Why is [NiF6]2- Diamagnetic Despite F- Being a Weak Field Ligand?

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SUMMARY

The discussion centers on the diamagnetism of the octahedral complex [NiF6]2-, despite fluoride (F-) being classified as a weak field ligand. Participants clarify that the oxidation state of nickel in this complex is +4, resulting in a d6 electron configuration. The key conclusion is that the effective atomic number (EAN) theory indicates that the complex behaves as if it has a filled d-orbital configuration, leading to its diamagnetic nature, contrary to expectations based on ligand field strength.

PREREQUISITES
  • Understanding of the spectrochemical series of ligands
  • Knowledge of octahedral complex geometry
  • Familiarity with electron configurations and oxidation states
  • Concept of effective atomic number (EAN) theory
NEXT STEPS
  • Study the spectrochemical series in detail to understand ligand field strength
  • Learn about the differences between high spin and low spin complexes
  • Research effective atomic number (EAN) theory and its applications in coordination chemistry
  • Explore the magnetic properties of transition metal complexes
USEFUL FOR

Chemistry students, particularly those studying coordination chemistry, as well as educators and researchers interested in the properties of transition metal complexes.

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Homework Statement



So I'm looking at the spectrochemical series of ligands which has that

I- < Br- < Cl- < F- < OH- < ox2- < H20 < NH3 < en <bpy< phen <CN-

Where the left side are weak field ligands and the right side are strong field ligands.

A lot of my homework problems involve me looking at an octahedral complex and deciding whether the complex is low or high spin and then figuring out if the complex is diamagnetic or not.


From problems I have been doing and google searches, I have found that H20 is a weak field ligand and NH3 is strong field.

I can't understand why [NiF6]2- is diamagnetic. F- should be a weak field ligand, which would mean it would lead to a high spin complex. The Ni should have an oxidation state of +4 making it d6, and in a high spin octahedral d6 complex it will not be diamagnetic. It can only be diamagnetic if it was low spin. But why is it low spin if F- is a weak field ligand?

Homework Equations





The Attempt at a Solution

 
Physics news on Phys.org
Actually We reasoned it out on the basis of Sidgwicks theory. the EAN( effective nuclear charge) it comes out to be 36 corresponding to Krypton
 
Last edited:

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