In chemistry the polyhedral skeletal electron pair theory (PSEPT) provides electron counting rules useful for predicting the structures of clusters such as borane and carborane clusters. The electron counting rules were originally formulated by Kenneth Wade,[1] and were further developed by others including Michael Mingos;[2] they are sometimes known as Wade's rules or the Wade–Mingos rules.[3] The rules are based on a molecular orbital treatment of the bonding.[4][5][6][7] These rules have been extended and unified in the form of the Jemmis mno rules.[8][9]

Predicting structures of cluster compounds

The structure of the butterfly cluster compound [Re4(CO)12]2− conforms to the predictions of PSEPT.
The structure of the butterfly cluster compound [Re4(CO)12]2− conforms to the predictions of PSEPT.

Different rules (4n, 5n, or 6n) are invoked depending on the number of electrons per vertex.

The 4n rules are reasonably accurate in predicting the structures of clusters having about 4 electrons per vertex, as is the case for many boranes and carboranes. For such clusters, the structures are based on deltahedra, which are polyhedra in which every face is triangular. The 4n clusters are classified as closo-, nido-, arachno- or hypho-, based on whether they represent a complete (closo-) deltahedron, or a deltahedron that is missing one (nido-), two (arachno-) or three (hypho-) vertices.

However, hypho clusters are relatively uncommon due to the fact that the electron count is high enough to start to fill antibonding orbitals and destabilize the 4n structure. If the electron count is close to 5 electrons per vertex, the structure often changes to one governed by the 5n rules, which are based on 3-connected polyhedra.

As the electron count increases further, the structures of clusters with 5n electron counts become unstable, so the 6n rules can be implemented. The 6n clusters have structures that are based on rings.

A molecular orbital treatment can be used to rationalize the bonding of cluster compounds of the 4n, 5n, and 6n types.

4n rules

Ball-and-stick models showing the structures of the boron skeletons of borane clusters.
Ball-and-stick models showing the structures of the boron skeletons of borane clusters.

The following polyhedra are closo polyhedra, and are the basis for the 4n rules; each of these have triangular faces.[10] The number of vertices in the cluster determines what polyhedron the structure is based on.

Number of vertices Polyhedron
4 Tetrahedron
5 Trigonal bipyramid
6 Octahedron
7 Pentagonal bipyramid
8 D2d (trigonal) dodecahedron (snub disphenoid)
9 Tricapped trigonal prism
10 Bicapped square antiprism
11 Edge-contracted icosahedron (octadecahedron)
12 Icosahedron (bicapped pentagonal antiprism)

Using the electron count, the predicted structure can be found. n is the number of vertices in the cluster. The 4n rules are enumerated in the following table.

Electron count Name Predicted structure
4n − 2 Bicapped closo n − 2 vertex closo polyhedron with 2 capped (augmented) faces
4n Capped closo n − 1 vertex closo polyhedron with 1 face capped
4n + 2 closo closo polyhedron with n vertices
4n + 4 nido n + 1 vertex closo polyhedron with 1 missing vertex
4n + 6 arachno n + 2 vertex closo polyhedron with 2 missing vertices
4n + 8 hypho n + 3 vertex closo polyhedron with 3 missing vertices
4n + 10 klado n + 4 vertex closo polyhedron with 4 missing vertices

When counting electrons for each cluster, the number of valence electrons is enumerated. For each transition metal present, 10 electrons are subtracted from the total electron count. For example, in Rh6(CO)16 the total number of electrons would be 6 × 9 + 16 × 2 − 6 × 10 = 86 – 60 = 26. Therefore, the cluster is a closo polyhedron because n = 6, with 4n + 2 = 26.


