Boranes

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Decaborane(14), B10H14

A borane is a compound with the formula BxHy or a related anion. Many such boranes are known. Most common are those with 1 to 12 boron atoms. Although they have few practical applications, the boranes exhibit structures and bonding that differs strongly from the patterns seen in hydrocarbons. Hybrids of boranes and hydrocarbons, the carboranes are also well developed.[1]

History

The development of the chemistry of boranes led to innovations in synthetic methods as well as structure and bonding. First, new synthetic techniques were required to handle diborane and many of its derivatives, which are both

pyrophoric and volatile. Alfred Stock invented the glass vacuum line for this purpose.[2]

The structure of diborane was correctly predicted in 1943 many years after its discovery.

Nobel prize in Chemistry in 1976 for this and many subsequent crystallographic investigations
. These investigations revealed the prevalence of deltahedral structures, i.e., networks of triangular arrays of BH centers.

The bonding of the clusters ushered in Polyhedral skeletal electron pair theory and Wade's rules, which can be used to predict the structures of boranes.[4] These rules were found to describe structures of many cluster compounds.

Interest in boranes increased during World War II due to the potential of

Nobel prize in Chemistry in 1979 for this work.[5]

Chemical formula and naming conventions

Borane clusters are classified as follows, where n is the number of boron atoms in a single cluster:[1][6][7]

Cluster type Chemical formula Example Notes
hypercloso- BnHn Unstable; derivatives are known[8]
closo- [BnHn]2− Caesium dodecaborate
nido- BnHn+4 pentaborane(9)
arachno- BnHn+6 pentaborane(11)
hypho- BnHn+8 Only found in adducts

The

systematic naming
is based on a prefix denoting a class of compound, followed by the number of boron atoms and finally the number of hydrogen atoms in parentheses. Various details can be omitted if there is no ambiguity about the meaning, for example, if only one structural type is possible. Some examples of the structures are shown below.

  • Hexaborate(6) [B6H6]2−
    Hexaborate(6)
    [B6H6]2−
  • Heptaborate(7) [B7H7]2−
    Heptaborate(7)
    [B7H7]2−
  • Octaborate(8) [B8H8]2−
    Octaborate(8)
    [B8H8]2−
  • Nonaborate(9) [B9H9]2−
    Nonaborate(9)
    [B9H9]2−
  • Decaborate(10) [B10H10]2−
    Decaborate(10)
    [B10H10]2−
  • Undecaborate(11) [B11H11]2−
    Undecaborate(11)
    [B11H11]2−
  • Dodecaborate(12) [B12H12]2−
    Dodecaborate(12)
    [B12H12]2−

The naming of anions is illustrated by

octahydridopentaborate, [B5H8]−

The hydrogen count is specified first followed by the boron count. The -ate suffix is applied with

anions
. The ionic charge value is included in the chemical formula but not as part of the systematic name.

Bonding in boranes

Boranes are nonclassically–bonded compounds, that is, there are not enough electrons to form 2-centre, 2-electron bonds between all pairs of adjacent atoms in the molecule. A description of the bonding in the larger boranes was formulated by William Lipscomb. It involved:

  • 3-center 2-electron B-H-B hydrogen bridges
  • 3-center 2-electron B-B-B bonds
  • 2-center 2-electron bonds (in B-B, B-H and BH2)

Lipscomb's methodology has largely been superseded by a molecular orbital approach. This allows the concept of multi-centre bonding to be extended. For example, in the icosahedral ion [B12H12]2−, the totally symmetric (Ag symmetry) molecular orbital is equally distributed among all 12 boron atoms. Wade's rules provide a powerful method that can be used to rationalize the structures in terms of the number of atoms and the connectivity between them.

Multicluster boranes

Structure of the conjuncto boron hydride cluster [B19H22]−.[9]

Although relatively rare, several multi-cluster boranes have been characterized. For example, reaction of a borane cluster with B2H6 (as a source of BH3) can lead to the formation of a conjuncto-borane species in which borane cluster sub-units are joined by the sharing of boron atoms.[10]

B6H10 + "BH3" → B7H11 + H2
B7H11 + B6H10 → B13H19 + H2

Other conjuncto-boranes, where the sub-units are joined by a B-B bond, can be made by ultra violet irradiation of nido-boranes. Some B-B coupled conjuncto-boranes can be produced using PtBr2 as catalyst.[11]

Analogous to Wade's Rules, electron counting scheme has been developed to predict or rationalize multicluster boranes.

