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Beryllium oxide

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Beryllium oxide
Unit cell, ball and stick model of beryllium oxide
Names
Preferred IUPAC name
Beryllium(II) monoxide
Systematic IUPAC name
Oxoberyllium
Other names
Beryllia, Thermalox, Bromellite, Thermalox 995.[1]
Identifiers
3D model (JSmol)
3902801
ChEBI
ChemSpider
ECHA InfoCard 100.013.758 Edit this at Wikidata
EC Number
  • 215-133-1
MeSH beryllium+oxide
RTECS number
  • DS4025000
UNII
UN number 1566
  • InChI=1S/Be.O checkY
    Key: LTPBRCUWZOMYOC-UHFFFAOYSA-N checkY
  • InChI=1/Be.O/rBeO/c1-2
    Key: LTPBRCUWZOMYOC-SRAGPBHZAE
  • [Be]=[O]
  • [Be-]#[O+]
Properties
BeO
Molar mass 25.011 g·mol−1
Appearance Colourless, vitreous crystals
Odor Odourless
Density 3.01 g/cm3[2]
Melting point 2,578 °C (4,672 °F; 2,851 K)[2]
Band gap 10.6 eV[3]
−11.9·10−6 cm3/mol[4]
Thermal conductivity 210 W/(m·K)[5]
n11.7184, n2=1.733[6][7]
Structure[8]
Hexagonal, zincite
P63mc
C6v
a = 2.6979 Å, c = 4.3772 Å
2
Linear
Thermochemistry[9]
25.6 J/(K·mol)
13.77±0.04 J/(K·mol)
−609.4±2.5 kJ/mol
−580.1 kJ/mol
Enthalpy of fusion (ΔfH⦵fus)
 86 kJ/mol
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Very toxic, Group 1B carcinogen
GHS labelling:
GHS06: Toxic GHS08: Health hazardGHS09: Environmental hazard
Danger
H301, H315, H317, H319, H330, H335, H350, H372
P201, P260, P280, P284, P301+P310, P305+P351+P338
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
4
0
0
Lethal dose or concentration (LD, LC):
15 mg/kg (mouse, oral)[11]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 0.002 mg/m3
C 0.005 mg/m3 (30 minutes), with a maximum peak of 0.025 mg/m3 (as Be)[10]
REL (Recommended)
 Ca C 0.0005 mg/m3 (as Be)[10]
IDLH (Immediate danger)
 Ca [4 mg/m3 (as Be)][10]
Related compounds
Other anions
 Beryllium telluride
Other cations
Supplementary data page
Beryllium oxide (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Beryllium oxide (BeO), also known as beryllia, is an inorganic compound with the formula BeO. This colourless solid is an electrical insulator with a higher thermal conductivity than any other non-metal except diamond, and exceeds that of most metals.[12] As an amorphous solid, beryllium oxide is white. Its high melting point leads to its use as a refractory material.[13] It occurs in nature as the mineral bromellite. Historically and in materials science, beryllium oxide was called glucina or glucinium oxide, owing to its sweet taste.

Preparation and chemical properties

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Beryllium oxide can be prepared by calcining (roasting) beryllium carbonate, dehydrating beryllium hydroxide, or igniting metallic beryllium:

BeCO3 → BeO + CO2
Be(OH)2 → BeO + H2O
2 Be + O2 → 2 BeO

Igniting beryllium in air gives a mixture of BeO and the nitride Be3N2.[12] Unlike the oxides formed by the other Group 2 elements (alkaline earth metals), beryllium oxide is amphoteric rather than basic.

Beryllium oxide formed at high temperatures (>800 °C) is inert, but dissolves easily in hot aqueous ammonium bifluoride (NH4HF2) or a solution of hot concentrated sulfuric acid (H2SO4) and ammonium sulfate ((NH4)2SO4).

Structure

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BeO crystallizes in the hexagonal wurtzite structure, featuring tetrahedral Be2+ and O2− centres, like lonsdaleite and w-BN (with both of which it is isoelectronic). In contrast, the oxides of the larger group-2 metals, i.e., MgO, CaO, SrO, BaO, crystallize in the cubic rock salt motif with octahedral geometry about the dications and dianions.[12] At high temperature the structure transforms to a tetragonal form.[14]

In the vapour phase, beryllium oxide is present as discrete diatomic molecules. In the language of valence bond theory, these molecules can be described as adopting sp orbital hybridisation on both atoms, featuring one σ bond (between one sp orbital on each atom) and one π bond (between aligned p orbitals on each atom oriented perpendicular to the molecular axis). Molecular orbital theory provides a slightly different picture with no net σ bonding (because the 2s orbitals of the two atoms combine to form a filled sigma bonding orbital and a filled sigma* anti-bonding orbital) and two π bonds formed between both pairs of p orbitals oriented perpendicular to the molecular axis. The sigma orbital formed by the p orbitals aligned along the molecular axis is unfilled. The corresponding ground state is ...(2sσ)2(2sσ*)2(2pπ)4 (as in the isoelectronic C2 molecule), where both bonds can be considered as dative bonds from oxygen towards beryllium.[15]

Applications

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High-quality crystals may be grown hydrothermally, or otherwise by the Verneuil method. For the most part, beryllium oxide is produced as a white amorphous powder, sintered into larger shapes. Impurities, like carbon, can give rise to a variety of colours to the otherwise colourless host crystals.

