Chemistry NCERT Exemplar Solutions Class 11th Chapter Eight

This is a Long answer type question as classified in NCERT Exemplar

We can calculate the oxidation states by - ]

NaClO₄ Oxidation no. of chlorine = +7 

Suppose oxidation number of chlorine is x then,  1 + x + 4 * (−2) = 0

∴ x - 7 = 0 

    x = +7

We can calculate, the oxidation states, as given below-

NaClO₃ Oxidation no. of chlorine = +5

? NaClO Oxidation no. of chlorine = +1

? KClO₂ Oxidation no. of chlorine = +3

? Cl₂O₇ Oxidation no. of chlorine = +7

ClO₃ Oxidation no. of chlorine = +6

Cl₂O Oxidation no. of chlorine = +1 

NaCl Oxidation no. of chlorine = −1

Cl₂ Oxidation no. of chlorine = 0

ClO₂ Oxidation no. of chlorine = +4.

Oxidation state (+2) is not present in any of the above compounds.

This is a Long answer type question as classified in NCERT Exemplar

Disproportionate is defined as the reaction in which one compound of intermediate oxidation state converts to two compounds, one of higher and one of lower oxidation states So, to occur such type of redox reaction, the element should exist in at least three oxidation states. So that element present in the intermediate state and it can change to both higher and lower oxidation state during disproportionate reaction. Fluorine is the most electronegative element and a strong oxidizing agent and is the smallest in size of all the halogens. It does not show a positive oxidation state (shows only −1 oxidation state) and hence, does not undergo disproportionate reaction.