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F r o m W i k i p e d i a , t h e f r e e e n c y c l o p e d i a
( R e d i r e c t e d f r o m B e r y l l i a )
Other names
Beryllia, Thermalox, Bromellite, Thermalox 995.[1]
3902801
100.013.758
beryllium+oxide
1566
InChI=1S/Be.O Y
Key: LTPBRCUWZOMYOC-UHFFFAOYSA-N Y
Key: LTPBRCUWZOMYOC-SRAGPBHZAE
[Be-]#[O+]
Be O
25.011 g·mol−1
Colourless, vitreous crystals
Odourless
3.01 g/cm3 [2]
2,578 °C (4,672 °F; 2,851 K )[2]
10.6 eV[3]
−11.9·10−6 cm 3 /mol[4]
210 W/(m·K)[5]
n 1 1.7184, n2 =1.733[6] [7]
Hexagonal, zincite
P63 mc
C 6v
a = 2.6979 Å, c = 4.3772 Å
2
Linear
25.6 J/(K·mol)
13.77±0.04 J/(K·mol)
−609.4±2.5 kJ/mol
−580.1 kJ/mol
86 kJ/mol
Very toxic, Group 1B carcinogen
Danger
H301 , H315 , H317 , H319 , H330 , H335 , H350 , H372
P201 , P260 , P280 , P284 , P301+P310 , P305+P351+P338
Lethal dose or concentration (LD, LC):
15 mg/kg (mouse, oral)[11]
NIOSH (US health exposure limits):
TWA 0.002 mg/m3 C 0.005 mg/m3 (30 minutes), with a maximum peak of 0.025 mg/m3 (as Be)[10]
Ca C 0.0005 mg/m3 (as Be)[10]
Ca [4 mg/m3 (as Be)][10]
Beryllium telluride
Strontium oxide
Barium oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
Chemical compound
Beryllium oxide (BeO ), also known as beryllia , is an inorganic compound with the formula BeO. This colourless solid is a 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 [ edit ]
Beryllium oxide can be prepared by calcining (roasting) beryllium carbonate , dehydrating beryllium hydroxide , or igniting metallic beryllium :
BeCO3 → BeO + CO2
Be(OH )2 → BeO + H2 O
2 Be + O2 → 2 BeO
Igniting beryllium in air gives a mixture of BeO and the nitride Be 3 N 2 .[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 (NH 4 HF 2 ) or a solution of hot concentrated sulfuric acid (H 2 SO 4 ) and ammonium sulfate ((NH 4 )2 SO 4 ).
Structure [ edit ]
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 C 2 molecule), where both bonds can be considered as dative bonds from oxygen towards beryllium.[15]
Applications [ edit ]
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[citation needed ] and as a transparent protective over-coating on aluminised telescope mirrors .
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 .[17] 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 , 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.[18]
BeO is carcinogenic in powdered form[19] 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.[20]
References [ edit ]
^ "beryllium oxide – Compound Summary" . PubChem Compound . USA: National Center for Biotechnology Information. 27 March 2005. Identification and Related records. Retrieved 8 November 2011 .
^ a b Haynes , p. 4.51
^ 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 .
^ Haynes , p. 4.126
^ Haynes , p. 12.222
^ Haynes , p. 10.248
^ Bromellite Mineral Data . webmineral
^ Haynes , p. 4.139
^ Haynes , pp. 5.1, 5.6, 6.155
^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0054" . National Institute for Occupational Safety and Health (NIOSH).
^ Beryllium oxide toxicity
^ a b c Greenwood, Norman N. ; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann . ISBN 978-0-08-037941-8 .
^ Higgins, Raymond Aurelius (2006). Materials for Engineers and Technicians . Newnes. p. 301 . ISBN 0-7506-6850-4 .
^ Wells, A. F. (1984). Structural Inorganic Chemistry (5 ed.). Oxford Science Publications. ISBN 0-19-855370-6 .
^ Fundamentals of Spectroscopy . Allied Publishers. p. 234. ISBN 978-81-7023-911-6 . Retrieved 29 November 2011 .
^ 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
^ 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 .
^ McClure, Patrick; Poston, David; Gibson, Marc; Bowman, Cheryl; Creasy, John (14 May 2014). "KiloPower Space Reactor Concept – Reactor Materials Study" . Retrieved 21 November 2017 .
^ "Hazardous Substance Fact Sheet" (PDF) . New Jersey Department of Health and Senior Services. Retrieved August 17, 2018 .
^ "Beryllium Oxide Safety" . American Beryllia . Retrieved 2018-03-29 .
