hard · MCAT chem-phys
The disproportionation reaction 3ClO^-(aq) rightarrow ClO_3^-(aq) + 2Cl^-(aq) occurs in basic solution.
What are the oxidation states of chlorine in each species, and does this reaction correctly represent a disproportionation?
- Cl is +1 in extClO^-, +5 in extClO_3^-, -1 in extCl^-; yes, the same element is oxidized and reduced.
- Cl is -1 in ClO^-, +3 in ClO_3^-, 0 in Cl^-; no, since only reduction occurs overall.
- Cl is +1 in ClO^-, +7 in ClO_3^-, -1 in Cl^-; yes, but electrons are not conserved as written.
- Cl is +1 in all three species since chlorine's oxidation state is fixed by the single negative charge on each ion.
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