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Beryllium
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<h2 id="characteristics">Characteristics</h2> <h3>Physical properties</h3> <p>Beryllium is a steel gray and hard <a href="/facts/Metal/PT8hNX6R">metal</a> that is brittle at room temperature and has a close-packed hexagonal <a href="/facts/Crystal_structure/bJ4bCeHd">crystal structure</a>.<a class="footnote-ref" id="fnref:9" href="#fn:9"><sup>9</sup></a> It has exceptional <a href="/facts/Stiffness/xlabLkfT">stiffness</a> (<a href="/facts/Young%27s_modulus/MV5JMCIM">Young's modulus</a> 287 GPa) and a <a href="/facts/Melting_point/MY0w0h0k">melting point</a> of 1287 °C. The <a href="/facts/Modulus_of_elasticity/Et73KjbT">modulus of elasticity</a> of beryllium is approximately 35% greater than that of steel. The combination of this modulus and a relatively low density results in an unusually fast <a href="/facts/Speed_of_sound/dYtbt1nf">sound conduction speed</a> in beryllium – about 12.9 km/s at <a href="/facts/Standard_temperature_and_pressure/JhJv9KFJ">ambient conditions</a>. Among all metals, beryllium dissipates the most heat per unit weight, with both high specific heat (1925 J·kg−1·K−1) and thermal conductivity (216 W·m−1·K−1). Beryllium's conductivity and relatively low coefficient of linear <a href="/facts/Thermal_expansion/BP2vjX0N">thermal expansion</a> (11.4 × 10−6 K−1), make it uniquely stable under extreme temperature differences.<a class="footnote-ref" id="fnref:10" href="#fn:10"><sup>10</sup></a>: 11.1 </p> <h3>Nuclear properties</h3> <p>Naturally occurring beryllium, save for slight contamination by the <a href="/facts/Cosmogenic_nuclide/TlJwc4wV">radioisotopes created by cosmic rays</a>, is isotopically pure beryllium-9,<a class="footnote-ref" id="fnref:11" href="#fn:11"><sup>11</sup></a> which has a <a href="/facts/Spin_(physics)/4Jvp7e8P">nuclear spin</a> of 3/2−.<a class="footnote-ref" id="fnref:12" href="#fn:12"><sup>12</sup></a> The inelastic scattering <a href="/facts/Cross_section_(physics)/lo014h2D">cross section</a> of beryllium increases with relation to neutron energy,<a class="footnote-ref" id="fnref:13" href="#fn:13"><sup>13</sup></a> allowing for significant slowing of higher-energy neutrons.<a class="footnote-ref" id="fnref:14" href="#fn:14"><sup>14</sup></a> Therefore, it works as a <a href="/facts/Neutron_reflector/yDkgmcrE">neutron reflector</a> and <a href="/facts/Neutron_moderator/1qa6YvDD">neutron moderator</a>; the exact strength of neutron slowing strongly depends on the purity and size of the crystallites in the material.<a class="footnote-ref" id="fnref:15" href="#fn:15"><sup>15</sup></a> </p><p>The single primordial beryllium isotope 9Be also undergoes a (n,2n) neutron reaction with neutron energies over about 1.9 MeV, to produce <a href="/facts/Beryllium-8/I8e5Isl0">8Be</a>, which almost immediately breaks into two alpha particles. Thus, for high-energy neutrons, beryllium is a neutron multiplier, releasing more neutrons than it absorbs. This nuclear reaction is:<a class="footnote-ref" id="fnref:16" href="#fn:16"><sup>16</sup></a> </p> 94Be + n → 2 42He + 2 n <p>Neutrons are liberated when beryllium <a href="/facts/Atomic_nucleus/orpIm5Xl">nuclei</a> are struck by energetic <a href="/facts/Alpha_particle/dzNMs9WP">alpha particles</a><a class="footnote-ref" id="fnref:17" href="#fn:17"><sup>17</sup></a> producing the nuclear reaction </p> 94Be + 42He → 126C + n <p>where 42He is an alpha particle and 126C is a <a href="/facts/Carbon-12/nJYECzEr">carbon-12</a> nucleus.