The cubic closest packet structure is a face-centered cubic cell in which atoms are on corners and faces.
Each atom on the corner is shared between 8 cells and each atom at the face is shared between 2 cells so the number of atoms per unit cell
8x1/8+6x1/2=1+3=4
The volume of the unit cell can be calculated from density.
d=m/V
m is mass of unit cell
m=4 xm(Cu)
m(Cu)=mass of one Cu atom=M(Cu)/NA=63.55 (g/mol) / ( 6.10 ^23 x1/ mol)
=10.59x 10^−23 g
V=m/d=42.37x10−23 g / 8.95( g/cm3) =4.733⋅10−23 cm3
The edge of the unit cell is equal to:
a= 3√V
=√47.33x10−24cm3
=3.62x 10−8 cm
=3.62x10−8 cm x 1 m /100 cmx 10^12 pm /1 m
=362 pm
radius of the copper : 4r^2 =a^2+a^2
16r^2=2a^2
8r^2=a^2
r=√a^2/8 =√(362)^2/8
where a =362 =127.9pm
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