BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Solutions

Chapter
Section
BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

The following are low-spin complexes. Use the ligand field model to find the electron configuration of the central metal ion in each ion. Determine which are diamagnetic. Give the number of unpaired electrons for the paramagnetic complexes.

(a) [Mn(CN)6]4−

(b) [Co(NH3)6]Cl3

(c) [Fe(H2O)6]3+

(d) [Cr(en)3]SO4

(a)

Interpretation Introduction

Interpretation: The electronic configuration, magnetic character and the number of unpaired electrons for the given set of low spin complexes has be determined.

Concept introduction: The transition metal atoms have tendency to form complex compounds that are linked to the certain neutral or ionic species which leads to the formation of coordination compounds. There exists a large number of coordination compounds that have a large number of applications in the chemical industry as well as in daily life.

The properties of the coordination compounds depend upon the primary and secondary valancy of the metal ion in the coordination sphere. The electrical conductivity depends upon the number of ions that are produced by complex.

The strong-field ligands results in pairing of electrons present in the complex and leads to diamagnetic species , while the low-field ligand do not have tendency to pair up the electrons therefore forms paramagnetic species.

The strong field ligands lead to splitting to a higher extent than the weak field ligands and the wavelength of light absorbed depends on the energy gap that is produced by a particular ligand.

The five d orbitals get divided into two sets that is dxy, dyz and dxz orbitals forms one set and dx2-y2and dz2 forms another set. The first set are oriented between the x, y and z axes whereas the second set gets oriented along the axis.

Electronic configuration: It is defined as the distribution of electrons present in the atom over orbitals following certain rules like electrons starts filling the lower energy orbital to higher energy, pairing of electrons does not occur until all the orbitals are singly filled and finally no electrons present in orbital can have same set of quantum numbers.

Oxidation state: It defines the number of electrons gained or lost by the chemical substance.

Explanation

Examining the given complex shows that manganese serves as the central metal atom since it is surrounded by 6 ligands with it. The periodic table clearly shows that the outer electronic configuration of Mn is 4s23d5.

The oxidation state for Mn in given complex is +2 since given complex has 6cyano groups and the charge of cyano group is 1 which is showed as follows,

[Mn(CN)6]4-Let x be charge of Mnx+(-6)= -4x = 2Therefore,oxidation state of Mn is +2.

Now considering the charge of metal atom the outer electrons present in the given complex is five distributed over d orbitals as follows,

__

(b)

Interpretation Introduction

Interpretation: The electronic configuration, magnetic character and the number of unpaired electrons for the given set of low spin complexes has be determined.

Concept introduction: The transition metal atoms have tendency to form complex compounds that are linked to the certain neutral or ionic species which leads to the formation of coordination compounds. There exists a large number of coordination compounds that have a large number of applications in the chemical industry as well as in daily life.

The properties of the coordination compounds depend upon the primary and secondary valancy of the metal ion in the coordination sphere. The electrical conductivity depends upon the number of ions that are produced by complex.

The strong-field ligands results in pairing of electrons present in the complex and leads to diamagnetic species , while the low-field ligand do not have tendency to pair up the electrons therefore forms paramagnetic species.

The strong field ligands lead to splitting to a higher extent than the weak field ligands and the wavelength of light absorbed depends on the energy gap that is produced by a particular ligand.

The five d orbitals get divided into two sets that is dxy, dyz and dxz orbitals forms one set and dx2-y2and dz2 forms another set. The first set are oriented between the x, y and z axes whereas the second set gets oriented along the axis.

Electronic configuration: It is defined as the distribution of electrons present in the atom over orbitals following certain rules like electrons starts filling the lower energy orbital to higher energy, pairing of electrons does not occur until all the orbitals are singly filled and finally no electrons present in orbital can have same set of quantum numbers.

Oxidation state: It defines the number of electrons gained or lost by the chemical substance.

(c)

Interpretation Introduction

Interpretation: The electronic configuration, magnetic character and the number of unpaired electrons for the given set of low spin complexes has be determined.

Concept introduction: The transition metal atoms have tendency to form complex compounds that are linked to the certain neutral or ionic species which leads to the formation of coordination compounds. There exists a large number of coordination compounds that have a large number of applications in the chemical industry as well as in daily life.

The properties of the coordination compounds depend upon the primary and secondary valancy of the metal ion in the coordination sphere. The electrical conductivity depends upon the number of ions that are produced by complex.

The strong-field ligands results in pairing of electrons present in the complex and leads to diamagnetic species , while the low-field ligand do not have tendency to pair up the electrons therefore forms paramagnetic species.

The strong field ligands lead to splitting to a higher extent than the weak field ligands and the wavelength of light absorbed depends on the energy gap that is produced by a particular ligand.

The five d orbitals get divided into two sets that is dxy, dyz and dxz orbitals forms one set and dx2-y2and dz2 forms another set. The first set are oriented between the x, y and z axes whereas the second set gets oriented along the axis.

Electronic configuration: It is defined as the distribution of electrons present in the atom over orbitals following certain rules like electrons starts filling the lower energy orbital to higher energy, pairing of electrons does not occur until all the orbitals are singly filled and finally no electrons present in orbital can have same set of quantum numbers.

Oxidation state: It defines the number of electrons gained or lost by the chemical substance.

(d)

Interpretation Introduction

Interpretation: The electronic configuration, magnetic character and the number of unpaired electrons for the given set of low spin complexes has be determined.

Concept introduction: The transition metal atoms have tendency to form complex compounds that are linked to the certain neutral or ionic species which leads to the formation of coordination compounds. There exists a large number of coordination compounds that have a large number of applications in the chemical industry as well as in daily life.

The properties of the coordination compounds depend upon the primary and secondary valancy of the metal ion in the coordination sphere. The electrical conductivity depends upon the number of ions that are produced by complex.

The strong-field ligands results in pairing of electrons present in the complex and leads to diamagnetic species , while the low-field ligand do not have tendency to pair up the electrons therefore forms paramagnetic species.

The strong field ligands lead to splitting to a higher extent than the weak field ligands and the wavelength of light absorbed depends on the energy gap that is produced by a particular ligand.

The five d orbitals get divided into two sets that is dxy, dyz and dxz orbitals forms one set and dx2-y2and dz2 forms another set. The first set are oriented between the x, y and z axes whereas the second set gets oriented along the axis.

Electronic configuration: It is defined as the distribution of electrons present in the atom over orbitals following certain rules like electrons starts filling the lower energy orbital to higher energy, pairing of electrons does not occur until all the orbitals are singly filled and finally no electrons present in orbital can have same set of quantum numbers.

Oxidation state: It defines the number of electrons gained or lost by the chemical substance.

Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Additional Science Solutions

Find more solutions based on key concepts

Show solutions add

Vitamin E is famous for its role: a. in maintaining bone tissue integrity. b. in maintaining connective tissue ...

Nutrition: Concepts and Controversies - Standalone book (MindTap Course List)

What is the life expectancy of a 16-solar-mass star?

Horizons: Exploring the Universe (MindTap Course List)

What impact has recombinant DNA technology had on genetics and society?

Human Heredity: Principles and Issues (MindTap Course List)

A rock is thrown downward from the top of a 40.0-in-tall tower with an initial speed of m/s. Assuming negligibl...

Physics for Scientists and Engineers, Technology Update (No access codes included)