Octahedral Void in Cubic Close-Packed (CCP) Structure

Cubic close-packed (CCP) structure is one of the three common crystal lattice structures. In a CCP structure, the atoms are arranged in a face-centered cubic (FCC) pattern. The FCC unit cell contains 4 atoms, which are located at the corners and the center of each face of the cube.

An octahedral void is a space between the atoms in a crystal lattice, which is shaped like an octahedron. It is formed by the closest-packed spheres in the lattice, and it is located at the center of six adjacent atoms.

In a CCP structure, the octahedral void is located at the center of the unit cell. It is surrounded by 6 atoms, which are located at the vertices of an octahedron. Therefore, each octahedral void is shared by 6 adjacent unit cells.

Number of Octahedral Voids per Atom in CCP Structure

To determine the number of octahedral voids per atom in a CCP structure, we can consider the following:

- Each atom in a CCP structure is in contact with 12 adjacent atoms.
- Each atom is located at the center of a tetrahedron formed by 4 adjacent atoms.
- Each tetrahedron shares its vertices with 4 adjacent tetrahedra.

Therefore, each atom in a CCP structure contributes to the formation of 8 tetrahedral voids, which are shared by 8 adjacent atoms. However, each atom is not located at the center of an octahedron, and therefore it does not contribute to the formation of octahedral voids.

Since there are no octahedral voids formed by the atoms in a CCP structure, the correct answer is option 'C': 1.