Question

Given below are two statements :
Statement I : The higher oxidation states are more stable down the group among transition elements unlike p-block elements.
Statement II : Copper can not liberate hydrogen from weak acids.
In the light of the above statements, choose the correct answer from the options given below

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

Answer 1

The Correct Option is C

Analysis of each statement for correctness:

1. Statement I: Higher oxidation states are more stable down the group for transition elements, unlike p-block elements.
   • In d-block elements, higher oxidation states generally stabilize moving down a group due to the increasing involvement of d orbitals in bonding.
   • For instance, Group 6 elements like Cr, Mo, and W all show stable +6 oxidation states (e.g., CrO₃, MoO₃, WO₃).
   • Conversely, in p-block elements (e.g., the nitrogen group), higher oxidation states become less stable down the group. Nitrogen's +5 state in N₂O₅ is stable, while Bismuth predominantly exhibits a +3 state, with +5 being less stable.
   • Conclusion: Statement I is true.
2. Statement II: Copper does not liberate hydrogen from weak acids.
   • Copper is less reactive than hydrogen in the electrochemical series, preventing it from displacing hydrogen ions from weak acids.
   • Copper requires a stronger impetus than weak acids provide to react with hydrogen ions. Reaction with stronger acids typically involves oxidation in the presence of an oxidizing agent, not simple hydrogen displacement.
   • Conclusion: Statement II is true.

Both Statement I and Statement II have been confirmed as true. Therefore, the correct conclusion is: Both Statement I and Statement II are true.