#Rank dmg in the spectrochemical series. series#
Some of the trends we see in the spectrochemical series arise from pi-donating and pi-accepting effects in the ligand. Show what happens to the energies of these two orbitals when they interact with each other. In the previous problem, a lower-energy atomic orbital on the metal interacts with a higher-energy antibonding orbital on the ligand. When orbitals on two different kinds of atoms combine, the bonding orbital is considered to be more like the orbital that was initially at lower energy.In this case, it is still close to a d orbital in energy, location, and shape.When orbitals on two different kinds of atoms combine, the antibonding orbital is considered to be more like the orbital that was initially at higher energy.
The d orbital is initially higher in energy than the ligand orbital, so an antibonding combination between these two orbitals is more like the initial d orbital, both in energy and location. This premise is based on the idea that a ligand orbital is initially lower in energy than the metal orbital, so a bonding combination between these two orbitals is more like the initial ligand orbital, both in energy and location. That bonding orbital would be more like the initial ligand orbital. In addition, there would also be a bonding combination for this interaction. The d orbitals that rise in energy in the presence of a ligand can be thought of as forming an antibonding molecular orbital combination with an orbital on the ligand. What empirical trends can you see within the spectrochemical series? Are there any factors that make something a stronger field ligand? The list can vary from one metal ion to another, since some ligands bind preferentially to certain metals (as seen in hard and soft acid and base chemistry). In which py = pyridine en = ethylenediamine bipy = 2,2'-bipyridine phen = 1,10-phenanthroline SCN means the ligand is bound via sulfur and NCS via nitrogen. < en < bipy < phen < NO 2 − < PPh 3 < CN − < CO I − < Br − < S 2− < SCN − < Cl − < NO 3 − < N 3 − < F − < OH − < C 2O 4 2− < H 2O < NCS − < CH 3CN < py < NH 3 It is often listed, from weaker to stronger ligands, something like this: The spectrochemical series is a list of ligands based on the strength of their interaction with metal ions. Ligands that interact only weakly produce little change in the d orbital energy levels, whereas ligands that interact strongly produce a larger change in d orbital energy levels. The d orbital energy splitting is influenced by how strongly the ligand interacts with the metal. Another factor that plays a key role in whether a transition metal complex is high- or low-spin is the nature of the ligands.
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