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IUPAC name
Systematic IUPAC name
Other names
tetrafluoridoberyllate(2-), BERYLLIUM TETRAFLUORIDE ION,[1][2] beryllium tetrafluoride, Tetrafluoroberyllate[3]
3D model (JSmol)
Molar mass 85.0068929 g·mol−1
Related compounds
tetrafluoroborate, tetrafluoromethane, tetrafluoroammonium
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 BeF2−
is an anion containing beryllium and fluorine. The ion has a tetrahedral shape, the same size and outer electron structure as sulfate. Therefore, many compounds that contain sulfate, have equivalents with tetrafluoroberyllate. Examples of these are the Langbeinites, and Tutton's salts.


The Be–F distance is between 1.45 and 1.53 Å. This bond is sp3 and has a longer length than the sp bond in BeF2 gas.[22] In trifluoroberyllates, there are actually BeF4 tetrahedra arranged in a triangle, so that three fluorine atoms are shared on two tetrahedra each, resulting in a formula of Be3F9.[23]

In the tetrafluoroberyllates the tetrahedra can rotate to various degrees. At room temperatures they are hindered from moving. But as temperature increases they can rotate around the three-fold axis, (ie a line through one fluorine atom and the beryllium atom) with a potential barrier of 12.5 kcal/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.[22]

Similar formula compounds have magnesium or zinc in a similar position to beryllium, e.g. K2MgF4 (Magnesium tetrafluoride) or (NH4)2ZnF4 (tetrafluorozincate) but these are not as stable.[23]

Tetrafluoroberyllate has a biological effect by inhibiting F-ATPase ATP 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.[24]

Simple salts[edit]

name formula molecular weight CAS crystal form density melting point solubility g/100ml
lithium tetrafluoroberyllate Li2BeF4 98.89 2.167[25] 472 °C[26]
lithium tetrafluoroberyllate Li2BeF4.H2O 116.89 1.944[25]
sodium tetrafluoroberyllate Na2BeF4 130.985333 13871-27-7 Orthorhombic[27] 2.47 575 °C slight 1.33 @0° 1.44 @20° 2.73 @90°[28]
potassium tetrafluoroberyllate K2BeF4 163.20 7787-50-0 orthorhombic a = 5.691Å, b = 7.278Å, c = 9.896Å[29] as for strontium orthosilicate[23] 2.64[29]
potassium tetrafluoroberyllate dihydrate K2BeF4.2(H2O) 199.233
ammonium tetrafluoroberyllate (NH4)2BeF4 121.0827 14874-86-3 orthorhombic a = 0.591 nm, b = 0.764 nm, c = 1.043 nm 1.71 d 280 °C[30] 323 g/l at 25°[31]
rubidium tetrafluoroberyllate Rb2BeF4 255.941 orthorhombic a = 5.87Å, b = 7.649Å, c = 10.184Å[29] 3.72[29]
caesium tetrafluoroberyllate Cs2BeF4 350.8167 orthorhomic a = 8.03Å, b = 10.81Å, c = 0.622Å 4.32
thallium tetrafluoroberyllate Tl2BeF4 493.7724 orthorhombic a=7.7238 b=5.9022 c=10.4499[32] 6.884[32]
silver tetrafluoroberyllate Ag2BeF4 300.7422
magnesium tetrafluoroberyllate MgBeF4 109.3108
calcium tetrafluoroberyllate CaBeF4 125.08 2.959[33]
strontium tetrafluoroberyllate SrBeF4 172.6 orthorhombic a = 0.5291 nm, b = 0.6787 nm, c = 0.8307 nm 3.84 ins
barium tetrafluoroberyllate BaBeF4 222.333 4.17[25] ins
radium tetrafluoroberyllate RaBeF4[34] 311.005795 ins
heptaqua ferrous tetrafluoroberyllate FeBe4.7H2O[33] 1.894
heptaqua nickel tetrafluoroberyllate NiBe4.7H2O[33]
hexaqua nickel tetrafluoroberyllate NiBe4.6H2O[33] 1.941
heptaqua cobalt tetrafluoroberyllate CoBe4.7H2O[33] 1.867
hexaqua cobalt tetrafluoroberyllate CoBe4.6H2O[33] 1.891
pentaqua copper tetrafluoroberyllate CuBe4.5H2O[33]
heptaqua zinc tetrafluoroberyllate ZnBe4.7H2O[33]
cadmium tetrafluoroberyllate CdBe4.8/3H2O[33]
lead tetrafluoroberyllate PbBeF4 292.2 6.135[25]
hydrazinium tetrafluoroberyllate N2H6BeF4 119.0668 a = 0.558 nm, b = 0.7337 nm, c = 0.9928 nm, α = 90 °, β = 98.22 °, γ = 90 °[29]
triglycine tetrafluoroberyllate (NH2CH2COOH)3.H2BeF4 312.221 2396-72-7 monoclinic[35][36]
ethylene diamine fluoroberyllate (NH2CH2CH2NH2).H2BeF4[37] d 330°
propylenediamine tetrafluoroberyllate (NH2CH2CH2CH2NH2).H2BeF4[38]
propylene-1,2-diamine tetrafluoroberyllate (NH2CH.(CH3)CH2NH2).H2BeF4[37] monoclinic a = 5.535 b = 13.560 c = 9.6048 β = 106.73 V = 690.4 Z = 4[39] 1.55
benzidine fluoroberyllate (NH2C6H4C6H4NH2).H2BeF4[37] ins
tetramethyl ammonium tetrafluoroberyllate [N(CH3)4]2BeF4[25]
tetramine silver tetrafluoroberyllate [Ag(NH3)2]2BeF4[40]

