Question

<!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> Explain redox reactions based on electron transfer. Give suitable examples.

Answer 1

<!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> In a redox reaction if one species loses electrons it’s considered to be undergoing oxidation reaction and acts as oxidising agent or oxidant. [0.5 mark]

The species who accepts electrons are said to undergo reduction and behave as a reducing agent. [0.5 mark]

For example:
$Zn+2HCl\to ZnC{l}_2+H_2$ [0.5 marks]

Here, zinc loses electrons to the electronegative atom Cl. The reduction and oxidation reaction involved are given below:
Oxidation: $Zn\to Z{n}^{2+}+2e^{-}$ [0.25 marks]
Reduction: $2H^{+}+2e^{-}\to H_2$ [0.25 marks]

Thus the transfer of electrons causes the redox reaction to occur.