Which of the following statement(s) is/are not true about the following decomposition reaction?

2KClO₃→ 2KCl + 3O₂

(i) Potassium is undergoing oxidation

Potassium has a general oxidation number of +1 as it as a group 1 alkali member. In KClO₃ and KCl the charge on potassium does not change so it is not going under oxidation but has same ON in both the compounds.

(ii) Chlorine is undergoing oxidation

The oxidation number of Cl in KClO₃ is

→

And that in KCl is -1, so the change is from +5 to -1 which shoes reduction in oxidation number thus the statement is wrong.

(iii) Oxygen is reduced

As only atom having high electronegativity in periodic table is F, only with fluorine compounds oxygen shows positive charge or oxidation number, thus oxygen here is not reduced as also justified that both reactant and product oxygen molecule shows -2 oxidation number.