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Tetrafluoroberyllate
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<h2 id="properties">Properties</h2> <p>The Be–F <a href="/facts/Bond_length/rHHIBH6q">bond length</a> is between 145 and 153 <a href="/facts/Picometre/Cb54mVBX">pm</a>. The beryllium is <a href="/facts/Orbital_hybridisation/Fl7sz8Jm">sp3 hybridized</a>, leading to a longer bond than in <a href="/facts/BeF2/4wkNdddq">BeF2</a>, where beryllium is <a href="/facts/Orbital_hybridisation/Fl7sz8Jm">sp hybridized</a>.<a class="footnote-ref" id="fnref:1" href="#fn:1"><sup>1</sup></a> 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.<a class="footnote-ref" id="fnref:2" href="#fn:2"><sup>2</sup></a> </p><p>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 <a href="/facts/Isotropic/mc3QEY2x">isotropic</a> (not limited to rotation on one axis) with a potential barrier of 14.5 kcal/mol (61 kJ/mol).<a class="footnote-ref" id="fnref:3" href="#fn:3"><sup>3</sup></a> </p><p>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.<a class="footnote-ref" id="fnref:4" href="#fn:4"><sup>4</sup></a> </p><p>Tetrafluoroberyllate has a biological effect by inhibiting <a href="/facts/F-ATPase/gw2r7PUE">F-ATPase</a> <a href="/facts/Adenosine_triphosphate/nB9bwgcU">adenosine triphosphate</a> producing enzymes in <a href="/facts/Mitochondria/ErHqrdJ1">mitochondria</a> and <a href="/facts/Bacteria/wC8xSCsU">bacteria</a>. It does this by attempting to react with <a href="/facts/Adenosine_diphosphate/JEDnsCjn">adenosine diphosphate</a> because it resembles <a href="/facts/Phosphate/FDGVCxUG">phosphate</a>. However once it does this it remains stuck in the <a href="/facts/F-ATPase/gw2r7PUE">F1</a> part of the enzyme and inhibits it from further function.<a class="footnote-ref" id="fnref:5" href="#fn:5"><sup>5</sup></a> </p> <h2 id="simple-salts">Simple salts</h2> <table><tbody><tr><th>Name</th><th><a href="/facts/Chemical_formula/hghUtthl">Chemical formula</a></th><th><a href="/facts/Molar_mass/m2laJErl">Molar mass</a> (g/mol)</th><th><a href="/facts/CAS_number/zjXjCGPx">CAS number</a></th><th><a href="/facts/Crystal_system/dMQLk1q4">Crystal system</a></th><th><a href="/facts/Density/92p6hh9I">Density</a> (g/cm3)</th><th><a href="/facts/Melting_point/MY0w0h0k">Melting point</a> (°C)</th><th><a href="/facts/Solubility/kLE9h3Jb">Solubility</a> in water(g/(100 ml))</th></tr><tr><td>lithium tetrafluoroberyllate</td><td>Li2[BeF4]</td><td>98.89</td><td></td><td></td><td>2.167<a class="footnote-ref" id="fnref:6" href="#fn:6"><sup>6</sup></a></td><td>472 °C<a class="footnote-ref" id="fnref:7" href="#fn:7"><sup>7</sup></a></td><td>slight (1.25 at 20 °C, 5.78 at 40 °C)<a class="footnote-ref" id="fnref:8" href="#fn:8"><sup>8</sup></a></td></tr><tr><td>sodium tetrafluoroberyllate</td><td>Na2BeF4</td><td>130.985333</td><td>13871-27-7</td><td>Orthorhombic<a class="footnote-ref" id="fnref:9" href="#fn:9"><sup>9</sup></a></td><td>2.47</td><td>575 °C</td><td>slight (1.33 at 0 °C, 1.44 at 20 °C, 2.73 at 90 °C)<a class="footnote-ref" id="fnref:10" href="#fn:10"><sup>10</sup></a></td></tr><tr><td>potassium tetrafluoroberyllate</td><td>K2BeF4</td><td>163.20</td><td>7787-50-0</td><td>orthorhombic <i>a</i> = 5.691 Å, <i>b</i> = 7.278 Å, <i>c</i> = 9.896 Å<a class="footnote-ref" id="fnref:11" href="#fn:11"><sup>11</sup></a> as for strontium orthosilicate<a class="footnote-ref" id="fnref:12" href="#fn:12"><sup>12</sup></a></td><td>2.64<a class="footnote-ref" id="fnref:13" href="#fn:13"><sup>13</sup></a></td><td></td><td></td></tr><tr><td>potassium tetrafluoroberyllate dihydrate</td><td>K2BeF4·2H2O</td><td>199.233</td><td></td><td></td><td></td><td></td></tr><tr><td>ammonium tetrafluoroberyllate</td><td>(NH4)2BeF4</td><td>121.0827</td><td>14874-86-3</td><td>orthorhombic a = 5.91 Å, b = 7.64 Å, c = 10.43 Å</td><td>1.71</td><td>decomposes 280 °C<a class="footnote-ref" id="fnref:14" href="#fn:14"><sup>14</sup></a></td><td>32.3 at 25 °C<a class="footnote-ref" id="fnref:15" href="#fn:15"><sup>15</sup></a></td></tr><tr><td>rubidium tetrafluoroberyllate</td><td>Rb2BeF4</td><td>255.941</td><td></td><td>orthorhombic <i>a</i> = 5.87 Å, <i>b</i> = 7.649 Å, <i>c</i> = 10.184 Å<a class="footnote-ref" id="fnref:16" href="#fn:16"><sup>16</sup></a></td><td>3.72<a class="footnote-ref" id="fnref:17" href="#fn:17"><sup>17</sup></a></td><td></td><td></td></tr><tr><td>caesium tetrafluoroberyllate</td><td>Cs2BeF4</td><td>350.8167</td><td></td><td>orthorhomic <i>a</i> = 8.03 Å, <i>b</i> = 10.81 Å, <i>c</i> = 0.622 