The electronic configuration ofhte elements. A, B and C are given below. Answer the question from 14 to 17 on the basis of these configuration.
`{:(A,1s^(2),2s^(2),2p^(6),,),(B,1s^(2),2s^(2),2p^(6),3s^(2),3p^(3)),(C,1s^(2),2s^(2),2p^(6),3s^(2),3p^(5)):}`
Stable form of A may be represented by the formula.

Options

A. A
B. `A_(2)`
C. `A_(3)`
D. `A_(4)`

Explanation

To determine the stable form of element A based on its electronic configuration, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Electronic Configuration of A**:
The electronic configuration of element A is given as \(1s^2, 2s^2, 2p^6\).

2. **Determine the Atomic Number**:
To find the atomic number, we add the total number of electrons in the configuration.
- \(1s^2\) contributes 2 electrons,
- \(2s^2\) contributes 2 electrons,
- \(2p^6\) contributes 6 electrons.
- Total = \(2 + 2 + 6 = 10\).
Therefore, the atomic number of A is 10.

3. **Identify the Element**:
The element with atomic number 10 is Neon (Ne), which is a noble gas.

4. **Analyze the Stability of A**:
Noble gases have complete outer electron shells (octet), which makes them very stable and unreactive. Since A has a complete octet, it does not need to gain, lose, or share electrons.

5. **Determine the Stable Form**:
Because A has a complete octet and does not need to bond with other elements, it will exist in a monoatomic form.

6. **Conclusion**:
The stable form of A can be represented by the formula \( \text{A} \) (as a monoatomic gas).

### Final Answer:
The stable form of A may be represented by the formula \( \text{A} \) (monoatomic).

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