How many unpaired electrons would you expect for the following complex ions?
1. [MnF6]^4-
2. [Ru(en)3]^2+
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!
2 Answers
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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.
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remember when they taught you about shells
1s
2s
2s2s
3s3p3d
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
