The species which does not undergo disproportionation reaction is:
Show Hint
- \( \text{ClO}_2^- \)
- \( \text{ClO}_4^- \)
- \( \text{ClO}_3^- \)
- \( \text{ClO}_2 \)
The Correct Option is B
Approach Solution - 1
To determine which species does not undergo a disproportionation reaction, we need to understand the concept of disproportionation. A disproportionation reaction is a type of redox reaction in which a single species undergoes both oxidation and reduction, forming two different products.
Let's analyze each given option in the context of chlorine compounds:
- \(\text{ClO}_2^-\): In the disproportionation reaction, this ion can form \(\text{ClO}_3^-\) (oxidation) and \(\text{Cl}^-\) (reduction).
- \(\text{ClO}_2\): This can disproportionate to form higher oxidation state species such as \(\text{ClO}_3^-\) and lower states such as \(\text{Cl}^-\).
- \(\text{ClO}_3^-\): This ion can also undergo disproportionation, forming \(\text{ClO}_4^-\) (oxidation) and \(\text{Cl}^-\) (reduction).
- \(\text{ClO}_4^-\): In this case, the oxidation state of chlorine in \(\text{ClO}_4^-\) is +7, which is its highest possible oxidation state. Because it cannot be oxidized further, it cannot undergo disproportionation.
Conclusion: Thus, the species that does not undergo a disproportionation reaction is \(\text{ClO}_4^-\) because it is already in its highest oxidation state.
Approach Solution -2
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