Beryllium nitride
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| Watchedfields = changed
| verifiedrevid = 428817099
| ImageFile = Tl2O3structure.jpg
| ImageSize =
| IUPACName = Beryllium nitride
| OtherNames = triberyllium dinitride
|Section1={{Chembox Identifiers
| CASNo_Ref = {{cascite|correct|??}}
| CASNo = 1304-54-7
| PubChem =
| SMILES = [Be]=N[Be]N=[Be]
| SMILES2 = [Be+2].[Be+2].[Be+2].[N-3].[N-3]
| SMILES3 = [Be]=[N-].[Be+2].[N-]=[Be]
| InChI = InChI=1S/3Be.2N
| InChI2 = InChI=1S/3Be.2N/q3*+2;2*-3
| InChI3 = InChI=1S/3Be.2N/q;;+2;2*-1
| EINECS = 215-132-6
| UNII = P0T5F6IUK4
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|Section2={{Chembox Properties
| Be=3|N=2
| Appearance = yellow or white powder
| Density = 2.71 g/cm3
| MeltingPtC = 2200
| BoilingPtC = 2240
| BoilingPt_notes = (decomposes)
| Solubility = decomposes
| Solubility1 = decomposes in solutions of acid and base
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|Section3={{Chembox Structure
| CrystalStruct = Cubic, cI80, SpaceGroup = Ia-3, No. 206 (α form)
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|Section7={{Chembox Hazards
| MainHazards =
| FlashPt =
| AutoignitionPt =
| REL = Ca C 0.0005 mg/m3 (as Be){{PGCH|0054}}
| PEL = TWA 0.002 mg/m3
C 0.005 mg/m3 (30 minutes), with a maximum peak of 0.025 mg/m3 (as Be)
}}
|Section8 = {{Chembox Related
| OtherCations = Calcium nitride
Magnesium nitride
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Beryllium nitride, Be3N2, is a nitride of beryllium. It can be prepared from the elements at high temperature (1100–1500 °C);Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier {{ISBN|0-12-352651-5}} unlike beryllium azide or BeN6, it decomposes in vacuum into beryllium and nitrogen. It is readily hydrolysed forming beryllium hydroxide and ammonia. It has two polymorphic forms cubic α-Be3N2 with a defect anti-fluorite structure, and hexagonal β-Be3N2. It reacts with silicon nitride, Si3N4 in a stream of ammonia at 1800–1900 °C to form BeSiN2.
Preparation
Beryllium nitride is prepared by heating beryllium metal powder with dry nitrogen in an oxygen-free atmosphere in temperatures between 700 and 1400 °C.
: 3Be + N2 → Be3N2
Uses
It is used in refractory ceramicsHugh O. Pierson, 1996, Handbook of Refractory Carbides and Nitrides: Properties, Characteristics, Processing, and Applications, William Andrew Inc.,{{ISBN|0-8155-1392-5}} as well as in nuclear reactors.
It is used to produce radioactive carbon-14 for tracer applications by the {{chem|14|7|N}} + n → {{chem|14|6|C}} + p reaction. It is favoured due to its stability, high nitrogen content (50%), and the very low capture cross section of beryllium for neutrons.{{Cite report |url=https://www.osti.gov/biblio/4324224 |title=THE PRODUCTION OF C$sup 14$ BY THE Be$sub 3$N$sub 2$ PROCESS |last=Shields |first=R. P. |date=1956-02-01 |publisher=Oak Ridge National Lab. (ORNL), Oak Ridge, TN (United States) |issue=ORNL-1962 |osti=4324224 |language=English}}
Reactions
Beryllium nitride reacts with mineral acids producing ammonia and the corresponding salts of the acids:
: Be3N2 + 6 HCl → 3 BeCl2 + 2 NH3
In strong alkali solutions, a beryllate forms, with evolution of ammonia:
: Be3N2 + 6 NaOH → 3 Na2BeO2 + 2 NH3
Both the acid and alkali reactions are brisk and vigorous. Reaction with water, however, is very slow:
: Be3N2 + 6 H2O → 3 Be(OH)2 + 2 NH3
Reactions with oxidizing agents are likely to be violent. It is oxidized when heated at 600 °C in air.
References
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{{Beryllium compounds}}
{{Nitrides}}
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