Question:
Given below are two statements:
Statement (I): Oxidising power of halogens decreases in the order
\[
F_2>Cl_2>Br_2>I_2
\]
which is the basis of the “Layer test”.
Statement (II): “Layer test” to identify \(Br_2\) and \(I_2\) in aqueous solution involves the oxidation of bromide or iodide into \(Br_2\) or \(I_2\) respectively with \(Cl_2\), which is a type of displacement redox reaction.
In the light of the above statements, choose the correct answer:
Given below are two statements:
Statement (I): Oxidising power of halogens decreases in the order
\[
F_2>Cl_2>Br_2>I_2
\]
which is the basis of the “Layer test”.
Statement (II): “Layer test” to identify \(Br_2\) and \(I_2\) in aqueous solution involves the oxidation of bromide or iodide into \(Br_2\) or \(I_2\) respectively with \(Cl_2\), which is a type of displacement redox reaction.
In the light of the above statements, choose the correct answer:
Updated On: Apr 10, 2026
- Both Statement I and Statement II are true
- Both Statement I and Statement II are false
- Statement I is true but Statement II is false
- Statement I is false but Statement II is true
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The Correct Option is A
Solution and Explanation
Concept:
Oxidising power of halogens decreases down the group.
\[
F_2>Cl_2>Br_2>I_2
\]
Step 1:Check Statement I} This trend arises because electron gain enthalpy becomes less negative down the group. Thus fluorine is the strongest oxidising agent. Hence Statement I is correct.
Step 2:Check Statement II} Chlorine can oxidise bromide and iodide ions: \[ Cl_2 + 2Br^- \rightarrow 2Cl^- + Br_2 \] \[ Cl_2 + 2I^- \rightarrow 2Cl^- + I_2 \] The liberated \(Br_2\) or \(I_2\) dissolves in an organic layer giving characteristic colours. Thus it is a displacement redox reaction. Hence Statement II is also correct. \[ \boxed{\text{Both statements are true}} \]
Step 1:Check Statement I} This trend arises because electron gain enthalpy becomes less negative down the group. Thus fluorine is the strongest oxidising agent. Hence Statement I is correct.
Step 2:Check Statement II} Chlorine can oxidise bromide and iodide ions: \[ Cl_2 + 2Br^- \rightarrow 2Cl^- + Br_2 \] \[ Cl_2 + 2I^- \rightarrow 2Cl^- + I_2 \] The liberated \(Br_2\) or \(I_2\) dissolves in an organic layer giving characteristic colours. Thus it is a displacement redox reaction. Hence Statement II is also correct. \[ \boxed{\text{Both statements are true}} \]
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