Å</td><td>4.32</td><td></td><td></td></tr><tr><td>thallium tetrafluoroberyllate</td><td>Tl2BeF4</td><td>493.7724</td><td></td><td>orthorhombic <i>a</i> = 7.7238 Å, <i>b</i> = 5.9022 Å, <i>c</i> = 10.4499 Å<a class="footnote-ref" id="fnref:18" href="#fn:18"><sup>18</sup></a></td><td>6.884<a class="footnote-ref" id="fnref:19" href="#fn:19"><sup>19</sup></a></td><td></td><td></td></tr><tr><td>silver tetrafluoroberyllate</td><td>Ag2BeF4</td><td>300.7422</td><td></td><td></td><td></td><td></td><td></td></tr><tr><td>magnesium tetrafluoroberyllate</td><td>MgBeF4</td><td>109.3108</td><td></td><td></td><td></td><td></td><td></td></tr><tr><td>calcium tetrafluoroberyllate</td><td>CaBeF4</td><td>125.08</td><td></td><td></td><td>2.959<a class="footnote-ref" id="fnref:20" href="#fn:20"><sup>20</sup></a></td><td></td><td></td></tr><tr><td>strontium tetrafluoroberyllate</td><td>SrBeF4</td><td>172.6</td><td></td><td>orthorhombic <i>a</i> = 5.291 Å, <i>b</i> = 6.787 Å, <i>c</i> = 8.307 Å</td><td>3.84</td><td></td><td>insoluble</td></tr><tr><td>barium tetrafluoroberyllate</td><td>BaBeF4</td><td>222.333</td><td></td><td></td><td>4.17<a class="footnote-ref" id="fnref:21" href="#fn:21"><sup>21</sup></a></td><td></td><td>insoluble</td></tr><tr><td>radium tetrafluoroberyllate</td><td>RaBeF4<a class="footnote-ref" id="fnref:22" href="#fn:22"><sup>22</sup></a></td><td>311.005795</td><td></td><td></td><td></td><td></td><td>insoluble</td></tr><tr><td>hexaqua ferrous tetrafluoroberyllate</td><td>FeBeF4·6H2O<a class="footnote-ref" id="fnref:23" href="#fn:23"><sup>23</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td>heptaqua ferrous tetrafluoroberyllate</td><td>FeBeF4·7H2O<a class="footnote-ref" id="fnref:24" href="#fn:24"><sup>24</sup></a></td><td></td><td></td><td></td><td>1.894</td><td></td><td></td></tr><tr><td>heptaqua nickel tetrafluoroberyllate</td><td>NiBeF4·7H2O<a class="footnote-ref" id="fnref:25" href="#fn:25"><sup>25</sup></a></td><td></td><td></td><td></td><td></td></tr><tr><td>hexaqua nickel tetrafluoroberyllate</td><td>NiBeF4·6H2O<a class="footnote-ref" id="fnref:26" href="#fn:26"><sup>26</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td>heptaqua cobalt tetrafluoroberyllate</td><td>CoBeF4·7H2O<a class="footnote-ref" id="fnref:27" href="#fn:27"><sup>27</sup></a></td><td></td><td></td><td></td><td>1.867</td><td></td><td></td></tr><tr><td>hexaqua cobalt tetrafluoroberyllate</td><td>CoBeF4·6H2O<a class="footnote-ref" id="fnref:28" href="#fn:28"><sup>28</sup></a></td><td></td><td></td><td></td><td>1.891</td><td></td><td></td></tr><tr><td>pentaqua copper tetrafluoroberyllate</td><td>CuBeF4·5H2O<a class="footnote-ref" id="fnref:29" href="#fn:29"><sup>29</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td>heptaqua zinc tetrafluoroberyllate</td><td>ZnBeFe4·7H2O<a class="footnote-ref" id="fnref:30" href="#fn:30"><sup>30</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td>lead tetrafluoroberyllate</td><td>PbBeF4</td><td>292.2</td><td></td><td></td><td>6.135<a class="footnote-ref" id="fnref:31" href="#fn:31"><sup>31</sup></a></td><td></td><td></td></tr><tr><td>hydrazinium tetrafluoroberyllate</td><td>N2H6BeF4</td><td>119.0668</td><td></td><td><i>a</i> = 5.58 Å, <i>b</i> = 7.337 Å, <i>c</i> = 9.928 Å, <i>α</i> = 90°, <i>β</i> = 98.22°, <i>γ</i> = 90°<a class="footnote-ref" id="fnref:32" href="#fn:32"><sup>32</sup></a></td><td></td><td></td><td></td></tr><tr><td>triglycine tetrafluoroberyllate</td><td>(NH2CH2COOH)3·H2BeF4</td><td>312.221</td><td>2396-72-7</td><td>monoclinic<a class="footnote-ref" id="fnref:33" href="#fn:33"><sup>33</sup></a><a class="footnote-ref" id="fnref:34" href="#fn:34"><sup>34</sup></a></td><td></td><td></td><td></td></tr><tr><td>ethylene diamine fluoroberyllate</td><td>(NH2CH2CH2NH2)·H2BeF4<a class="footnote-ref" id="fnref:35" href="#fn:35"><sup>35</sup></a></td><td></td><td></td><td></td><td></td><td>decomposes 330 °C</td><td></td></tr><tr><td>propylenediamine tetrafluoroberyllate</td><td>(NH2CH2CH2CH2NH2)·H2BeF4<a class="footnote-ref" id="fnref:36" href="#fn:36"><sup>36</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td>propylene-1,2-diamine tetrafluoroberyllate</td><td>(NH2CH(CH3)CH2NH2)·H2BeF4<a class="footnote-ref" id="fnref:37" href="#fn:37"><sup>37</sup></a></td><td></td><td></td><td>monoclinic <i>a</i> = 5.535 Å, <i>b</i> = 13.560 Å, <i>c</i> = 9.6048 Å, <i>β</i> = 106.73 Å, <i>V</i> = 690.4 Å3, <i>Z</i> = 4<a class="footnote-ref" id="fnref:38" href="#fn:38"><sup>38</sup></a></td><td>1.55</td><td></td><td></td></tr><tr><td>benzidine fluoroberyllate</td><td>(NH2C6H4C6H4NH2)·H2BeF4<a