Chemistry & Chemical Reactivity

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



Chemistry & Chemical Reactivity

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

How many unpaired electrons are expected for high-spin and low-spin complexes of Fe2+?

Interpretation Introduction

Interpretation: The number of unpaired electrons presents in the high and low spin of iron +2 complexes has to 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.


The periodic table clearly shows that the outer electronic configuration of Fe is 4s23d6 which is with d6 configuration.

The high spin complex of Fe+2 complex electronic configuration is as follows,

Oxidation state of Fe is +2No. of valence electrons is 6

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


The above configuration clearly shows that there exist 4 unpaired electrons since the given condition says that it is high spin complex where pairing of electrons does occurs and the electrons tends to present at lower level of d orbitals hence the given complex is diamagnetic

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