The atom having the valence shell electronic configuration` 4s^(2) 4p^2` would be in

Options

A. group-II A and period 3
B. group-II B and period 4
C. group-IV A and period 4
D. group-IV A and period 3

Explanation

To determine the group and period of the atom with the valence shell electronic configuration of \(4s^2 4p^2\), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Electronic Configuration**: The given electronic configuration is \(4s^2 4p^2\). This indicates that the atom has two electrons in the \(4s\) subshell and two electrons in the \(4p\) subshell.

2. **Determine the Family**: The general electronic configuration for the carbon family (Group 14) is \(ns^2 np^2\). Here, \(n\) is 4 (since we have \(4s\) and \(4p\)), which means this atom belongs to the carbon family.

3. **Identify the Element**: The specific element with the configuration \(4s^2 4p^2\) is Germanium (Ge). This can be confirmed by looking at the complete electronic configuration of Germanium, which is \( [Ar] 3d^{10} 4s^2 4p^2 \).

4. **Determine the Period**: The period of an element is determined by the highest principal quantum number \(n\) in its electron configuration. In this case, the maximum value of \(n\) is 4 (from \(4s\) and \(4p\)), indicating that the element is in the 4th period.

5. **Determine the Group**: The group can be determined from the valence shell configuration. Since the configuration is \(4s^2 4p^2\), it falls under Group 14 (or 4A in older notation) of the periodic table.

6. **Conclusion**: Therefore, the atom with the valence shell electronic configuration \(4s^2 4p^2\) is in Group 14 (4A) and Period 4.

### Final Answer:
The atom having the valence shell electronic configuration \(4s^2 4p^2\) would be in Group 14 (4A) and Period 4.

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