class="footnote-ref" id="fnref:39" href="#fn:39"><sup>39</sup></a></td><td></td><td></td><td></td><td></td><td></td><td>ins</td></tr><tr><td>tetramethyl ammonium tetrafluoroberyllate</td><td>[N(CH3)4]2BeF4<a class="footnote-ref" id="fnref:40" href="#fn:40"><sup>40</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td>tetramine silver tetrafluoroberyllate</td><td>[Ag(NH3)2]2BeF4<a class="footnote-ref" id="fnref:41" href="#fn:41"><sup>41</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td></td><td>[Cu(NH3)2]2BeF4<a class="footnote-ref" id="fnref:42" href="#fn:42"><sup>42</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td></td><td>[Cu(NH3)4]2BeF4·H2O<a class="footnote-ref" id="fnref:43" href="#fn:43"><sup>43</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td></td><td>[Zn(NH3)4]2BeF4<a class="footnote-ref" id="fnref:44" href="#fn:44"><sup>44</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td></td><td>[Cd(NH3)4]2BeF4<a class="footnote-ref" id="fnref:45" href="#fn:45"><sup>45</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td></td><td>[Ni(NH3)6]2BeF4<a class="footnote-ref" id="fnref:46" href="#fn:46"><sup>46</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td></td><td>[Ni(NH3)4]2BeF4·2H2O<a class="footnote-ref" id="fnref:47" href="#fn:47"><sup>47</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td></td><td>[Ni(NH3)2]2BeF4<a class="footnote-ref" id="fnref:48" href="#fn:48"><sup>48</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr><tr><td></td><td>[Co(NH3)6]2BeF4·3H2O<a class="footnote-ref" id="fnref:49" href="#fn:49"><sup>49</sup></a></td><td></td><td></td><td></td><td></td><td></td><td></td></tr></tbody></table> <p>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.<a class="footnote-ref" id="fnref:50" href="#fn:50"><sup>50</sup></a> It can be formed by melting <a href="/facts/Sodium_fluoride/HHcvwK7s">sodium fluoride</a> and <a href="/facts/Beryllium_fluoride/4wkNdddq">beryllium fluoride</a>.<a class="footnote-ref" id="fnref:51" href="#fn:51"><sup>51</sup></a> The gas above molten sodium tetrafluoroberyllate contains BeF2 and NaF gas.<a class="footnote-ref" id="fnref:52" href="#fn:52"><sup>52</sup></a> </p><p>Lithium tetrafluoroberyllate takes on the same crystal form as the mineral <a href="/facts/Phenacite/f7w8BeD5">phenacite</a>. As a liquid it is proposed for the <a href="/facts/Molten_salt_reactor/aSvp1qTG">molten salt reactor</a>, in which it is called <a href="/facts/FLiBe/z8wD05ur">FLiBe</a>. 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.<a class="footnote-ref" id="fnref:53" href="#fn:53"><sup>53</sup></a> Li2BeF4 can be crystallised from aqueous solution using (NH4)2BeF4 and LiCl.<a class="footnote-ref" id="fnref:54" href="#fn:54"><sup>54</sup></a> </p><p>Potassium tetrafluoroberyllate has the same structure as anhydrous <a href="/facts/Potassium_sulfate/amB6UMaI">potassium sulfate</a>, as does rubidium and caesium tetrafluoroberyllate. Potassium tetrafluoroberyllate can make solid solutions with potassium sulfate.<a class="footnote-ref" id="fnref:55" href="#fn:55"><sup>55</sup></a> 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.<a class="footnote-ref" id="fnref:56" href="#fn:56"><sup>56</sup></a> It is quite soluble in water, so beryllium can be extracted from soil in this form.<a class="footnote-ref" id="fnref:57" href="#fn:57"><sup>57</sup></a> </p><p>Ammonium tetrafluoroberyllate decomposes on heating by losing NH4F vapour, progressively forming NH4BeF3, then NH4Be2F5 and finally BeF2.<a class="footnote-ref" id="fnref:58" href="#fn:58"><sup>58</sup></a> </p><p>Thallium tetrafluoroberyllate can be made by dissolving <a href="/facts/Beryllium_fluoride/4wkNdddq">beryllium fluoride</a> and <a href="/facts/Thallium_carbonate/EETHpomH">thallium carbonate</a> together in <a href="/facts/Hydrofluoric_acid/wdXqu4bE">hydrofluoric acid</a> and then evaporating the solution.<a class="footnote-ref" id="fnref:59" href="#fn:59"><sup>59</sup></a> </p><p>Radium tetrafluoroberyllate is used as a standard neutron source. The <a href="/facts/Alpha_particle/dzNMs9WP">alpha particles</a> from the <a href="/facts/Radium/VWo5gkzn">radium</a> cause <a href="/facts/Neutron/oRCM1geb">neutrons</a> to be emitted from the beryllium. It is precipitated from a <a href="/facts/Radium_chloride/MaChrTh6">radium chloride</a> solution mixed with potassium tetrafluoroberyllate.<a class="footnote-ref" id="fnref:60" href="#fn:60"><sup>60</sup></a> </p><p>Magnesium tetrafluoroberyllate can be precipitated from a hot saturated solution of ammonium tetrafluoroberyllate and a magnesium salt.