Chemistry:Tetrafluoroberyllate

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Short description: Anion
Tetrafluoroberyllate
Tetrafluoroberyllate.png
Names
IUPAC name
Tetrafluoroberyllate(2−)[2][3][4]
Systematic IUPAC name
Tetrafluoroberyllate(2−)[5]
Other names
Tetrafluoroberyllate[1]
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
2035[10]
UNII
Properties
[BeF
4]2−
Molar mass 85.0057958 g·mol−1
Structure
Td
tetrahedral
Related compounds
Related isoelectronic
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Tetrafluoroberyllate or orthofluoroberyllate is an anion with the chemical formula [[[Beryllium|Be]]F
4]2−. It contains beryllium and fluorine. This fluoroanion has a tetrahedral shape, with the four fluorine atoms surrounding a central beryllium atom. It has the same size, charge, and outer electron structure as sulfate SO2−
4. Therefore, many compounds that contain sulfate have equivalents with tetrafluoroberyllate. Examples of these are the langbeinites, and Tutton's salts.

Properties

The Be–F bond length is between 145 and 153 pm. The beryllium is sp3 hybridized, leading to a longer bond than in BeF
2, where beryllium is sp hybridized.[11] In trifluoroberyllates, there are actually BeF
4 tetrahedra arranged in a triangle, so that three fluorine atoms are shared on two tetrahedra each, resulting in a formula of Be
3F
9.[12]

In the tetrafluoroberyllates, the tetrahedra can rotate to various degrees. At room temperature, they are hindered from moving. But as temperature increases, they can rotate around the threefold axis, (i.e. a line through one fluorine atom and the beryllium atom) with a potential barrier of 12.5 kcal/mol (52 kJ/mol). At higher temperatures, the movement can become isotropic (not limited to rotation on one axis) with a potential barrier of 14.5 kcal/mol (61 kJ/mol).[11]

Similar compounds have magnesium or zinc in a similar position as beryllium, e.g. K
2[MgF
4] (potassium tetrafluoromagnesate) or [NH
4]
2[ZnF
4] (ammonium tetrafluorozincate) but these are not as stable.[12]

Tetrafluoroberyllate has a biological effect by inhibiting F-ATPase adenosine triphosphate producing enzymes in mitochondria and bacteria. It does this by attempting to react with adenosine diphosphate because it resembles phosphate. However once it does this it remains stuck in the F1 part of the enzyme and inhibits it from further function.[13]

