Beryllium nitrate

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Names
Systematic IUPAC name
Beryllium nitrate
Other names
Beryllium dinitrate
Identifiers
  • 13597-99-4 checkY
  • 7787-55-5 (trihydrate) checkY
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.033.678 Edit this at Wikidata
EC Number
  • 237-062-5
UNII
UN number 2464
  • InChI=1S/Be.2NO3/c;2*2-1(3)4/q+2;2*-1 checkY
    Key: RFVVBBUVWAIIBT-UHFFFAOYSA-N checkY
  • [Be+2].[O-][N+]([O-])=O.[O-][N+]([O-])=O
Properties
Be(NO3)2
Molar mass 133.021982 g/mol
Appearance white solid
Odor odorless
Density 1.56 g/cm3
Melting point 60.5 °C (140.9 °F; 333.6 K)
Boiling point 142 °C (288 °F; 415 K) (decomposes)
166 g/100 mL
Thermochemistry
Std enthalpy of
formation (ΔfH⦵298)
 -700.4 kJ/mol
Hazards
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)[1]
REL (Recommended)
 Ca C 0.0005 mg/m3 (as Be)[1]
IDLH (Immediate danger)
 Ca [4 mg/m3 (as Be)][1]
Related compounds
Other cations
 Magnesium nitrate
Calcium nitrate
Strontium nitrate
Barium nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N  (what is checkY☒N ?)
Infobox references

Beryllium nitrate is an inorganic compound with the idealized chemical formula Be(NO3)2. The formula suggests a salt, but, as for many beryllium compounds, the compound is highly covalent. Little of its chemistry is well known. "When added to water, brown fumes are evolved; when hydrolyzed in sodium hydroxide solution, both nitrate and nitrite ions are produced. "[2]

Structure of basic berylliium nitrate.[3] Color scheme: red = O, blue = N, turquoise = Be.

Synthesis and reactions[]

The straw-colored adduct Be(NO3)2(N2O4) forms upon treatment of beryllium chloride with dinitrogen tetroxide:

BeCl2 + 3 N2O4 → Be(NO3)2(N2O4) + 2 NOCl

Upon heating, this adduct loses N2O4 and produces colorless Be(NO3)2. Further heating of Be(NO3)2 induces conversion to basic beryllium nitrate, which adopts a structure akin to that for basic berylium acetate.[4]

Unlike the basic acetate, with its six lipophilic methyl groups, the basic nitrate is insoluble in most solvents.

References[]

  1. ^ a b c NIOSH Pocket Guide to Chemical Hazards. "#0054". National Institute for Occupational Safety and Health (NIOSH).
  2. ^ Addison, C.C.; Logan, N. (1964). Anhydrous Metal Nitrates. Advances in Inorganic Chemistry and Radiochemistry. 6. pp. 71–142. doi:10.1016/S0065-2792(08)60225-3. ISBN 9780120236060.
  3. ^ Haley, M. J.; Wallwork, S. C.; Duffin, B.; Logan, N.; Addison, C. C. (1997). "Hexa-μ-nitrato-μ4-oxo-tetraberyllium". Acta Crystallographica Section C Crystal Structure Communications. 53 (7): 829–830. doi:10.1107/S010827019700303X.
  4. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 122. ISBN 978-0-08-037941-8.
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Salts and covalent derivatives of the nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO
3)−
4 		RONO2 NO−
3
NH4NO3 		HOONO2 FNO3 Ne
NaNO3 Mg(NO3)2 Al(NO3)3 Si P S ClONO2 Ar
KNO3 Ca(NO3)2 Sc(NO3)3 Ti(NO3)4 VO(NO3)3 Cr(NO3)3 Mn(NO3)2 Fe(NO3)2
Fe(NO3)3 		Co(NO3)2
Co(NO3)3 		Ni(NO3)2 CuNO3
Cu(NO3)2 		Zn(NO3)2 Ga(NO3)3 Ge As Se BrNO3 Kr
RbNO3 Sr(NO3)2 Y(NO3)3 Zr(NO3)4 Nb Mo Tc Ru(NO3)3 Rh(NO3)3 Pd(NO3)2
 AgNO3
 Cd(NO3)2 In(NO3)3 Sn(NO3)4 Sb(NO3)3 Te INO3 Xe(NO3)2
CsNO3 Ba(NO3)2   Hf(NO3)4 Ta W Re Os Ir
Au(NO3)3 Hg2(NO3)2
Hg(NO3)2
Tl(NO3)3 		Pb(NO3)2 Bi(NO3)3
BiO(NO3) 		Po(NO3)4 At Rn
  Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La(NO3)3 Ce(NO3)3
Ce(NO3)4 		Pr(NO3)3 Nd(NO3)3 Pm(NO3)3 Sm(NO3)3 Eu(NO3)3 Gd(NO3)3 Tb(NO3)3 Dy(NO3)3 Ho(NO3)3 Er(NO3)3 Tm(NO3)3 Yb(NO3)3 Lu(NO3)3
Ac(NO3)3 Th(NO3)4 UO2(NO3)2 Np(NO3)4 Pu(NO3)4 Am(NO3)3 Cm(NO3)3 Bk Cf Es Fm Md No Lr
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