Orbitals complex

Oudeman law physchem The law that the molecular rotations of the various salts of an acid or base tend toward an identical limiting value as the concentration of the solution is reduced to zero. od-a-man, I6 ) outer orbital complex phys chem A metal coordination compound in which the d orbital used in forming the coordinate bond is at the same energy level as the s and p orbitals. aud-or 6rb-od-3l kam.pleks) overall stability constant analychem Reaction equilibrium constant for the reaction... 

E. Brandas, P. Froelich, Continuum Orbitals, Complex Scaling, and the Extended Virial Theorem, Phys. Rev. A16 (1977) 2207. 

The electron arrangement in an outer orbital complex such as [Mn(ox)3]3 can be shown as follows ... 

Some complexes utilize inner d orbitals of the central ion, while others are outer-orbital complexes ... 

Crystal field designation for an outer orbital complex all t2g and eg orbitals are singly occupied before any pairing occurs. 

For more information see Colloidal Chemistry Inner Orbital Complex... 

Crystal field designation for an inner orbital complex contains electrons paired t2g orbitals before eg orbitals are occupied in octahedral complexes. 

Henry Taube Itmer and outer orbital complexes... 

FIGURE 10-2 Inner and Outer Orbital Complexes. In each case, ligand electrons fill the d sp bonding orbitals. The remaining orbitals contain the electrons from the metal. 

Inner-orbital complexes are formed by ions of the transition metals, regardless of the nature of the ligands, provided ( —l)d orbitals can be made available... 

But 6-co-ordinate inner-orbital complexes of Co and NF+ are unlikely since they would require the promotion of one or two electrons to the 4d level. 

Copper(I) and zinc do not form inner-orbital complexes the promotion of four electrons would be required in each case ... 

In those instances where a cation forms both an inner (spin-paired) and an outer (spin-free) orbital complex, the former usually appears with easily-polarisable ligands containing directed lone pairs such as H2O, NH3 and CN, and the latter with ligands such as F (p. 133). 

The inner-orbital complexes show a sharp decrease in lability at the stage where no d orbital is left vacant. A pronounced difference in bond type cannot be expected in the following ... 

For outer-orbital 6-co-ordinate complexes, lability is associated with a charge of under four on the central ion, and inertness with one of four or over. These outer-orbital complexes probably undergo unimolecular dissociation and the ligand is easier to remove when the central charge is low. It is characteristic of the metals which give outer-orbital, 6-co-ordinate complexes readily, that they should also form 4-co-ordinate complexes. 

Care should be taken to distinguish these terms from the expressions inner orbital and outer orbital complex ions which have been introduced recently for an entirely different purpose 45). 

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