Simple salts

Name Chemical formula Molar mass (g/mol) CAS number Crystal system Density (g/cm3) Melting point (°C) Solubility in water
(g/(100 ml))
lithium tetrafluoroberyllate Li
2[BeF
4] 		98.89 2.167[14] 472 °C[15] slight (1.25 at 20 °C, 5.78 at 40 °C)[16]
sodium tetrafluoroberyllate Na
2BeF
4 		130.985333 13871-27-7 Orthorhombic[17] 2.47 575 °C slight (1.33 at 0 °C, 1.44 at 20 °C, 2.73 at 90 °C)[18]
potassium tetrafluoroberyllate K
2BeF
4 		163.20 7787-50-0 orthorhombic a = 5.691 Å, b = 7.278 Å, c = 9.896 Å[19] as for strontium orthosilicate[12] 2.64[19]
potassium tetrafluoroberyllate dihydrate K
2BeF
4 · 2H2O 		199.233
ammonium tetrafluoroberyllate (NH
4)
2BeF
4 		121.0827 14874-86-3 orthorhombic a = 5.91 Å, b = 7.64 Å, c = 10.43 Å 1.71 decomposes 280 °C[20] 32.3 at 25 °C[21]
rubidium tetrafluoroberyllate Rb
2BeF
4 		255.941 orthorhombic a = 5.87 Å, b = 7.649 Å, c = 10.184 Å[19] 3.72[19]
caesium tetrafluoroberyllate Cs
2BeF
4 		350.8167 orthorhomic a = 8.03 Å, b = 10.81 Å, c = 0.622 Å 4.32
thallium tetrafluoroberyllate Tl
2BeF
4 		493.7724 orthorhombic a = 7.7238 Å, b = 5.9022 Å, c = 10.4499 Å[22] 6.884[22]
silver tetrafluoroberyllate Ag
2BeF
4 		300.7422
magnesium tetrafluoroberyllate MgBeF
4 		109.3108
calcium tetrafluoroberyllate CaBeF
4 		125.08 2.959[23]
strontium tetrafluoroberyllate SrBeF
4 		172.6 orthorhombic a = 5.291 Å, b = 6.787 Å, c = 8.307 Å 3.84 insoluble
barium tetrafluoroberyllate BaBeF
4 		222.333 4.17[14] insoluble
radium tetrafluoroberyllate RaBeF
4[24] 		311.005795 insoluble
hexaqua ferrous tetrafluoroberyllate FeBeF
4 · 6H2O[25]
heptaqua ferrous tetrafluoroberyllate FeBeF
4 · 7H2O[23] 		1.894
heptaqua nickel tetrafluoroberyllate NiBeF
4 · 7H2O[23]
hexaqua nickel tetrafluoroberyllate NiBeF
4 · 6H2O[23]
heptaqua cobalt tetrafluoroberyllate CoBeF
4 · 7H2O[23] 		1.867
hexaqua cobalt tetrafluoroberyllate CoBeF
4 · 6H2O[23] 		1.891
pentaqua copper tetrafluoroberyllate CuBeF
4 · 5H2O[23]
heptaqua zinc tetrafluoroberyllate ZnBeFe
4 · 7H2O[23]
lead tetrafluoroberyllate PbBeF
4 		292.2 6.135[14]
hydrazinium tetrafluoroberyllate N
2H
6BeF
4 		119.0668 a = 5.58 Å, b = 7.337 Å, c = 9.928 Å, α = 90°, β = 98.22°, γ = 90°[19]
triglycine tetrafluoroberyllate (NH
2CH
2COOH)
3 · H
2BeF
4 		312.221 2396-72-7 monoclinic[26][27]
ethylene diamine fluoroberyllate (NH
2CH
2CH
2NH
2) · H
2BeF
4[28] 		decomposes 330 °C
propylenediamine tetrafluoroberyllate (NH
2CH
2CH
2CH
2NH
2) · H
2BeF
4[29]
propylene-1,2-diamine tetrafluoroberyllate (NH
2CH(CH
3)CH
2NH
2) · H
2BeF
4[28] 		monoclinic a = 5.535 Å, b = 13.560 Å, c = 9.6048 Å, β = 106.73 Å, V = 690.4 Å3, Z = 4[30] 1.55
benzidine fluoroberyllate (NH
2C
6H
4C
6H
4NH
2) · H
2BeF
4[28] 		ins
tetramethyl ammonium tetrafluoroberyllate [N(CH
3)
4]
2BeF
4[14]
tetramine silver tetrafluoroberyllate [Ag(NH
3)
2]
2BeF
4[31]
[Cu(NH
3)
2]
2BeF
4[31]
[Cu(NH
3)
4]
2BeF
4 · H2O[31]
[Zn(NH
3)
4]
2BeF
4[31]
[Cd(NH
3)
4]
2BeF
4[31]
[Ni(NH
3)
6]
2BeF
4[31]
[Ni(NH
3)
4]
2BeF
4 · 2H2O[31]
[Ni(NH
3)
2]
2BeF
4[31]
[Co(NH
3)
6]
2BeF
4 · 3H2O[31]

Sodium tetrafluoroberyllate has several crystalline forms. Below 220 °C it takes the same form as orthorhombic olivine, and this is called γ phase. Between 220 °C and 320 °C it is in the α′ form. When temperature is raised above 320 °C it changes to the hexagonal α form. When cooled the α′ form changes to β form at 110 °C and this can be cooled to 70 °C before changing back to the γ form.[32] It can be formed by melting sodium fluoride and beryllium fluoride.[32] The gas above molten sodium tetrafluoroberyllate contains BeF
2 and NaF gas.[11]