Other rules may be considered when predicting the structure of clusters:

  1. For clusters consisting mostly of transition metals, any main group elements present are often best counted as ligands or interstitial atoms, rather than vertices.
  2. Larger and more electropositive atoms tend to occupy vertices of high connectivity and smaller more electronegative atoms tend to occupy vertices of low connectivity.
  3. In the special case of boron hydride clusters, each boron atom connected to 3 or more vertices has one terminal hydride, while a boron atom connected to two other vertices has two terminal hydrogen atoms. If more hydrogen atoms are present, they are placed in open face positions to even out the coordination number of the vertices.
  4. For the special case of transition metal clusters, ligands are added to the metal centers to give the metals reasonable coordination numbers, and if any hydrogen atoms are present they are placed in bridging positions to even out the coordination numbers of the vertices.

In general, closo structures with n vertices are n-vertex polyhedra.

To predict the structure of a nido cluster, the closo cluster with n + 1 vertices is used as a starting point; if the cluster is composed of small atoms a high connectivity vertex is removed, while if the cluster is composed of large atoms a low connectivity vertex is removed.

To predict the structure of an arachno cluster, the closo polyhedron with n + 2 vertices is used as the starting point, and the n + 1 vertex nido complex is generated by following the rule above; a second vertex adjacent to the first is removed if the cluster is composed of mostly small atoms, a second vertex not adjacent to the first is removed if the cluster is composed mostly of large atoms.

Os6(CO)18, carbonyls omitted
Os6(CO)18, carbonyls omitted

Example: Pb2−

Electron count: 10 × Pb + 2 (for the negative charge) = 10 × 4 + 2 = 42 electrons.
Since n = 10, 4n + 2 = 42, so the cluster is a closo bicapped square antiprism.

Example: S2+

Electron count: 4 × S – 2 (for the positive charge) = 4 × 6 – 2 = 22 electrons.
Since n = 4, 4n + 6 = 22, so the cluster is arachno.
Starting from an octahedron, a vertex of high connectivity is removed, and then a non-adjacent vertex is removed.

Example: Os6(CO)18

Electron count: 6 × Os + 18 × CO – 60 (for 6 osmium atoms) = 6 × 8 + 18 × 2 – 60 = 24
Since n = 6, 4n = 24, so the cluster is capped closo.
Starting from a trigonal bipyramid, a face is capped. The carbonyls have been omitted for clarity.
B5H4−5, hydrogen atoms omitted
, hydrogen atoms omitted

Example:[11] B

Electron count: 5 × B + 5 × H + 4 (for the negative charge) = 5 × 3 + 5 × 1 + 4 = 24
Since n = 5, 4n + 4 = 24, so the cluster is nido.
Starting from an octahedron, one of the vertices is removed.

The rules are useful in also predicting the structure of carboranes. Example: C2B7H13

Electron count = 2 × C + 7 × B + 13 × H = 2 × 4 + 7 × 3 + 13 × 1 = 42
Since n in this case is 9, 4n + 6 = 42, the cluster is arachno.

The bookkeeping for deltahedral clusters is sometimes carried out by counting skeletal electrons instead of the total number of electrons. The skeletal orbital (electron pair) and skeletal electron counts for the four types of deltahedral clusters are:

The skeletal electron counts are determined by summing the total of the following number of electrons:

5n rules

As discussed previously, the 4n rule mainly deals with clusters with electron counts of 4n + k, in which approximately 4 electrons are on each vertex. As more electrons are added per vertex, the number of the electrons per vertex approaches 5. Rather than adopting structures based on deltahedra, the 5n-type clusters have structures based on a different series of polyhedra known as the 3-connected polyhedra, in which each vertex is connected to 3 other vertices. The 3-connected polyhedra are the duals of the deltahedra. The common types of 3-connected polyhedra are listed below.

5n cluster: P4
5n cluster: P4
5n + 3 cluster: P4S3
5n + 3 cluster: P4S3
5n + 6 cluster: P4O6
5n + 6 cluster: P4O6
Number of vertices Type of 3-connected polyhedron
4 Tetrahedron
6 Trigonal prism
8 Cube
10 Pentagonal prism
12 D2d pseudo-octahedron (dual of snub disphenoid)
14 Dual of triaugmented triangular prism (K5 associahedron)
16 Square truncated trapezohedron
18 Dual of edge-contracted icosahedron
20 Dodecahedron

The 5n rules are as follows.

