Complete the exercises below. Draw the crystal-field energy-level diagrams and show the placement of electrons for each of the following complexes: 
a. [VCl₆]^3–,
b. [FeF₆]^3– (a high-spin complex),

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1. Identify the metal ion and its oxidation state in each complex. For [VCl6]3–, vanadium (V) is the metal, and for [FeF6]3–, iron (Fe) is the metal. Determine the oxidation state by considering the charge of the complex and the known charges of the ligands (Cl- and F-).
2. Determine the electron configuration of the metal ion in its oxidation state. For example, V3+ and Fe3+ have specific electron configurations that can be derived from their neutral atom configurations by removing electrons from the outermost orbitals.
3. Consider the geometry of the complex. Both [VCl6]3– and [FeF6]3– are octahedral complexes, which means the d-orbitals will split into two sets: t2g (lower energy) and eg (higher energy) due to the crystal field splitting.
4. For [VCl6]3–, place the electrons in the crystal-field energy-level diagram according to the electron configuration of V3+. Since Cl- is a weak field ligand, the splitting will be small, and electrons will fill the t2g and eg orbitals according to Hund's rule.
5. For [FeF6]3–, determine the placement of electrons in the crystal-field energy-level diagram for Fe3+. As a high-spin complex with F- as a weak field ligand, the electrons will occupy the orbitals to maximize unpaired electrons, following Hund's rule and the small splitting energy.