The electronic configuration of the `Mn^(4+)` ion is -

Options

A. `3d^(4)4s^(0)`
B. `3d^(2)4s^(1)`
C. `3d^(1)4s^(2)`
D. `3d^(3)4s^(0)`

Explanation

To determine the electronic configuration of the \( \text{Mn}^{4+} \) ion, we will follow these steps:

### Step 1: Identify the Atomic Number of Manganese
Manganese (Mn) has an atomic number of 25. This means that a neutral manganese atom has 25 electrons.

### Step 2: Write the Electronic Configuration of Neutral Manganese
The electronic configuration of a neutral manganese atom can be written as:
\[ \text{Mn}: [\text{Ar}] 3d^5 4s^2 \]
Here, [Ar] represents the electron configuration of argon, which accounts for the first 18 electrons. The remaining 7 electrons are distributed in the 3d and 4s orbitals.

### Step 3: Determine the Configuration After Losing Electrons
The \( \text{Mn}^{4+} \) ion indicates that manganese has lost 4 electrons. Electrons are removed first from the outermost shell (4s) before the 3d subshell.

1. Start with the outermost shell:
- Remove the 2 electrons from the 4s orbital.
2. Next, remove 2 electrons from the 3d orbital:
- From \( 3d^5 \), removing 2 electrons leaves \( 3d^3 \).

### Step 4: Write the Electronic Configuration of \( \text{Mn}^{4+} \)
After losing 4 electrons, the electronic configuration of \( \text{Mn}^{4+} \) becomes:
\[ \text{Mn}^{4+}: [\text{Ar}] 3d^3 4s^0 \]
Since the 4s orbital is now empty, we can simply write:
\[ \text{Mn}^{4+}: [\text{Ar}] 3d^3 \]

### Final Answer
The electronic configuration of the \( \text{Mn}^{4+} \) ion is:
\[ [\text{Ar}] 3d^3 \]

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