OXIDIZING AGENT & REDUCING AGENT( in term of electron gain and loss)/Definition, Concept points, & Examples/

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 Definition

An oxidizing agent -also known as "OXIDIZER" and "OXIDANT"-is a reactant that oxidizes other reactant, by accepting its electron/s. So, oxidizing agent is electron acceptor in  REDOX Reactions.

Examples: O2, O3, Halogens, Sulphuric acid, Nitric acid, and Potassium nitrate.

A Reducing agent - also known as "REDUCTANT" - is a reactant that reduces other reactant, by donating electron/s in REDOX Reactions. So, reducing agent is electron donor in REDOX Reactions.

Examples: H2, CO, Fe, Zn, Formic acid, Alkali metals and Sulphites etc

Concept Points to remember

  • In an oxidizing or reducing agent only one atom is accepting or losing electron/s respectively, not the whole agent.
  • That atom - electron acceptor atom- usually exist in highest oxidation state in Oxidizing agent 
  • That atom - electron donor atom- typically exist in lowest possible oxidation state in reducing agent.   
  • Oxidation number/state of that atom- that accepts electron/s- decreases.
  • Oxidation number/state of atom- that donates electron/s - increases.



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