Answer: d3 (t2g3, CFSE = -1.2 Delta_o) and d6 low spin (t2g6, CFSE = -2.4 Delta_o).
- A d3 (t2g3, CFSE = -1.2 Delta_o) and d6 low spin (t2g6, CFSE = -2.4 Delta_o)
- B d0, which by definition has zero d electrons and therefore zero CFSE
- C d10, which has all orbitals fully occupied giving zero net CFSE
- D d5 high spin, which has one electron in every orbital giving zero net CFSE
Correct answer: A. d3 (t2g3, CFSE = -1.2 Delta_o) and d6 low spin (t2g6, CFSE = -2.4 Delta_o)
Explanation: d6 low spin (t2g6 eg0): CFSE = 6(-0.4) = -2.4 Delta_o, the maximum CFSE for any dn in octahedral field. d3 gives -1.2 Delta_o (all in t2g).
The three common coordination geometries: octahedral (6 ligands), tetrahedral (4 ligands), and square planar (4 ligands in one plane).
Concept context
Study of compounds where a central metal atom is bonded to surrounding ligands. Covers nomenclature, types of isomerism, bonding theories (VBT, CFT), and applications in medicine, photography, and industry.