Which one of the following metals exhibits the highest oxidation state?

Options

A. Mn
B. Cr
C. Fe
D. V

Answer

To determine which of the metals exhibits the highest oxidation state among Magnesium, Chromium, Iron, and Vanadium, we can analyze the oxidation states of each metal based on their electron configurations.

### Step-by-Step Solution:

1. **Identify the Electron Configurations**:
- **Magnesium (Mg)**: The electron configuration is \( [Ne] 3s^2 \). The maximum oxidation state is +2 (by losing its two 3s electrons).
- **Chromium (Cr)**: The electron configuration is \( [Ar] 4s^1 3d^5 \). The maximum oxidation state is +6 (by losing one 4s electron and all five 3d electrons).
- **Iron (Fe)**: The electron configuration is \( [Ar] 4s^2 3d^6 \). The maximum oxidation state is +6 (by losing both 4s electrons and all six 3d electrons).
- **Vanadium (V)**: The electron configuration is \( [Ar] 4s^2 3d^3 \). The maximum oxidation state is +5 (by losing both 4s electrons and all three 3d electrons).

2. **Compare the Maximum Oxidation States**:
- Magnesium: +2
- Chromium: +6
- Iron: +6
- Vanadium: +5

3. **Determine the Highest Oxidation State**:
- The highest oxidation state among the metals is +6, which is exhibited by both Chromium and Iron.

4. **Conclusion**:
- Therefore, the metals that exhibit the highest oxidation state are Chromium and Iron, both having an oxidation state of +6.

### Final Answer:
**Chromium and Iron exhibit the highest oxidation state of +6.**