Which one of the following species is NOT capable of showing disproportionation reaction?
Understanding Disproportionation Reactions
A disproportionation reaction is a specific type of redox reaction where an element in a particular oxidation state is simultaneously oxidized to a higher oxidation state and reduced to a lower oxidation state. For an element to undergo disproportionation, it must be in an intermediate oxidation state. This means the element can be both increased and decreased in oxidation number from its current state.
Let's examine the oxidation state of chlorine in each of the given species to determine which one cannot undergo disproportionation.
Calculating Oxidation States of Chlorine in Oxyanions
We can calculate the oxidation state of chlorine in each oxyanion. Oxygen typically has an oxidation state of -2 in these compounds.
| Species | Oxidation State Calculation | Oxidation State of Cl |
|---|---|---|
| \(ClO^-\) | Let oxidation state of Cl be \(x\). \(x + (-2) = -1\) \(x = -1 + 2\) \(x = +1\) |
+1 |
| \(ClO_2^-\) | Let oxidation state of Cl be \(x\). \(x + 2(-2) = -1\) \(x - 4 = -1\) \(x = -1 + 4\) \(x = +3\) |
+3 |
| \(ClO_3^-\) | Let oxidation state of Cl be \(x\). \(x + 3(-2) = -1\) \(x - 6 = -1\) \(x = -1 + 6\) \(x = +5\) |
+5 |
| \(ClO_4^-\) | Let oxidation state of Cl be \(x\). \(x + 4(-2) = -1\) \(x - 8 = -1\) \(x = -1 + 8\) \(x = +7\) |
+7 |
Analyzing Chlorine Oxidation States and Disproportionation
Chlorine exhibits several common oxidation states, including:
- -1 (e.g., in chlorides like NaCl)
- 0 (elemental Cl\(_2\))
- +1 (e.g., in \(ClO^-\))
- +3 (e.g., in \(ClO_2^-\))
- +5 (e.g., in \(ClO_3^-\))
- +7 (e.g., in \(ClO_4^-\))
For disproportionation to occur, the element must be in an intermediate oxidation state. Let's look at the oxidation state of chlorine in each given species:
- In \(ClO^-\), chlorine is in the +1 oxidation state. This is an intermediate state, as chlorine can be reduced (e.g., to 0 or -1) and oxidized (e.g., to +3, +5, or +7). Thus, \(ClO^-\) can undergo disproportionation.
- In \(ClO_2^-\), chlorine is in the +3 oxidation state. This is an intermediate state, as chlorine can be reduced (e.g., to +1, 0, or -1) and oxidized (e.g., to +5 or +7). Thus, \(ClO_2^-\) can undergo disproportionation.
- In \(ClO_3^-\), chlorine is in the +5 oxidation state. This is an intermediate state, as chlorine can be reduced (e.g., to +3, +1, 0, or -1) and oxidized (to +7). Thus, \(ClO_3^-\) can undergo disproportionation.
- In \(ClO_4^-\), chlorine is in the +7 oxidation state. This is the maximum possible oxidation state for chlorine. Since chlorine is already in its highest oxidation state, it cannot be oxidized further. It can only be reduced to a lower oxidation state. Therefore, \(ClO_4^-\) cannot undergo disproportionation because disproportionation requires both oxidation and reduction of the same element from an intermediate state.
Conclusion: Which Species Cannot Disproportionate?
The species that is NOT capable of showing a disproportionation reaction is the one where chlorine is in its highest oxidation state (+7). Based on our analysis, this is \(ClO_4^-\) (perchlorate ion).
Similar Questions
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Important Questions from Chemical Reaction
Which of the following statement is/are true?
I. In physical change new substance is formed. substance is formed.
II. In chemical change no new substance is formed.
Which of the following cells involves similar chemical reactions?
The information not obtained from balanced chemical equation is
Oxygen cannot be obtained by which one of the following methods?
Which is the most reactive metal?