Cited sources [ edit ]
External links [ edit ]
BeBr2
BeCO3
BeCl2
BeF2
BeH2
BeI2
Be(N 3 )2
Be(NO 3 )2
Be 4 O(C 2 H 3 O 2 )6
BeC2 O 4
BeO
Be(OH )2
BeS
BeSO4
BeTe
Be 2 C
BeCrO4
Be 3 N 2
Boron suboxide (B 12 O 2 )
Carbon suboxide (C 3 O 2 )
Chlorine perchlorate (Cl 2 O 4 )
Chloryl perchlorate (Cl 2 O 6 )
Cobalt(II,III) oxide (Co 3 O 4 )
Dichlorine pentoxide (Cl 2 O 5 )
Iron(II,III) oxide (Fe 3 O 4 )
Lead(II,IV) oxide (Pb 3 O 4 )
Manganese(II,III) oxide (Mn 3 O 4 )
Mellitic anhydride (C 12 O 9 )
Praseodymium(III,IV) oxide (Pr 6 O 11 )
Silver(I,III) oxide (Ag 2 O 2 )
Terbium(III,IV) oxide (Tb 4 O 7 )
Tribromine octoxide (Br 3 O 8 )
Triuranium octoxide (U 3 O 8 )
Copper(I ) oxide (Cu 2 O )
Caesium monoxide (Cs 2 O )
Dicarbon monoxide (C 2 O )
Dichlorine monoxide (Cl 2 O )
Gallium(I ) oxide (Ga 2 O )
Iodine(I ) oxide (I 2 O )
Lithium oxide (Li 2 O )
Mercury(I ) oxide (Hg 2 O )
Nitrous oxide (N 2 O )
Potassium oxide (K 2 O )
Rubidium oxide (Rb 2 O )
Silver oxide (Ag 2 O )
Thallium(I ) oxide (Tl 2 O )
Sodium oxide (Na 2 O )
Water (hydrogen oxide) (H 2 O )
Barium oxide (Ba O )
Berkelium monoxide (Bk O )
Beryllium oxide (Be O )
Bromine monoxide (Br O )
Cadmium oxide (Cd O )
Calcium oxide (Ca O )
Carbon monoxide (C O )
Chlorine monoxide (Cl O )
Chromium(II ) oxide (Cr O )
Cobalt(II ) oxide (Co O )
Copper(II ) oxide (Cu O )
Dinitrogen dioxide (N 2 O 2 )
Europium(II ) oxide (Eu O )
Germanium monoxide (Ge O )
Iron(II ) oxide (Fe O )
Iodine monoxide (I O )
Lead(II ) oxide (Pb O )
Magnesium oxide (Mg O )
Manganese(II ) oxide (Mn O )
Mercury(II ) oxide (Hg O )
Nickel(II ) oxide (Ni O )
Nitric oxide (N O )
Palladium(II ) oxide (Pd O )
Phosphorus monoxide (P O )
Polonium monoxide (Po O )
Protactinium monoxide (Pa O )
Radium oxide (Ra O )
Silicon monoxide (Si O )
Strontium oxide (Sr O )
Sulfur monoxide (S O )
Disulfur dioxide (S 2 O 2 )
Thorium monoxide (Th O )
Tin(II ) oxide (Sn O )
Titanium(II ) oxide (Ti O )
Vanadium(II ) oxide (V O )
Yttrium(II ) oxide (Y O )
Zinc oxide (Zn O )
Aluminium oxide (Al 2 O 3 )
Americium(III) oxide (Am 2 O 3 )
Antimony trioxide (Sb 2 O 3 )
Arsenic trioxide (As 2 O 3 )
Berkelium(III) oxide (Bk 2 O 3 )
Bismuth(III) oxide (Bi 2 O 3 )
Boron trioxide (B 2 O 3 )
Caesium sesquioxide (Cs 2 O 3 )
Californium(III) oxide (Cf 2 O 3 )
Cerium(III) oxide (Ce 2 O 3 )
Chromium(III) oxide (Cr 2 O 3 )
Cobalt(III) oxide (Co 2 O 3 )
Dinitrogen trioxide (N 2 O 3 )
Dysprosium(III) oxide (Dy 2 O 3 )
Einsteinium(III) oxide (Es 2 O 3 )
Erbium(III) oxide (Er 2 O 3 )
Europium(III) oxide (Eu 2 O 3 )
Gadolinium(III) oxide (Gd 2 O 3 )
Gallium(III) oxide (Ga 2 O 3 )
Gold(III) oxide (Au 2 O 3 )
Holmium(III) oxide (Ho 2 O 3 )
Indium(III) oxide (In 2 O 3 )
Iron(III) oxide (Fe 2 O 3 )
Lanthanum oxide (La 2 O 3 )
Lutetium(III) oxide (Lu 2 O 3 )
Manganese(III) oxide (Mn 2 O 3 )
Neodymium(III) oxide (Nd 2 O 3 )
Nickel(III) oxide (Ni 2 O 3 )
Phosphorus trioxide (P 4 O 6 )
Praseodymium(III) oxide (Pr 2 O 3 )
