Question

In the reaction, \[C{l_2} + O{H^ - } \to C{l^ - } + Cl{O_3}^ - + {H_2}O\] chlorine is :
A. Oxidized
B. Reduced
C. Oxidized as well as reduced
D. Neither oxidized or reduced

Answer 1

Hint: We also remember that the chlorine gas reacts in different ways according to the temperature and concentration of the solution and it gives different products. The reaction undergoes disproportionation but in presence of the alkali the halogen is oxidized or reduced let’s see. We have to remember that the substance which gets reduced is known as oxidising agent while the substance which gets oxidised is known as reducing agent.

Complete step by step answer:
Firstly, let’s have a clear idea about oxidation and reduction and how redox occurs.
Reduction: It is a process during which an atom gains an electron and therefore decreases (or reduces its oxidation number). In the words, the positive character of the species is reduced.
Oxidation: It is a process during which an atom loses an electron and therefore increases its oxidation number.
So basically, redox reactions are reactions in which one species is reduced while the other is oxidized in which the oxidation states of the species changes ultimately.
\[C{l_2} + O{H^ - } \to C{l^ - } + Cl{O^ - }_3 + {H_2}O\]
Since, there is both decrease and increase of oxidation states so \[Cl\] is undergoing oxidation as well as reduction.
Option A: Cl is not only oxidised but also reduced. So this option is wrong.
Option B: Cl is not only reduced but also oxidised. So this option is wrong.
Option C: Cl is both oxidised and reduced. So this option is correct.
Option D: Cl is not only oxidised but also reduced. So this option is wrong.

So, the correct answer is Option C.

Note: We must remember that the same reaction will give different products when temperature and concentrations are changed. Cold dilute sodium hydroxide will give sodium chloride, and water products. We have to know that there are some general rules to be followed when we calculate oxidising agents of substance. There are two points which we need to remember that are,
For a neutral compound, oxidation number for all is zero which also does not have any charge.
In an ion, the oxidation number must have charge of an ion.