Comprehension # 1
Read the following rules and answer the questions at the end of it.
Electrons in various suborbits of an filled in increasing order to their energies.
Pairing of electrons in various orbitals of a suborbit takes places only after each orbital is half-filled.
No two electrons in an atom can have the same set of quantum number.
Which of these ions are expected to be paramagnetic and coloured in aqueous solution ?

Options

A. `Fe^(3+),Ti^(3+),Co^(3+)`
B. `Cu^(+),Ti^(4+),Sc^(3+)`
C. `Fe^(3+),Ni^(2+),V^(5+)`
D. `Cu^(+),Cu^(2+),Fe^(2+)`

Explanation

To determine which ions are expected to be paramagnetic and colored in aqueous solution, we need to analyze the electronic configurations of the ions provided. The key points to remember are:

1. Paramagnetism is exhibited by species with unpaired electrons.
2. Colored solutions are typically associated with transition metal ions that have unpaired electrons.

### Step-by-Step Solution:

1. **Identify the Ions**: Let's consider the ions mentioned in the video transcript:
- Fe³⁺ (Iron)
- Ti³⁺ (Titanium)
- Co³⁺ (Cobalt)
- Cu⁺ (Copper)
- V⁵⁺ (Vanadium)

2. **Determine the Electronic Configuration**:
- **Fe³⁺**: Atomic number = 26. After losing 3 electrons, the configuration is:
- 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s⁰
- Thus, Fe³⁺ = 3d⁵ (5 unpaired electrons)
- **Ti³⁺**: Atomic number = 22. After losing 3 electrons, the configuration is:
- 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹ 4s⁰
- Thus, Ti³⁺ = 3d¹ (1 unpaired electron)
- **Co³⁺**: Atomic number = 27. After losing 3 electrons, the configuration is:
- 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ 4s⁰
- Thus, Co³⁺ = 3d⁶ (4 unpaired electrons)
- **Cu⁺**: Atomic number = 29. After losing 1 electron, the configuration is:
- 1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s⁰
- Thus, Cu⁺ = 3d¹⁰ (0 unpaired electrons)
- **V⁵⁺**: Atomic number = 23. After losing 5 electrons, the configuration is:
- 1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁰ 4s⁰
- Thus, V⁵⁺ = 3d⁰ (0 unpaired electrons)

3. **Count Unpaired Electrons**:
- **Fe³⁺**: 5 unpaired electrons (paramagnetic)
- **Ti³⁺**: 1 unpaired electron (paramagnetic)
- **Co³⁺**: 4 unpaired electrons (paramagnetic)
- **Cu⁺**: 0 unpaired electrons (not paramagnetic)
- **V⁵⁺**: 0 unpaired electrons (not paramagnetic)

4. **Conclusion**: The ions that are expected to be paramagnetic and colored in aqueous solution are:
- Fe³⁺
- Ti³⁺
- Co³⁺

### Final Answer:
The ions expected to be paramagnetic and colored in aqueous solution are **Fe³⁺, Ti³⁺, and Co³⁺**.