Valence electron in the element A are 3 and that in element B are 6. Most probable compound formed from A and B is

Options

A. `A_(2) B`
B. `AB_(2)`
C. `A_(6)B_(3)`
D. `A_(2)B_(3)`

Explanation

To determine the most probable compound formed from elements A and B, we need to analyze the valence electrons of each element and how they can combine to form a stable compound.

### Step-by-Step Solution:

1. **Identify the Valence Electrons**:
- Element A has 3 valence electrons.
- Element B has 6 valence electrons.

2. **Determine the Valence**:
- For element A (with 3 valence electrons), the valence is equal to the number of valence electrons. Therefore, the valence of A is 3.
- For element B (with 6 valence electrons), since the number of valence electrons is greater than 4, we use the formula:
\[ \text{Valence} = 8 - \text{Valence Electrons} \]
Thus, the valence of B is:
\[ 8 - 6 = 2 \]

3. **Combine the Valences**:
- To form a compound, we need to balance the total positive and negative charges from the valences of A and B.
- Element A has a valence of 3, and element B has a valence of 2.

4. **Use the Crisscross Method**:
- The crisscross method involves taking the valence of one element and using it as the subscript for the other element.
- From A (valence 3) and B (valence 2), we can write the formula:
- A will have a subscript of 2 (from B's valence).
- B will have a subscript of 3 (from A's valence).
- Therefore, the compound formed will be:
\[ \text{A}_2\text{B}_3 \]

5. **Conclusion**:
- The most probable compound formed from elements A and B is \( \text{A}_2\text{B}_3 \).

### Final Answer:
The most probable compound formed from elements A and B is \( \text{A}_2\text{B}_3 \).

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