In a compound, atoms A occupy `3//4` of the tetrahedral voids and atoms B from ccp lattice. The empirical formula of the compound is

Options

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

Explanation

To solve the problem, we need to determine the empirical formula of a compound where atoms A occupy \( \frac{3}{4} \) of the tetrahedral voids and atoms B form a close-packed (CCP) lattice.

### Step-by-Step Solution:

1. **Understanding the CCP Lattice:**
- In a CCP (Cubic Close Packing) structure, the number of atoms (let's denote it as \( N \)) is equal to the number of octahedral voids.
- The number of tetrahedral voids is twice the number of octahedral voids, which means there are \( 2N \) tetrahedral voids.

2. **Calculating the Number of Tetrahedral Voids Occupied by A:**
- Given that atoms A occupy \( \frac{3}{4} \) of the tetrahedral voids, we can calculate the number of tetrahedral voids occupied by A:
\[ \text{Number of A atoms} = \frac{3}{4} \times \text{Total Tetrahedral Voids} = \frac{3}{4} \times 2N = \frac{3N}{2} \]

3. **Calculating the Number of B Atoms:**
- Since atoms B form the CCP lattice, the number of B atoms is simply \( N \).

4. **Finding the Ratio of A to B:**
- Now, we need to find the ratio of the number of A atoms to the number of B atoms:
\[ \text{Ratio of A to B} = \frac{\text{Number of A atoms}}{\text{Number of B atoms}} = \frac{\frac{3N}{2}}{N} = \frac{3}{2} \]

5. **Simplifying the Ratio:**
- The ratio \( \frac{3}{2} \) can be expressed as:
\[ 3 : 2 \]

6. **Writing the Empirical Formula:**
- Based on the ratio of A to B, we can write the empirical formula as:
\[ \text{Empirical Formula} = A_3B_2 \]

### Final Answer:
The empirical formula of the compound is \( A_3B_2 \).