easechemistry

  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-Reduction Reactions REDOX Reactions Oxidation reduction reactions are also known as REDOX reactions. In oxidation reduction reactions electrons move between the atoms. In the figure below atom "A" giving electron,so in atom "A" oxidation is taking place and atom B is receiving that electron so in atom "B" reduction is taking place.As atom "A" is giving electron so its positive charge increases i.e its OXIDATION NUMBER is increasing and atom " B" is receiving electron so its positive charge decreases i.e its OXIDATION NUMBER is decreasing. Oxidation and reduction are the name of processes. Atom  "A" in which oxidation occurs get oxidized and the atom "B" in which reduction occurs get reduced. So, we can define as " Oxidation is loss of electrons and increase of oxidation number and reduction is gain of electrons and decrease in oxidation number." Table is giving summary Of definition for REDOX REA...