Editing Isolobal principle (section)

===Non-octahedral complexes===

{|style="float: left;" class=wikitable border="1"
|+Figure 7: Isolobal relationship between octahedral and square planar complexes.
!Octahedral<br>ML<sub>''n''</sub>
!Square-planar<br>ML<sub>''n''−2</sub>
|-
|d<sup>6</sup>: Mo(CO)<sub>5</sub>
|d<sup>8</sup>: [PdCl<sub>3</sub>]<sup>−</sup>
|-
|d<sup>8</sup>: Os(CO)<sub>4</sub>
|d<sup>10</sup>: Ni(PR<sub>3</sub>)<sub>2</sub>
|}

[[Image:Isolobal Figure8.tif|thumb|250px|right|'''Figure 8:''' Examples of non-basic shapes in the isolobal analogy.]] 
The analogy applies to other shapes besides tetrahedral and octahedral geometries. The derivations used in octahedral geometry are valid for most other geometries. The exception is square-planar because [[square-planar complex]]es typically abide by the 16-electron rule. Assuming ligands act as two-electron donors the metal center in square-planar molecules is d<sup>8</sup>. To relate an octahedral fragment, ML<sub>''n''</sub>, where M has a d<sup>''x''</sup> electron configuration to a square planar analogous fragment, the formula ML<sub>''n''−2</sub> where M has a d<sup>''x''+2</sup> electron configuration should be followed.

Further examples of the isolobal analogy in various shapes and forms are shown in figure 8.
{{clear}}