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 and 320 it is in the α' form. When temperature is raised above 320 it changes to the hexagonal α form. When cooled the α' form changes to β form at 110° and this can be cooled to 70° before changing back to the γ form.[41] It can be formed by melting sodium fluoride and beryllium fluoride.[41] The gas above molten sodium tetrafluoroberyllate contains BeF2 and NaF gas.[22]

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.[26] Li2BeF4 can be crystallised from aqueous solution using (NH4)2BeF4 and LiCl.[42]

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.[22] It can be used as a starting point to make the non-linear optic crystal KBe2BO3F2 which has the highest power handling capacity and shortest UV performance of any borate.[43] It is quite soluble in water, so beryllium can be extracted from soil this in this form.[44]

Ammonium tetrafluoroberyllate decomposes on heating by losing NH4F vapour, progressively forming NH4BeF3, then NH4Be2F5 and finally BeF2.[22]

Thallium tetrafluoroberyllate can be made by dissolving beryllium fluoride and thallium carbonate together in hydrofluoric acid and then evaporating the solution.[32]

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.[23]

Magnesium tetrafluoroberyllate can be precipitated from a hot saturated solution of ammonium tetrafluoroberyllate and a magnesium salt.[22] However, if the temperature reaches boiling point MgF2 is precipitated instead.[45]

Calcium tetrafluoroberyllate resembles zircon in the way it melts and crystallises.[22]

Strontium tetrafluoroberyllate can be made in several forms. The Ύ is produced by cooling a melt of SrF2 and Be2 and the β from is made by precipitating from a water solution. When melted and heated to 850-1145° Be2 gas evaporates leaving behind molten SrF2.[22]

The barium tetrafluoroberyllate is very insoluble and can be used for gravimetric analysis of beryllium.[22]

H2BeF4 is an acid that can be produced from Ag2BeF4 and HCl. It only exists dissolved in water.[22]

Triglycine tetrafluoroberyllate (TGFB) is ferroelectric with a transition point of 70 °C.[35] The crystals can be formed by dissolving BeF2 in water, adding HF and then glycine. When the solution is cooled triglycine tetrafluoroberyllate forms. Cs2BeF4 and Tl2BeF4 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%.[46]

Double salts[edit]

Tuttons salts[edit]

The Tuttons salt (NH4)2Mn(BeF4)2.6(H2O) is made from a solution of NH4BeF3 mixed with NH4MnF3.[22] 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.[47]

