- Oxidation: The loss of electrons by a substance.
- Reduction: The gain of electrons by a substance.
- Oxidizing Agent: A substance that causes another substance to be oxidized by accepting electrons itself (it is reduced).
- Reducing Agent: A substance that causes another substance to be reduced by donating electrons itself (it is oxidized).
- 1. Can be an oxidizing agent for Pb but not Sn²⁺: A species with a reduction potential higher than Pb²⁺/Pb but lower than Sn⁴⁺/Sn²⁺ (e.g., Cu²⁺).
- 2. Can be reduced by I⁻ but not by Fe²⁺: A species with a reduction potential lower than I₂/I⁻ but higher than Fe³⁺/Fe²⁺ (e.g., Br₂).
- 3. Can be oxidized by I₂ but not acidic SO₄²⁻: A species with a reduction potential lower than I₂/I⁻ but higher than SO₄²⁻/SO₂ (e.g., Fe²⁺).
- 4. Can oxidize Co and reduce H⁺: A species with a reduction potential higher than Co²⁺/Co but lower than H⁺/H₂ (e.g., Zn²⁺).
- Cr³⁺(aq) + e⁻ → Cr²⁺(aq): Reduction
- Li(s) → Li⁺(aq) + e⁻: Oxidation
- S(s) + 2e⁻ → S²⁻(aq): Reduction
- Sn²⁺(aq) → Sn⁴⁺(aq) + 2e⁻: Oxidation
Parent Tip: Review the logic above to help your child master the concept of oxidation and reduction worksheet.
