Master this deck with 31 terms through effective study methods.
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Octahedral due to hybridisation of 3d orbitals.
Absence of unpaired electrons.
[CoF6]3- is paramagnetic; [Co(NH3)6]3+ is diamagnetic.
Involves sp3 hybridisation.
Electrons occupy e_g orbitals, forming high spin complexes.
Ranks ligands by their field strength effects.
Indicates presence of five unpaired electrons.
Repulsion between d electrons and ligand charges.
Color results from d-d electron transitions.
Involves dsp2 hybridisation.
Electrons pair up in lower energy orbitals.
They cause larger splitting of d orbitals.
dsp2 hybridisation leading to square planar geometry.
Low spin configurations are rarely observed.
They facilitate bonding between metal and ligands.
Nickel in +2 state leads to paramagnetism.
The substance becomes colorless due to no crystal field splitting.
The hydrated form is blue, while the anhydrous form is white.
The color changes from green to pale blue.
The presence of unpaired electrons in [NiCl4]2– causes paramagnetism.
It suggests anionic ligands should cause the greatest splitting, which is not observed.
Emerald transmits green light due to Cr3+ ions, while ruby appears red.
It has a tetrahedral structure.
They are used for qualitative and quantitative analysis through color reactions.
It forms stable complexes with Ca2+ and Mg2+ ions for titration.
They are essential for functions like oxygen transport in hemoglobin.
Gold forms a soluble complex, [Au(CN)2]–, facilitating extraction.
It involves synergic bonding that strengthens the M–C bond.
Inner orbital complexes use d orbitals for bonding, while outer do not.
It removes toxic metal ions from biological systems using ligands.
It appears blue/purple due to ligand substitution.