Oxidizing and Reducing Agent
Oxidation reduction reaction or Oxidizing and reducing agents are always going hand to hand in the chemical process or redox reactions. In learning chemistry, the oxidation reduction process or reaction, one element, or molecule oxidizing agent, another chemical element or molecule must be simultaneously reducing agent. According to the electronic concept, the oxidizing agent gains electrons and is reduced to the lower oxidation number or state but the reducing agent losses electrons and oxidized to the higher oxidation state or number in the chemical reaction.
For example, the formation of crystalline solid magnesium oxide by an oxidation reduction reaction. Each magnesium atom loses two electrons to form a magnesium ion and a neutral oxygen atom gains two electrons to form an oxygen ion. These two ions bonding to form a closed packed type crystal lattice. Oxidation reduction reaction going hand to hand with the formation of magnesium oxide (MgO).
Classical Concept of Oxidation Reduction
Oxidation is classically defined as the combination of oxygen or electronegative element with another element or compound or the removal of hydrogen or electropositive element from a chemical compound. In the same way, reduction has defined as the combination of hydrogen or electropositive element with another element or compound or the removal of oxygen or electronegative element from a chemical compound. In oxidation reduction reaction, magnesium metal, burns in oxygen to produce magnesium oxide with the addition of oxygen is called oxidation.
Electronic Concept of Oxidation Reduction
The electronic structure of elements gives the quantitative relations between classical and electronic concept oxidation and reduction reaction.
2Mg → 2Mg+2 + 4e
O2 + 4e → 2O-2
In the above balancing equations, oxygen has to lead to the removal of two valence orbital electron particles from magnesium metal to form a stable zero-valance Mg (II) ion. On the other hand, the lost electron have found new homes in oxygen to form O-2 ions. Therefore, the classical definition and examples of oxidation reduction reactions have an intimate connection with the electronics concept.
Examples of Oxidizing Agent
Combination of Oxygen examples
All the hydrocarbon like methane, ethane, propane, etc readily burns in excess air or oxygen to form carbon dioxide and water but controlled oxidation gives various products. For example, oxidation in the presence of boric acid produces a mixture of secondary alcohols. Oxidizing reagents such as potassium permanganate really oxidizes tertiary hydrogen atoms to form the hydroxyl group.
CH3-CH3 + 3[O] → 2CO2 + 3H2O
(CH3)3CH + [O] → (CH3)3COH
Combination of electronegative element
Group-17 elements in the periodic table stable on negative oxidation state and oxidation power decreases from fluorine to iodine. Therefore, the electronegative elements chlorine oxidizes the colorless FeCl2 solution to red FeCl3.
2FeCl2 + Cl2 ⇆ 2FeCl3
Removal of hydrogen examples
4HCl + MnO2 ⇆ MnCl2 + Cl2 + H2O
Oxidation of hydrogen sulfide to sulfur in the presence of nitric acid. In this oxidation reduction reaction, hydrogen can remove from the hydrogen sulfide molecule.
H2S + 2HNO3 ⇆ S↓ + 2NO2 + 2H2O
Removal of electro-positive elements
2[Fe(CN)6]4- + H2O2 +2H+ → 2[Fe(CN)6]4- + 2H2O
Example of Reducing Agent
Addition of hydrogen examples
Alkenes are rapidly added hydrogen atom or hydrogenated under pressure in the presence of chemical catalyst like platinum or palladium surface in oxidation reduction reaction (C2H4 + H2 → C2H6). Reduction of monocarboxylic acid in organic chemistry. The deduction of monocarboxylic acid depends on the nature of reducing agents, heat, and catalyst used. Therefore, monocarboxylic acid like acetic acid heating with hydrogen iodide and red phosphorus under pressure or with hydrogen under pressure at specific heat in the presence of nickel catalyst produces an alkane or RCO2H + 3H2 → RCH3 + 2H2O.
Addition of electro-positive elements examples
2K3[Fe(CN)6] + 2KOH + H2O2 ⇆ 2K4[Fe(CN)6] + 2H2O + O2
In the above oxidation reduction reaction, potassium ferricyanide combines with the electro-positive element potassium to produce potassium ferrocyanide.
Removal of oxygen oxidizing agent
CuO + H2 ⇆ Cu +H2O
Removal of electro-negative elements
When SO2 passes through a red ferric sulfate solution, it turns into a greenish ferrous sulfate and sulfuric acid.
Fe2(SO4)3 + 2SO2 + H2O ⇆ 2FeSO4 + 2H2SO4
In the above reaction, electronegative sulfate removes from ferric sulfate and ferric sulfate is reduced to form ferrous sulfate in oxidation reduction or redox reaction.