Chemistry:Beryllium nitride

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Beryllium nitride
Names
IUPAC name
Beryllium nitride
Other names
triberyllium dinitride
Identifiers
3D model (JSmol)
EC Number
  • 215-132-6
UNII
Properties
Be3N2
Molar mass 55.051 g·mol−1
Appearance yellow or white powder
Density 2.71 g/cm3
Melting point 2,200 °C (3,990 °F; 2,470 K)
Boiling point 2,240 °C (4,060 °F; 2,510 K) (decomposes)
decomposes
Solubility decomposes in solutions of acid and base
Structure[citation needed]
Cubic, cI80, SpaceGroup = Ia-3, No. 206 (α form)
Hazards
NIOSH (US health exposure limits):Template:Chembox NIOSH (set)/formatPocketGuideLink
PEL (Permissible)
  • TWA 0.0002 mg/m3
  • STEL 0.002 mg/m3 (15 minutes)
IDLH (Immediate danger)
 4 mg/m3 (as Be)
Related compounds
Other cations
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Beryllium nitride, Be
3N
2, is a nitride of beryllium. It can be prepared from the elements at high temperature (1,100–1,500 °C (2,010–2,730 °F)); unlike beryllium azide or BeN
6, it decomposes in vacuum into beryllium and nitrogen. It is readily hydrolysed forming beryllium hydroxide and ammonia. It has two polymorphic forms: cubic α–Be
3N
2 with a defect anti-fluorite structure, and hexagonal β–Be
3N
2. It reacts with silicon nitride, Si
3N
4 in a stream of ammonia at 1,800–1,900 °C (3,270–3,450 °F) to form BeSiN
2.[1]

Preparation

Beryllium nitride is prepared by heating beryllium metal powder with dry nitrogen in an oxygen-free atmosphere at temperatures between 700 and 1,400 °C (1,292 and 2,552 °F):[2]

3 Be + N
2 → B
3N
2

Uses

It is used in refractory ceramics[3] as well as in nuclear reactors.

It is used to produce radioactive carbon-14 for tracer applications by the 147N + neutron Template:Arrow 146C + proton reaction. It is favored due to its stability, high nitrogen content (50%), and the very low capture cross section of beryllium for neutrons.[4]

Reactions

Beryllium nitride reacts with mineral acids producing ammonia and the corresponding salts of the acids:

Be
3N
2 + 6 HCl → 3 BeCl
2 + 2 NH
3

In strong alkali solutions, a beryllate forms, with evolution of ammonia:

Be
3N
2 + 6 NaOH → 3 Na
2BeO
2 + 2 NH
3

Both the acid and alkali reactions are brisk and vigorous. Reaction with water, however, is very slow:

Be
3N
2 + 6 H
2O → 3 Be(OH)
2 + 2 NH
3

Reactions with oxidizing agents are likely to be violent. It is oxidized when heated at 600 °C (1,112 °F) in air.[5]

References

  1. ↑ Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils, ed., Inorganic Chemistry, San Diego/Berlin: Academic Press/De Gruyter, ISBN 0-12-352651-5 
  2. ↑ "Crystal structure and Uses of Beryllium nitride_Chemicalbook". https://www.chemicalbook.com/article/crystal-structure-and-uses-of-beryllium-nitride.htm. 
  3. ↑ Pierson, Hugh O. (1996). Handbook of refractory carbides and nitrides: properties, characteristics, processing, and applications. Park Ridge, N.J: Noyes Publications. ISBN 0-8155-1392-5. 
  4. ↑ Shields, R. P. (1956-02-01) (in English). The Production of C14 by the Be3N2 Process (Report). Oak Ridge National Lab. (ORNL), Oak Ridge, TN (United States). doi:10.2172/4324224. https://www.osti.gov/biblio/4324224. 
  5. ↑ "Beryllium Nitride" (in en). https://qsstudy.com/beryllium-nitride/. 
Salts and covalent derivatives of the nitride ion
NH3 He(N2)11
Li3N Be3N2 BN β-C3N4
g-C3N4 		N2 NxOy NF3 Ne
Na3N Mg3N2 AlN Si3N4 PN
P3N5 		SxNy
SN
S4N4 		NCl3 Ar
K3N Ca3N2 ScN TiN VN CrN
Cr2N 		MnxNy FexNy CoN Ni3N CuN Zn3N2 GaN Ge3N4 As Se NBr3 Kr
Rb3N Sr3N2 YN ZrN NbN β-Mo2N Tc Ru Rh PdN Ag3N CdN InN Sn Sb Te NI3 Xe
Cs3N Ba3N2   Hf3N4 TaN WN Re Os Ir Pt Au Hg3N2 TlN Pb BiN Po At Rn
Fr3N Ra3N   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La CeN Pr Nd Pm Sm Eu GdN Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UN Np Pu Am Cm Bk Cf Es Fm Md No Lr




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