In the following balanced equation: Cl 2 aq + 2 KI aq → 2 KCl aq + I 2 aq Deduce the oxidation states of chlorine and iodine in the reactants and products.

The total number of electrons gains or losses by an element in a chemical reaction are called oxidation state or oxidation number. Cl 2 aq + 2 KI aq → 2 KCl aq + I 2 aq In the above given reaction the oxidation states of chlorine and iodine are as follows, Name of the element Oxidation state in the reactants Oxidation state in the products Chlorine 0 in Cl 2 - 1 in KCl Iodine - 1 in KI 0 in I 2

In the following balanced equation: Cl 2 aq + 2 KI aq → 2 KCl aq + I 2 aq Deduce the oxidation states of chlorine and iodine in the reactants and products.

The total number of electrons gains or losses by an element in a chemical reaction are called oxidation state or oxidation number. Cl 2 aq + 2 KI aq → 2 KCl aq + I 2 aq In the above given reaction the oxidation states of chlorine and iodine are as follows, Name of the element Oxidation state in the reactants Oxidation state in the products Chlorine 0 in Cl 2 - 1 in KCl Iodine - 1 in KI 0 in I 2

In the following balanced equation: Cl 2 aq + 2 KI aq → 2 KCl aq + I 2 aq State which element is oxidised and which element is reduced.

The element which losses electrons is oxidised and the one which gets electrons will be reduced. Cl 2 aq + 2 KI aq → 2 KCl aq + I 2 aq In the above given reaction the oxidation states of chlorine and iodine are as follows, Name of the element Oxidation state in the reactants Oxidation state in the products Chlorine 0 in Cl 2 - 1 in KCl Iodine - 1 in KI 0 in I 2 From the above table it is observed that the oxidation state of chlorine changed from 0 to - 1 , so chlorine reduced by gaining one electron and the oxidation state of iodine changed from - 1 to 0 . Hence, iodine oxidised by losing one electron. So it is a redox reaction.

In the following balanced equation: Cl 2 aq + 2 KI aq → 2 KCl aq + I 2 aq Identify the oxidising agent and reducing agent.

The element which has the ability to oxidise other element is called oxidising agent and the element which has the ability to reduce other element is called reducing agent. Cl 2 aq + 2 KI aq → 2 KCl aq + I 2 aq In the above given redox reaction the oxidation states of chlorine and iodine are as follows, Name of the element Oxidation state in the reactants Oxidation state in the products Chlorine 0 in Cl 2 - 1 in KCl Iodine - 1 in KI 0 in I 2 Oxidising agent undergoes reduction and reducing agent undergoes oxidation. From the above table it is observed that C l 2 oxidises I - , so Cl 2 is the oxidising agent. And indirectly, I - causes reduction of Cl 2 . Hence, I - is the reducing agent.