The electronic configuration of an clement is `1s^(2), 2s^(2), 2p^(6), 3s^(2), 3p^(4)`. The atomic number and the group number of the element 'X' which is just below the above element in the periodic table are respectively.

Options

A. 24 & 6
B. 24 & 15
C. 34 & 16
D. 34 & 8

Answer

To solve the problem, we need to analyze the given electronic configuration and determine the atomic number and group number of the element 'X' that is directly below it in the periodic table.

### Step-by-Step Solution:

1. **Identify the Given Electronic Configuration**:
The electronic configuration provided is:
\[ 1s^2, 2s^2, 2p^6, 3s^2, 3p^4 \]

2. **Count the Total Number of Electrons**:
We need to sum up the electrons in the given configuration:
- From \(1s^2\): 2 electrons
- From \(2s^2\): 2 electrons
- From \(2p^6\): 6 electrons
- From \(3s^2\): 2 electrons
- From \(3p^4\): 4 electrons

Adding these together:
\[ 2 + 2 + 6 + 2 + 4 = 16 \text{ electrons} \]

3. **Determine the Element**:
The total number of electrons (16) corresponds to the atomic number of sulfur (S). Therefore, the element with the given electronic configuration is sulfur (S).

4. **Find the Element Below Sulfur**:
The element directly below sulfur in the periodic table is selenium (Se). To find its atomic number, we add 18 to the atomic number of sulfur:
\[ 16 + 18 = 34 \]
Thus, the atomic number of selenium is 34.

5. **Determine the Group Number**:
Selenium is located in Group 16 of the periodic table, which is the same group as sulfur.

### Final Answer:
The atomic number of element 'X' (selenium) is 34, and the group number is 16.

### Summary:
- Atomic Number: 34
- Group Number: 16