AuCl}}_{\text{2}}\right]}^{\text{-}}\\ \text{4}& \text{Square}\text{planar}& {\left[\text{Ni}{\left(\text{CN}\right)}_{\text{4}}\right]}^{2-}\text{,}{\left[{\text{PdCl}}_{\text{4}}\right]}^{\text{2-}}\\ \text{4}& \text{Tetrahedral}& {\left[Zn{\left(OH\right)}_{\text{4}}\right]}^{2-}\text{,}{\left[{\text{CdCl}}_{\text{4}}\right]}^{\text{2-}}\\ \text{6}& \text{Octahedral}& {\left[\text{Ti}{\left({\text{H}}_{\text{2}}\text{O}\right)}_{\text{6}}\right]}^{\text{3+}}\text{,}{\left[\text{Co}{\left(\text{en}\right)}_{\text{3}}\right]}^{\text{3+}}\end{array}$

(b)

Interpretation Introduction

Interpretation: The structure of the given coordination complex has to be drawn. The oxidation state, coordination number and the coordination geometry of the metal should be determined.

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.

Oxidation number is the charge of the central atom of a coordination complex and it is represented by roman numerals. The geometry of a transition metal complex depends on the coordination number and nature of the metal ion.

Coordination number of complexes, shape with example are listed below,

$\begin{array}{ccc}\text{Coordination}\text{number}& \text{Shape}& \text{Examples}\\ \text{2}& \text{Linear}& {\left[{\text{CuCl}}_{\text{2}}\right]}^{\text{-}}\text{,}{\left[\text{Ag}{\left({\text{NH}}_{\text{3}}\right)}_{\text{2}}\right]}^{\text{+}}\text{,}{\left[{\text{AuCl}}_{\text{2}}\right]}^{\text{-}}\\ \text{4}& \text{Square}\text{planar}& {\left[\text{Ni}{\left(\text{CN}\right)}_{\text{4}}\right]}^{2-}\text{,}{\left[{\text{PdCl}}_{\text{4}}\right]}^{\text{2-}}\\ \text{4}& \text{Tetrahedral}& {\left[Zn{\left(OH\right)}_{\text{4}}\right]}^{2-}\text{,}{\left[{\text{CdCl}}_{\text{4}}\right]}^{\text{2-}}\\ \text{6}& \text{Octahedral}& {\left[\text{Ti}{\left({\text{H}}_{\text{2}}\text{O}\right)}_{\text{6}}\right]}^{\text{3+}}\text{,}{\left[\text{Co}{\left(\text{en}\right)}_{\text{3}}\right]}^{\text{3+}}\end{array}$

(c)

Interpretation Introduction

Interpretation: The structure of the given coordination complex has to be drawn. The oxidation state, coordination number and the coordination geometry of the metal should be determined.

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.

Oxidation number is the charge of the central atom of a coordination complex and it is represented by roman numerals.

The geometry of a transition metal complex depends on the coordination number and nature of the metal ion.

Coordination number of complexes, shape with example are listed below,

$\begin{array}{ccc}\text{Coordination}\text{number}& \text{Shape}& \text{Examples}\\ \text{2}& \text{Linear}& {\left[{\text{CuCl}}_{\text{2}}\right]}^{\text{-}}\text{,}{\left[\text{Ag}{\left({\text{NH}}_{\text{3}}\right)}_{\text{2}}\right]}^{\text{+}}\text{,}{\left[{\text{AuCl}}_{\text{2}}\right]}^{\text{-}}\\ \text{4}& \text{Square}\text{planar}& {\left[\text{Ni}{\left(\text{CN}\right)}_{\text{4}}\right]}^{2-}\text{,}{\left[{\text{PdCl}}_{\text{4}}\right]}^{\text{2-}},\left[Pt\left(en\right)C{l}_2\right]\\ \text{4}& \text{Tetrahedral}& {\left[Zn{\left(OH\right)}_{\text{4}}\right]}^{2-}\text{,}{\left[{\text{CdCl}}_{\text{4}}\right]}^{\text{2-}}\\ \text{6}& \text{Octahedral}& {\left[\text{Ti}{\left({\text{H}}_{\text{2}}\text{O}\right)}_{\text{6}}\right]}^{\text{3+}}\text{,}{\left[\text{Co}{\left(\text{en}\right)}_{\text{3}}\right]}^{\text{3+}}\end{array}$

(d)

Interpretation Introduction

Interpretation: The structure of the given coordination complex has to be drawn. The oxidation state, coordination number and the coordination geometry of the metal should be determined.

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.

Oxidation number is the charge of the central atom of a coordination complex and it is represented by roman numerals.

The geometry of a transition metal complex depends on the coordination number and nature of the metal ion.

Coordination number of complexes, shape with example are listed below,

$\begin{array}{ccc}\text{Coordination}\text{number}& \text{Shape}& \text{Examples}\\ \text{2}& \text{Linear}& {\left[{\text{CuCl}}_{\text{2}}\right]}^{\text{-}}\text{,}{\left[\text{Ag}{\left({\text{NH}}_{\text{3}}\right)}_{\text{2}}\right]}^{\text{+}}\text{,}{\left[{\text{AuCl}}_{\text{2}}\right]}^{\text{-}}\\ \text{4}& \text{Square}\text{planar}& {\left[\text{Ni}{\left(\text{CN}\right)}_{\text{4}}\right]}^{2-}\text{,}{\left[{\text{PdCl}}_{\text{4}}\right]}^{\text{2-}}\\ \text{4}& \text{Tetrahedral}& {\left[Zn{\left(OH\right)}_{\text{4}}\right]}^{2-}\text{,}{\left[{\text{CdCl}}_{\text{4}}\right]}^{\text{2-}}\\ \text{6}& \text{Octahedral}& {\left[\text{Ti}{\left({\text{H}}_{\text{2}}\text{O}\right)}_{\text{6}}\right]}^{\text{3+}}\text{,}{\left[\text{Co}{\left(\text{en}\right)}_{\text{3}}\right]}^{\text{3+}}\end{array}$