Total electron count Predicted structure
5n n-vertex 3-connected polyhedron
5n + 1 n – 1 vertex 3-connected polyhedron with one vertex inserted into an edge
5n + 2 n – 2 vertex 3-connected polyhedron with two vertices inserted into edges
5n + k nk vertex 3-connected polyhedron with k vertices inserted into edges

Example: P4

Electron count: 4 × P = 4 × 5 = 20
It is a 5n structure with n = 4, so it is tetrahedral

Example: P4S3

Electron count 4 × P + 3 × S = 4 × 5 + 3 × 6 = 38
It is a 5n + 3 structure with n = 7. Three vertices are inserted into edges

Example: P4O6

Electron count 4 × P + 6 × O = 4 × 5 + 6 × 6 = 56
It is a 5n + 6 structure with n = 10. Six vertices are inserted into edges

6n rules

As more electrons are added to a 5n cluster, the number of electrons per vertex approaches 6. Instead of adopting structures based on 4n or 5n rules, the clusters tend to have structures governed by the 6n rules, which are based on rings. The rules for the 6n structures are as follows.

S8 crown
S8 crown
Total electron count Predicted structure
6n – k n-membered ring with k2 transannular bonds
6n – 4 n-membered ring with 2 transannular bonds
6n – 2 n-membered ring with 1 transannular bond
6n n-membered ring
6n + 2 n-membered chain (n-membered ring with 1 broken bond)

Example: S8

Electron count = 8 × S = 8 × 6 = 48 electrons.
Since n = 8, 6n = 48, so the cluster is an 8-membered ring.
6n + 2 cluster: hexane
6n + 2 cluster: hexane

Hexane (C6H14)

Electron count = 6 × C + 14 × H = 6 × 4 + 14 × 1 = 38
Since n = 6, 6n = 36 and 6n + 2 = 38, so the cluster is a 6-membered chain.

Isolobal vertex units

Provided a vertex unit is isolobal with BH then it can, in principle at least, be substituted for a BH unit, even though BH and CH are not isoelectronic. The CH+ unit is isolobal, hence the rules are applicable to carboranes. This can be explained due to a frontier orbital treatment.[10] Additionally there are isolobal transition-metal units. For example, Fe(CO)3 provides 2 electrons. The derivation of this is briefly as follows:

Bonding in cluster compounds

MO diagram of B6H2−6 showing the orbitals responsible for forming the cluster. Pictorial representations of the orbitals are shown; the MO sets of T and E symmetry will each have two or one additional pictorial representation, respectively, that are not shown here.
MO diagram of B
showing the orbitals responsible for forming the cluster. Pictorial representations of the orbitals are shown; the MO sets of T and E symmetry will each have two or one additional pictorial representation, respectively, that are not shown here.
The boron atoms lie on each vertex of the octahedron and are sp hybridized.[11] One sp-hybrid radiates away from the structure forming the bond with the hydrogen atom. The other sp-hybrid radiates into the center of the structure forming a large bonding molecular orbital at the center of the cluster. The remaining two unhybridized orbitals lie along the tangent of the sphere like structure creating more bonding and antibonding orbitals between the boron vertices.[9] The orbital diagram breaks down as follows:
The 18 framework molecular orbitals, (MOs), derived from the 18 boron atomic orbitals are:
  • 1 bonding MO at the center of the cluster and 5 antibonding MOs from the 6 sp-radial hybrid orbitals
  • 6 bonding MOs and 6 antibonding MOs from the 12 tangential p-orbitals.
The total skeletal bonding orbitals is therefore 7, i.e. n + 1.

