I have been given a complex coordination entity [Cu(NH3)4]2+
I have to find its hybridization by valence bond theory.
Now NH3 is a weak field ligand. But its a square planar compound. In one book its shown that it is sp2d and in other it is given
dsp2..
Which is correct ? Oxidation of Cu is +2.. Will electron in Cu2+ be promoted from 3d orbital to 4p in presence of the given ligand ? Which
book is correct ?
But its a square planar compound. In one book its shown that it is sp2d and in other it is given dsp2..
Which is correct ?
Explain what you consider the difference between these two.
Cu has electronic configuration 1s22s22p63s23p63d104s1
Cu(2+) will have, 1s22s22p63s23p63d9
Now there is one unpaired electron in 3d orbital. Now it is said in one book that the one electron from 3d orbital promotes itself to 4p because as
per crystal field theory one d orbital in square planar has very high energy. Hence hybridization is dsp2, d orbital from inner 3d
subshell.
In other book it was given that the unpaired electron if permanently promoted to 4p will get lost and so it remains in 3d and 4p both..keeps
oscillating. Hence we leave 3d and 4p out and hence the hybridization sp2d with d orbital from 4d subshell.
