Electronic configuration of Ferrous ion is

Options

A. `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(6)4s^(0)`
B. `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(6)4s^(2)`
C. `1s^(2)2s^(2)2p^(6)3s^(2)3p^(6)3d^(5)4s^(1)`
D. `1s^(2)2s^(2)2p^(6)2p^(6)3s^(2)3p^(6)3d^(5)4s^(0)`

Answer

To find the electronic configuration of the ferrous ion (Fe²⁺), we can follow these steps:

### Step 1: Determine the Atomic Number of Iron
Iron (Fe) has an atomic number of 26. This means that a neutral iron atom has 26 electrons.

### Step 2: Write the Electronic Configuration of Neutral Iron
The electronic configuration of neutral iron can be written as follows:
- The first shell can hold a maximum of 2 electrons: 1s²
- The second shell can hold a maximum of 8 electrons: 2s² 2p⁶
- The third shell can hold a maximum of 18 electrons, but we will fill it according to the Aufbau principle: 3s² 3p⁶ 4s² 3d⁶

Thus, the electronic configuration of neutral iron (Fe) is:
\[ \text{Fe: } 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 4s^2 \, 3d^6 \]

### Step 3: Identify the Electronic Configuration of the Ferrous Ion (Fe²⁺)
The ferrous ion (Fe²⁺) means that iron has lost 2 electrons. According to the Aufbau principle, when electrons are removed, they are taken from the outermost shell first. In the case of iron, the 4s orbital is filled before the 3d orbital, so the two electrons will be removed from the 4s orbital.

Thus, the electronic configuration of Fe²⁺ will be:
- Remove 2 electrons from the 4s orbital:
\[ \text{Fe}^{2+}: 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 3d^6 \, 4s^0 \]

### Final Answer
The electronic configuration of the ferrous ion (Fe²⁺) is:
\[ \text{Fe}^{2+}: 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 3d^6 \]