The orbital splitting energies (∆ₜ) in tetrahedral coordination entities are not large enough to force electron pairing, resulting in low spin configurations. The relationship is given by ∆ₜ = (4/9) ∆₀ for the same metal, ligands, and metal-ligand distances.

In [PtCl₆]²⁻, Pt has a coordination number of 6, and in [Ni(NH₃)₄]²⁺, Ni has a coordination number of 4. Similarly, [Fe(C₂O₄)₃]₃³⁻ and [Co(en)₃]³⁺ both have a coordination number of 6.

The coordination number (CN) of a metal ion in a complex is the count of ligand donor atoms directly bonded to the metal. It determines the spatial arrangement around the central metal ion.

Ambidentate ligands, like NO₂⁻ and SCN⁻ ions, have two different donor atoms. NO₂⁻ can coordinate through nitrogen or oxygen, while SCN⁻ can coordinate through sulfur or nitrogen, offering flexibility in metal binding.

Chelate ligands, like EDTA⁴⁻, use two or more donor atoms simultaneously to bind a metal ion, forming more stable complexes than those with unidentate ligands. The denticity of the ligand is the number of such ligating groups.