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Clear, school‑friendly notes on redox reactions: definitions, oxidation numbers, balancing redox equations, tests and nomenclature.
A redox (oxidation–reduction) reaction is any chemical change where electrons are transferred between species. One species loses electrons (oxidation) while another gains electrons (reduction).
Oxidation is when a substance loses electrons. Other easy ways to spot oxidation are when a substance gains oxygen or loses hydrogen.
Reduction is when a substance gains electrons. It can also be seen as loss of oxygen or gain of hydrogen.
Oxidation numbers help us track electron transfer. Use these simple rules:
For reactions in acidic solution use H⁺ and H₂O to balance oxygen and hydrogen. For basic solutions, after balancing in acid, neutralize H⁺ with OH⁻ to form water.
The oxidizing agent is the species reduced (gains electrons). The reducing agent is the species oxidized (loses electrons).
When a metal has variable oxidation states, indicate the state in Roman numerals in brackets after the metal name.
Balance: Fe²⁺ + MnO₄⁻ → Fe³⁺ + Mn²⁺ in acidic medium.\p>
Balanced: 5Fe²⁺ + MnO₄⁻ + 8H⁺ → 5Fe³⁺ + Mn²⁺ + 4H₂O (electrons balanced: 5e⁻).
Identify oxidizing and reducing agents: Cu + 2Ag⁺ → Cu²⁺ + 2Ag
Ag⁺ is reduced (oxidizing agent); Cu is oxidized (reducing agent).
Clear, school‑friendly notes on redox reactions with a timed practice quiz.
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