Multi-cluster descriptors[12]
Prefix Meaning Example
klado- branched clusters
conjuncto- conjoined clusters
megalo- multiple conjoined clusters

Reactivity of boranes

For reactions of diborane, see diborane.

The lowest borane, BH3 exists only transiently,

DMSO are sufficiently stable to be used in hydroboration
reactions. Reminiscent of the behavior of diborane, some lower boranes react with air very exothermically, even explosively. By contrast, many closo-borane cluster, such as [B12H12]2−, do not react with air.

The boron hydride clusters are so diverse that generalizations on their reactions are not possible.

Lewis acid/base behavior

Some function as electron donors owing to the relative basic character of the B−Hterminal groups. Boranes can function as

coordination compounds.[13] Hapticities of η1 to η6 have been found, with electron donation involving bridging H atoms or donation from B-B bonds. For example, nido-B6H10 can replace ethene in Zeise's salt to produce trans-Pt(η2-B6H10)Cl2.[13]

They can also act as

Lewis acids, with concomitant opening of the cluster. An example involving trimethylphosphine
:

B5H9 + 2 P(CH3)3 → B5H9·2P(CH3)3

Brønsted acid/base behavior

Some higher boranes, especially those with bridging hydrogen atoms, can be deprotonated with a strong base. An example:

B5H9 + NaH → Na[B5H8] + H2

Acidity increases with the size of the borane, with B10H14 having a

pKa value of 2.7.[14][15]

B10H14 < B16H20 < B18H22

Aufbau reactions

Structure of [(CH3)4N+]2[Fe(C2B9H11)2]+, showing only one Me4N+.[16]

For the boron hydride chemist, one of the most important reactions is the building up process by which smaller boron hydride clusters add borane to give larger clusters. This approach also applies to the synthesis of metallaboranes,

Hydroboration

Reminiscent of the behavior of diborane and its adducts, higher boranes participate in hydroboration. When boron hydrides add an alkyne, the carbon becomes incorporated into the cluster, producing carboranes, e.g. C2B10H12.[17]

Applications

Diborane and its monomeric adducts

borane–dimethylsulfide are useful reagents. They are often used for hydroboration in organic synthesis. Some cobalt derivatives of carboranes have been commercialized for sequestering 137Cs from radioactive waste.[18]

Boranes have a high specific energy of combustion compared to hydrocarbons, making them potentially attractive as fuels or igniters. Intense research was carried out in the 1950s into their use as jet fuel additives, but the effort did not lead to practical results.

Aspirational uses

Because 10B has a very high

neutron-capture cross section, boron-hydride derivatives have often been investigated for applications in Neutron capture therapy of cancer.[19]

10B + 1n → (11B*) → 4He + 7Li + γ (2.4 Mev)

See also

References

  1. ^
    ISBN 978-0-08-037941-8
    . pp 151-195
  2. ^ Stock, Alfred (1933). The Hydrides of Boron and Silicon. New York: Cornell University Press.
  3. doi:10.1039/JR9430000250
    .
  4. S2CID 98202127
    .
  5. ISBN 0-471-11280-1
    .
  6. ISBN 0-471-19957-5
  7. ^ Lipscomb W. N. Boron Hydrides. Benjamin, New York (1963).
  8. PMID 11353472
    .
  9. PMID 20349936
    .
  10. ISBN 978-0-08-037941-8
    . p. 162
  11. S2CID 55817512
    .
  12. doi:10.1016/S0020-1693(99)00071-7
    .
  13. ^
    ISBN 978-0-08-037941-8
    .
  14. ^ temperature not stated
  15. ISBN 978-0-08-037941-8
    . p. 171
  16. doi:10.1021/ic00009a015
    .
  17. doi:10.1021/ja00389a021
    .
  18. PMID 25299942
    .
  19. ISBN 978-3-642-31333-2
    .
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