Borazine

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Borazine
Names
Preferred IUPAC name
1,3,5,2,4,6-Triazatriborinane (only preselected[1])
Other names
Cyclotriborazaneborazol
Inorganic benzene
Borazole
Identifiers
3D model (
JSmol
)
ChEBI
ChemSpider
ECHA InfoCard
 100.169.303 Edit this at Wikidata
UNII
  • InChI=1S/B3H6N3/c1-4-2-6-3-5-1/h1-6H checkY
    Key: BGECDVWSWDRFSP-UHFFFAOYSA-N checkY
  • InChI=1/B3H6N3/c1-4-2-6-3-5-1/h1-6H
    Key: BGECDVWSWDRFSP-UHFFFAOYAU
  • [BH-]1-[NH+]=[BH-]-[NH+]=[BH-]-[NH+]=1
Properties
B3H6N3
Molar mass 80.50 g/mol
Appearance Colorless liquid
Density 0.81 g/cm3
Melting point −58 °C (−72 °F; 215 K)
Boiling point 53 °C (127 °F; 326 K) (55 °C at 105 Pa)
-49.6·10−6 cm3/mol
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 2: Must be moderately heated or exposed to relatively high ambient temperature before ignition can occur. Flash point between 38 and 93 °C (100 and 200 °F). E.g. diesel fuelInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
2
2
1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Borazine, also known as borazole, is an

isoelectronic and isostructural with benzene. For this reason borazine is sometimes referred to as “inorganic benzene”. Like benzene, borazine is a colourless liquid[2]
with an aromatic odor.

Synthesis

The compound was reported in 1926 by the chemists Alfred Stock and Erich Pohland by a reaction of diborane with ammonia.[3]

Borazine can be synthesized by treating diborane and ammonia in a 1:2 ratio at 250–300 °C with a conversion of 50%.

3 B2H6 + 6 NH3 → 2 B3H6N3 + 12 H2

An alternative more efficient route begins with sodium borohydride and ammonium sulfate:[4]

6 NaBH4 + 3 (NH4)2SO4 → 2 B3N3H6 + 3 Na2SO4 + 18 H2

In a two-step process to borazine, boron trichloride is first converted to trichloroborazine:

3 BCl3 + 3 NH4Cl → Cl3B3H3N3 + 9 HCl

The B-Cl bonds are subsequently converted to B-H bonds:

2 Cl3B3H3N3 + 6 NaBH4 → 2 B3H6N3 + 3 B2H6 + 6 NaCl

Structure

Borazine is isoelectronic with benzene and has similar connectivity, so it is sometimes referred to as "inorganic benzene". This comparison is not rigorously valid due to the electronegativity difference between boron and nitrogen. X-ray crystallographic structural determinations show that the bond lengths within the borazine ring are all equivalent at 1.429 Å, a property shared by benzene.[5] However, the borazine ring does not form a perfect hexagon. The bond angle is 117.1° at the boron atoms and 122.9° at the nitrogens, giving the molecule the D3h symmetry point group.

The

mesomer
structures for borazine.

Boron behaves as a

Lewis base
.

Aromaticity

Due to its similarities to benzene, there have been a number of computational and experimental analyses of borazine's

standard enthalpy change of formation
ΔfH of −531 kJ/mol, is thermally very stable.

Natural bond orbitals (NBO)

Natural bond orbital (NBO) analysis suggests weak aromaticity in borazine.[6] In the NBO model, B-N bonds in the ring are slightly displaced from the nuclear axes, and B and N have large differences in charge. Natural chemical shielding (NCS) analysis provides some further evidence for aromaticity based on a contribution of the B-N π bond to magnetic shielding. Computations based on NBO orbitals show that this π bond allows for weak ring current which somewhat counteracts a magnetic field simulated at the center of the borazine ring. A small ring current does suggest some delocalization.

Electron localization function (ELF)

Topological analysis of bonding in borazine by the electron localization function (ELF) indicates that borazine can be described as a π aromatic compound. However, the bonding in borazine is less delocalized than in benzene based on a difference in bifurcation values of the electron basins. Larger bifurcation values indicate better electron delocalization, and it is argued that when this bifurcation value is greater than 0.70, the delocalization is sufficient to designate a compound aromatic.[7] For benzene, this value is 0.91, but the borazine π system bifurcates at the ELF value 0.682.[8] This is caused by the difference in electronegativity between B and N, which produces a weaker bond interaction than the C-C interaction in benzene, leading to increased localization of electrons on the B-H and N-H units. The bifurcation value is slightly below the limit of 0.70 which suggests moderate aromaticity.

Reactivity

Hydrolysis

Borazine hydrolyzes readily, yielding boric acid, ammonia, and hydrogen.

Polymerization

Polyborazylene

Heating borazine at 70 °C expels hydrogen with formation of polyborazylene:

n B3N3H6 → 1/n[B3N3H4]n

With hydrogen halides and halogens

With hydrogen chloride it forms an adduct.

B3N3H6 + 3 HCl → B3N3H9Cl3
Addition reaction of borazine with hydrogen chloride
B3N3H9Cl3 + NaBH4 → (BH4N)3
Reduction with sodium borohydride

The addition reaction with

catalyst. Borazines undergo nucleophilic attack at boron and electrophilic
attack at nitrogen.

Ceramic precursor

Boron nitride can be prepared by heating polyborazylene to 1000 °C.[4]

Borazines are also starting materials for other potential ceramics such as boron carbonitrides. Borazine can also be used as a precursor to grow hexagonal boron nitride (h-BN) thin films and single layers on catalytic surfaces such as copper,[9] platinum,[10] nickel[11] iron[12] and many more, with chemical vapor deposition (CVD).

synthetic route to boron carbonitrides, first step a hydroboration reaction to an oligomeric precursor followed by step two: pyrolysis
synthetic route to boron carbonitrides, first step a hydroboration reaction to an oligomeric precursor followed by step two: pyrolysis

Polyborazylene has been proposed as a recycled

hydrogen fuel cell vehicle applications, using a "single pot" process for digestion and reduction to recreate ammonia borane.[13]

Among other B-N type compounds mixed amino-nitro substituted borazines have been predicted to outperform carbon based explosives such as

CL-20.[14][15]

Related compounds

Main article:
Heterocyclic compounds

(C
2H
2B
2N
2) is a six-membered aromatic ring with two carbon atoms, two nitrogen atoms, and two boron atoms in opposing pairs.[16][17]

1,2-Dihydro-1,2-azaborine (C
4BNH
6) is a six-membered ring with four carbon atoms, one nitrogen atom, and one boron atom.

See also

Further reading

  • Nelson, Ralph; et al. (September 1, 1967). "Selected values of electric dipole moments for molecules in the gas phase" (PDF). American National Bureau of Standards (10): 17.

References

  1. ISBN 978-0-85404-182-4
    .
  2. ISBN 978-1429218207
    .
  3. doi:10.1002/cber.19260590906
    .
  4. ^
    ISBN 9780470132630
    .
  5. doi:10.1002/cber.19941271011
    .
  6. doi:10.1016/j.ica.2006.08.028
    .
  7. PMID 15268298
    .
  8. S2CID 95098134
    .
  9. PMID 25673919
    .
  10. PMID 23527543
    .
  11. ISSN 0897-4756
    .
  12. PMID 25664483
    .
  13. PMID 19514023
    .
  14. doi:10.1002/prep.201100157
    .
  15. S2CID 9774352
    .
  16. S2CID 94792421
    .
  17. PMID 26411675
    .

Further reading

External links

Media related to borazine at Wikimedia Commons

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