Tetrafluoroberyllate
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
  • InChI=1S/Be.4FH/h;4*1H/q+2;;;;/p-4
    Key: UUMYFIKVCFICLB-UHFFFAOYSA-J
  • InChI=1S/Be.4FH/h;4*1H/q+2;;;;/p-4
    Key: UUMYFIKVCFICLB-UHFFFAOYSA-J
  • [8]: [Be-2](F)(F)(F)F
  • [9]: F[Be--](F)(F)F
Properties
[BeF4]2−
Molar mass 85.0057958 g·mol−1
Structure
Td
tetrahedral
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Tetrafluoroberyllate or orthofluoroberyllate is an anion with the chemical formula [BeF4]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 BeF2, where beryllium is sp hybridized.[11] 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.[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. K2[MgF4] (potassium tetrafluoromagnesate) or [NH4]2[ZnF4] (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 Li2[BeF4] 98.89 2.167[14] 472 °C[15] slight (1.25 at 20 °C, 5.78 at 40 °C)[16]
sodium tetrafluoroberyllate Na2BeF4 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 K2BeF4 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 K2BeF4·2H2O 199.233
ammonium tetrafluoroberyllate (NH4)2BeF4 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 Rb2BeF4 255.941 orthorhombic a = 5.87 Å, b = 7.649 Å, c = 10.184 Å[19] 3.72[19]
caesium tetrafluoroberyllate Cs2BeF4 350.8167 orthorhomic a = 8.03 Å, b = 10.81 Å, c = 0.622 Å 4.32
thallium tetrafluoroberyllate Tl2BeF4 493.7724 orthorhombic a = 7.7238 Å, b = 5.9022 Å, c = 10.4499 Å[22] 6.884[22]
silver tetrafluoroberyllate Ag2BeF4 300.7422
magnesium tetrafluoroberyllate MgBeF4 109.3108
calcium tetrafluoroberyllate CaBeF4 125.08 2.959[23]
strontium tetrafluoroberyllate SrBeF4 172.6 orthorhombic a = 5.291 Å, b = 6.787 Å, c = 8.307 Å 3.84 insoluble
barium tetrafluoroberyllate BaBeF4 222.333 4.17[14] insoluble
radium tetrafluoroberyllate RaBeF4[24] 311.005795 insoluble
hexaqua ferrous tetrafluoroberyllate FeBeF4·6H2O[25]
heptaqua ferrous tetrafluoroberyllate FeBeF4·7H2O[23] 1.894
heptaqua nickel tetrafluoroberyllate NiBeF4·7H2O[23]
hexaqua nickel tetrafluoroberyllate NiBeF4·6H2O[23]
heptaqua cobalt tetrafluoroberyllate CoBeF4·7H2O[23] 1.867
hexaqua cobalt tetrafluoroberyllate CoBeF4·6H2O[23] 1.891
pentaqua copper tetrafluoroberyllate CuBeF4·5H2O[23]
heptaqua zinc tetrafluoroberyllate ZnBeFe4·7H2O[23]
lead tetrafluoroberyllate PbBeF4 292.2 6.135[14]
hydrazinium tetrafluoroberyllate N2H6BeF4 119.0668 a = 5.58 Å, b = 7.337 Å, c = 9.928 Å, α = 90°, β = 98.22°, γ = 90°[19]
triglycine tetrafluoroberyllate (NH2CH2COOH)3·H2BeF4 312.221 2396-72-7 monoclinic[26][27]
ethylene diamine fluoroberyllate (NH2CH2CH2NH2)·H2BeF4[28] decomposes 330 °C
propylenediamine tetrafluoroberyllate (NH2CH2CH2CH2NH2)·H2BeF4[29]
propylene-1,2-diamine tetrafluoroberyllate (NH2CH(CH3)CH2NH2)·H2BeF4[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 (NH2C6H4C6H4NH2)·H2BeF4[28] ins
tetramethyl ammonium tetrafluoroberyllate [N(CH3)4]2BeF4[14]
tetramine silver tetrafluoroberyllate [Ag(NH3)2]2BeF4[31]
[Cu(NH3)2]2BeF4[31]
[Cu(NH3)4]2BeF4·H2O[31]
[Zn(NH3)4]2BeF4[31]
[Cd(NH3)4]2BeF4[31]
[Ni(NH3)6]2BeF4[31]
[Ni(NH3)4]2BeF4·2H2O[31]
[Ni(NH3)2]2BeF4[31]
[Co(NH3)6]2BeF4·3H2O[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 BeF2 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] Li2BeF4 can be crystallised from aqueous solution using (NH4)2BeF4 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 KBe2BO3F2 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 NH4F vapour, progressively forming NH4BeF3, then NH4Be2F5 and finally BeF2.[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 MgF2 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 SrF2 and Be2 and the β form is made by precipitating from a water solution. When melted and heated to 850–1145 °C, Be2 gas evaporates leaving behind molten SrF2.[11]

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

H2BeF4 is an acid that can be produced from Ag2BeF4 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 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%.[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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