which of the following group of ion is paramagnetic in nature:

Options

A. `Cu^(+),Zn^(2+)Sc^(2+)`
B. `Mn^(2+),Fe^(3+),Ni^(2+)`
C. `Cr^(2+),Mn^(3+),Sc^(3+)`
D. `Cu^(2+),Ni^(2+),Ti^(4+)`

Explanation

To determine which group of ions is paramagnetic in nature, we need to analyze the electronic configurations of each ion and identify the presence of unpaired electrons. Paramagnetic ions have unpaired electrons, while diamagnetic ions do not.

### Step-by-Step Solution:

1. **Understand Paramagnetism**:
- Paramagnetic substances have one or more unpaired electrons in their electronic configuration.
- Diamagnetic substances have all electrons paired, resulting in no net magnetic moment.

2. **Analyze Each Ion Group**:
- We will examine each group of ions provided in the question.

3. **Group 1: Cu⁺, Zn²⁺, Sc²⁺**
- **Cu⁺**: Electronic configuration is [Ar] 3d¹⁰ 4s⁰. (No unpaired electrons, diamagnetic)
- **Zn²⁺**: Electronic configuration is [Ar] 3d¹⁰ 4s⁰. (No unpaired electrons, diamagnetic)
- **Sc²⁺**: Electronic configuration is [Ar] 3d¹ 4s⁰. (1 unpaired electron, paramagnetic)
- **Conclusion**: Not all are paramagnetic (2 are diamagnetic).

4. **Group 2: Mn²⁺, Fe³⁺, Ni²⁺**
- **Mn²⁺**: Electronic configuration is [Ar] 3d⁵ 4s⁰. (5 unpaired electrons, paramagnetic)
- **Fe³⁺**: Electronic configuration is [Ar] 3d⁵ 4s⁰. (5 unpaired electrons, paramagnetic)
- **Ni²⁺**: Electronic configuration is [Ar] 3d⁸ 4s⁰. (2 unpaired electrons, paramagnetic)
- **Conclusion**: All are paramagnetic.

5. **Group 3: Cr²⁺, Mn³⁺, Sc³⁺**
- **Cr²⁺**: Electronic configuration is [Ar] 3d⁴ 4s⁰. (4 unpaired electrons, paramagnetic)
- **Mn³⁺**: Electronic configuration is [Ar] 3d⁴ 4s⁰. (4 unpaired electrons, paramagnetic)
- **Sc³⁺**: Electronic configuration is [Ar] 3d⁰ 4s⁰. (No unpaired electrons, diamagnetic)
- **Conclusion**: Not all are paramagnetic (1 is diamagnetic).

6. **Group 4: Cu²⁺, Ni²⁺, Ti⁴⁺**
- **Cu²⁺**: Electronic configuration is [Ar] 3d⁹ 4s⁰. (1 unpaired electron, paramagnetic)
- **Ni²⁺**: Electronic configuration is [Ar] 3d⁸ 4s⁰. (2 unpaired electrons, paramagnetic)
- **Ti⁴⁺**: Electronic configuration is [Ar] 3d⁰ 4s⁰. (No unpaired electrons, diamagnetic)
- **Conclusion**: Not all are paramagnetic (1 is diamagnetic).

### Final Conclusion:
The only group of ions that is entirely paramagnetic is **Group 2: Mn²⁺, Fe³⁺, Ni²⁺**.