<a class="footnote-ref" id="fnref:61" href="#fn:61"><sup>61</sup></a> However, if the temperature reaches boiling point MgF2 is precipitated instead.<a class="footnote-ref" id="fnref:62" href="#fn:62"><sup>62</sup></a> </p><p>Calcium tetrafluoroberyllate resembles <a href="/facts/Zircon/84APfbLt">zircon</a> in the way it melts and crystallises.<a class="footnote-ref" id="fnref:63" href="#fn:63"><sup>63</sup></a> </p><p>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.<a class="footnote-ref" id="fnref:64" href="#fn:64"><sup>64</sup></a> </p><p>The barium tetrafluoroberyllate is very insoluble and can be used for <a href="/facts/Gravimetric_analysis/FtMjzQly">gravimetric analysis</a> of beryllium.<a class="footnote-ref" id="fnref:65" href="#fn:65"><sup>65</sup></a> </p><p>H2BeF4 is an acid that can be produced from Ag2BeF4 and <a href="/facts/HCl/7Wzkhomd">HCl</a>. It only exists in aqueous solution.<a class="footnote-ref" id="fnref:66" href="#fn:66"><sup>66</sup></a> </p><p>Triglycine tetrafluoroberyllate (TGFB) is <a href="/facts/Ferroelectric/DLVYFNQT">ferroelectric</a> with a transition point of 70 °C.<a class="footnote-ref" id="fnref:67" href="#fn:67"><sup>67</sup></a> 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%.<a class="footnote-ref" id="fnref:68" href="#fn:68"><sup>68</sup></a> </p> <h2 id="double-salts">Double salts</h2> <h3>Tuttons salts</h3> <p>The Tuttons salt (NH4)2Mn(BeF4)2·6(H2O) is made from a solution of NH4BeF3 mixed with NH4MnF3.<a class="footnote-ref" id="fnref:69" href="#fn:69"><sup>69</sup></a> 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.<a class="footnote-ref" id="fnref:70" href="#fn:70"><sup>70</sup></a> </p><p>Tutton's salts (also called schoenites) containing magnesium with <a href="/facts/Fluoroberyllate/vBDSyz9X">fluoroberyllate</a> are difficult to produce, as the solutions tend to precipitate insoluble <a href="/facts/Magnesium_fluoride/nGsPQuRz">MgF2</a>.<a class="footnote-ref" id="fnref:71" href="#fn:71"><sup>71</sup></a> </p> <table><tbody><tr><th>name</th><th>formula</th><th>molecular weight</th><th>CAS</th><th>crystal form</th><th>density</th><th>melting point</th><th>solubility g/100ml</th></tr><tr><td>potassium lithium tetrafluoroberyllate</td><td>KLiBeF4</td><td>131.05</td><td></td><td><i>P</i>63, <i>a</i> = 8.781 Å, <i>b</i> = 5.070 Å <i>c</i> = 8.566 Å<a class="footnote-ref" id="fnref:72" href="#fn:72"><sup>72</sup></a></td><td></td><td></td></tr><tr><td>rubidium lithium tetrafluoroberyllate</td><td>RbLiBeF4</td><td>177.41</td><td></td><td><i>P</i>6322, <i>a</i> = 8.980 Å, <i>b</i> = 5.185 Å<i> </i>c<i> = 8.751 Å<a class="footnote-ref" id="fnref:73" href="#fn:73"><sup>73</sup></a></i></td><td></td><td></td></tr><tr><td>caesium lithium tetrafluoroberyllate</td><td>CsLiBeF4</td><td>224.852</td><td></td><td><i>P</i>21/n, <i>a</i> = 9.328 Å <i>b</i> = 5.356 Å, <i>c</i> = 8.736 Å, <i>γ</i> = 89.82°<a class="footnote-ref" id="fnref:74" href="#fn:74"><sup>74</sup></a></td><td></td><td></td></tr><tr><td>acid chromium fluoroberyllate tetracosihydrate</td><td>H2Cr2(BeF4)4·24H2O<a class="footnote-ref" id="fnref:75" href="#fn:75"><sup>75</sup></a></td><td>878.40</td></tr><tr><td>ammonium chromium fluoroberyllate tetracosihydrate</td><td>(NH4)2Cr2(BeF4)4·24H2O<a class="footnote-ref" id="fnref:76" href="#fn:76"><sup>76</sup></a></td><td>912.46</td></tr><tr><td>rubidium chromium fluoroberyllate tetracosihydrate</td><td>Rb2Cr2(BeF4)4·24H2O<a class="footnote-ref" id="fnref:77" href="#fn:77"><sup>77</sup></a></td><td>1047.32</td></tr><tr><td>manganese ammonium fluoroberyllate hydrate</td><td>(NH4)2Mn(BeF4)2·6H2O<a class="footnote-ref" id="fnref:78" href="#fn:78"><sup>78</sup></a></td><td>369.118</td><td></td><td></td><td>1.758<a class="footnote-ref" id="fnref:79" href="#fn:79"><sup>79</sup></a></td></tr><tr><td></td><td>Rb2Fe(BeF4)2·6H2O<a class="footnote-ref" id="fnref:80" href="#fn:80"><sup>80</sup></a></td><td>504.884</td></tr><tr><td>ferrous ammonium fluoroberyllate hydrate</td><td>(NH4)2Fe(BeF4)2·6H2O<a class="footnote-ref" id="fnref:81" href="#fn:81"><sup>81</sup></a></td><td>370.025<a class="footnote-ref" id="fnref:82" href="#fn:82"><sup>82</sup></a></td></tr><tr><td>nickel potassium fluoroberyllate hydrate</td><td>K2Ni(BeF4)2·6H2O<a class="footnote-ref" id="fnref:83" href="#fn:83"><sup>83</sup></a></td><td>414.913<a class="footnote-ref" id="fnref:84" href="#fn:84"><sup>84</sup></a></td></tr><tr><td>nickel rubidium fluoroberyllate hydrate</td><td>Rb2Ni(BeF4)2·6H2O<a