[{"data":1,"prerenderedAt":104},["ShallowReactive",2],{"reference-spectrochemical-series":3},{"table":4},{"id":5,"slug":6,"title":7,"shortTitle":8,"category":9,"description":10,"metaDescription":11,"columns":12,"rows":28,"notes":75,"source":82,"relatedTopics":85,"relatedElements":86,"seoKeywords":93,"relatedReferences":100,"tableTitle":102,"tableDescription":103,"seoTitle":8},11,"spectrochemical-series","Spectrochemical Series and Spin States","Spectrochemical Series","coordination-chemistry","A general-chemistry reference for comparing ligand field strength and deciding when octahedral complexes can be high spin or low spin.","Spectrochemical series of ligands from weak to strong field, with the Δoct-versus-pairing-energy rule for high-spin and low-spin complexes.",[13,17,21,25],{"key":14,"label":15,"type":16},"position","Order","number",{"key":18,"label":19,"type":20},"ligand","Ligand","chem",{"key":22,"label":23,"type":24},"name","Name","text",{"key":26,"label":27,"type":24},"trend","Field-strength trend",[29,34,39,43,47,51,55,59,63,67,71],{"position":30,"ligand":31,"name":32,"trend":33},1,"I⁻","iodide","weaker end",{"position":35,"ligand":36,"name":37,"trend":38},2,"Br⁻","bromide","increasing Δoct →",{"position":40,"ligand":41,"name":42,"trend":38},3,"Cl⁻","chloride",{"position":44,"ligand":45,"name":46,"trend":38},4,"F⁻","fluoride",{"position":48,"ligand":49,"name":50,"trend":38},5,"OH⁻","hydroxide",{"position":52,"ligand":53,"name":54,"trend":38},6,"C₂O₄²⁻","oxalate (bidentate)",{"position":56,"ligand":57,"name":58,"trend":38},7,"H₂O","aqua",{"position":60,"ligand":61,"name":62,"trend":38},8,"NH₃","ammine",{"position":64,"ligand":65,"name":66,"trend":38},9,"en","ethylenediamine",{"position":68,"ligand":69,"name":70,"trend":38},10,"NO₂⁻","nitro (N-bound nitrite)",{"position":5,"ligand":72,"name":73,"trend":74},"CN⁻","cyanide","stronger end",[76,77,78,79,80,81],"The order runs from smaller to larger crystal-field splitting for otherwise comparable complexes. It is qualitative, not a universal numerical scale.","For octahedral d⁴, d⁵, d⁶, and d⁷ complexes, compare Δoct with the electron-pairing energy P: Δoct \u003C P gives high spin; Δoct > P gives low spin.","Metal identity, oxidation state, 3d/4d/5d row, geometry, and the full ligand environment all affect Δ. A ligand name alone is not a complete spin-state calculation.","For a mixed-ligand complex, there is no strongest-ligand-wins rule. Use a supplied Δoct/P comparison or experimental spin information. If neither is available and the d count is spin-sensitive, the spin state may be underdetermined.","For octahedral d⁰ to d³ and d⁸ to d¹⁰ configurations, field strength does not create two alternative high-spin and low-spin fillings.","Tetrahedral complexes are ordinarily treated as high spin in general chemistry because Δtet is small. Square-planar d⁸ complexes use a different splitting pattern and should be analyzed separately.",{"label":83,"url":84},"Ligand ordering based on OpenStax Chemistry 2e, Section 19.3 (Spectroscopic and Magnetic Properties of Coordination Compounds), extended with OH⁻ and oxalate per the standard spectrochemical series.","https://openstax.org/books/chemistry-2e/pages/19-3-spectroscopic-and-magnetic-properties-of-coordination-compounds",[9],[87,88,89,90,91,92],"Mn","Fe","Co","Ni","Cu","Pt",[94,95,96,97,98,99],"spectrochemical series","strong field ligands","weak field ligands","high spin low spin","crystal field splitting","coordination chemistry",[101],"formation-constants","Ligand Field Strength (Weak to Strong)","Compare Δoct with the pairing energy P: Δoct \u003C P gives high spin, Δoct > P gives low spin.",1787246032631]