Oxidation and Reduction Reactions Electronic Interpretations

Oxidation is the process which results in the loss of one or more electrons by atoms or ions. Reduction is the process which results in the gain of one or more electrons by atoms or ions. An oxidising agent is one that gains electrons and is reduced, like potassium permanga- 

The equation 4.6.17.1 and 4.6.17.2 must be balanced not only with regard to the number and kind of atoms, but also electrically, that is the not electric charge on each side must be the same. Equation 4.6.17.1 can be balanced by adding one electron to the left hand side and 4.6.17.2 by adding two electrons to the right hand side. 

These partial equations are then multiplied by the coefficients which result in the number of electrons utilised in one reaction being equal to those liberated in the other. 

cancelling the electrons common to both sides, the simple ionic equation is obtained 

all strong electrolytes are completely dissociated, hence only the ions actually taking part or resulting from the reaction need appear in the equation. Substances which are only slightly ionised such as water or which are sparingly soluble and thus yield only as small concentration of ions e.g. silver chloride and barium sulphate are in general written as molecular formulae because they are present mainly in the undissociated state. Equation 4.6.17.4 is an example to prove that oxidation and reductions occurs simultaneously. Ion-electron balance therefore can be performed based on the step mentioned below  

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