Promethium(III) oxide (Pm 2 O 3 )
Rhodium(III) oxide (Rh 2 O 3 )
Samarium(III) oxide (Sm 2 O 3 )
Scandium oxide (Sc 2 O 3 )
Terbium(III) oxide (Tb 2 O 3 )
Thallium(III) oxide (Tl 2 O 3 )
Thulium(III) oxide (Tm 2 O 3 )
Titanium(III) oxide (Ti 2 O 3 )
Tungsten(III) oxide (W 2 O 3 )
Vanadium(III) oxide (V 2 O 3 )
Ytterbium(III) oxide (Yb 2 O 3 )
Yttrium(III) oxide (Y 2 O 3 )
Berkelium(IV ) oxide (Bk O 2 )
Bromine dioxide (Br O 2 )
Californium dioxide (Cf O 2 )
Carbon dioxide (C O 2 )
Carbon trioxide (C O 3 )
Cerium(IV ) oxide (Ce O 2 )
Chlorine dioxide (Cl O 2 )
Chromium(IV ) oxide (Cr O 2 )
Curium(IV ) oxide (Cm O 2 )
Dinitrogen tetroxide (N 2 O 4 )
Germanium dioxide (Ge O 2 )
Iodine dioxide (I O 2 )
Hafnium(IV ) oxide (Hf O 2 )
Lead dioxide (Pb O 2 )
Manganese dioxide (Mn O 2 )
Neptunium(IV ) oxide (Np O 2 )
Nitrogen dioxide (N O 2 )
Osmium dioxide (Os O 2 )
Plutonium(IV ) oxide (Pu O 2 )
Polonium dioxide (Po O 2 )
Praseodymium(IV ) oxide (Pr O 2 )
Protactinium(IV ) oxide (Pa O 2 )
Rhodium(IV ) oxide (Rh O 2 )
Ruthenium(IV ) oxide (Ru O 2 )
Selenium dioxide (Se O 2 )
Silicon dioxide (Si O 2 )
Sulfur dioxide (S O 2 )
Technetium(IV ) oxide (Tc O 2 )
Tellurium dioxide (Te O 2 )
Terbium(IV ) oxide (Tb O 2 )
Thorium dioxide (Th O 2 )
Tin dioxide (Sn O 2 )
Titanium dioxide (Ti O 2 )
Tungsten(IV ) oxide (W O 2 )
Uranium dioxide (U O 2 )
Vanadium(IV ) oxide (V O 2 )
Zirconium dioxide (Zr O 2 )
Arsenic pentoxide (As 2 O 5 )
Bismuth pentoxide (Bi 2 O 5 )
Dinitrogen pentoxide (N 2 O 5 )
Niobium pentoxide (Nb 2 O 5 )
Phosphorus pentoxide (P 2 O 5 )
Protactinium(V ) oxide (Pa 2 O 5 )
Tantalum pentoxide (Ta 2 O 5 )
Vanadium(V ) oxide (V 2 O 5 )
Molybdenum trioxide (Mo O 3 )
Polonium trioxide (Po O 3 )
Rhenium trioxide (Re O 3 )
Selenium trioxide (Se O 3 )
Sulfur trioxide (S O 3 )
Tellurium trioxide (Te O 3 )
Tungsten trioxide (W O 3 )
Uranium trioxide (U O 3 )
Xenon trioxide (Xe O 3 )
Manganese heptoxide (Mn 2 O 7 )
Rhenium(VII) oxide (Re 2 O 7 )
Technetium(VII) oxide (Tc 2 O 7 )
Osmium tetroxide (Os O 4 )
Ruthenium tetroxide (Ru O 4 )
Xenon tetroxide (Xe O 4 )
Hassium tetroxide (Hs O 4 )
Suboxide
Oxyanion
Ozonide
Peroxide
Superoxide
Oxypnictide
AmO2
Am 2 O 3
As 2 O 3
As 2 O 5
Au 2 O 3
B 2 O 3
BaO
BeO
Bi 2 O 3
BiO2
Bi 2 O 5
BrO2
Br 2 O 3
Br 2 O 5
Br 3 O 8
CO
CO 2
C 3 O 2
CaO
CaO2
CdO
CeO2
Ce 3 O 4
Ce 2 O 3
ClO2
Cl 2 O
Cl 2 O 2
Cl 2 O 3
Cl 2 O 4
Cl 2 O 6
Cl 2 O 7
CoO
Co 2 O 3
Co 3 O 4
CrO3
Cr 2 O 3
Cr 2 O 5
Cr 5 O 12
CsO2
Cs 2 O 3
CuO
Dy 2 O 3
Er 2 O 3
Eu 2 O 3
FeO
Fe 2 O 3
Fe 3 O 4
Ga 2 O
Ga 2 O 3
GeO
GeO2
H 2 O
2 H 2 O
3 H 2 O
H 2 18 O
H 2 O 2
HfO2
HgO
Hg 2 O
Ho 2 O 3
IO
I 2 O 4
I 2 O 5
I 2 O 6
I 4 O 9
In 2 O 3
IrO2
KO 2
K 2 O 2
La 2 O 3
Li 2 O
Li 2 O 2
Lu 2 O 3
MgO
Mg 2 O 3
MnO
MnO2
Mn 2 O 3
Mn 2 O 7
MoO2
MoO3
Mo 2 O 3
NO
NO 2
N 2 O
N 2 O 3
N 2 O 4
N 2 O 5
NaO2
Na 2 O
Na 2 O 2
NbO
NbO2
Nd 2 O 3
O 2 F
OF
OF 2
O 2 F 2
O 3 F 2
O 4 F 2
O 5 F 2
O 6 F 2
O 2 PtF6
more...
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