Atomic packing factor Information & Atomic packing factor Links at HealthHaven.com

In crystallography, atomic packing factor (APF) or packing fraction is the fraction of volume in a crystal structure that is occupied by atoms. It is dimensionless and always less than unity. For practical purposes, the APF of a crystal structure is determined by assuming that atoms are rigid spheres. For one-component crystals (those that contain only one type of atom), the APF is represented mathematically by

$\mathrm{APF} = \frac{N_\mathrm{atoms} V_\mathrm{atom}}{V_\mathrm{unit cell}}$

where N_atoms is the number of atoms in the unit cell, V_atom is the volume of an atom, and V_{unit cell} is the volume occupied by the unit cell. It can be proven mathematically that for one-component structures, the most dense arrangement of atoms has an APF of about 0.74. In reality, this number can be higher due to specific intermolecular factors. For multiple-component structures, the APF can exceed 0.74.

[edit] Worked out example

BCC structure

The primitive unit cell for the body-centered cubic (BCC) crystal structure contains nine atoms: one on each corner of the cube and one atom in the center. Because the volume of each corner atom is shared between adjacent cells, each BCC cell contains two atoms.

Each corner atom touches the center atom. A line that is drawn from one corner of the cube through the center and to the other corner passes through 4r, where r is the radius of an atom. By geometry, the length of the diagonal is a√3. Therefore, the length of each side of the BCC structure can be related to the radius of the atom by

$a = \frac{4r}{\sqrt{3}}.$

Knowing this and the formula for the volume of a sphere( $(4 / 3)$ pi r³), it becomes possible to calculate the APF as follows:

$\mathrm{APF} = \frac{N_\mathrm{atoms} V_\mathrm{atom}}{V_\mathrm{crystal}}$

$= \frac{2 (4/3)\pi r^3}{(4r/\sqrt{3})^3}$

$= \frac{\pi\sqrt{3}}{8}$

$\approx 0.68.\,\!$

For the hexagonal close-packed (HCP) structure the derivation is similar. The side length of the hexagon will be denoted as a while the height of the hexagon will be denoted as c. Then:

$a = 2 \times r$

$c = (\sqrt{\frac{2}{3}})(4r).$

It is then possible to calculate the APF as follows:

$\mathrm{APF} = \frac{N_\mathrm{atoms} V_\mathrm{atom}}{V_\mathrm{crystal}}$

$= \frac{6 (4/3)\pi r^3}{[(3\sqrt{3})/2](a^2)(c)}$

$= \frac{6 (4/3)\pi r^3}{[(3\sqrt{3})/2](2r)^2(\sqrt{\frac{2}{3}})(4r)}$

$= \frac{6 (4/3)\pi r^3}{[(3\sqrt{3})/2](\sqrt{\frac{2}{3}})(16r^3)}$

$= \frac{\pi}{\sqrt{18}}$

$\approx 0.74.\,\!$

[edit] APF of common structures

By similar procedures, the ideal atomic packing factors of all crystal structures can be found. The common ones are collected here as reference, rounded to the nearest hundredth.

[edit] See also

Crystal

[edit] References

Schaffer, Saxena, Antolovich, Sanders, and Warner (1999). The Science and Design of Engineering Materials (Second Edition ed.). New York: WCB/McGraw-Hill. pp. 81–88.
Callister, W. (2002). Materials Science and Engineering (Sixth Edition ed.). San Francisco: John Wiley and Sons. pp. 105–114.

[edit] External links

Contents

[edit] Worked out example

[edit] APF of common structures

[edit] See also

[edit] References

[edit] External links