Lithium tetrafluoroberyllate takes on the same crystal form as the mineral phenacite. As a liquid it is proposed for the molten salt reactor, in which it is called FLiBe. The liquid salt has a high specific heat, similar to that of water. The molten salt has a very similar density to the solid. The solid has continuous void channels through it, which reduces its density.[15] Li
2BeF
4 can be crystallised from aqueous solution using (NH
4)
2BeF
4 and LiCl.[33]

Potassium tetrafluoroberyllate has the same structure as anhydrous potassium sulfate, as does rubidium and caesium tetrafluoroberyllate. Potassium tetrafluoroberyllate can make solid solutions with potassium sulfate.[11] It can be used as a starting point to make the non-linear optic crystal KBe
2BO
3F
2 which has the highest power handling capacity and shortest UV performance of any borate.[34] It is quite soluble in water, so beryllium can be extracted from soil in this form.[35]

Ammonium tetrafluoroberyllate decomposes on heating by losing NH
4F vapour, progressively forming NH
4BeF
3, then NH
4Be
2F
5 and finally BeF
2.[11]

Thallium tetrafluoroberyllate can be made by dissolving beryllium fluoride and thallium carbonate together in hydrofluoric acid and then evaporating the solution.[22]

Radium tetrafluoroberyllate is used as a standard neutron source. The alpha particles from the radium cause neutrons to be emitted from the beryllium. It is precipitated from a radium chloride solution mixed with potassium tetrafluoroberyllate.[12]

Magnesium tetrafluoroberyllate can be precipitated from a hot saturated solution of ammonium tetrafluoroberyllate and a magnesium salt.[11] However, if the temperature reaches boiling point MgF
2 is precipitated instead.[36]

Calcium tetrafluoroberyllate resembles zircon in the way it melts and crystallises.[11]

Strontium tetrafluoroberyllate can be made in several forms. The γ form is produced by cooling a melt of SrF
2 and Be
2 and the β form is made by precipitating from a water solution. When melted and heated to 850–1145 °C, Be
2 gas evaporates leaving behind molten SrF
2.[11]

The barium tetrafluoroberyllate is very insoluble and can be used for gravimetric analysis of beryllium.[11]

H
2BeF
4 is an acid that can be produced from Ag
2BeF
4 and HCl. It only exists in aqueous solution.[11]

Triglycine tetrafluoroberyllate (TGFB) is ferroelectric with a transition point of 70 °C.[26] The crystals can be formed by dissolving BeF
2 in water, adding HF and then glycine. When the solution is cooled triglycine tetrafluoroberyllate forms. Cs
2BeF
4 and Tl
2BeF
4 in the solution reduce growth on the 001 direction so that tabular shaped crystals of TGFB form. The thallium compound can cut growth on the 001 axis by 99%.[37]

Double salts

Tuttons salts

The Tuttons salt (NH4)2Mn(BeF4)2·6(H2O) is made from a solution of NH4BeF3 mixed with NH4MnF3.[11] The equivalent of alums are hard to make because the trivalent ion will often form a complex with fluoride in preference to the beryllium fluoride. However the violet coloured acid and rubidium chrome alum exist at chilly temperatures for a few hours.[38]

Tutton's salts (also called schoenites) containing magnesium with fluoroberyllate are difficult to produce, as the solutions tend to precipitate insoluble MgF2.[39]

