Indicate the likely coordination number of the metal in each of the following complexes:
(a) \(\left[\operatorname{Rh}(\text { bipy })_{3}\right]\left(\mathrm{NO}_{3}\right)_{3}\)
(b) \(\mathrm{Na}_{3}\left[\mathrm{Co}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{2} \mathrm{Cl}_{2}\right]\)
(c) \(\left[\mathrm{Cr}(o \text {-phen })_{3}\right]\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{3}\)
(d) \(\mathrm{Na}_{2}[\mathrm{Co}(\mathrm{EDTA}) \mathrm{Br}]\)
Text Transcription:
[Rh(bipy)3](NO3)3
Na3[Co(C2O4)2Cl2]
[Cr(o-phen)3\(CH3COO)3
Na2[Co(EDTA)Br]
Step 1 of 5) Shows that the lobes of the dz2 and dx2 - y2 orbitals are directed along the x-, y-, and z-axes and so point directly toward the ligand point charges. The lobes of the dxy, dxz, and dyz orbitals, however, are directed between the axes and so do not point directly toward the charges. The result of this difference in orientation—dx2 - y2 and dz2 lobes point directly toward the ligand charges; dxy, dxz, and dyz lobes do not—is that an electron residing in either the dx2 - y2 or dz2 orbitals feels more repulsion from the negatively charged ligands. Hence the energy of the dx2 - y2 and dz2 orbitals is higher than the energy of the dxy, dxz, and dyz orbitals. This difference in energy is represented by the red boxes in the energy diagram of Figure 23.28.
