What determines the size of an ion in an octahedral complex?

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SUMMARY

In octahedral complexes, the ionic radius of Fe2+ is larger than that of Co2+ due to the differences in their electronic configurations and the effects of strong field ligands. Strong field ligands cause greater splitting of the d-orbitals, leading to a higher effective nuclear charge experienced by the electrons in Co2+, which results in a smaller ionic radius compared to Fe2+. Understanding the influence of ligand field strength on ionic size is crucial for predicting the behavior of transition metal complexes.

PREREQUISITES
  • Understanding of octahedral coordination geometry
  • Knowledge of ligand field theory
  • Familiarity with transition metal electronic configurations
  • Concept of ionic radii and their measurement
NEXT STEPS
  • Research the impact of ligand field strength on ionic radii in transition metal complexes
  • Study the electronic configurations of transition metals, focusing on Fe2+ and Co2+
  • Learn about the differences between strong field and weak field ligands
  • Explore the concept of crystal field splitting and its implications in coordination chemistry
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Chemistry students, researchers in coordination chemistry, and professionals working with transition metal complexes will benefit from this discussion.

lord12
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An an octahedral complex with all strong field ligands, which ion has the larger radius, Fe2+ or Co2+? What are the rules for known the size of the ion with respect if its a weak or strong field ligand?
 
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