Tutton's salts (also called schoenites) containing magnesium with fluoroberyllate are difficult to produce, as the solutions tend to precipitate insoluble MgF2.[48]

name formula molecular weight CAS crystal form density melting point solubility g/100ml
potassium lithium tetrafluoroberyllate KLiBeF4 131.05 P63 a=8.781 b=5.070 c=8.566[49]
rubidium lithium tetrafluoroberyllate RbLiBeF4 177.41 P6322 a=8.980 b=5.185 c=8.751[49]
caesium lithium tetrafluoroberyllate CsLiBeF4 224.852 P21/n a=9.328 b=5.356 c=8.736 γ=89°49′[49]
acid chromium fluoroberyllate tetracosihydrate H2Cr2(BeF4)4.24H2O[47] 878.40
ammonium chromium fluoroberyllate tetracosihydrate (NH4)2Cr2(BeF4)4.24H2O[47] 912.46
rubidium chromium fluoroberyllate tetracosihydrate Rb2Cr2(BeF4)4.24H2O[47] 1047.32
manganese ammonium fluoroberyllate hydrate (NH4)2Mn(BeF4)2.6H2O[48] 369.118 1.758[50]
Rb2Fe(BeF4)2.6H2O[48] 504.884
ferrous ammonium fluoroberyllate hydrate (NH4)2Fe(BeF4)2.6H2O[48] 370.025[50]
nickel potassium fluoroberyllate hydrate K2Ni(BeF4)2.6H2O[48] 414.913[50]
nickel rubidium fluoroberyllate hydrate Rb2Ni(BeF4)2.6H2O[48] 507.732
Cs2Ni(BeF4)2.6H2O[48] 602.608
nickel ammonium fluoroberyllate hydrate (NH4)2Ni(BeF4)2.6H2O[48] 372.874 P21/a a=9.201 b=12.482 c=6.142 β=106.57 V=676.0 Z=2[51] 1.843[50]
cobalt potassium fluoroberyllate hydrate K2Co(BeF4)2.6H2O[48] 415.233[50]
cobalt rubidium fluoroberyllate hydrate Rb2Co(BeF4)2.6H2O[48] 507.972
cobalt ammonium fluoroberyllate hydrate (NH4)2Co(BeF4)2.6H2O[48] 372.874 1.821[50]
copper rubidium fluoroberyllate hydrate Rb2Cu(BeF4)2.6H2O[48] 512.585
copper ammonium fluoroberyllate hydrate (NH4)2Cu(BeF4)2.6H2O[48] 377.726 1.858[50]
zinc rubidium fluoroberyllate hydrate Rb2Zn(BeF4)2.6H2O[48] 514.42
zinc ammonium fluoroberyllate hydrate (NH4)2Zn(BeF4)2.6H2O[48] 379.56 1.859[50]
cadmium rubidium fluoroberyllate hydrate Rb2Cd(BeF4)2.6H2O[48] 561.45
cadmium ammonium fluoroberyllate hydrate (NH4)2Cd(BeF4)2.6H2O[48] 426.591


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.[52] The unit cell dimensions are slightly smaller (0.03 to 0.05 Å) than the corresponding sulfate alums.[52]

name formula molecular weight CAS crystal form density melting point solubility g/100ml
ammonium aluminium tetrafluoroberyllate alum NH4AlBeF4•12H2O [52]
potassium aluminium tetrafluoroberyllate alum KAlBeF4•12H2O [52]
potassium chromium tetrafluoroberyllate alum KCrBeF4•12H2O [52]
ammonium chromium tetrafluoroberyllate alum NH4CrBeF4•12H2O cubic a=12.218 Å 4 formulas per cell[52]
rubidium chromium tetrafluoroberyllate alum RbCrBeF4•12H2O 12.214 Å[52]
caesium chromium tetrafluoroberyllate alum CsCrBeF4•12H2O 12.323 Å[52]
thallium chromium tetrafluoroberyllate alum TlCrBeF4•12H2O 12.195 Å[52]
rubidium iron tetrafluoroberyllate alum RbFeBeF4•12H2O [52]
caesium iron tetrafluoroberyllate alum CsFeBeF4•12H2O [52]
monomethyl chromium tetrafluoroberyllate alum CH3NH3CrBeF4•12H2O 12.496 Å[53]
guanidium chromium tetrafluoroberyllate alum C(NH2)3CrBeF4•12H2O 12.538 Å[53] on heating forms a rhombohedral hexahydrate stable from 30° to 90 °C


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  8. ^ "Tetrafluoroberyllate(2-) | BeF4 | ChemSpider". www.chemspider.com. p. Data Sources. Retrieved 30 January 2019. 30497
  9. ^ "tetrafluoroberyllate(2-) (CHEBI:30497)". www.ebi.ac.uk. 26 January 2009. Retrieved 30 January 2019. ChEBI ID CHEBI:30497
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