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How does ligand field strength and stoichiometry affect the electronic spectrum
Accepted Answer
Ligand field strength and stoichiometry significantly influence the electronic spectrum of a transition metal complex. Here's how:
Ligand Field Strength: Stronger field ligands (e.g., CN-, CO) cause a larger splitting of the d orbitals. This leads to higher energy transitions, resulting in absorption of higher energy light (shorter wavelengths). Conversely, weaker field ligands (e.g., H2O, Cl-) create smaller splitting, leading to lower energy transitions and absorption of lower energy light (longer wavelengths).
Stoichiometry: The number and types of ligands bound to the metal ion influence the ligand field strength and symmetry of the complex. Different stoichiometries can lead to different electronic configurations and splitting patterns, resulting in distinct absorption spectra.
For example, [Co(NH3)6]3+ (six ammonia ligands) has a stronger ligand field than [Co(H2O)6]3+ (six water ligands), leading to different colors and absorption maxima in their electronic spectra.
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