Oxidation and Reduction

  • Oxidation and Reduction, often referred to as Redox, are two fundamental concepts in Chemistry.

  • Oxidation is defined as the loss of electrons, which can lead to an increase in oxidation state. It involves the addition of oxygen or removal of hydrogen.

  • Reduction is the gain of electrons leading to a decrease in the oxidation state. It involves the removal of oxygen or addition of hydrogen.

  • Redox reactions are vital in many chemical processes, including battery operations, reactions in biological systems or industrial processes like the extraction of metals from ores.

  • The Redox concept is also applied in electrochemical cells, where spontaneous Redox reactions occur, generating electrical energy.

  • Oxidation and Reduction always occur simultaneously. A species cannot be oxidised unless another is reduced. This is because the electrons lost by one species in the oxidation half-reaction are gained by another species in the reduction half-reaction.

  • In Redox reactions, the substance that is oxidised is the reducing agent, as it reduces the other substance by donating its electrons to it.

  • Similarly, the substance that is reduced is the oxidising agent, as it oxidises the other substance by accepting its electrons.

  • Oxidation numbers (states) are used to keep track of the electrons in a Redox reaction. The rules for assigning these numbers can be a useful tool for determining if a Redox reaction has taken place and to what extent.

  • A Redox equation can be balanced by the half-reaction method, separating the overall reaction into an oxidation half-reaction and a reduction half-reaction.

  • Remember to consider the atom economy and the energy requirements of the Redox reactions, particularly in the context of sustainable chemistry.

  • Familiarize yourself with common oxidising and reducing agents, their properties,Applications, and the potential hazards associated with their use.

  • Practice with various examples of redox reactions, balancing redox equations, and drawing electrochemical cells to ensure full understanding and retain the information.