Redox reactions

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contains explanation of redox reaction, differences between oxidation and reduction, related pictures and solved examples along with test your understanding section.

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Redox reactions

  1. 1. aNUSHIKA bANSAL lAKSHMI sURESH VAIBHAVI pATEL sHREYA sHARMA VANSHIKA sHARMA Redox reactions
  2. 2. REDOXREACTIONS Oxidation reactions are common events in everyday life : Example- combustion of fossil fuel, Corrosion of metals, Dry cells and accumulators, Metabolism of nutrients in human bodies, Photosynthesis in green plants
  3. 3. Redoxreaction
  4. 4. Oxidation-ReductionReactions  Redox reactions are electron transfer reactions.  The process may involve the complete transfer of electrons to form ionic bonds or only a partial transfer or shift of electrons to form covalent bonds.  In terms of electronic concept, oxidation is the process which involves loss of electrons whereas reduction is the process which involves gain of electrons.
  5. 5. OXIDATION REDUCTION  Oxidation is the loss of electrons by a particle in a reaction, resulting in an increase in the oxidation number.  Ex., Ared – n e- -> Aox  Reduction is the gain of electrons by a particle in a reaction that results in a decrease in the oxidation number.  Ex., BOX + n e- -> Bred
  6. 6. Balancing redox reactions  Describing the overall electrochemical reaction for a redox process requires a balancing of the component half-reactions for oxidation and reduction. In general, for reactions in aqueous solution, this involves adding H+, OH−, H2O, and electrons to compensate for the oxidation changes.
  7. 7. A few examples-
  8. 8. Example 2Al + 6HCl → 2AlCl3 + 3H2 2Al → 2Al3+ + 6e- (oxidation) 6e- + 6H+ → 3H2 (reduction) Al is getting oxidized to 2Al3+. As all metals are reducing agents & 6H+ gets reduced to 3H2. Therefore HCl is the oxidizing agent.
  9. 9. TESTYOURUNDERSTANDING Name the substance oxidized, reduced, oxidizing agent and reducing agent in the following reactions: i. 3MnO2 + 4Al → 3Mn + 2Al2O3 a) MnO2 has lost oxygen to form Mn. Hence MnO2 has been reduced. b) Al has gained oxygen to form 2Al2O3. Hence, Al has been oxidized. c) MnO2 is the oxidizing agent. d) Al is the reducing agent.
  10. 10. ii. 2Na +Cl2 → 2NaCl a) Sodium loses electron to form Na+. Hence, sodium has been oxidized. b) Chlorine gains electrons to form Cl-. Hence, chlorine has been reduced. c) Sodium is the reducing agent.. d) Chlorine is the oxidizing agent.. iii. Cu + 2AgNO3 → Cu(NO3)2 + 2Ag a) Copper has lost electrons to form Cu2+. Hence, copper has been oxidized &, therefore, is a reducing agent.. b) AgNO3 (Ag+ ion) gains electron to form Ag. Hence, AgNO3 has been reduced &, therefore, is an oxidizing agent..

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