class="footnote-ref" id="fnref:85" href="#fn:85"><sup>85</sup></a></td><td>507.732</td></tr><tr><td></td><td>Cs2Ni(BeF4)2·6H2O<a class="footnote-ref" id="fnref:86" href="#fn:86"><sup>86</sup></a></td><td>602.608</td></tr><tr><td>nickel ammonium fluoroberyllate hydrate</td><td>(NH4)2Ni(BeF4)2·6H2O<a class="footnote-ref" id="fnref:87" href="#fn:87"><sup>87</sup></a></td><td>372.874</td><td></td><td><i>P</i>21/a, <i>a</i> = 9.201 Å, <i>b</i> = 12.482 Å, <i>c</i> = 6.142 Å, <i>β</i> = 106.57 Å, <i>V</i> = 676.0 Å3 <i>Z</i> = 2<a class="footnote-ref" id="fnref:88" href="#fn:88"><sup>88</sup></a></td><td>1.843<a class="footnote-ref" id="fnref:89" href="#fn:89"><sup>89</sup></a></td></tr><tr><td>cobalt potassium fluoroberyllate hydrate</td><td>K2Co(BeF4)2·6H2O<a class="footnote-ref" id="fnref:90" href="#fn:90"><sup>90</sup></a></td><td>415.233<a class="footnote-ref" id="fnref:91" href="#fn:91"><sup>91</sup></a></td></tr><tr><td>cobalt rubidium fluoroberyllate hydrate</td><td>Rb2Co(BeF4)2·6H2O<a class="footnote-ref" id="fnref:92" href="#fn:92"><sup>92</sup></a></td><td>507.972</td></tr><tr><td>cobalt ammonium fluoroberyllate hydrate</td><td>(NH4)2Co(BeF4)2·6H2O<a class="footnote-ref" id="fnref:93" href="#fn:93"><sup>93</sup></a></td><td>372.874</td><td></td><td></td><td>1.821<a class="footnote-ref" id="fnref:94" href="#fn:94"><sup>94</sup></a></td></tr><tr><td>copper rubidium fluoroberyllate hydrate</td><td>Rb2Cu(BeF4)2·6H2O<a class="footnote-ref" id="fnref:95" href="#fn:95"><sup>95</sup></a></td><td>512.585</td></tr><tr><td>copper ammonium fluoroberyllate hydrate</td><td>(NH4)2Cu(BeF4)2·6H2O<a class="footnote-ref" id="fnref:96" href="#fn:96"><sup>96</sup></a></td><td>377.726</td><td></td><td></td><td>1.858<a class="footnote-ref" id="fnref:97" href="#fn:97"><sup>97</sup></a></td></tr><tr><td>zinc rubidium fluoroberyllate hydrate</td><td>Rb2Zn(BeF4)2·6H2O<a class="footnote-ref" id="fnref:98" href="#fn:98"><sup>98</sup></a></td><td>514.42</td></tr><tr><td>zinc ammonium fluoroberyllate hydrate</td><td>(NH4)2Zn(BeF4)2·6H2O<a class="footnote-ref" id="fnref:99" href="#fn:99"><sup>99</sup></a></td><td>379.56</td><td></td><td></td><td>1.859<a class="footnote-ref" id="fnref:100" href="#fn:100"><sup>100</sup></a></td></tr><tr><td>cadmium rubidium fluoroberyllate hydrate</td><td>Rb2Cd(BeF4)2·6H2O<a class="footnote-ref" id="fnref:101" href="#fn:101"><sup>101</sup></a></td><td>561.45</td></tr><tr><td>cadmium ammonium fluoroberyllate hydrate</td><td>(NH4)2Cd(BeF4)2·6H2O<a class="footnote-ref" id="fnref:102" href="#fn:102"><sup>102</sup></a></td><td>426.591</td></tr></tbody></table> <h3>Alums</h3> <p>Tetrafluoroberyllate salts equivalent to <a href="/facts/Alums/ULAn0XRB">alums</a> 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.<a class="footnote-ref" id="fnref:103" href="#fn:103"><sup>103</sup></a> The unit cell dimensions are slightly smaller (by 0.03–0.05 Å) than the corresponding sulfate alums.<a class="footnote-ref" id="fnref:104" href="#fn:104"><sup>104</sup></a> </p> <table><tbody><tr><th>name</th><th>formula</th><th>molecular weight</th><th>CAS</th><th>crystal form</th><th>density</th><th>melting point</th><th>solubility g/100ml</th></tr><tr><td>ammonium aluminium tetrafluoroberyllate alum</td><td>NH4AlBeF4·12H2O</td><td></td><td></td><td><a class="footnote-ref" id="fnref:105" href="#fn:105"><sup>105</sup></a></td><td></td><td></td></tr><tr><td>potassium aluminium tetrafluoroberyllate alum</td><td>KAlBeF4·12H2O</td><td></td><td></td><td><a class="footnote-ref" id="fnref:106" href="#fn:106"><sup>106</sup></a></td><td></td><td></td></tr><tr><td>potassium chromium tetrafluoroberyllate alum</td><td>KCrBeF4·12H2O</td><td></td><td></td><td><a class="footnote-ref" id="fnref:107" href="#fn:107"><sup>107</sup></a></td><td></td><td></td></tr><tr><td>ammonium chromium tetrafluoroberyllate alum</td><td>NH4CrBeF4·12H2O</td><td></td><td></td><td>cubic <i>a</i> = 12.218 Å, <i>Z</i> = 4<a class="footnote-ref" id="fnref:108" href="#fn:108"><sup>108</sup></a></td><td></td><td></td></tr><tr><td>rubidium chromium tetrafluoroberyllate alum</td><td>RbCrBeF4·12H2O</td><td></td><td></td><td>12.214 Å<a class="footnote-ref" id="fnref:109" href="#fn:109"><sup>109</sup></a></td><td></td><td></td></tr><tr><td>caesium chromium tetrafluoroberyllate alum</td><td>CsCrBeF4·12H2O</td><td></td><td></td><td>12.323 Å<a class="footnote-ref" id="fnref:110" href="#fn:110"><sup>110</sup></a></td><td></td><td></td></tr><tr><td>thallium chromium tetrafluoroberyllate alum</td><td>TlCrBeF4·12H2O</td><td></td><td></td><td>12.195 Å<a