<a class="footnote-ref" id="fnref:18" href="#fn:18"><sup>18</sup></a> Beryllium also releases neutrons under bombardment by gamma rays.<a class="footnote-ref" id="fnref:19" href="#fn:19"><sup>19</sup></a> Thus, natural beryllium bombarded either by alphas or gammas from a suitable radioisotope is a key component of most radioisotope-powered <a href="/facts/Nuclear_reaction/202yClUr">nuclear reaction</a> <a href="/facts/Neutron_source/4BTQAu9l">neutron sources</a> for the laboratory production of free neutrons.<a class="footnote-ref" id="fnref:20" href="#fn:20"><sup>20</sup></a><a class="footnote-ref" id="fnref:21" href="#fn:21"><sup>21</sup></a> </p><p>Small amounts of <a href="/facts/Tritium/HWSa6EHy">tritium</a> are liberated when 94Be nuclei absorb low energy neutrons in the three-step nuclear reaction </p> 94Be + n → 42He + 62He, 62He → 63Li + β−, 63Li + n → 42He + 31H <p>62He has a half-life of only 0.8 seconds, β− is an electron, and 63Li has a high neutron absorption cross section. Tritium is a radioisotope of concern in nuclear reactor waste streams.<a class="footnote-ref" id="fnref:22" href="#fn:22"><sup>22</sup></a> </p> <h3>Optical properties</h3> <p>As a metal, beryllium is <a href="/facts/Transparency_and_translucency/PRryNNW6">transparent or translucent</a> to most wavelengths of <a href="/facts/X-ray/wseP79cN">X-rays</a> and <a href="/facts/Gamma_ray/5Drf913J">gamma rays</a>, making it useful for the output windows of <a href="/facts/X-ray_tube/tx0dTDqp">X-ray tubes</a> and other such apparatus.<a class="footnote-ref" id="fnref:23" href="#fn:23"><sup>23</sup></a> </p> <h3>Isotopes and nucleosynthesis</h3> <p class="note">Main article: <a href="/facts/Isotopes_of_beryllium/bNvHB5xg">Isotopes of beryllium</a></p> <p>Both stable and unstable isotopes of beryllium are created in stars, but the radioisotopes do not last long. It is believed that the beryllium in the universe was created in the interstellar medium when <a href="/facts/Cosmic_rays/uxCVdTKd">cosmic rays</a> induced fission in heavier elements found in interstellar gas and dust, a process called <a href="/facts/Cosmic_ray_spallation/gSlq9VEP">cosmic ray spallation</a>.<a class="footnote-ref" id="fnref:24" href="#fn:24"><sup>24</sup></a><a class="footnote-ref" id="fnref:25" href="#fn:25"><sup>25</sup></a> Natural beryllium is solely made up of the stable isotope beryllium-9. Beryllium is the only <a href="/facts/Monoisotopic_element/WzpKpVfg">monoisotopic element</a> with an even atomic number.<a class="footnote-ref" id="fnref:26" href="#fn:26"><sup>26</sup></a> </p><p>A very small fraction – 10−9 – of the primordial atoms created in the <a href="/facts/Big_Bang_nucleosynthesis/IvM4gbKH">Big Bang nucleosynthesis</a> were 7Be. This is a consequence of the low density of matter when the temperature of the universe cooled enough for small nuclei to be stable. Creating such nuclei require nuclear collisions that are rare at low density.<a class="footnote-ref" id="fnref:27" href="#fn:27"><sup>27</sup></a>: 297 7Be is unstable and decays by <a href="/facts/Electron_capture/EIccoV1u">electron capture</a> into 7Li with a half-life of 53 days, but in the early universe this decay channel was unavailable due to atoms being fully ionized. The conversion of 7Be to Li was only complete near the time of <a href="/facts/Recombination_(cosmology)/cUGysC0q">recombination</a>.