You can use any elements you want, but the complexes electronic configuration must be
unmistakably d8 Pt(II) by the counting rules
(If you have literature data for the complex, please provide it so I can cite it
Due to the large ligand field splitting there will be never a terahedral Pt(II) complex.
Even [PtF4]2- with fluoride as the weakest ligand you can imagine, the geometry is square planar.
You might force the tilt angle L2Pt/PtL2 from 0° to some degrees using extremely bulky ligands, but I would guess you cannot exceed more than 15 degrees (as an estimate).
So, if somebody has published a tetrahedral Pt(II) complex you should check the crystal structure for correctness (presumably the space group is wrong in such a case).
Hello, its difficult because Pt position is in the 3rd transition metals series which cause low spin case and provide empty d-orbital to form dsp2-hybridization
Yes it is not only difficult but almost impossible due to the large ligand field splitting. Thanks Axel Klein
Just to add to the answer of Md. Kudrat-E-Zahan: The ligand field splitting depends on essentially three parameters:
a) position in the d series. As a rule of thumb, the splitting energy doubles from 3d to 4d and again from 4d to 5d - this is the decisive part
b) the charge of the metal ion. As a rule of thumb, the energies are 1x - 2x - 3x for a series of metal ions M+, M2+, M3+. This is more important than c)
c) and finally, there are the ligands. They can cover a range from 5000 cm-1 to 15000 cm-1
Students in chemistry always start thinking about the ligand strength c) while a) and also b) are far more important for the estimation of the ligand field splitting
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