class="footnote-ref" id="fnref:111" href="#fn:111"><sup>111</sup></a></td><td></td><td></td></tr><tr><td>rubidium iron tetrafluoroberyllate alum</td><td>RbFeBeF4·12H2O</td><td></td><td></td><td><a class="footnote-ref" id="fnref:112" href="#fn:112"><sup>112</sup></a></td><td></td><td></td></tr><tr><td>caesium iron tetrafluoroberyllate alum</td><td>CsFeBeF4·12H2O</td><td></td><td></td><td><a class="footnote-ref" id="fnref:113" href="#fn:113"><sup>113</sup></a></td><td></td><td></td></tr><tr><td>monomethyl chromium tetrafluoroberyllate alum</td><td>CH3NH3CrBeF4·12H2O</td><td></td><td></td><td>12.496 Å<a class="footnote-ref" id="fnref:114" href="#fn:114"><sup>114</sup></a></td><td></td><td></td></tr><tr><td>guanidium chromium tetrafluoroberyllate alum</td><td>C(NH2)3CrBeF4·12H2O</td><td></td><td></td><td>12.538 Å<a class="footnote-ref" id="fnref:115" href="#fn:115"><sup>115</sup></a></td><td></td><td>on heating forms a rhombohedral hexahydrate stable from 30 °C to 90 °C</td></tr></tbody></table> <h2 id="references">References</h2> <ol> <li id="fn:1"><p>Emeléus, Harry Julius; Sharpe, A. G. (1972-12-06). ADVANCES IN INORGANIC CHEMISTRY AND RADIOCHEMISTRY. Academic Press. pp. 271–275. ISBN 9780080578637. Retrieved 13 July 2013. <a href="9780080578637" target="_blank">9780080578637</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li> <li id="fn:2"><p>Simons, J.H. (1954-01-01). Fluorine Chemistry. Elsevier. p. 5. ISBN 9780323145435. Retrieved 13 July 2013. {{cite book}}: ISBN / Date incompatibility (help) <a href="9780323145435" target="_blank">9780323145435</a> <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li> <li id="fn:3"><p>Emeléus, Harry Julius; Sharpe, A. G. (1972-12-06). ADVANCES IN INORGANIC CHEMISTRY AND RADIOCHEMISTRY. Academic Press. pp. 271–275. ISBN 9780080578637. Retrieved 13 July 2013. <a href="9780080578637" target="_blank">9780080578637</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li> <li id="fn:4"><p>Simons, J.H. (1954-01-01). Fluorine Chemistry. Elsevier. p. 5. ISBN 9780323145435. 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"Powder neutron diffraction of Tl2BeF4 at six temperatures from room temperature to 1.5 K". Acta Crystallographica Section C. 61 (12): i113 – i116. Bibcode:2005AcCrC..61I.113D. doi:10.1107/S010827010503249X. ISSN 0108-2701. PMID 16330826. <a href="/wiki/Bibcode_(identifier)" target="_blank">/wiki/Bibcode_(identifier)</a> <a href="#fnref:19" class="footnote-back-ref">↩</a></p></li> <li id="fn:20"><p>Rây, Nirmalendu Nath (1932). "Fluoberyllate und ihre Analogie mit den Sulfaten. II. Fluoberyllate einiger zweiwertiger Metalle". Zeitschrift für anorganische und allgemeine Chemie (in German). 205 (3): 257–267. doi:10.1002/zaac.19322050307. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:20" class="footnote-back-ref">↩</a></p></li> <li id="fn:21"><p>Rây, Nirmalendu Nath (1931). "Fluoberyllate und ihre Analogie mit Sulfaten. I". Zeitschrift für anorganische und allgemeine Chemie. 201 (1): 289–300. doi:10.1002/zaac.19312010126. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:21" class="footnote-back-ref">↩</a></p></li> <li id="fn:22"><p>Sastri, Malladi Narasimha (1958). Radiochemical measurements on neutron sources (PDF) (Thesis). Durham University. pp. 18–20. <a href="http://etheses.dur.ac.uk/2013/1/2013_20.pdf" target="_blank">http://etheses.dur.ac.uk/2013/1/2013_20.pdf</a> <a href="#fnref:22" class="footnote-back-ref">↩</a></p></li> <li id="fn:23"><p>Kaduk, J. A. (2019). "Section 4.9.4. Chemical reasonableness". In Gilmore, C. J.; Kaduk, J. A.; Schenk, H. (eds.). International Tables for Crystallography Volume H Powder diffraction. pp. 496–508. doi:10.1107/97809553602060000964. <a href="https://onlinelibrary.wiley.com/iucr/itc/Ha/ch4o9v0001/sec4o9o4/" target="_blank">https://onlinelibrary.wiley.com/iucr/itc/Ha/ch4o9v0001/sec4o9o4/</a> <a href="#fnref:23" class="footnote-back-ref">↩</a></p></li> <li id="fn:24"><p>Rây, Nirmalendu Nath (1932). 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ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:82" class="footnote-back-ref">↩</a></p></li> <li id="fn:83"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:83" class="footnote-back-ref">↩</a></p></li> <li id="fn:84"><p>Nath Rây, Nirmalendu (1932). "Fluoberyllate und ihre Analogie mit Sulfaten. III. Doppelsalze der Fluoberyllate". Zeitschrift für anorganische und allgemeine Chemie (in German). 206 (2): 209–216. doi:10.1002/zaac.19322060209. