Octahedral Voids in CCP Unit Cell

A cubic close-packed (ccp) unit cell is a three-dimensional arrangement of atoms such that the atoms are touching along the face diagonal of the cube. In this structure, there are octahedral voids present that are formed by the overlapping of six atoms.

Body Diagonal in CCP Unit Cell

A body diagonal is a line that passes through the center of a cube and connects opposite corners. In a ccp unit cell, there are four body diagonals present. These diagonals pass through the center of the unit cell and connect opposite corners of the cube.

Number of Octahedral Voids in Body Diagonal

The number of octahedral voids present in a ccp unit cell along the body diagonal can be calculated using the following formula:

Number of octahedral voids = 1/4 * number of atoms

In a ccp unit cell, there are 4 atoms present per unit cell. Therefore, the number of octahedral voids present in the body diagonal can be calculated as follows:

Number of octahedral voids = 1/4 * 4

Number of octahedral voids = 1

Therefore, there is only one octahedral void present along the body diagonal of a ccp unit cell. This void is formed by the overlapping of six atoms along the body diagonal.

Conclusion

In conclusion, a ccp unit cell has octahedral voids present that are formed by the overlapping of six atoms. Along the body diagonal of the cube, there is only one octahedral void present. This void is formed by the overlapping of six atoms along the body diagonal.

At one body diagonal, one octahedral void is present which is at its centerthere are 4 octahedral voids in 1 unit cell of ccp, out of which 1 is at centre of cell and others are at all edge centers [ 12(1/4)]=3Thus, total 1+3=4 octahedral void