Sintered beryllium oxide is a very stable ceramic.[16] Beryllium oxide is used in rocket engines[17] and as a transparent protective over-coating on aluminised telescope mirrors. Metal-coated beryllium oxide (BeO) plates are used in the control systems of aircraft drive devices.[18]

Beryllium oxide is used in many high-performance semiconductor parts for applications such as radio equipment because it has good thermal conductivity while also being a good electrical insulator. It is used as a filler in some thermal interface materials such as thermal grease.[19] It is also employed in heat sinks and spreaders that cool electronic devices, such as CPUs, lasers, and power amplifiers.[20] Some power semiconductor devices have used beryllium oxide ceramic between the silicon chip and the metal mounting base of the package to achieve a lower value of thermal resistance than a similar construction of aluminium oxide. It is also used as a structural ceramic for high-performance microwave devices, vacuum tubes, cavity magnetrons [citation needed], and gas lasers. BeO has been proposed as a neutron moderator for naval marine high-temperature gas-cooled reactors (MGCR), as well as NASA's Kilopower nuclear reactor for space applications.[21]

Safety

[edit]

BeO is carcinogenic in powdered form[22] and may cause a chronic allergic-type lung disease berylliosis. Once fired into solid form, it is safe to handle if not subjected to machining that generates dust. Clean breakage releases little dust, but crushing or grinding actions can pose a risk.[23]

References

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  1. ^ "beryllium oxide – Compound Summary". PubChem Compound. USA: National Center for Biotechnology Information. 27 March 2005. Identification and Related records. Retrieved 8 November 2011.
  2. ^ a b Haynes, p. 4.51
  3. ^ Ryu, Y. R.; Lee, T. S.; Lubguban, J. A.; Corman, A. B.; White, H. W.; Leem, J. H.; Han, M. S.; Park, Y. S.; Youn, C. J.; Kim, W. J. (2006). "Wide-band gap oxide alloy: BeZnO". Applied Physics Letters. 88 (5): 052103. Bibcode:2006ApPhL..88e2103R. doi:10.1063/1.2168040.
  4. ^ Haynes, p. 4.126
  5. ^ Haynes, p. 12.222
  6. ^ Haynes, p. 10.248
  7. ^ Bromellite Mineral Data. webmineral
  8. ^ Haynes, p. 4.139
  9. ^ Haynes, pp. 5.1, 5.6, 6.155
  10. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0054". National Institute for Occupational Safety and Health (NIOSH).
  11. ^ Beryllium oxide toxicity
  12. ^ a b c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  13. ^ Higgins, Raymond Aurelius (2006). Materials for Engineers and Technicians. Newnes. p. 301. ISBN 0-7506-6850-4.
  14. ^ Wells, A. F. (1984). Structural Inorganic Chemistry (5 ed.). Oxford Science Publications. ISBN 0-19-855370-6.
  15. ^ Fundamentals of Spectroscopy. Allied Publishers. p. 234. ISBN 978-81-7023-911-6. Retrieved 29 November 2011.
  16. ^ Petzow, Günter; Aldinger, Fritz; Jönsson, Sigurd; Welge, Peter; van Kampen, Vera; Mensing, Thomas; Brüning, Thomas (2005) "Beryllium and Beryllium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim. doi:10.1002/14356007.a04_011.pub2
  17. ^ Ropp, R.C. (2023). "Chapter 3 - Group 16 (O, S, Se, Te) Alkaline Earth Compounds". Encyclopedia of the Alkaline Earth Compounds. Elsevier. pp. 105–197. doi:10.1016/B978-0-444-59550-8.00003-X. ISBN 9780444595508.
  18. ^ Trento, Chin (Dec 27, 2023). "What Are the Ceramic Materials With High Thermal Conductivity?". Stanford Advanced Materials. Retrieved Sep 3, 2024.
  19. ^ Greg Becker; Chris Lee; Zuchen Lin (2005). "Thermal conductivity in advanced chips — Emerging generation of thermal greases offers advantages". Advanced Packaging: 2–4. Archived from the original on June 21, 2000. Retrieved 2008-03-04.
  20. ^ "Beryllia (BeO)". Advanced Ceramic Materials. Retrieved Oct 18, 2024.
  21. ^ McClure, Patrick; Poston, David; Gibson, Marc; Bowman, Cheryl; Creasy, John (14 May 2014). "KiloPower Space Reactor Concept – Reactor Materials Study". Retrieved 21 November 2017.
  22. ^ "Hazardous Substance Fact Sheet" (PDF). New Jersey Department of Health and Senior Services. Retrieved August 17, 2018.
  23. ^ "Beryllium Oxide Safety". American Beryllia. Retrieved 2018-03-29.

Cited sources

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