Which one of the following shows the correct electronic configuration of the outermost shell in inert gases ?

Options

A. `ns^(2), np^(6)`
B. `ns^(2), np^(3)`
C. `ns^(2), np^(5)`
D. `ns^(2), np^(4)`

Answer

To determine the correct electronic configuration of the outermost shell in inert gases, follow these steps:

### Step 1: Understand the Characteristics of Inert Gases
Inert gases, also known as noble gases, are elements in Group 18 of the periodic table. They are characterized by their non-reactivity due to having a complete outermost shell of electrons.

### Step 2: Identify the Electron Configuration of Inert Gases
The outermost shell of inert gases contains a total of 8 electrons, which is known as the octet rule. The electronic configurations for the first few inert gases are:
- Helium (He): 1s² (2 electrons)
- Neon (Ne): 1s² 2s² 2p⁶ (8 electrons)
- Argon (Ar): 1s² 2s² 2p⁶ 3s² 3p⁶ (8 electrons)
- Krypton (Kr): 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4p⁶ (8 electrons)

### Step 3: Analyze the Given Options
Now, look at the options provided in the question. We need to find the one that shows a total of 8 electrons in the outermost shell.

1. **Option A**: 2 + 6 = 8 electrons (Correct)
2. **Option B**: 5 electrons (Incorrect)
3. **Option C**: 7 electrons (Incorrect)
4. **Option D**: 6 electrons (Incorrect)

### Step 4: Conclusion
The only option that shows the correct electronic configuration of the outermost shell in inert gases is Option A, which has a total of 8 electrons.

### Final Answer:
**Option A: 2 + 6 (Total 8 electrons)**

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