The electronic configuration of an element is written as follows: `1s^2 2s^2 2p^6 3s^2 3p^6 3d^8 4s^2`
On removal of two electrons, the electronic configuration will become 

Options

A. `1s^2 2s^2 2p^6 3s^2 3p^6 3d^7 4s^2`
B. `1s^2 2s^2 2p^6 3s^2 3p^6 3d^8 4s^0`
C. `1s^2 2s^2 2p^6 3s^2 3p^6 3d^9 4s^0`
D. None of these.

Answer

To determine the electronic configuration of the element after the removal of two electrons, we will follow these steps:

### Step-by-Step Solution:

1. **Identify the Initial Electronic Configuration**:
The given electronic configuration is:
\[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 3d^8 \, 4s^2 \]

2. **Determine Which Electrons to Remove**:
When removing electrons, we typically remove them from the highest energy level first. In this case, the highest energy level is 4s, followed by 3d. Therefore, we will remove the two electrons from the 4s subshell.

3. **Remove the Electrons**:
By removing two electrons from the 4s subshell, we get:
\[ 4s^0 \, (or \, no \, 4s \, electrons) \]
The remaining configuration will now be:
\[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 3d^8 \]

4. **Write the Final Electronic Configuration**:
After removing the two electrons, the final electronic configuration becomes:
\[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 3d^8 \, 4s^0 \]
However, it is conventional to omit the \(4s^0\) when writing electronic configurations, so we can simply write:
\[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 3d^8 \]

### Final Answer:
The electronic configuration after the removal of two electrons is:
\[ 1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^6 \, 3d^8 \]