Question

Given below are two statements.
Statement I: Iron (III) catalyst, acidified \(K_2Cr_2O_7\) and neutral \(KMnO_4\) have the ability to oxidise \(I^–\) to \(I_2\) independently.
Statement II: Manganate ion is paramagnetic in nature and involves \(pπ – pπ\) bonding.
In the light of the above statements, choose the correct answer from the options given below.

• A. Both Statement I and Statement II are true
• B. Both Statement I and Statement II are false
• C. Statement I is true but Statement II is false
• D. Statement I is false but Statement II is true

Answer 1

The Correct Option is B

To address the question, let's analyze both statements separately:

Statement I: Iron (III) catalyst, acidified \(K_2Cr_2O_7\) and neutral \(KMnO_4\) have the ability to oxidise \(I^–\) to \(I_2\) independently.

Oxidation of iodide ions \((I^-)\) to iodine \((I_2)\) is a redox reaction. Acidified potassium dichromate \((K_2Cr_2O_7)\) is a well-known oxidizing agent, which indeed can oxidize \(I^–\) to \(I_2\). However, neutral potassium permanganate \((KMnO_4)\) is not effective without acidic conditions to oxidize \(I^–\). Thus, the statement that neutral KMnO_4 can independently oxidize \(I^–\) is incorrect.

Statement II: Manganate ion is paramagnetic in nature and involves \(pπ – pπ\) bonding.

Manganate ion \((MnO_4^{2-})\) has a \(d^0\) configuration because Mn is in the +6 oxidation state. A \(d^0\) electronic configuration implies that there are no unpaired electrons, hence it is diamagnetic, not paramagnetic. The term "\(pπ – pπ\) bonding" is generally used for overlapping of p orbitals in conjugated systems, which is not applicable to manganate ions. Therefore, this statement is also false.

Conclusion: Based on the analysis, both statements are false. Therefore, the correct answer is:

Both Statement I and Statement II are false