[{"data":1,"prerenderedAt":94},["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":68,"source":75,"relatedTopics":79,"relatedElements":80,"seoKeywords":87},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 reference table with increasing ligand field strength, the Δoct versus pairing-energy rule, and guidance for high-spin, low-spin, and mixed-ligand 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],{"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,"H₂O","aqua",{"position":52,"ligand":53,"name":54,"trend":38},6,"NH₃","ammine",{"position":56,"ligand":57,"name":58,"trend":38},7,"en","ethylenediamine",{"position":60,"ligand":61,"name":62,"trend":38},8,"NO₂⁻","nitro (N-bound nitrite)",{"position":64,"ligand":65,"name":66,"trend":67},9,"CN⁻","cyanide","stronger end",[69,70,71,72,73,74],"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–d³ and d⁸–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":76,"url":77,"license":78},"OpenStax Chemistry 2e, Section 19.3 — Spectroscopic and Magnetic Properties of Coordination Compounds","https://openstax.org/books/chemistry-2e/pages/19-3-spectroscopic-and-magnetic-properties-of-coordination-compounds","CC BY 4.0",[9],[81,82,83,84,85,86],"Mn","Fe","Co","Ni","Cu","Pt",[88,89,90,91,92,93],"spectrochemical series","strong field ligands","weak field ligands","high spin low spin","crystal field splitting","coordination chemistry",1785108608438]