name formula molecular weight CAS crystal form density melting point solubility g/100ml
potassium lithium tetrafluoroberyllate KLiBeF4 131.05 P63, a = 8.781 Å, b = 5.070 Å c = 8.566 Å[40]
rubidium lithium tetrafluoroberyllate RbLiBeF4 177.41 P6322, a = 8.980 Å, b = 5.185 Å c = 8.751 Å[40]
caesium lithium tetrafluoroberyllate CsLiBeF4 224.852 P21/n, a = 9.328 Å b = 5.356 Å, c = 8.736 Å, γ = 89.82°[40]
acid chromium fluoroberyllate tetracosihydrate H2Cr2(BeF4)4·24H2O[38] 878.40
ammonium chromium fluoroberyllate tetracosihydrate (NH4)2Cr2(BeF4)4·24H2O[38] 912.46
rubidium chromium fluoroberyllate tetracosihydrate Rb2Cr2(BeF4)4·24H2O[38] 1047.32
manganese ammonium fluoroberyllate hydrate (NH4)2Mn(BeF4)2·6H2O[39] 369.118 1.758[41]
Rb2Fe(BeF4)2·6H2O[39] 504.884
ferrous ammonium fluoroberyllate hydrate (NH4)2Fe(BeF4)2·6H2O[39] 370.025[41]
nickel potassium fluoroberyllate hydrate K2Ni(BeF4)2·6H2O[39] 414.913[41]
nickel rubidium fluoroberyllate hydrate Rb2Ni(BeF4)2·6H2O[39] 507.732
Cs2Ni(BeF4)2·6H2O[39] 602.608
nickel ammonium fluoroberyllate hydrate (NH4)2Ni(BeF4)2·6H2O[39] 372.874 P21/a, a = 9.201 Å, b = 12.482 Å, c = 6.142 Å, β = 106.57 Å, V = 676.0 Å3 Z = 2[42] 1.843[41]
cobalt potassium fluoroberyllate hydrate K2Co(BeF4)2·6H2O[39] 415.233[41]
cobalt rubidium fluoroberyllate hydrate Rb2Co(BeF4)2·6H2O[39] 507.972
cobalt ammonium fluoroberyllate hydrate (NH4)2Co(BeF4)2·6H2O[39] 372.874 1.821[41]
copper rubidium fluoroberyllate hydrate Rb2Cu(BeF4)2·6H2O[39] 512.585
copper ammonium fluoroberyllate hydrate (NH4)2Cu(BeF4)2·6H2O[39] 377.726 1.858[41]
zinc rubidium fluoroberyllate hydrate Rb2Zn(BeF4)2·6H2O[39] 514.42
zinc ammonium fluoroberyllate hydrate (NH4)2Zn(BeF4)2·6H2O[39] 379.56 1.859[41]
cadmium rubidium fluoroberyllate hydrate Rb2Cd(BeF4)2·6H2O[39] 561.45
cadmium ammonium fluoroberyllate hydrate (NH4)2Cd(BeF4)2·6H2O[39] 426.591

Alums

Tetrafluoroberyllate salts equivalent to alums also exist with formula MABF4·12H2O, where M is univalent, and A trivalent. These are not common as fluoride often form insoluble products with the trivalent ions. Methods to produce these include evaporating mixed fluoride solutions under reduced pressure at 0 °C, or dissolving beryllium and other metal hydroxides in hydrofluoric acid at room temperature, cooled, and them mixing with cold ethyl alcohol, causing cooling and crystallisation.[43] The unit cell dimensions are slightly smaller (by 0.03–0.05 Å) than the corresponding sulfate alums.[43]

name formula molecular weight CAS crystal form density melting point solubility g/100ml
ammonium aluminium tetrafluoroberyllate alum NH4AlBeF4·12H2O [43]
potassium aluminium tetrafluoroberyllate alum KAlBeF4·12H2O [43]
potassium chromium tetrafluoroberyllate alum KCrBeF4·12H2O [43]
ammonium chromium tetrafluoroberyllate alum NH4CrBeF4·12H2O cubic a = 12.218 Å, Z = 4[43]
rubidium chromium tetrafluoroberyllate alum RbCrBeF4·12H2O 12.214 Å[43]
caesium chromium tetrafluoroberyllate alum CsCrBeF4·12H2O 12.323 Å[43]
thallium chromium tetrafluoroberyllate alum TlCrBeF4·12H2O 12.195 Å[43]
rubidium iron tetrafluoroberyllate alum RbFeBeF4·12H2O [43]
caesium iron tetrafluoroberyllate alum CsFeBeF4·12H2O [43]
monomethyl chromium tetrafluoroberyllate alum CH3NH3CrBeF4·12H2O 12.496 Å[44]
guanidium chromium tetrafluoroberyllate alum C(NH2)3CrBeF4·12H2O 12.538 Å[44] on heating forms a rhombohedral hexahydrate stable from 30 °C to 90 °C