<a class="footnote-ref" id="fnref:28" href="#fn:28"><sup>28</sup></a> </p><p>The isotope 7Be (half-life 53 days) is also a <a href="/facts/Cosmogenic_nuclide/TlJwc4wV">cosmogenic nuclide</a>, and also shows an atmospheric abundance inversely proportional to solar activity.<a class="footnote-ref" id="fnref:29" href="#fn:29"><sup>29</sup></a> The 2s electrons of beryllium may contribute to chemical bonding. Therefore, when 7Be decays by L-<a href="/facts/Electron_capture/EIccoV1u">electron capture</a>, it does so by taking electrons from its <a href="/facts/Atomic_orbital/tKhgl6mL">atomic orbitals</a> that may be participating in bonding. This makes its decay rate dependent to a measurable degree upon its chemical surroundings – a rare occurrence in nuclear decay.<a class="footnote-ref" id="fnref:30" href="#fn:30"><sup>30</sup></a> </p><p>8Be is unstable but has a ground state <a href="/facts/Resonance_(particle_physics)/aBEXCbzT">resonance</a> with an important role in the <a href="/facts/Triple-alpha_process/wV6lacSF">triple-alpha process</a> in helium-fueled stars. As first proposed by British <a href="/facts/Astronomer/ronF8j4a">astronomer</a> Sir <a href="/facts/Fred_Hoyle/tXjJ0Lbd">Fred Hoyle</a> based solely on astrophysical analysis, the energy levels of 8Be and 12C allow carbon nucleosynthesis by increasing the contact time for two of the three alpha particles in the carbon production process. The main carbon producing reaction in the universe is 4 He + 8 Be → 12 C + γ {\displaystyle ^{4}{\textrm {He}}\ +\ ^{8}{\textrm {Be}}\rightarrow \ ^{12}{\textrm {C}}+\gamma } where 4-He is an alpha particle.<a class="footnote-ref" id="fnref:31" href="#fn:31"><sup>31</sup></a> </p> <p>Radioactive cosmogenic <a href="/facts/Beryllium-10/oz3rQBLB">10Be</a> is produced in the <a href="/facts/Earth%27s_atmosphere/FV97Am25">atmosphere of the Earth</a> by the <a href="/facts/Cosmic_ray_spallation/gSlq9VEP">cosmic ray spallation</a> of <a href="/facts/Oxygen/acyn6o8r">oxygen</a>.<a class="footnote-ref" id="fnref:32" href="#fn:32"><sup>32</sup></a> 10Be accumulates at the <a href="/facts/Soil/5Ddpr3QM">soil</a> surface, where its relatively long <a href="/facts/Half-life/kGVH8BAB">half-life</a> (1.36 million years) permits a long <a href="/facts/Residence_time_(fluid_dynamics)/Y9TGuxyv">residence time</a> before decaying to <a href="/facts/Boron/Pmwgd7Mf">boron</a>-10. Thus, 10Be and its daughter products are used to examine natural <a href="/facts/Soil_erosion/pbwuyY5H">soil erosion</a>, <a href="/facts/Soil_formation/sJty93z9">soil formation</a> and the development of <a href="/facts/Laterite/3FYFwspo">lateritic soils</a>, and as a <a href="/facts/Proxy_(climate)/kuCVBpBL">proxy</a> for measurement of the variations in <a href="/facts/Solar_variation/QrP4Egea">solar activity</a> and the age of <a href="/facts/Ice_core/QnzraAoN">ice cores</a>.<a class="footnote-ref" id="fnref:33" href="#fn:33"><sup>33</sup></a> The production of 10Be is inversely proportional to solar activity, because increased <a href="/facts/Solar_wind/BvuB3dT8">solar wind</a> during periods of high solar activity decreases the flux of galactic cosmic rays that reach the Earth.<a class="footnote-ref" id="fnref:34" href="#fn:34"><sup>34</sup></a> Nuclear explosions also form 10Be by the reaction of fast neutrons with 13C in the carbon dioxide in air. This is one of the indicators of past activity at <a href="/facts/Nuclear_weapon_test/s2srGDFP">nuclear weapon test</a> sites.