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:84" class="footnote-back-ref">↩</a></p></li> <li id="fn:85"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:85" class="footnote-back-ref">↩</a></p></li> <li id="fn:86"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:86" class="footnote-back-ref">↩</a></p></li> <li id="fn:87"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:87" class="footnote-back-ref">↩</a></p></li> <li id="fn:88"><p>Montgomery, H. (15 September 1980). "Diammonium nickel bis(tetrafluoroberyllate)hexahydrate" (PDF). Acta Crystallographica Section B. 36 (9): 2121–2123. Bibcode:1980AcCrB..36.2121M. doi:10.1107/S0567740880008060. <a href="http://journals.iucr.org/b/issues/1980/09/00/a19083/a19083.pdf" target="_blank">http://journals.iucr.org/b/issues/1980/09/00/a19083/a19083.pdf</a> <a href="#fnref:88" class="footnote-back-ref">↩</a></p></li> <li id="fn:89"><p>Nath Rây, Nirmalendu (1932). "Fluoberyllate und ihre Analogie mit Sulfaten. III. Doppelsalze der Fluoberyllate". Zeitschrift für anorganische und allgemeine Chemie (in German). 206 (2): 209–216. doi:10.1002/zaac.19322060209. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:89" class="footnote-back-ref">↩</a></p></li> <li id="fn:90"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:90" class="footnote-back-ref">↩</a></p></li> <li id="fn:91"><p>Nath Rây, Nirmalendu (1932). "Fluoberyllate und ihre Analogie mit Sulfaten. III. Doppelsalze der Fluoberyllate". Zeitschrift für anorganische und allgemeine Chemie (in German). 206 (2): 209–216. doi:10.1002/zaac.19322060209. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:91" class="footnote-back-ref">↩</a></p></li> <li id="fn:92"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:92" class="footnote-back-ref">↩</a></p></li> <li id="fn:93"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:93" class="footnote-back-ref">↩</a></p></li> <li id="fn:94"><p>Nath Rây, Nirmalendu (1932). "Fluoberyllate und ihre Analogie mit Sulfaten. III. Doppelsalze der Fluoberyllate". Zeitschrift für anorganische und allgemeine Chemie (in German). 206 (2): 209–216. doi:10.1002/zaac.19322060209. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:94" class="footnote-back-ref">↩</a></p></li> <li id="fn:95"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:95" class="footnote-back-ref">↩</a></p></li> <li id="fn:96"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:96" class="footnote-back-ref">↩</a></p></li> <li id="fn:97"><p>Nath Rây, Nirmalendu (1932). "Fluoberyllate und ihre Analogie mit Sulfaten. III. Doppelsalze der Fluoberyllate". Zeitschrift für anorganische und allgemeine Chemie (in German). 206 (2): 209–216. doi:10.1002/zaac.19322060209. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:97" class="footnote-back-ref">↩</a></p></li> <li id="fn:98"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:98" class="footnote-back-ref">↩</a></p></li> <li id="fn:99"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:99" class="footnote-back-ref">↩</a></p></li> <li id="fn:100"><p>Nath Rây, Nirmalendu (1932). "Fluoberyllate und ihre Analogie mit Sulfaten. III. Doppelsalze der Fluoberyllate". Zeitschrift für anorganische und allgemeine Chemie (in German). 206 (2): 209–216. doi:10.1002/zaac.19322060209. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:100" class="footnote-back-ref">↩</a></p></li> <li id="fn:101"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:101" class="footnote-back-ref">↩</a></p></li> <li id="fn:102"><p>Rây, Nirmalendunath (1936). "Fluoberyllate und ihre Analogie mit Sulfaten. IV. Doppelsalze mit Rubidium- und Cäsiumfluoberyllaten". Zeitschrift für anorganische und allgemeine Chemie (in German). 227 (1): 32–36. doi:10.1002/zaac.19362270105. ISSN 0863-1786. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:102" class="footnote-back-ref">↩</a></p></li> <li id="fn:103"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" [Preparation and X-ray crystallographic study of crome fluoroberyllate alums]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C268. Paris: 1782–1784. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image</a> <a href="#fnref:103" class="footnote-back-ref">↩</a></p></li> <li id="fn:104"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" [Preparation and X-ray crystallographic study of crome fluoroberyllate alums]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C268. Paris: 1782–1784. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image</a> <a href="#fnref:104" class="footnote-back-ref">↩</a></p></li> <li id="fn:105"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" [Preparation and X-ray crystallographic study of crome fluoroberyllate alums]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C268. Paris: 1782–1784. