Atomic packing factor

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In crystallography, atomic packing factor (APF), packing efficiency or packing fraction is the fraction of volume in a crystal structure that is occupied by constituent particles. It is dimensionless and always less than unity. In atomic systems, by convention, the APF is determined by assuming that atoms are rigid spheres. The radius of the spheres is taken to be the maximal value such that the atoms do not overlap. For one-component crystals (those that contain only one type of particle), the packing fraction is represented mathematically by

\mathrm{APF} = \frac{N_\mathrm{particle} V_\mathrm{particle}}{V_\mathrm{unit cell}}

where Nparticle is the number of particles in the unit cell, Vparticle is the volume of each particle, and Vunit 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, obtained by the close-packed structures. For multiple-component structures, the APF can exceed 0.74.

Single component crystal structures[edit]

Common sphere packings taken on by atomic systems are listed below with their corresponding packing fraction.

The majority of metals take on either the hcp, ccp or bcc structure.[2]

Body-centered cubic[edit]

BCC structure

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

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, 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.\,\!

Hexagonal close-packed[edit]

HCP structure

For the hexagonal close-packed structure the derivation is similar. Here the unit cell is a hexagonal prism containing six atoms. Let a be the side length of its base and c be its height. Then:

a = 2r


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

It is then possible to calculate the APF as follows:

\mathrm{APF} = \frac{N_\mathrm{atoms}\cdot 
V_\mathrm{atom}}{V_\mathrm{crystal}} = \frac{6\cdot (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.\,\!

See also[edit]

References[edit]

  1. ^ a b c d Ellis, Arthur B. [et al.] (1995). Teaching general chemistry : a materials science companion (3. print ed.). Washington: American Chemical Soceity. ISBN 084122725X. 
  2. ^ Moore, Lesley E. Smart; Elaine A. (2005). Solid state chemistry : an introduction (3. ed. ed.). Boca Raton, Fla. [u.a.]: Taylor & Francis, CRC. p. 8. ISBN 0748775161. 

Further Reading[edit]

  1. 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. 
  2. Callister, W. (2002). Materials Science and Engineering (Sixth Edition ed.). San Francisco: John Wiley and Sons. pp. 105–114.