<a class="footnote-ref" id="fnref:35" href="#fn:35"><sup>35</sup></a> </p><p>The exotic isotopes 11Be and 14Be are known to exhibit a <a href="/facts/Halo_nucleus/1oKv2Cmw">nuclear halo</a>. This phenomenon can be understood as the nuclei of 11Be and 14Be have, respectively, 1 and 4 neutrons orbiting substantially outside the expected nuclear radius.<a class="footnote-ref" id="fnref:36" href="#fn:36"><sup>36</sup></a> </p> <h2 id="occurrence">Occurrence</h2> <p>Beryllium is found in over 100 minerals,<a class="footnote-ref" id="fnref:37" href="#fn:37"><sup>37</sup></a> but most are uncommon to rare. The more common beryllium containing minerals include: <a href="/facts/Bertrandite/RKJvfCDC">bertrandite</a> (Be4Si2O7(OH)2), <a href="/facts/Beryl/Fl7q1Hl9">beryl</a> (Al2Be3Si6O18), <a href="/facts/Chrysoberyl/RRDtRWJE">chrysoberyl</a> (Al2BeO4) and <a href="/facts/Phenakite/f7w8BeD5">phenakite</a> (Be2SiO4). Precious forms of beryl are <a href="/facts/Aquamarine_(gemstone)/Fl7q1Hl9">aquamarine</a>, <a href="/facts/Red_beryl/Fl7q1Hl9">red beryl</a> and <a href="/facts/Emerald/pr52yTAD">emerald</a>.<a class="footnote-ref" id="fnref:38" href="#fn:38"><sup>38</sup></a><a class="footnote-ref" id="fnref:39" href="#fn:39"><sup>39</sup></a><a class="footnote-ref" id="fnref:40" href="#fn:40"><sup>40</sup></a> The green color in gem-quality forms of beryl comes from varying amounts of chromium (about 2% for emerald).<a class="footnote-ref" id="fnref:41" href="#fn:41"><sup>41</sup></a> </p><p>The two main ores of beryllium, beryl and bertrandite, are found in Argentina, Brazil, India, Madagascar, Russia and the United States.<a class="footnote-ref" id="fnref:42" href="#fn:42"><sup>42</sup></a> Total world reserves of beryllium ore are greater than 400,000 tonnes.<a class="footnote-ref" id="fnref:43" href="#fn:43"><sup>43</sup></a> </p><p>The Sun has a concentration of 0.1 <a href="/facts/Parts_per_billion/PozRuoLM">parts per billion</a> (ppb) of beryllium.<a class="footnote-ref" id="fnref:44" href="#fn:44"><sup>44</sup></a> Beryllium has a concentration of 2 to 6 <a href="/facts/Parts_per_million/PozRuoLM">parts per million</a> (ppm) in the Earth's crust and is the 47th most abundant element.<a class="footnote-ref" id="fnref:45" href="#fn:45"><sup>45</sup></a><a class="footnote-ref" id="fnref:46" href="#fn:46"><sup>46</sup></a> It is most concentrated in the soils at 6 ppm.<a class="footnote-ref" id="fnref:47" href="#fn:47"><sup>47</sup></a> Trace amounts of 9Be are found in the Earth's atmosphere.<a class="footnote-ref" id="fnref:48" href="#fn:48"><sup>48</sup></a> The concentration of beryllium in sea water is 0.2–0.6 <a href="/facts/Parts_per_trillion/PozRuoLM">parts per trillion</a>.<a class="footnote-ref" id="fnref:49" href="#fn:49"><sup>49</sup></a><a class="footnote-ref" id="fnref:50" href="#fn:50"><sup>50</sup></a> In stream water, however, beryllium is more abundant with a concentration of 0.1 ppb.<a class="footnote-ref" id="fnref:51" href="#fn:51"><sup>51</sup></a> </p> <h2 id="extraction">Extraction</h2> <p>The extraction of beryllium from its compounds is a difficult process due to its high affinity for oxygen at elevated temperatures, and its ability to reduce water when its oxide film is removed. Currently the United States, China and Kazakhstan are the only three countries involved in the industrial-scale extraction of beryllium.<a class="footnote-ref" id="fnref:52" href="#fn:52"><sup>52</sup></a> Kazakhstan produces beryllium from a concentrate stockpiled before the <a href="/facts/Dissolution_of_the_Soviet_Union/Fyn5jw3n">breakup of the Soviet Union</a> around 1991. This resource had become nearly depleted by mid-2010s.