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Oxidation-Reduction (Redox) Reactions

Redox reactions involve the transfer of electrons between species, resulting in changes in oxidation states. They are essential for energy production, corrosion, and many chemical processes.

Key Concepts

  • Oxidation: Loss of electrons (increase in oxidation state)
  • Reduction: Gain of electrons (decrease in oxidation state)
  • Oxidizing agent: Species that is reduced, causes oxidation
  • Reducing agent: Species that is oxidized, causes reduction

Identifying Redox Reactions

  1. Assign oxidation numbers to all elements in the reaction.
  2. Look for changes in oxidation numbers.
  3. Determine which species is oxidized and which is reduced.

Example

Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s)

  • Zn: 0 → +2 (oxidation)
  • Cu: +2 → 0 (reduction)
  • Zn is the reducing agent; Cu²⁺ is the oxidizing agent

Types of Redox Reactions

  • Combination reactions: Two elements combine, electrons are transferred
  • Decomposition reactions: Single compound breaks down, electron transfer occurs
  • Displacement reactions: One element replaces another in a compound
  • Combustion reactions: Rapid oxidation producing energy

Importance

  • Fundamental to batteries, corrosion, metabolism, and industrial processes
  • Helps predict reaction feasibility and electron flow in chemical systems

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