How many unpaired electrons would you expect for the following complex ions?
I know that #1 is high spin and #2 is low spin, but somehow I still don’t get how many unpaired electrons there are. Please help!
oxidation state of manganese here is +2 that is 3d^5 . flourides are poor ligands and can not force the outer electrons in Manganese to be paired up. Mn^2+ undergoes sp^3d^2 hybridisation to accommodate six ligand pairs. Hence the complex contains five unpaired electrons in the central atom. ethylene diamine (en) is a neutral ligand. Oxidation state of Ruthenium is +2 it contains six valence electrons . en is a strong ligand and can force the electrons to pair up. So the central atom undergoes d^2sp^3 hybridisation and contains no unpaired electrons.
remember when they taught you about shells
something like that?
use that in order to draw the whole thing when you finish you will have some e- unpaired I believe
remember ? like only one arrow up instead of one up one down?
sorry I don’t know how to explain it any further but that is how I would do it