Transition metal clusters

Transition metal clusters use the d orbitals for bonding. Thus, they have up to nine bonding orbitals, instead of only the four present in boron and main group clusters.[12][13] PSEPT also applies to metallaboranes

Clusters with interstitial atoms

Owing their large radii, transition metals generally form clusters that are larger than main group elements. One consequence of their increased size, these clusters often contain atoms at their centers. A prominent example is [Fe6C(CO)16]2-. In such cases, the rules of electron counting assume that the interstitial atom contributes all valence electrons to cluster bonding. In this way, [Fe6C(CO)16]2- is equivalent to [Fe6(CO)16]6- or [Fe6(CO)18]2-.[14]


  1. ^ Wade, K. (1971). "The structural significance of the number of skeletal bonding electron-pairs in carboranes, the higher boranes and borane anions, and various transition-metal carbonyl cluster compounds". J. Chem. Soc. D. 1971 (15): 792–793. doi:10.1039/C29710000792.
  2. ^ Mingos, D. M. P. (1972). "A General Theory for Cluster and Ring Compounds of the Main Group and Transition Elements". Nature Physical Science. 236 (68): 99–102. Bibcode:1972NPhS..236...99M. doi:10.1038/physci236099a0.
  3. ^ Welch, Alan J. (2013). "The significance and impact of Wade's rules". Chem. Commun. 49 (35): 3615–3616. doi:10.1039/C3CC00069A. PMID 23535980.
  4. ^ Wade, K. (1976). "Structural and Bonding Patterns in Cluster Chemistry". Adv. Inorg. Chem. Radiochem. Advances in Inorganic Chemistry and Radiochemistry. 18: 1–66. doi:10.1016/S0065-2792(08)60027-8. ISBN 9780120236183.
  5. ^ Girolami, G. (Fall 2008). "Lecture notes distributed at the University of Illinois, Urbana-Champaign". ((cite journal)): Cite journal requires |journal= (help) These notes contained original material that served as the basis of the sections on the 4n, 5n, and 6n rules.
  6. ^ Gilespie, R. J. (1979). "Nyholm Memorial Lectures". Chem. Soc. Rev. 8 (3): 315–352. doi:10.1039/CS9790800315.
  7. ^ Mingos, D. M. P. (1984). "Polyhedral Skeletal Electron Pair Approach". Acc. Chem. Res. 17 (9): 311–319. doi:10.1021/ar00105a003.
  8. ^ Jemmis, Eluvathingal D.; Balakrishnarajan, Musiri M.; Pancharatna, Pattath D. (2001). "A Unifying Electron-counting rule for Macropolyhedral Boranes, Metallaboranes, and Metallocenes". J. Am. Chem. Soc. 123 (18): 4313–4323. doi:10.1021/ja003233z. PMID 11457198.
  9. ^ a b Jemmis, Eluvathingal D.; Balakrishnarajan, Musiri M.; Pancharatna, Pattath D. (2002). "Electronic Requirements for Macropolyhedral Boranes". Chem. Rev. 102 (1): 93–144. doi:10.1021/cr990356x. PMID 11782130.
  10. ^ a b Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5
  11. ^ a b Cotton, Albert (1990). Chemical Applications of Group Theory. John Wiley & Sons. pp. 205–251. ISBN 0-471-51094-7.
  12. ^ King, R. B.; Rouvray, D. H. (1977). "Chemical Applications of Group Theory and Topology.7. A Graph-Theoretical Interpretation of the Bonding Topology in Polyhedral Boranes, Carboranes, and Metal Clusters". J. Am. Chem. Soc. 99 (24): 7834–7840. doi:10.1021/ja00466a014.
  13. ^ Kostikova, G. P.; Korolkov, D. V. (1985). "Electronic Structure of Transition Metal Cluster Complexes with Weak- and Strong-field Ligands". Russ. Chem. Rev. 54 (4): 591–619. Bibcode:1985RuCRv..54..344K. doi:10.1070/RC1985v054n04ABEH003040. S2CID 250797537.
  14. ^ Fehlner, Thomas P. (2006). "Cluster Compounds: Inorganometallic Compounds Containing Transition Metal & Main Group Elements". Encyclopedia of Inorganic Chemistry. doi:10.1002/0470862106.ia097. ISBN 0470860782.

General references