References

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  2. ↑ "tetrafluoroberyllate(2−) (CHEBI:30497)" (table). 26 January 2009. https://www.ebi.ac.uk/chebi/searchId.do?chebiId=CHEBI:30497. Retrieved 30 January 2019. "Synonyms Sources tetrafluoroberyllate(2−) IUPAC" 
  3. ↑ "Tetrafluoroberyllate(2−)". p. Names. http://www.chemspider.com/Chemical-Structure.15238330.html. Retrieved 30 January 2019. "Tetrafluoroberyllate(2-) [ACD/IUPAC Name]" 
  4. ↑ "tetrafluoroberyllate(2−) (CHEBI:30497)". 26 January 2009. https://www.ebi.ac.uk/chebi/searchId.do?chebiId=CHEBI:30497. Retrieved 30 January 2019. "IUPAC Name tetrafluoridoberyllate(2−)" 
  5. ↑ "Tetrafluoroberyllate(2−)". p. More details. http://www.chemspider.com/Chemical-Structure.15238330.html. Retrieved 30 January 2019. "Systematic name Tetrafluoroberyllate(2−)" 
  6. ↑ "Tetrafluoroberyllate(2−)". p. Data Sources. http://www.chemspider.com/Chemical-Structure.15238330.html. Retrieved 30 January 2019. "30497" 
  7. ↑ "tetrafluoroberyllate(2-) (CHEBI:30497)". 26 January 2009. https://www.ebi.ac.uk/chebi/searchId.do?chebiId=CHEBI:30497. Retrieved 30 January 2019. "ChEBI ID CHEBI:30497" 
  8. ↑ "Tetrafluoroberyllate(2−)". p. More details. http://www.chemspider.com/Chemical-Structure.15238330.html. Retrieved 30 January 2019. "SMILES [Be-2](F)(F)(F)F" 
  9. ↑ "tetrafluoroberyllate(2−) (CHEBI:30497)" (table). 26 January 2009. https://www.ebi.ac.uk/chebi/searchId.do?chebiId=CHEBI:30497. Retrieved 30 January 2019. "SMILES F[Be--](F)(F)F" 
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  15. ↑ 15.0 15.1 Douglas, Thomas B.; William H. Payne (May 20, 1969). "Measured Solid Enthalpy and Derived Thermodynamic Properties of and Liquid Lithium Tetrafluoroberyllate, Li2BeF4 from 273 to 900 K". Journal of Research of the National Bureau of Standards Section A (Washington, D.C.: Institute for Basic Standards, National Bureau of Standards) 73A (5). 
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  18. ↑ Perry, Dale L. (2011-05-19). Handbook of Inorganic Compounds, Second Edition. Taylor & Francis. p. 394. ISBN 9781439814611. https://books.google.com/books?id=SFD30BvPBhoC&pg=PA50. Retrieved 13 July 2013. 
  19. ↑ 19.0 19.1 19.2 19.3 19.4 Villars, P.. "AtomWork Materials Database". Nationional Institute of Materials Science. http://crystdb.nims.go.jp/crystdb/search-materials. Retrieved 17 July 2013. 
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  21. ↑ Dyachenko, A.N.; Kraydenko, R.I.; Petlin, I.V.; Malyutin, L.N. (2016). "The Research of (NH4)2BeF4 Solution Purification Effectiveness". Procedia Engineering 152: 51–58. doi:10.1016/j.proeng.2016.07.624. open access
  22. ↑ 22.0 22.1 22.2 da Silva, Iván; González Silgo, Cristina; González Platas, Javier; Rodríguez Carvajal, Juan; Martínez Sarrión, María Luisa; Mestres, Lourdes (2005). "Powder neutron diffraction of Tl2BeF4 at six temperatures from room temperature to 1.5 K". Acta Crystallographica Section C 61 (12): i113–i116. doi:10.1107/S010827010503249X. ISSN 0108-2701. PMID 16330826. 
