Share
Consider a hypothetical metal that has a density of 3.55 g/cm3, an atomic weight of 40.48 g/mol, and an atomic radius of 0.135 nm. Compute t
Question
Consider a hypothetical metal that has a density of 3.55 g/cm3, an atomic weight of 40.48 g/mol, and an atomic radius of 0.135 nm. Compute the atomic packing factor if the unit cell has tetragonal symmetry, values for the a and c lattice parameters are 0.545 and 0.255, respectively.
in progress
0
Chemistry
3 years
2021-07-29T01:12:54+00:00
2021-07-29T01:12:54+00:00 1 Answers
51 views
0
Answers ( )
Answer:
0.5447
Explanation:
The atomic packing fraction factor is given by
APF = Volume of sphere/ Volume of unit cell
The atomic radius = 0.135 nm
The Density of the metal = 3.55 g/cm^3
To calculate the number of atoms
= desnsity/(atomic radius×Avagadro’s number)
Putting values and solving we get
the number of atoms = 4
Now,
Solving we get
APF = 0.54427