Mn, Fe, and Co in the +2 and +3 oxidation states all form hexaaquacomplexes in acidic aqueous solution. The reduction reactions of the three species are represented schematically below, where the water ligands are not shown for simplicity. It is an experimental fact from elec- trochemistry that Mn2+ and Co²+ are more easily reduced than Fe3+; that is, they will more readily accept an elec- tron. Based on the electron configurations of the ions involved, explain why Fe³+ is harder to reduce than Mn2+ and Co²+. Mn3+ + e – Mn²+ Fe* + e –→ Fe²+ Co³+ + e → Co²+

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Mn, Fe, and Co in the +2 and +3 oxidation states all
form hexaaquacomplexes in acidic aqueous solution. The
reduction reactions of the three species are represented
schematically below, where the water ligands are not
shown for simplicity. It is an experimental fact from elec-
trochemistry that Mn2+ and Co²+ are more easily reduced
than Fe3+; that is, they will more readily accept an elec-
tron. Based on the electron configurations of the ions
involved, explain why Fe³+ is harder to reduce than Mn2+
and Co²+.
Mn3+ + e – Mn²+
Fe* + e –→ Fe²+
Co³+
+ e → Co²+
Transcribed Image Text:Mn, Fe, and Co in the +2 and +3 oxidation states all form hexaaquacomplexes in acidic aqueous solution. The reduction reactions of the three species are represented schematically below, where the water ligands are not shown for simplicity. It is an experimental fact from elec- trochemistry that Mn2+ and Co²+ are more easily reduced than Fe3+; that is, they will more readily accept an elec- tron. Based on the electron configurations of the ions involved, explain why Fe³+ is harder to reduce than Mn2+ and Co²+. Mn3+ + e – Mn²+ Fe* + e –→ Fe²+ Co³+ + e → Co²+
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