  23. ↑ 23.0 23.1 23.2 23.3 23.4 23.5 23.6 23.7 Rây, Nirmalendu Nath (1932). "Fluoberyllate und ihre Analogie mit den Sulfaten. II. Fluoberyllate einiger zweiwertiger Metalle" (in German). Zeitschrift für anorganische und allgemeine Chemie 205 (3): 257–267. doi:10.1002/zaac.19322050307. ISSN 0863-1786. 
  24. ↑ Sastri, Malladi Narasimha (1958). Radiochemical measurements on neutron sources (PDF) (Thesis). Durham University. pp. 18–20.
  25. ↑ Kaduk, J. A. (2019). "Section 4.9.4. Chemical reasonableness". in Gilmore, C. J.; Kaduk, J. A.; Schenk, H.. International Tables for Crystallography Volume H Powder diffraction. pp. 496–508. https://onlinelibrary.wiley.com/iucr/itc/Ha/ch4o9v0001/sec4o9o4/. 
  26. ↑ 26.0 26.1 Zarembovskaya, T. A.; V. M. Varikash; P. A. Pupkevich (1972). "Thermal expansion of triglycine fluoroberyllate crystals near the ferroelectric transition point". Soviet Physics Journal 15 (6): 920–922. doi:10.1007/BF00912245. ISSN 0038-5697. Bibcode: 1972SvPhJ..15..920Z. 
  27. ↑ Ghazaryan, V.V.; Fleck, M.; Petrosyan, A.M. (September 2014). "New chemical analogs of triglycine sulfate". Journal of Crystal Growth 401: 857–862. doi:10.1016/j.jcrysgro.2013.11.054. Bibcode: 2014JCrGr.401..857G. 
  28. ↑ 28.0 28.1 28.2 Ghosh, Amiya Kanti (1959). "Fluoberyllates of Organic Bases. I". Zeitschrift für anorganische und allgemeine Chemie 300 (1–2): 98–101. doi:10.1002/zaac.19593000110. ISSN 0044-2313. 
  29. ↑ Kanti Ghosh, Amiya; Nirmalendu Nath Ráy (1959). "Fluoberyllates and their Analogy with Sulphates. XII. Complex Compounds of Zinc and Cadmium Fluoberyllate with Organic Bases". Zeitschrift für anorganische und allgemeine Chemie 300 (1–2): 109–112. doi:10.1002/zaac.19593000112. ISSN 0044-2313. 
  30. ↑ Gerrard, Lee A.; Weller, Mark T. (30 September 2002). "Propane-1,2-diammonium tetrafluoroberyllate". Acta Crystallographica Section C 58 (10): m504–m505. doi:10.1107/S0108270102015718. PMID 12359927. 
  31. ↑ 31.0 31.1 31.2 31.3 31.4 31.5 31.6 31.7 31.8 Rây, Nirmalendunath (1939). "Fluoberyllate und ihre Analogie mit Sulfaten. VI. Die Fluoberyllate von Metallamminkomplexen". Zeitschrift für anorganische und allgemeine Chemie 241 (2–3): 165–171. doi:10.1002/zaac.19392410203. ISSN 0863-1786. 
  32. ↑ 32.0 32.1 Holm, J. L.; K. Lønvik (1982). "Studies of the polymorphic transformations of dicalcium silicate (Ca2SiO4) and sodium tetrafluoroberyllate (Na2BeF4) by Thermosonimetry and differential scanning calorimetry". Journal of Thermal Analysis 25 (1): 109–115. doi:10.1007/BF01913059. ISSN 0368-4466. 
  33. ↑ Simons, J.H. (1964-01-01). Fluorine Chemistry. Elsevier. pp. 20–22. ISBN 9780323147248. https://books.google.com/books?id=9AbqU4cI93wC&pg=PA21. Retrieved 13 July 2013. 
