Chemistry

The magnetic moment tells you how many unpaired electrons are in the complex—use the formula $\mu = \sqrt{n(n+2)}$ BM, where $n$ is the number of unpaired electrons. Work backwards from 5.9 BM to find $n$, then determine which d-orbital configuration of Mn matches that count. Finally, consider whether the ligand (a halide, a weak-field ligand) causes pairing or leaves electrons unpaired, which reveals the geometry: tetrahedral complexes typically remain high-spin with weak-field ligands, while square planar or octahedral geometries might pair electrons differently.

The magnetic moment tells you how many unpaired electrons are in the complex—use the formula $\mu = \sqrt{n(n+2)}$ BM, where $n$ is the number of unpaired electrons. Work backwards from 5.9 BM to find $n$, then determine which d-orbital configuration of Mn matches that count. Finally, consider whether the ligand (a halide, a weak-field ligand) causes pairing or leaves electrons unpaired, which reveals the geometry: tetrahedral complexes typically remain high-spin with weak-field ligands, while square planar or octahedral geometries might pair electrons differently.