Which of the following is coloured

Options

A. `ScCl_(3)`
B. `TiO_(2)`
C. `MnSO_(4)`
D. `ZnSO_(4)`

Explanation

To determine which of the given compounds is colored, we need to analyze the oxidation states and electronic configurations of the elements involved, particularly focusing on the presence of unpaired electrons in their d-orbitals. Compounds with unpaired electrons typically exhibit color due to d-d transitions.

### Step-by-Step Solution:

1. **Identify the Compounds**: The compounds given are SCCl3, TiO2, MnSO4, and ZnSO4.

2. **Analyze SCCl3**:
- **Element**: Scandium (Sc)
- **Oxidation State**: +3
- **Electronic Configuration**: Sc (atomic number 21) has the configuration 4s² 3d¹.
- **For Sc +3**: The configuration becomes 4s⁰ 3d⁰.
- **Unpaired Electrons**: There are no unpaired electrons (0 unpaired).
- **Color**: Colorless.

3. **Analyze TiO2**:
- **Element**: Titanium (Ti)
- **Oxidation State**: +4
- **Electronic Configuration**: Ti (atomic number 22) has the configuration 4s² 3d².
- **For Ti +4**: The configuration becomes 4s⁰ 3d⁰.
- **Unpaired Electrons**: There are no unpaired electrons (0 unpaired).
- **Color**: Colorless.

4. **Analyze MnSO4**:
- **Element**: Manganese (Mn)
- **Oxidation State**: +2
- **Electronic Configuration**: Mn (atomic number 25) has the configuration 4s² 3d⁵.
- **For Mn +2**: The configuration becomes 4s⁰ 3d⁵.
- **Unpaired Electrons**: There are 5 unpaired electrons (5 unpaired).
- **Color**: Colored (due to unpaired electrons).

5. **Analyze ZnSO4**:
- **Element**: Zinc (Zn)
- **Oxidation State**: +2
- **Electronic Configuration**: Zn (atomic number 30) has the configuration 4s² 3d¹⁰.
- **For Zn +2**: The configuration becomes 4s⁰ 3d¹⁰.
- **Unpaired Electrons**: There are no unpaired electrons (0 unpaired).
- **Color**: Colorless.

6. **Conclusion**: Among the compounds analyzed, only MnSO4 has unpaired electrons and is therefore colored.

### Final Answer:
The colored compound is **MnSO4**.