  34. ↑ Karas, George V. (2005). New Developments in Crystal Growth Research. Nova Publishers. pp. 24–26. ISBN 9781594545399. https://books.google.com/books?id=PjpWUwI7VSgC&pg=PA26. Retrieved 14 July 2013. 
  35. ↑ Stone, John (May 2004). "Extraction ofBeryllium-10 from Soil by Fusion". http://depts.washington.edu/cosmolab/chem/fusionmethod.pdf. Retrieved 14 July 2013. 
  36. ↑ Walsh, Kenneth A. (2009-01-01). Beryllium Chemistry and Processing. ASM International. p. 100. ISBN 9780871707215. https://books.google.com/books?id=3-GbhmSfyeYC&pg=PA100. Retrieved 14 July 2013. 
  37. ↑ Wieder, H.H.; C.R. Parkerson (1966). "Some ferroelectric and dielectric properties of triglycine fluoberyllate". Journal of Physics and Chemistry of Solids 27 (2): 247–252. doi:10.1016/0022-3697(66)90029-1. ISSN 0022-3697. Bibcode: 1966JPCS...27..247W. 
  38. ↑ 38.0 38.1 38.2 38.3 Ghosh, Amiya Kanti (1959). "Complex Chromic Fluoberyllates. I". Zeitschrift für anorganische und allgemeine Chemie 300 (1–2): 102–108. doi:10.1002/zaac.19593000111. ISSN 0044-2313. 
  39. ↑ 39.00 39.01 39.02 39.03 39.04 39.05 39.06 39.07 39.08 39.09 39.10 39.11 39.12 39.13 39.14 39.15 39.16 Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten" (in German). Zeitschrift für anorganische und allgemeine Chemie 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. 
  40. ↑ 40.0 40.1 40.2 Hahn, Th.; G. Lohre; S. J. Chung (1969). "A new tetrahedral framework structure in sulfates and fluoberyllates". Die Naturwissenschaften 56 (9): 459. doi:10.1007/bf00601063. ISSN 0028-1042. Bibcode: 1969NW.....56Q.459H. 
  41. ↑ 41.0 41.1 41.2 41.3 41.4 41.5 41.6 41.7 Nath Rây, Nirmalendu (1932). "Fluoberyllate und ihre Analogie mit Sulfaten. III. Doppelsalze der Fluoberyllate" (in German). Zeitschrift für anorganische und allgemeine Chemie 206 (2): 209–216. doi:10.1002/zaac.19322060209. ISSN 0863-1786. 
  42. ↑ Montgomery, H. (15 September 1980). "Diammonium nickel bis(tetrafluoroberyllate)hexahydrate". Acta Crystallographica Section B 36 (9): 2121–2123. doi:10.1107/S0567740880008060. http://journals.iucr.org/b/issues/1980/09/00/a19083/a19083.pdf. 
  43. ↑ 43.00 43.01 43.02 43.03 43.04 43.05 43.06 43.07 43.08 43.09 43.10 Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" (in fr). Comptes rendus hebdomadaires des séances de l'Académie des sciences (Paris) C268: 1782–1784. https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image. 
  44. ↑ 44.0 44.1 Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (15 June 1970). "Sur l'existence et la cristallographie de quelques nouveaux fluorobéryllates doubles de chrome [CH3NH3Cr(BeF4)2·12H2O, [C(NH2)3]Cr(BeF4)2·12H2O et [C(NH2)3]Cr(BeF4)2·6H2O"] (in fr). Comptes rendus hebdomadaires des séances de l'Académie des sciences (Paris) C270: 1973–1975. https://gallica.bnf.fr/ark:/12148/bpt6k480278s/f2016.image. 



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