Textbook Question
Draw the crystal-field energy-level diagrams and show the placement of electrons for each of the following complexes:
d. [NiCl4]2+ (tetrahedral),
24. Transition Metals and Coordination Compounds
Crystal Field Theory: Tetrahedral Complexes
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For which of the following complexes, the energies of the dx2−y2 and dz2 orbitals will be lower than the other three d orbitals?
A
[Co(en)3]3+
B
[Ni(CN)4]2–
C
[Zn(H2O)4]2+
D
[AuCl2]–
Verified step by step guidance1
Identify the geometry of each complex. The geometry affects the splitting of the d orbitals. For example, [Co(en)3]3+ is octahedral, [Ni(CN)4]2– is square planar, [Zn(H2O)4]2+ is tetrahedral, and [AuCl2]– is linear.
Understand the concept of crystal field splitting. In octahedral complexes, the dx2−y2 and dz2 orbitals are higher in energy compared to the other three d orbitals (dxy, dxz, dyz). In tetrahedral complexes, the opposite is true; the dx2−y2 and dz2 orbitals are lower in energy.
Analyze the electronic configuration of the metal ions in each complex. This helps in understanding how the d orbitals are filled and which orbitals are affected by the ligand field.
Consider the ligand field strength. Strong field ligands like CN- in [Ni(CN)4]2– can cause significant splitting of the d orbitals, affecting their relative energies.
Determine which complex has a geometry that results in the dx2−y2 and dz2 orbitals being lower in energy. Based on the geometry and ligand field strength, [Zn(H2O)4]2+ is tetrahedral, where the dx2−y2 and dz2 orbitals are lower in energy compared to the other three d orbitals.
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