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image</a> <a href="#fnref:105" class="footnote-back-ref">↩</a></p></li> <li id="fn:106"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" [Preparation and X-ray crystallographic study of crome fluoroberyllate alums]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C268. Paris: 1782–1784. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image</a> <a href="#fnref:106" class="footnote-back-ref">↩</a></p></li> <li id="fn:107"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" [Preparation and X-ray crystallographic study of crome fluoroberyllate alums]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C268. Paris: 1782–1784. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image</a> <a href="#fnref:107" class="footnote-back-ref">↩</a></p></li> <li id="fn:108"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" [Preparation and X-ray crystallographic study of crome fluoroberyllate alums]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C268. Paris: 1782–1784. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image</a> <a href="#fnref:108" class="footnote-back-ref">↩</a></p></li> <li id="fn:109"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" [Preparation and X-ray crystallographic study of crome fluoroberyllate alums]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C268. Paris: 1782–1784. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image</a> <a href="#fnref:109" class="footnote-back-ref">↩</a></p></li> <li id="fn:110"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" [Preparation and X-ray crystallographic study of crome fluoroberyllate alums]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C268. Paris: 1782–1784. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image</a> <a href="#fnref:110" class="footnote-back-ref">↩</a></p></li> <li id="fn:111"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" [Preparation and X-ray crystallographic study of crome fluoroberyllate alums]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C268. Paris: 1782–1784. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image</a> <a href="#fnref:111" class="footnote-back-ref">↩</a></p></li> <li id="fn:112"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" [Preparation and X-ray crystallographic study of crome fluoroberyllate alums]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C268. Paris: 1782–1784. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image</a> <a href="#fnref:112" class="footnote-back-ref">↩</a></p></li> <li id="fn:113"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (19 May 1969). "Préparation et étude radiocristallographique des aluns fluorobéryllates de chrome" [Preparation and X-ray crystallographic study of crome fluoroberyllate alums]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C268. Paris: 1782–1784. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k4802761/f1805.image</a> <a href="#fnref:113" class="footnote-back-ref">↩</a></p></li> <li id="fn:114"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (15 June 1970). "Sur l'existence et la cristallographie de quelques nouveaux fluorobéryllates doubles de chrome [CH3NH3]Cr(BeF4)2·12H2O, [C(NH2)3]Cr(BeF4)2·12H2O et [C(NH2)3]Cr(BeF4)2·6H2O" [On the existence and crystallography of several new double chrome fluoroberyllates [CH3NH3]Cr(BeF4)2·12H2O, [C(NH2)3]Cr(BeF4)2·12H2O and [C(NH2)3]Cr(BeF4)2·6H2O]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C270. Paris: 1973–1975. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k480278s/f2016.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k480278s/f2016.image</a> <a href="#fnref:114" class="footnote-back-ref">↩</a></p></li> <li id="fn:115"><p>Lari-Lavassani, Abbasse; Avinens, Christian; Cot, Louis (15 June 1970). "Sur l'existence et la cristallographie de quelques nouveaux fluorobéryllates doubles de chrome [CH3NH3]Cr(BeF4)2·12H2O, [C(NH2)3]Cr(BeF4)2·12H2O et [C(NH2)3]Cr(BeF4)2·6H2O" [On the existence and crystallography of several new double chrome fluoroberyllates [CH3NH3]Cr(BeF4)2·12H2O, [C(NH2)3]Cr(BeF4)2·12H2O and [C(NH2)3]Cr(BeF4)2·6H2O]. Comptes rendus hebdomadaires des séances de l'Académie des sciences (in French). C270. Paris: 1973–1975. <a href="https://gallica.bnf.fr/ark:/12148/bpt6k480278s/f2016.image" target="_blank">https://gallica.bnf.fr/ark:/12148/bpt6k480278s/f2016.image</a> <a href="#fnref:115" class="footnote-back-ref">↩</a></p></li> </ol>