The coordination number of an atom in a molecule or a crystal is the number of its nearest neighbours. This number is determined somewhat differently for molecules and for crystals. In chemistry the emphasis is on molecules (or ions) with defined bonding structures, and the coordination number of an atom is determined by simply counting the other atoms to which it is bonded (by either single or multiple bonds).

However the solid-state structures of crystallography often have less clearly defined bonds, so a simpler model is used in which the atoms are represented by touching spheres. In this model the coordination number of an atom is the number of other atoms which it touches.

Chemistry usage

In chemistry, coordination number (c.n.), defined originally in 1893 by Alfred Werner, is the total number of neighbours of a central atom in a molecule or ion. Although a carbon atom has four chemical bonds in most stable molecules, the coordination number of each carbon is four in methane (CH₄), three in ethylene (H₂C=CH₂, each C is bonded to 2H + 1C = 3 atoms), and two in acetylene. In effect we count the first bond (or sigma bond) to each neighbouring atom, but not the other bonds (pi bonds).

In inorganic chemistry also, only the first or sigma bond between each ligand and the central atom counts, but not any pi bonds to the same ligands. In tungsten hexacarbonyl, W(CO)₆, the coordination number of tungsten (W) is counted as six although pi as well as sigma bonding is important in such metal carbonyls.

Examples of high coordination number complexes are the ions formed by uranium and thorium with bidentate nitrate ion ligands, U(NO₃)₆²⁻ and Th(NO₃)₆²⁻. Here each nitrate ligand is bound to the metal by two oxygen atoms, so that the total coordination number of the U or Th atom is 12.

When the surrounding ligands get smaller even higher coordination numbers may be possible. One in silico computational chemistry study predicted a particularly stable PbHe₁₅²⁺ ion composed of a central lead ion coordinated with no less than 15 helium atoms..

Crystallography usage

In materials science, the bulk coordination number of a given atom in the interior of a crystal lattice is the number of atoms touching the given atom. Iron at 20^oC has a body-centered cubic (BCC) crystal in which each interior iron atom occupies the centre of a cube formed by eight neighbouring iron atoms. The bulk coordination number for this structure is therefore 8.

The highest bulk coordination number is 12, found in both hexagonal close-packed (HCP) and cubic close-packed (CCP) (also known as face-centered cubic or FCC) structures. This value of 12 corresponds to the theoretical limit of the kissing number problem when all spheres are identical.

The two most common allotropes of carbon have different coordination numbers. In diamond each carbon atom is at the centre of a tetrahedron formed by four other carbon atoms, so the coordination number is four as for methane. Graphite is made of two-dimensional layers in which each carbon is covalently bonded to three other carbons. Atoms in other layers are much further away and are not nearest neighbours, so the coordination number of a carbon atom in graphite is 3 as in ethylene.

Simple ionic structures are described by two coordination numbers, one for each type of ion. Calcium fluoride (CaF₂) is an (8, 4) structure, meaning that each cation Ca²⁺ is surrounded by eight F⁻ anion neighbors, and each anion F⁻ by four Ca²⁺. For sodium chloride (NaCl) the numbers of cations and anions are equal, and both coordination numbers are six so that the structure is (6, 6).

For an atom at a surface of a crystal, the surface coordination number is always less than the bulk coordination number. The surface coordination number is dependent on which Miller index the surface uses. In a body-centered cubic (BCC) crystal, the bulk coordination number is 8, whereas for the (100) surface, the surface coordination number is 4.

References

External links

• Meteorite Book-Glossary C
• A website on Coordination Numbers