text: In the case of octahedral complexes, the question of high spin vs low spin first arises for d, since it has more than the 3 electrons to fill the non-bonding d orbitals according to ligand field theory or the stabilized d orbitals according to crystal field splitting.
  All complexes of second and third row metals are low-spin.
  ;d: 
  :Octahedral high-spin: 4 unpaired electrons, paramagnetic, substitutionally labile. Includes Cr (many complexes assigned as Cr(II) are however Cr(III) with reduced ligands), Mn.
  :Octahedral low-spin: 2 unpaired electrons, paramagnetic, substitutionally inert. Includes Cr, Mn.
  ;d: 
  :Octahedral high-spin: 5 unpaired electrons, paramagnetic, substitutionally labile. Includes Fe, Mn. Example: Tris(acetylacetonato)iron(III).
  :Octahedral low-spin: 1 unpaired electron, paramagnetic, substitutionally inert. Includes Fe.  Example: [[ferricyanide|[Fe(CN)]]].
  ;d: 
  :Octahedral high-spin: 4 unpaired electrons, paramagnetic, substitutionally labile. Includes Fe, Co.  Examples: [Fe(HO)], [CoF].
  :Octahedral low-spin: no unpaired electrons, diamagnetic, substitutionally inert. Includes Fe, Co, Ni. Example: [[Hexamminecobalt(III) chloride|[Co(NH)]]].
  ;d:
  :Octahedral high-spin: 3 unpaired electrons, paramagnetic, substitutionally labile. Includes Co, Ni.
  :Octahedral low-spin:1 unpaired electron, paramagnetic, substitutionally labile. Includes Co, Ni. Example: [Co(NH)].
  ;d:Octahedral high-spin: 2 unpaired electrons, paramagnetic, substitutionally labile. Includes Ni. Example: [[Hexaamminenickel chloride|[Ni(NH)]]].
  :Tetrahedral high-spin: 2 unpaired electrons, paramagnetic, substitutionally labile. Includes Ni. Example: [[Tetrachloronickelate|[NiCl]]].
  :Square planar low-spin: no unpaired electrons, diamagnetic, substitutionally inert. Includes Ni. Example: [[Cyanonickelate|[Ni(CN)]]].