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 find the electronic configuration of the `Mn^(4+)` ion, we will follow these steps:

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

### Step 2: Write the Electron Configuration of Neutral Manganese
The electron configuration of a neutral manganese atom can be written as follows:
- Fill the 1s orbital: 1s²
- Fill the 2s orbital: 2s²
- Fill the 2p orbital: 2p⁶
- Fill the 3s orbital: 3s²
- Fill the 3p orbital: 3p⁶
- Fill the 4s orbital: 4s²
- Fill the 3d orbital: 3d⁵

Putting it all together, the electron configuration for neutral manganese is:
\[ \text{Mn: } 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^5 \]

### Step 3: Determine the Electron Configuration of Mn^(4+)
The `Mn^(4+)` ion means that manganese has lost 4 electrons. When forming cations, electrons are removed first from the outermost shell. In this case, the electrons will be removed from the 4s and then from the 3d orbitals.

1. Remove 2 electrons from the 4s orbital:
- From 4s², we remove 2 electrons: 4s² → 4s⁰
2. Remove 2 electrons from the 3d orbital:
- From 3d⁵, we remove 2 electrons: 3d⁵ → 3d³

So, after removing 4 electrons, the electron configuration for `Mn^(4+)` becomes:
\[ \text{Mn}^{4+}: 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 3d^3 \]

### Final Answer
The electronic configuration of the `Mn^(4+)` ion is:
\[ \text{Mn}^{4+}: 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 3d^3 \]

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