12: simply because if Δo<P,then the electrons occupying the upper eg orbitals will have lesser energy than those which are forced to pair up..(by applying more energy)
can there be covalent interaction between orbitals of the metal and ligand in coordination compounds?????????explain briefly
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12. why if Δ0 <P(pairing energy),it will be more favourable energetically to occupy the upper eg level rather than to pair electron ???????
11SEE,ACC TO VALENCE BOND THEORY THERE IS COVALENT INTERACTIONS BETWEEN CENTRAL METAL ION AND THE LIGANDS
NOW IF U CONSIDER THE CRYSTAL FIELD THEORY IT CONSIDERS
THE BOND BET THE METAL AND LIGAND TO BE IONIC .if Δ<P
THE ELECTRON OCUUPIES Eg level so that cfse level is low and the configuration is more stable.
remember if Δ is small high spin state more stable
and if Δ large then low spin state more stable
11: ya..for example in case of dimethylglyoxime, one N atom coordinates and the other forms a covalent bond.
1NO WE NEED to have a donating electron to the ligand rather than a co-ordinate bond(sharing electrons) there
But if the metal has more electrons to donate with other ligands then it will