In tetrahedral complexes, one s and three p orbitals undergo hybridization to form four equivalent orbitals arranged tetrahedrally. This hybridization is demonstrated in [NiCl₄]²⁻, where nickel is in the +2 oxidation state.
How are orbitals hybridized in tetrahedral complexes, illustrated using [NiCl₄]²⁻ as an example?
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In tetrahedral complexes like [NiCl₄]²⁻, orbitals undergo hybridization to form four equivalent hybrid orbitals oriented tetrahedrally. The nickel ion in +2 oxidation state has the electronic configuration 3d⁸. The hybridization involves one s orbital and three p orbitals of the nickel ion, resulting in four equivalent sp³ hybrid orbitals. Each chloride ion donates a pair of electrons for bonding. This hybridization scheme leads to the tetrahedral geometry of the complex. The complex [NiCl₄]²⁻ is paramagnetic due to the presence of two unpaired electrons in the hybrid orbitals, resulting from the pairing of electrons from the chloride ligands.