Oxidizing and Reducing agent
Oxidation and reduction reactions are always found to go hand in hand during a redox reaction. Thus in the oxidation-reduction process, one element or compound oxidizing agent, another element or compound must be simultaneously reducing agent.
- According to the electronic concept, the oxidizing agent gains electrons and reduced to a lower oxidation number or state.
- A reducing agent losses electrons and oxidized to a higher oxidation state or number.
Concept of oxidation and reduction reaction
Classically oxidation has defined as the combination of oxygen or electronegative element with another element or compound or as the removal of hydrogen or electropositive element from a chemical compound.
In the same way, the reduction has defined as the combination of hydrogen or electropositive element with another element or compound or as the removal of oxygen or electronegative element from a chemical compound.
The electronic structure of elements gives the quantitative relations between classical and electronic concept oxidation and reduction reaction.
2Mg + O2 ⇆ 2MgO
On the above reaction magnesium metal burns in oxygen to produce magnesium oxide with the addition of oxygen. Thus the balanced chemical equations of the above reaction
2Mg → 2Mg+2 + 4e
O2 + 4e → 2O-2
In this reaction, oxygen led to the removal of two electrons from zerovalent magnesium metal by forming magnesium(II) ion. On the other hand, the lost electrons accept oxygen by forming oxide ion.
Thus shows that the classical definition of oxidation-reduction has an intimate connection with the electronics concept.
Oxidation of the reducing agent
Combination of oxygen examples
- Carbon burns in oxygen to produce carbon dioxide. Here oxygen forming chemical bonds with carbon to produce carbon dioxide. Thus carbon can be act as a reducing agent in this oxidation process.
C + O2 ⇆ CO2
- Magnesium metal reacts with chlorine to produce magnesium chloride. In this reaction, magnesium combines with oxygen to produced magnesium oxide. Thus magnesium can be oxidized.
Mg + Cl2 ⇆ MgCl2
- When ferrous oxide heated in oxygen to produce ferric oxide. Here ferrous oxide oxidized.
4FeO + O2 ⇆ 2Fe2O3
Combination of electronegative element examples
When Cl2 passes through the colorless FeCl2 solution, it turns red FeCl3. This is the example of oxidation, by the addition of the electronegative elements.
2FeCl2 + Cl2 ⇆ 2FeCl3
Removal of hydrogen examples
- When MnO2 reacts with concentrated HCl, it produces greenish-red Cl2 gas. Here hydrogen can be removed from HCl to form Cl2, hence the removal of hydrogen means oxidation. Thus HCl can be oxidized.
4HCl + MnO2 ⇆ MnCl2 + Cl2 + H2O
- H2S reacts with Cl2 to produce sulfur. In this reaction, remove hydrogen from H2S. Thus H2S oxidized to form sulfur.
H2S + Cl2 ⇆ 2HCl + S↓
Removal of electro-positive elements examples
When KI reacts with hydrogen peroxide, it produces iodine. Here electro-positive potassium removes from KI to form iodine. Thus KI can be oxidized.
2KI + H2O2 ⇆ 2KOH + I2
Reduction of the oxidizing agent
Addition of hydrogen examples
- When bromine reacts with hydrogen, it produces hydrogen bromide. Here bromine can be act as an oxidizing agent in this reduction process.
H2 + Br2 ⇆ 2HBr
- When H2S reacts with chlorine to produce hydrogen chloride and sulfur. Here chlorine combines with hydrogen and reduced.
H2S + Cl2 ⇆ HCl + S↓
Addition of electro-positive elements examples
In the above reaction potassium ferricyanide combine with electro-positive element potassium to produce potassium ferrocyanide. Thus potassium ferricyanide reduced.
Removal of oxygen reduction examples
When hydrogen passes through black heated CuO, oxygen removes from CuO to form red copper. Thus CuO is reduced.
CuO + H2 ⇆ Cu +H2O
Removal of electro-negative elements examples
When SO2 passes through a red ferric sulfate solution, it turns into a greenish ferrous sulfate solution.
Fe₂(SO₄)₃ + 2SO₂ + H₂O ⇆ 2FeSO₄ + 2H₂SO₄
In the above reaction, electronegative sulfate removes form ferric sulfate. Thus ferric sulfate reduced to form ferrous sulfate.