Discussion of the results
Reduction of dichromate in acidic media often is described
by the following half-reaction:
Cr2O72-(aq) +
14H+(aq) + 6e-
→ 2Cr3+(aq) + 7H2O
The ion Cr2O72-(aq)
is bright orange and the ion Cr3+(aq)
is dull bluish/violet.
In many cases, the half-reaction, given above, apparently
is too much of a simplification and in reality things are more complex.
When dichromate is reduced by ethanol in nitric acid or
sulphuric acid, then the half-reaction is a reasonable approximation. The
observed colors are close to the color of a plain hydrated chromium (III) salt,
when it is dissolved in water. When hydrochloric acid is used as the donor for
the required H+ ions, then the newly formed chromium ions are
coordinated to chloride ions and a green compound is formed. When dilute
hydrochloric acid is added to a dull bluish solution of a chromium (III) salt,
then no change of color from bluish/violet to green is observed, so one can
conclude that the formation of a chloride-chromium (III) complex is combined
with the redox reaction.
Reduction of dichromate by sulfite in acidic media can
better be regarded as reduction of dichromate by sulphur dioxide. When
dichromate is reduced by sulphur dioxide, then a green chromium (III) compound
is formed, regardless of the acid, used for supplying the H+ ions.
Probably a chromium-sulfate complex is formed, with the sulphur dioxide being
transformed to sulfate by transfer of electrons to the SO2 molecule
and addition of oxygen ligands from the dichromate ion. On formation of the
chromium (III) core, the newly formed sulfate ion may be coordinated. More
research, however, is necessary to see whether this theory is correct or not.
The observation, that reduction and coordination are
combined in a single reaction, is used in preparative chemistry. Frequently,
chromium (III) complexes are made, either by reducing dichromate by a certain
reductor, or in the presence of a certain ligand, or by oxidizing chromium (II)
in the presence of a certain ligand.
Chromium (III) complexes are inert, meaning that ligands
are exchanged only very slowly. This also explains why simple addition of
hydrochloric acid to a plain aqueous chromium (III) solution does not result in
formation of the green chloro-complex. The Cr3+(aq)
ion, better described as Cr(H2O)63+ is quite
stable and the H2O ligands are only replaced slowly. When, however,
chromium (III) is formed, then the ligands are coordinated on formation and then
the presence of a certain ligand may favor the formation of certain complexes
over formation of other complexes.
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