<a class="footnote-ref" id="fnref:53" href="#fn:53"><sup>53</sup></a> </p><p>Production of beryllium in Russia was halted in 1997, and is planned to be resumed in the 2020s.<a class="footnote-ref" id="fnref:54" href="#fn:54"><sup>54</sup></a><a class="footnote-ref" id="fnref:55" href="#fn:55"><sup>55</sup></a> </p> <p>Beryllium is most commonly extracted from the mineral <a href="/facts/Beryl/Fl7q1Hl9">beryl</a>, which is either <a href="/facts/Sintering/Y4eGLzFf">sintered</a> using an extraction agent or melted into a soluble mixture. The sintering process involves mixing beryl with <a href="/facts/Sodium_fluorosilicate/XWoBQPwK">sodium fluorosilicate</a> and soda at 770 °C (1,420 °F) to form <a href="/facts/Tetrafluoroberyllate/gSmGknKr">sodium fluoroberyllate</a>, <a href="/facts/Aluminium_oxide/wXM9P6pI">aluminium oxide</a> and <a href="/facts/Silicon_dioxide/A3WILp6J">silicon dioxide</a>.<a class="footnote-ref" id="fnref:56" href="#fn:56"><sup>56</sup></a> <a href="/facts/Beryllium_hydroxide/4CBISdYQ">Beryllium hydroxide</a> is precipitated from a solution of sodium fluoroberyllate and <a href="/facts/Sodium_hydroxide/xjtdYtq7">sodium hydroxide</a> in water. The extraction of beryllium using the melt method involves grinding beryl into a powder and heating it to 1,650 °C (3,000 °F). The melt is quickly cooled with water and then reheated 250 to 300 °C (482 to 572 °F) in concentrated <a href="/facts/Sulfuric_acid/Wom6fymJ">sulfuric acid</a>, mostly yielding <a href="/facts/Beryllium_sulfate/8pgGhaBn">beryllium sulfate</a> and <a href="/facts/Aluminium_sulfate/Jz6FlVb5">aluminium sulfate</a>. Aqueous <a href="/facts/Ammonia/MtLtJFtz">ammonia</a> is then used to remove the aluminium and sulfur, leaving beryllium hydroxide.<a class="footnote-ref" id="fnref:57" href="#fn:57"><sup>57</sup></a> </p><p>Beryllium hydroxide created using either the sinter or melt method is then converted into <a href="/facts/Beryllium_fluoride/4wkNdddq">beryllium fluoride</a> or <a href="/facts/Beryllium_chloride/2uepR11V">beryllium chloride</a>. To form the fluoride, aqueous <a href="/facts/Ammonium_hydrogen_fluoride/F433DsdE">ammonium hydrogen fluoride</a> is added to beryllium hydroxide to yield a precipitate of ammonium <a href="/facts/Tetrafluoroberyllate/gSmGknKr">tetrafluoroberyllate</a>, which is heated to 1,000 °C (1,830 °F) to form beryllium fluoride.<a class="footnote-ref" id="fnref:58" href="#fn:58"><sup>58</sup></a> Heating the fluoride to 900 °C (1,650 °F) with <a href="/facts/Magnesium/XyIhd2FG">magnesium</a> forms finely divided beryllium, and additional heating to 1,300 °C (2,370 °F) creates the compact metal.<a class="footnote-ref" id="fnref:59" href="#fn:59"><sup>59</sup></a> Heating beryllium hydroxide forms <a href="/facts/Beryllium_oxide/o3VnG96d">beryllium oxide</a>, which becomes beryllium chloride when combined with carbon and chlorine. <a href="/facts/Electrolysis/pU75nCDI">Electrolysis</a> of molten beryllium chloride is then used to obtain the metal.<a class="footnote-ref" id="fnref:60" href="#fn:60"><sup>60</sup></a> </p> <h2 id="chemical-properties">Chemical properties</h2> <p class="note">See also: Category:Beryllium compounds</p> <p>A beryllium atom has the electronic configuration [He] 2s2. The predominant <a href="/facts/Oxidation_state/W53W6s6V">oxidation state</a> of beryllium is +2; the beryllium atom has lost both of its valence electrons. Lower oxidation states complexes of beryllium are exceedingly rare. For example, a stable complex with a Be-Be bond, which formally features beryllium in the +1 oxidation state, has been described.