Cubic Crystal System
In crystallography, the cubic (or isometric) crystal system is a crystal system where the unit cell is in the shape of a cube. This is one of the most common and simplest shapes found in crystals and minerals.
There are three main varieties of these crystals, called simple cubic (sc), body-centered cubic (bcc), and face-centered cubic (fcc, also known as cubic close-packed or ccp), plus a number of other variants listed below. Note that although the unit cell in these crystals is conventionally taken to be a cube, the primitive unit cell often is not. This is related to the fact that in most cubic crystal systems, there is more than one atom per cubic unit cell.
Cubic space groups
The three Bravais lattices which form cubic crystal systems are:
|Primitive (P)||Body-centered (I)||Face-centered (F)|
The simple cubic system (P) consists of one lattice point on each corner of the cube. Each atom at a lattice point is then shared equally between eight adjacent cubes, and the unit cell therefore contains in total one atom (1⁄8 × 8).
The body-centered cubic system (I) has one lattice point in the center of the unit cell in addition to the eight corner points. It has a net total of 2 lattice points per unit cell (1⁄8 × 8 + 1).
The face-centered cubic system (F) has lattice points on the faces of the cube, that each gives exactly one half contribution, in addition to the corner lattice points, giving a total of 4 atoms per unit cell (1⁄8 × 8 from the corners plus 1⁄2× 6 from the faces).
The isometric crystal system class names, examples, Schönflies notation, Hermann-Mauguin notation, point groups, International Tables for Crystallography space group number, orbifold, type, and space groups are listed in the table below. There are a total 36 cubic space groups.
|#||Point group||Example||Type||Space groups|
Other terms for hexoctahedral are: normal class, holohedral, ditesseral central class, galena type.
Atomic packing factors and examples
One important characteristic of a crystalline structure is its atomic packing factor. This is calculated by assuming that all the atoms are identical spheres, with a radius large enough that each sphere abuts the next. The atomic packing factor is the proportion of space filled by these spheres.
Assuming one atom per lattice point, in a simple cubic lattice with cube side length a, the sphere size would be a⁄2 and the atomic packing factor turns out to be about 0.524 (which is quite low). Similarly, in a bcc lattice, the atomic packing factor is 0.680, and in fcc it is 0.740. The fcc value is the highest theoretically possible value for any lattice, although there are other lattices which also achieve the same value, such as hexagonal close packed and one version of tetrahedral bcc.
As a rule, since atoms in a solid attract each other, the more tightly-packed arrangements of atoms tend to be more common. (Loosely packed arrangements do occur, though, for example if the orbital hybridization demands certain bond angles.) Accordingly, the simple-cubic structure, with especially low atomic packing factor, is rare in nature, but is found in polonium. The bcc and fcc, with their higher densities, are both quite common in nature. Examples of bcc include iron, chromium, tungsten, and niobium. Examples of fcc include lead (for example in lead(II) nitrate), aluminum, copper, gold and silver.
Compounds that consist of more than one element (e.g. binary compounds) often have crystal structures based on a cubic crystal system. Some of the more common ones are listed here.
Interpenetrating simple cubic (caesium chloride) structure
One structure is the “interpenetrating simple cubic” structure, also called the “caesium chloride” structure. Each of the two atom types forms a separate simple cubic lattice, with an atom of one type at the center of each cube of the other type. Altogether, the arrangement of atoms is the same as body-centered cubic, but with alternating types of atoms at the different lattice sites. (See picture here.)
Examples of compounds with this structure include caesium chloride itself, as well as certain other alkali halides when prepared at low temperatures or high pressures. More generally, this structure is more likely to be formed from two elements whose ions are of roughly the same size (for example, ionic radius of Cs+ = 167 pm, and Cl− = 181 pm) .
The coordination number of each atom in the structure is 8: the central cation is coordinated to 8 anions on the corners of a cube as shown, and similarly, the central anion is coordinated to 8 cations on the corners of a cube.
Another structure is the “rock salt” or “sodium chloride” (halite) structure. In this, each of the two atom types forms a separate face-centered cubic lattice, with the two lattices interpenetrating so as to form a 3D checkerboard pattern. (See picture here.)
Examples of compounds with this structure include sodium chloride itself, along with almost all other alkali halides, and “many divalent metal oxides, sulfides, selenides, and tellurides”. More generally, this structure is more likely to be formed if the cation is slightly smaller than the anion (a cation/anion radius ratio of 0.414 to 0.732).
The coordination number of each atom in this structure is 6: each cation is coordinated to 6 anions at the vertices of an octahedron, and similarly, each anion is coordinated to 6 cations at the vertices of an octahedron.
The interatomic distance (distance between cation and anion, or half the unit cell length a) in some rock-salt-structure crystals are: 2.3 Å (2.3 × 10−10 m) for NaF, 2.8 Å for NaCl, and 3.2 Å for SnTe.
Another common structure is the “zincblende” structure (also spelled “zinc blende”), named after the mineral zincblende (sphalerite). As in the rock-salt structure, the two atom types form two interpenetrating face-centered cubic lattices. However, it differs from rock-salt structure in how the two lattices are positioned relative to one another. Altogether, the arrangement of atoms is the same as diamond cubic structure, but with alternating types of atoms at the different lattice sites. (See picture here.)
- Diamond cubic
- Reciprocal lattice
- Atomium: building which is a model of a bcc unit cell, with vertical body diagonal.
- Crystal structure
- ^ Prince, E., ed (2006). International Tables for Crystallography. International Union of Crystallography. doi:10.1107/97809553602060000001. ISBN 978-1-4020-4969-9.
- ^ Crystallography and Minerals Arranged by Crystal Form, Webmineral
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Oxford: Butterworth-Heinemann. ISBN 0080379419. . The original discovery was in J. Chem. Phys. 14, 569 (1946), web link. Also see this more recent non-technical article.
- ^ a b Seitz, Modern Theory of Solids (1940), p.49
- ^ The CsCl (B2) Structure
- ^ The NaCl (B1) Structure
- ^ Sundquist, J. J.; Lin, C. C. (1981). “Electronic structure of the F centre in a sodium fluoride crystal”. Journal of Physics C: Solid State Physics 14 (32): 4797–4805. Bibcode 1981JPhC…14.4797S. doi:10.1088/0022-3719/14/32/016.
- ^ Abrahams, S. C.; Bernstein, J. L. (1965). “Accuracy of an automatic diffractometer. Measurement of the sodium chloride structure factors”. Acta Cryst. 18: 926–932. doi:10.1107/S0365110X65002244.
- ^ Kao, W.; Peretti, E. (1970). “The ternary subsystem Sn4As3-SnAs-SnTe”. Journal of the Less Common Metals 22: 39–50. doi:10.1016/0022-5088(70)90174-8.
- ^ L. Kantorovich (2004). Quantum Theory of the Solid State. Springer. p. 32. ISBN 1402021534. http://books.google.com/?id=YoI2-QvDoUAC&pg=PA32.
- ^ Birkbeck College, University of London
- ^ The Zincblende (B3) Structure
- Hurlbut, Cornelius S.; Klein, Cornelis, 1985, Manual of Mineralogy, 20th ed., Wiley, ISBN 0-471-80580-7
This information originally retrieved from http://en.wikipedia.org/wiki/Cubic_crystal_system
on Wednesday 3rd August 2011 6:17 pm EDT
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