What is the electronic configuration of `Mn^(2+)`

Options

A. `[Ne]3d^(5)4s^(0)`
B. `[Ar]3d^(5)4s^(2)`
C. `[Ar]3d^(5)4s^(0)`
D. `[Ne]3d^(5)4s^(2)`

Explanation

To find the electronic configuration of \( \text{Mn}^{2+} \), we can follow these steps:

### Step 1: Determine the atomic number of manganese (Mn).
- Manganese has an atomic number of 25.

### Step 2: Write the electronic configuration of neutral manganese (Mn).
- The electronic configuration of manganese (Mn) is:
\[ \text{Mn}: 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^5 \]
- This can also be expressed using the noble gas shorthand notation:
\[ \text{Mn}: [\text{Ar}] \, 4s^2 \, 3d^5 \]

### Step 3: Account for the \(2+\) oxidation state.
- When manganese is in the \(2+\) oxidation state (\( \text{Mn}^{2+} \)), it loses two electrons.
- The electrons are removed first from the \(4s\) orbital before the \(3d\) orbital.

### Step 4: Write the electronic configuration for \( \text{Mn}^{2+} \).
- After removing two electrons from the \(4s\) orbital, the electronic configuration becomes:
\[ \text{Mn}^{2+}: [\text{Ar}] \, 3d^5 \, 4s^0 \]

### Final Answer:
- The electronic configuration of \( \text{Mn}^{2+} \) is:
\[ [\text{Ar}] \, 3d^5 \, 4s^0 \]