Predict which of the following will be coloured in aqueous solution ?
`Ti^(3+) , V^(3+) , Sc^(3+) , Mn^(2+) , Fe^(3+) , Co^(2+) ` and `MnO_(4)^(-)`

Explanation

To determine which of the given ions will be colored in aqueous solution, we need to analyze the electronic configurations of each ion and check for the presence of unpaired electrons. The presence of unpaired electrons in the d-orbitals is what typically gives rise to color in transition metal ions.

### Step-by-Step Solution:

1. **Identify the Electronic Configurations:**
- **Ti^(3+):** Titanium (Ti) has an atomic number of 22. The electronic configuration of Ti is [Ar] 3d² 4s². For Ti^(3+), we remove three electrons, resulting in [Ar] 3d¹.
- **V^(3+):** Vanadium (V) has an atomic number of 23. The electronic configuration of V is [Ar] 3d³ 4s². For V^(3+), we remove three electrons, resulting in [Ar] 3d².
- **Sc^(3+):** Scandium (Sc) has an atomic number of 21. The electronic configuration of Sc is [Ar] 3d¹ 4s². For Sc^(3+), we remove three electrons, resulting in [Ar] 3d⁰ (no unpaired electrons).
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