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Assertion (A): I(2) can displace Cl(2) ...

Assertion (A): `I_(2)` can displace `Cl_(2)` form `NaClO_(3)`.
Reason (R ): I is more electronegative than CI.

If both (A) and (R) are correct, and (R) is the correct explanation of (A)
If both (A) and (R) are correct, but (R) is not the correct explanation of (A).
If (A) is correct, but (R) is incorrect.
If (A) is incorrect, but (R) is correct.

Text Solution

AI Generated Solution

The correct Answer is:
To solve the given question, we need to analyze both the assertion and the reason provided and determine their correctness. ### Step 1: Analyze the Assertion (A) The assertion states that \( I_2 \) can displace \( Cl_2 \) from \( NaClO_3 \). - **Understanding the Reaction**: In \( NaClO_3 \), chlorine is in the +5 oxidation state. When \( I_2 \) (iodine in the 0 oxidation state) reacts with \( NaClO_3 \), it can potentially reduce chlorine. - **Displacement Reaction**: For \( I_2 \) to displace \( Cl_2 \), it must act as a reducing agent. In this case, \( I_2 \) can reduce \( Cl \) from +5 to 0, while itself being oxidized to +5. - **Conclusion**: Therefore, the assertion is **true**. ### Step 2: Analyze the Reason (R) The reason states that iodine (I) is more electronegative than chlorine (Cl). - **Electronegativity Values**: The electronegativity of chlorine is higher than that of iodine. Chlorine is more electronegative because it is higher up in the periodic table. - **Periodic Trend**: As we move down the group in the periodic table, electronegativity decreases. Hence, iodine, being below chlorine, is less electronegative. - **Conclusion**: Therefore, the reason is **false**. ### Final Conclusion - Since the assertion (A) is true and the reason (R) is false, the correct option is: - **If (A) is correct, but (R) is incorrect.** ### Answer: **Option 3: If (A) is correct, but (R) is incorrect.** ---
To solve the given question, we need to analyze both the assertion and the reason provided and determine their correctness. ### Step 1: Analyze the Assertion (A) The assertion states that \( I_2 \) can displace \( Cl_2 \) from \( NaClO_3 \). - **Understanding the Reaction**: In \( NaClO_3 \), chlorine is in the +5 oxidation state. When \( I_2 \) (iodine in the 0 oxidation state) reacts with \( NaClO_3 \), it can potentially reduce chlorine. - **Displacement Reaction**: For \( I_2 \) to displace \( Cl_2 \), it must act as a reducing agent. In this case, \( I_2 \) can reduce \( Cl \) from +5 to 0, while itself being oxidized to +5. - **Conclusion**: Therefore, the assertion is **true**. ...
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