Consider the octahedral complex [FeBr6] 4−. In water solution it has an absorption peak at 864 nm with a molar absorptivity (ε) of 3.6 L mol-1 cm-1 . (a) What is the energy (in wavenumbers, cm-1 ) of the absorption peak? Show all work. (b) How many valence d electrons does the metal center have? Justify your answer. (c) How many unpaired electrons per molecule would a magnetic susceptibility experiment predict? What would the S number be for this transition metal center? Justify your answers. (d) What electronic transition results from absorption of 864-nm light? (e) Calculate the ligand stabilization energy (in units of ∆o) and units of coulombic (Πc) energy. (f) How would the ligand field strengths (∆o) of [Fe(NH3)6] 2+ and [Fe(bipy)3] 2+ differ from that of [FeBr6] 4−? Why?

Principles of Modern Chemistry
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ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter8: Bonding In Transition Metal Compounds And Coordination Complexes
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Consider the octahedral complex [FeBr6] 4−. In water solution it has an absorption peak at 864 nm with a molar absorptivity (ε) of 3.6 L mol-1 cm-1 .

(a) What is the energy (in wavenumbers, cm-1 ) of the absorption peak? Show all work.

(b) How many valence d electrons does the metal center have? Justify your answer.

(c) How many unpaired electrons per molecule would a magnetic susceptibility experiment predict? What would the S number be for this transition metal center? Justify your answers.

(d) What electronic transition results from absorption of 864-nm light?

(e) Calculate the ligand stabilization energy (in units of ∆o) and units of coulombic (Πc) energy.

(f) How would the ligand field strengths (∆o) of [Fe(NH3)6] 2+ and [Fe(bipy)3] 2+ differ from that of [FeBr6] 4−? Why?

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