The total number of points of attachment to the central element is termed the coordination number and this can vary from 2 to as many as 16, but is usually 6. In simple terms, the coordination number of a complex is influenced by the relative sizes of the metal ion and the ligands and by electronic factors, such as charge which is dependent on the electronic configuration of the metal ion. These competing effects are described by the term ionic potential which is defined as the charge to radius ratio (q/r).
Based on the radius ratio, it can be seen that the bigger the charge on the central ion, the more attraction there will be for negatively charged ligands, however at the same time, the bigger the charge the smaller the ion becomes which then limits the number of groups able to coordinate.
This arrangement is not very common for first row transition metal ion complexes and some of the best known examples are for Silver(I). In this case we have a low charge and an ion at the right hand side of the d-block indicating smaller size
A method often employed for the detection of chloride ions involves the formation of the linear diamminesilver(I) complex.
The first step is:
Ag+ + Cl- → AgCl (white ppt)
and to ensure that the precipitate is really the chloride salt, two further tests must be done:
AgCl + 2 NH3 → [Ag(NH3)2]+
[Ag(NH3)2]+ + HNO3 → AgCl (re-ppts)
The reaction of a bidentate ligand such as 1,2-diaminoethane with Ag(I) does not lead to chelated ring systems, but instead to linear two coordinate complexes. One reason for this is that bidentate ligands can NOT exist in trans arrangements, that is they can NOT span 180 degrees.
Once again, this is not very common for first row transition metal ions. Examples with three different geometries have been identified:
Well known for main group species like CO32- etc., this geometry has the four atoms in a plane with the bond angles between the ligands at 120 degrees.
More common with main group ions.
The first example of a rare T-shaped molecule was found in 1977.
Two different geometries are possible. The tetrahedron is the more common while the square planar is found almost exclusively with metal ions having a d8 electronic configuration.
The chemistry of molecules centered around a tetrahedral C atom is covered in organic courses. To be politically correct, please change all occurrences of C to Co. There are large numbers of tetrahedral Cobalt(II) complexes known.
This is fairly rare and is included only because some extremely important molecules exist with this shape.
The structure of [Cr(en)3][Ni(CN)5] 1.5 H2O was reported in 1968 to be a remarkable example of a complex exhibiting both types of geometry in the same crystal. The reaction of cyanide ion with Ni2+ proceeds via several steps:
Ni2+ + 2 CN- → Ni(CN)2
Ni(CN)2 + 2 CN- → [Ni(CN)4]2-
log(β4) = 30.1
[Ni(CN)4]2- + CN- → [Ni(CN)5]3-
Oxovanadium salts (Vanadyl, VO2+) often show square pyramidal geometry, for example, VO(acac)2. Note that the Vanadium(IV) can be considered coordinatively unsaturated and addition of pyridine leads to the formation of an octahedral complex.
Unknown for first row transition metal ions, although the arrangement of six groups in a plane is found in some higher coordination number geometries.
Most trigonal prismatic compounds have three bidentate ligands such as dithiolates or oxalates and few are known for first row transition metal ions.
The most common geometry found for first row transition metal ions, including all aqua ions.
In some cases distortions are observed and these can sometimes be explained in terms of the Jahn-Teller Theorem.
Three geometries are possible:
Not very common for 1st row complexes and the energy difference between the structures seems small and distortions occur so that prediction of the closest "idealised" shape is generally difficult.
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