<a class="footnote-ref" id="fnref:61" href="#fn:61"><sup>61</sup></a> Beryllium in the 0 oxidation state is also known in a complex with a Mg-Be bond.<a class="footnote-ref" id="fnref:62" href="#fn:62"><sup>62</sup></a> Beryllium's chemical behavior is largely a result of its small <a href="/facts/Atomic_radius/0mQaIJX9">atomic</a> and <a href="/facts/Ionic_radius/C3dwKrrB">ionic</a> radii. It thus has very high <a href="/facts/Ionization_potential/lezUajfA">ionization potentials</a> and does not form divalent cations. Instead it forms two covalent bonds with a tendency to polymerize, as in solid BeCl2.<a class="footnote-ref" id="fnref:63" href="#fn:63"><sup>63</sup></a>.: 37 Its chemistry has similarities to that of aluminium, an example of a <a href="/facts/Diagonal_relationship/jMMvw2lt">diagonal relationship</a>.<a class="footnote-ref" id="fnref:64" href="#fn:64"><sup>64</sup></a>: 107 </p><p>At room temperature, the surface of beryllium forms a 1−10 nm-thick oxide <a href="/facts/Passivation_(chemistry)/tPADJj5G">passivation</a> layer that prevents further reactions with air, except for gradual thickening of the oxide up to about 25 nm. When heated above about 500 °C, oxidation into the bulk metal progresses along grain boundaries.<a class="footnote-ref" id="fnref:65" href="#fn:65"><sup>65</sup></a> Once the metal is ignited in air by heating above the oxide melting point around 2500 °C, beryllium burns brilliantly,<a class="footnote-ref" id="fnref:66" href="#fn:66"><sup>66</sup></a> forming a mixture of <a href="/facts/Beryllium_oxide/o3VnG96d">beryllium oxide</a> and <a href="/facts/Beryllium_nitride/pQaMV5wt">beryllium nitride</a>. Beryllium dissolves readily in non-<a href="/facts/Oxidizing_acid/cCr2nwAy">oxidizing acids</a>, such as HCl and diluted H2SO4, but not in <a href="/facts/Nitric_acid/UDbwGp6s">nitric acid</a> or water as this forms the oxide. This behavior is similar to that of aluminium. Beryllium also dissolves and reacts with alkali solutions.<a class="footnote-ref" id="fnref:67" href="#fn:67"><sup>67</sup></a><a class="footnote-ref" id="fnref:68" href="#fn:68"><sup>68</sup></a>: 112 </p><p>Binary compounds of beryllium(II) are polymeric in the solid state. <a href="/facts/Beryllium_fluoride/4wkNdddq">BeF2</a> has a <a href="/facts/Silica/A3WILp6J">silica</a>-like structure with corner-shared BeF4 tetrahedra. <a href="/facts/Beryllium_chloride/2uepR11V">BeCl2</a> and <a href="/facts/Beryllium_bromide/1JmjCQBz">BeBr2</a> have chain structures with edge-shared tetrahedra. <a href="/facts/Beryllium_oxide/o3VnG96d">Beryllium oxide</a>, BeO, is a white <a href="/facts/Refractory/LoKrzGkR">refractory</a> solid which has a <a href="/facts/Zinc_sulfide/K8l5AF3K">wurtzite</a> crystal structure and a thermal conductivity as high as some metals. BeO is <a href="/facts/Amphoteric/2UrXEsyl">amphoteric</a>. <a href="/facts/Beryllium_sulfide/KKdR9lWg">Beryllium sulfide</a>, selenide and <a href="/facts/Beryllium_telluride/wPxfq3oh">telluride</a> are known, all having the <a href="/facts/Cubic_crystal_system/92Co7BKM">zincblende structure</a>.<a class="footnote-ref" id="fnref:69" href="#fn:69"><sup>69</sup></a> <a href="/facts/Beryllium_nitride/pQaMV5wt">Beryllium nitride</a>, Be3N2, is a high-melting-point compound which is readily hydrolyzed. <a href="/facts/Beryllium_azide/bd7R2mEH">Beryllium azide</a>, BeN6 is known and beryllium phosphide, Be3P2 has a similar structure to Be3N2. A number of beryllium <a href="/facts/Boride/Cf1ephFt">borides</a> are known, such as Be5B, Be4B, Be2B, BeB2, BeB6 and BeB12. <a href="/facts/Beryllium_carbide/4hy75uyX">Beryllium carbide</a>, Be2C, is a refractory brick-red compound that reacts with water to give <a href="/facts/Methane/kBHneYnh">methane</a>.