Applying VB theory

  We illustrate the applications and limitations of VB theory by considering octahedral complexes of Cr(III) (d³) and Fe(III) (d⁵) and octahedral, tetrahedral and square planar complexes of Ni(II) (d⁸). The atomic orbitals required for hybridization in an octahedral complex are the 3d_z² , 3d_x²_-y², 4s, 4p_x, 4p_y and 4p_z (Table 20.1); these orbitals must be unoccupied so as to be available to accept six pairs of electrons from the ligands. The Cr^3‏+ ion has three unpaired electrons and these are accommodated in the 3d_xy, 3d_xz and 3d_yz orbitals:

Table 1.1 Hybridization schemes for the σ-bonding frameworks of different geometrical configurations of ligand donor atoms.

  With the electrons from the ligands included and a hybridization scheme applied for an octahedral complex, the diagram becomes:

   This diagram is appropriate for all octahedral Cr(III) complexes because the three 3d electrons always singly occupy different orbitals. For octahedral Fe(III) complexes, we must account for  the existence of both high- and low-spin complexes. The electronic configuration of the free Fe^3‏+ ion is:

   For a high-spin octahedral complex such as [FeF₆]^3-, the five 3d electrons occupy the five 3d atomic orbitals (as in the free ion shown above) and the two d orbitals required for the sp³d² hybridization scheme must come from the 4d set. With the ligand electrons included, valence bond theory describes the bonding as follows leaving three empty 4d atomic orbitals (not shown):

   This scheme, however, is unrealistic because the 4d orbitals are at a significantly higher energy than the 3d atomic orbitals. Nickel(II) (d⁸) forms paramagnetic tetrahedral and octahedral complexes, and diamagnetic square planar complexes.  Bonding in a tetrahedral complex can be represented as follows (ligand electrons are shown in red):

and an octahedral complex can be described by the diagram:

in which the three empty 4d atomic orbitals are not shown.  For diamagnetic square planar complexes, valence bond theory gives the following picture:

     Valence bond theory may rationalize stereochemical and magnetic properties, but only at a simplistic level. It can say nothing about electronic spectroscopic properties or about the kinetic inertness that is a characteristic of the low-spin d⁶ configuration. Furthermore, the model implies a distinction between high- and low-spin complexes that is actually misleading. Finally, it cannot tell us why certain ligands are associated with the formation of high- (or low-)spin complexes. We therefore move on to alternative approaches to the bonding.

مواضيع ذات صلة

ايجاد الصيغة التركيبية للمعقدات

معقدات الخارصين

معقدات النحاس

كيمياء ومعقدات بعض عناصر السلسلة الانتقالية الاولى

تعريف المركبات المعقدة

Crystal Field Stabilization Energies

Colors of Transition-Metal Complexes

The Nature of the Ligands

Principal Quantum Number of the Metal

Charge on the Metal Ion

Factors That Affect the Magnitude of Δo

Electronic Structures of Metal Complexes