Nine of a possible eleven solid complexes were tested for magnetic properties using a magnetic susceptibility balance. From this data, the number of unpaired electrons were calculated using an estimate value of √(1+ μeff2)-1. These experimental numbers were compared to the calculated number of unpaired electrons simply using ligand charges. Both values showed similar results.
[...] For the purpose of this experiment, we are measuring the magnetic susceptibility of a material and to measure this accurately we need to zero the balance for the materials that have this susceptibility, namely the paramagnetic compounds Complete the table below, following the methods in the lab instructions (m0 is the mass of the empty tube) 4. Choose one of the transition metal compounds from the table above, and be sure that your lab partner chooses a different one. Determine the number of unpaired electrons, showing all calculations, and using both calculation schemes: the first being the number of unpaired electrons based on the charge on the ligands; the second method being described in the lab instructions. [...]
[...] The following are paramagnetic (unpaired d-electrons): HgCo(SCN)4, MnSO4◦2H20, MnO Cu(HCOO)2◦2H Mn2O Ni(en)3S2O Co(NH4)2(SO4)2◦6H Fe(NH4)2(SO4)2◦6H In K4Fe(CN) 6.3 H2O, the oxidation state of Fe is and in Fe(NH4)2(S04) 2.6 H2O the oxidation of Fe is also +2. However, K4Fe(CN) 6.3 H2O has 6 low spin CN- ligands and will show an octahedral complex. These low spin ligands will split the d-orbitals into a low energy t2g and a high energy eg. As a result, the d6 electrons from the Fe2+ will fully fill the lower energy t2g level, resulting in all paired electrons. [...]
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