Copper crystallizes in a face-centered cubic cell. Copper's density is 8.92 g?cm3, and its molar mass is 63.55 g/mol. Determine the radius (in pm) of a copper atom.
since the cubic cell is Face Centred Cubic, the value of Z=4
Molar mass = 63.55 g/mol
d = (Z*M)/(a^3*NA)
8.92 = (4*63.55)/(a^3*(6.022*10^23))
a^3 = 4.732*10^-23 cm^3
a = 3.617*10^-8 cm
a = 361.7 pm
for FCC:
length of face diagonal = sqrt(a^2+a^2)
length of face diagonal = a*sqrt(2)
use:
For FCC Lattice
length of face diagonal = 4*r
a*sqrt(2) = 4*r
361.7*sqrt(2) = 4*r
r = 128 pm
Answer: 128 pm
Copper crystallizes in a face-centered cubic cell. Copper's density is 8.92 g?cm3, and its molar mass...
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