The complex ion Fe(CN)6 3− is paramagnetic with one unpaired electron. The complex ion Fe(SCN)6 3− has five unpaired electrons. Where does SCN− lie in the spectrochemical series relative to CN−?
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Fe(CN)6 3− has one unpaired electron, which means that the ligand CN− causes a strong crystal field splitting. This results in the d-electrons being paired up in the lower energy orbitals, leaving only one unpaired electron. Show more…
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The complex ion $\mathrm{Fe}(\mathrm{CN})_{6}^{3-}$ is paramagnetic with one unpaired electron. The complex ion Fe(SCN) $_{6}^{3-}$ has five unpaired electrons. Where does $\mathrm{SCN}^{-}$ lie in the spectrochemical series relative to $\mathrm{CN}^{-} ?$
The ion $\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}$ has one unpaired electron, whereas $\left[\mathrm{Fe}(\mathrm{NCS})_{6}\right]^{3-}$ has five unpaired electrons. From these results, what can you conclude about whether each complex is high spin or low spin? What can you say about the placement of $\mathrm{NCS}^{-}$ in the spectrochemical series?
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