<a class="footnote-ref" id="fnref:70" href="#fn:70"><sup>70</sup></a> Beryllium <a href="/facts/Silicide/NyxslNNN">silicides</a> have been identified in the form of variously sized <a href="/facts/Nanocluster/k8kNxX4E">nanoclusters</a>,<a class="footnote-ref" id="fnref:71" href="#fn:71"><sup>71</sup></a> formed through a spontaneous reaction between pure beryllium and silicon.<a class="footnote-ref" id="fnref:72" href="#fn:72"><sup>72</sup></a> The halides BeX2 (X = F, Cl, Br, and I) have a linear monomeric molecular structure in the gas phase.<a class="footnote-ref" id="fnref:73" href="#fn:73"><sup>73</sup></a>: 117 </p><p>Beryllium is a strong electron acceptor leading to Be bonding effects similar to <a href="/facts/Hydrogen_bonding/85V86IIg">hydrogen bonding</a>.<a class="footnote-ref" id="fnref:74" href="#fn:74"><sup>74</sup></a> </p> <h3>Aqueous solutions</h3> <p>Solutions of beryllium salts, such as <a href="/facts/Beryllium_sulfate/8pgGhaBn">beryllium sulfate</a> and <a href="/facts/Beryllium_nitrate/tubgUYbQ">beryllium nitrate</a>, are acidic because of hydrolysis of the [Be(H2O)4]2+ ion. The concentration of the first hydrolysis product, [Be(H2O)3(OH)]+, is less than 1% of the beryllium concentration. The most stable hydrolysis product is the <a href="/facts/Trimer_(chemistry)/ws3JkjuQ">trimeric</a> ion [Be3(OH)3(H2O)6]3+. <a href="/facts/Beryllium_hydroxide/4CBISdYQ">Beryllium hydroxide</a>, Be(OH)2, is insoluble in water at pH 5 or more. Consequently, beryllium compounds are generally insoluble at biological pH. Because of this, inhalation of beryllium metal dust leads to the development of the fatal condition of <a href="/facts/Berylliosis/yELbTj7r">berylliosis</a>. Be(OH)2 dissolves in strongly <a href="/facts/Alkalinity/qWjbkx33">alkaline</a> solutions.<a class="footnote-ref" id="fnref:75" href="#fn:75"><sup>75</sup></a> </p><p>Beryllium(II) forms few complexes with monodentate ligands because the water molecules in the aquo-ion, [Be(H2O)4]2+ are bound very strongly to the beryllium ion. Notable exceptions are the series of water-soluble complexes with the <a href="/facts/Fluoride/LpqNMzwa">fluoride</a> ion:<a class="footnote-ref" id="fnref:76" href="#fn:76"><sup>76</sup></a> </p> [Be(H2O)4]2+ + <i>n</i> F− ⇌ Be[(H2O)2−<i>n</i>F<i>n</i>]2− + <i>n</i> H2O <p>Beryllium(II) forms many complexes with bidentate ligands containing oxygen-donor atoms.<a class="footnote-ref" id="fnref:77" href="#fn:77"><sup>77</sup></a> The species [Be3O(H2PO4)6]2- is notable for having a 3-coordinate oxide ion at its center. <a href="/facts/Basic_beryllium_acetate/2x9W0Ljg">Basic beryllium acetate</a>, Be4O(OAc)6, has an oxide ion surrounded by a tetrahedron of beryllium atoms.<a class="footnote-ref" id="fnref:78" href="#fn:78"><sup>78</sup></a> </p><p>With organic ligands, such as the <a href="/facts/Malonate/rIrVbMpm">malonate</a> ion, the acid deprotonates when forming the complex. The donor atoms are two oxygens. </p> H2A + [Be(H2O)4]2+ ⇌ [BeA(H2O)2] + 2 H+ + 2 H2O H2A + [BeA(H2O)2] ⇌ [BeA2]2− + 2 H+ + 2 H2O <p>The formation of a complex is in competition with the metal ion-hydrolysis reaction and mixed complexes with both the anion and the hydroxide ion are also formed. For example, derivatives of the cyclic trimer are known, with a bidentate ligand replacing one or more pairs of water molecules.