(A): `Sc^(+3)` ion in aqueous solutions is colorless
(R) : Ions with `d^o` configuration are colorless 

Options

A. Both A & R are true, R is the correct explanation of A
B. Both A & R are true, R is not correct explanation of A
C. A is true, R is false
D. A is false, R is true

Answer

To solve the question step by step, we will analyze both statements A and R regarding the Scandium ion and its electronic configuration.

### Step 1: Analyze Statement A
**Statement A**: Sc^(+3) ion in aqueous solutions is colorless.

- The Scandium ion (Sc^(+3)) has lost three electrons from its neutral atom.
- The electronic configuration of neutral Scandium (Sc) is:
- 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹ 4s²
- When Sc loses three electrons to form Sc^(+3), the electrons are removed from the outermost shell first:
- The configuration becomes: 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁰ (removing 2 electrons from 4s and 1 from 3d).
- Therefore, the electronic configuration of Sc^(+3) is 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁰.

### Step 2: Analyze Statement R
**Statement R**: Ions with d⁰ configuration are colorless.

- Ions with a d⁰ configuration have no unpaired electrons in their d orbitals.
- Since Sc^(+3) has a d⁰ configuration (3d⁰), it means there are no unpaired electrons.
- Color in transition metal ions is typically due to the presence of unpaired electrons that can absorb visible light.
- Since Sc^(+3) has no unpaired electrons, it does not absorb visible light, making it colorless.

### Step 3: Conclusion
- Both statements A and R are true.
- Statement R correctly explains why statement A is true, as the absence of unpaired electrons in Sc^(+3) (d⁰ configuration) leads to it being colorless.

### Final Answer
Both A and R are correct, and R is the correct explanation of A.

### Answer Option
The correct option is: **Option 1** - Both A and R are true, and R is the correct explanation of A.

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