The more paramagnetic in the following is

Options

A. Mn
B. Cr
C. `Fe^(2+)`
D. `Fe^(3+)`

Explanation

To determine which of the given elements or ions is the most paramagnetic, we need to analyze their electronic configurations and count the number of unpaired electrons. Paramagnetism arises from the presence of unpaired electrons in an atom or ion.

### Step-by-Step Solution:

1. **Identify the Elements and Their Electronic Configurations**:
- Manganese (Mn): Atomic number = 25
- Electronic configuration: \( [Ar] 3d^5 4s^2 \)
- Chromium (Cr): Atomic number = 24
- Electronic configuration: \( [Ar] 3d^5 4s^1 \)
- Iron (Fe): Atomic number = 26
- Electronic configuration: \( [Ar] 3d^6 4s^2 \)
- Iron (Fe²⁺): When iron loses 2 electrons, it loses the 4s electrons first.
- Electronic configuration: \( [Ar] 3d^6 \)
- Iron (Fe³⁺): When iron loses 3 electrons, it loses both 4s and one 3d electron.
- Electronic configuration: \( [Ar] 3d^5 \)

2. **Count the Unpaired Electrons**:
- **Manganese (Mn)**:
- Configuration: \( 3d^5 4s^2 \)
- Unpaired electrons: 5 (all 5 d electrons are unpaired)
- **Chromium (Cr)**:
- Configuration: \( 3d^5 4s^1 \)
- Unpaired electrons: 6 (5 unpaired d electrons + 1 unpaired s electron)
- **Iron (Fe²⁺)**:
- Configuration: \( 3d^6 \)
- Unpaired electrons: 4 (the 6 electrons fill the d orbitals, resulting in 4 unpaired electrons)
- **Iron (Fe³⁺)**:
- Configuration: \( 3d^5 \)
- Unpaired electrons: 5 (all 5 d electrons are unpaired)

3. **Compare the Number of Unpaired Electrons**:
- Manganese: 5 unpaired electrons
- Chromium: 6 unpaired electrons
- Iron (Fe²⁺): 4 unpaired electrons
- Iron (Fe³⁺): 5 unpaired electrons

4. **Conclusion**:
- The element with the highest number of unpaired electrons is Chromium (Cr) with 6 unpaired electrons. Therefore, Chromium is the most paramagnetic among the given options.

### Final Answer:
**Chromium (Cr) is the more paramagnetic of the following.**