Which of the following atoms are involved in the formation of Tetrahedral voids (T-voids)?

One corner atom and three adjacent face-centered atoms of cubic unit cell

The correct answer is option 2. One corner atom and three adjacent face-centered atoms of cubic unit cell.

Tetrahedral voids (T-voids) are formed within the crystal lattice structure and are surrounded by four atoms in a tetrahedral arrangement. Let's analyze the given options to determine which atoms are involved in the formation of tetrahedral voids:

1. Four corner atoms of cubic unit cell:

This option suggests that the tetrahedral void is formed by the four corner atoms of the cubic unit cell. However, this arrangement does not result in a tetrahedral void; instead, it forms the body center of the unit cell.

2. One corner atom and three adjacent face-centered atoms of cubic unit cell:

This option describes an arrangement where one corner atom and three adjacent face-centered atoms of the cubic unit cell form a tetrahedral void. This arrangement creates a tetrahedral void, with the corner atom at the center and the three face-centered atoms surrounding it.

3. Two edge-centered atoms and two face-centered atoms:

This arrangement does not form a tetrahedral void. It describes an arrangement of atoms along the edges and faces of the unit cell but does not result in a tetrahedral void.

4. Three corner atoms and body-centered atom:

Similar to option 1, this arrangement does not result in a tetrahedral void. It forms the body center of the unit cell.

The correct option describing the atoms involved in the formation of tetrahedral voids is option 2. One corner atom and three adjacent face-centered atoms of cubic unit cell.