Question

Match List I with List II

Choose the correct answer from the options given below :

• A. A-III, B-II, C-IV, D-I
• B. A-IV, B-I, C-II, D-III
• C. A-IV, B-III, C-I, D-II
• D. A-II, B-III, C-IV, D-I

Answer 1

The Correct Option is D

To resolve this, we must correlate the complex ions in List I with their corresponding electronic configurations from List II.

Each complex ion's electronic configuration will be determined by its central metal's oxidation state and coordination chemistry principles.

1. A. \([\text{Cr}(\text{H}_2\text{O})_6]^{3+}\)
   • Cr exhibits a +3 oxidation state.
   • Cr's electronic configuration is \([\text{Ar}] 3d^5 4s^1\).
   • Cr³⁺ achieves a \(3d^3\) configuration by losing 3 electrons.
   • For octahedral complexes, the electron configuration is \(t_{2g}^3 e_g^0\).
   • This corresponds to II.
2. B. \([\text{Fe}(\text{H}_2\text{O})_6]^{3+}\)
   • Fe is in the +3 oxidation state.
   • Fe's electronic configuration is \([\text{Ar}] 3d^6 4s^2\).
   • Fe³⁺ has a \(3d^5\) configuration after losing 3 electrons.
   • In octahedral complexes, the electron configuration is \(t_{2g}^3 e_g^2\).
   • This corresponds to III.
3. C. \([\text{Ni}(\text{H}_2\text{O})_6]^{2+}\)
   • Ni has a +2 oxidation state.
   • Ni's electronic configuration is \([\text{Ar}] 3d^8 4s^2\).
   • Ni²⁺, after losing 2 electrons, has a \(3d^8\) configuration.
   • For octahedral complexes, the electron configuration is \(t_{2g}^6 e_g^2\).
   • This corresponds to IV.
4. D. \([\text{V}(\text{H}_2\text{O})_6]^{3+}\)
   • V is in the +3 oxidation state.
   • V's electronic configuration is \([\text{Ar}] 3d^3 4s^2\).
   • V³⁺ loses 3 electrons, resulting in a \(3d^2\) configuration.
   • In octahedral complexes, the electron configuration is \(t_{2g}^2 e_g^0\).
   • This corresponds to I.

The derived matching is:

A-II, B-III, C-IV, D-I

Therefore, the correct answer is:

A-II, B-III, C-IV, D-I