<a class="footnote-ref" id="fnref:79" href="#fn:79"><sup>79</sup></a> </p><p>Aliphatic <a href="/facts/Hydroxycarboxylic_acid/Wrpznrje">hydroxycarboxylic acids</a> such as <a href="/facts/Glycolic_acid/Y0urKYuy">glycolic acid</a> form rather weak monodentate complexes in solution, in which the hydroxyl group remains intact. In the solid state, the hydroxyl group may deprotonate: a hexamer, Na4[Be6(OCH2(O)O)6], was isolated long ago.<a class="footnote-ref" id="fnref:80" href="#fn:80"><sup>80</sup></a><a class="footnote-ref" id="fnref:81" href="#fn:81"><sup>81</sup></a> Aromatic hydroxy ligands (i.e. <a href="/facts/Phenol/ACJs5NIU">phenols</a>) form relatively strong complexes. For example, log K1 and log K2 values of 12.2 and 9.3 have been reported for complexes with <a href="/facts/Tiron_(chemical)/7jIvm2pq">tiron</a>.<a class="footnote-ref" id="fnref:82" href="#fn:82"><sup>82</sup></a><a class="footnote-ref" id="fnref:83" href="#fn:83"><sup>83</sup></a> </p><p>Beryllium has generally a rather poor affinity for <a href="/facts/Ammine/xvd6F14I">ammine</a> ligands.<a class="footnote-ref" id="fnref:84" href="#fn:84"><sup>84</sup></a><a class="footnote-ref" id="fnref:85" href="#fn:85"><sup>85</sup></a> There are many early reports of complexes with amino acids, but unfortunately they are not reliable as the concomitant hydrolysis reactions were not understood at the time of publication. Values for log β of ca. 6 to 7 have been reported. The degree of formation is small because of competition with hydrolysis reactions.<a class="footnote-ref" id="fnref:86" href="#fn:86"><sup>86</sup></a><a class="footnote-ref" id="fnref:87" href="#fn:87"><sup>87</sup></a> </p> <h3>Organic chemistry</h3> <p class="note">Main article: <a href="/facts/Organoberyllium_chemistry/HBe5FuvD">Organoberyllium chemistry</a></p> <p>Organometallic beryllium compounds are known to be highly reactive.<a class="footnote-ref" id="fnref:88" href="#fn:88"><sup>88</sup></a> Examples of known organoberyllium compounds are dineopentylberyllium,<a class="footnote-ref" id="fnref:89" href="#fn:89"><sup>89</sup></a> beryllocene (Cp2Be),<a class="footnote-ref" id="fnref:90" href="#fn:90"><sup>90</sup></a><a class="footnote-ref" id="fnref:91" href="#fn:91"><sup>91</sup></a><a class="footnote-ref" id="fnref:92" href="#fn:92"><sup>92</sup></a><a class="footnote-ref" id="fnref:93" href="#fn:93"><sup>93</sup></a> diallylberyllium (by exchange reaction of diethyl beryllium with triallyl boron),<a class="footnote-ref" id="fnref:94" href="#fn:94"><sup>94</sup></a> bis(1,3-trimethylsilylallyl)beryllium,<a class="footnote-ref" id="fnref:95" href="#fn:95"><sup>95</sup></a> Be(<a href="/facts/Mesitylene/4JCRbj1Y">mes</a>)2,<a class="footnote-ref" id="fnref:96" href="#fn:96"><sup>96</sup></a> and (beryllium(I) complex) diberyllocene.<a class="footnote-ref" id="fnref:97" href="#fn:97"><sup>97</sup></a> Ligands can also be aryls<a class="footnote-ref" id="fnref:98" href="#fn:98"><sup>98</sup></a> and alkynyls.<a class="footnote-ref" id="fnref:99" href="#fn:99"><sup>99</sup></a> </p> <h2 id="history">History</h2> <p>The mineral <a href="/facts/Beryl/Fl7q1Hl9">beryl</a>, which contains beryllium, has been used at least since the <a href="/facts/Ptolemaic_dynasty/xqbNcghq">Ptolemaic dynasty</a> of Egypt.<a class="footnote-ref" id="fnref:100" href="#fn:100"><sup>100</sup></a> In the first century <a href="/facts/Common_Era/e5DpqUoe">CE</a>, Roman naturalist <a href="/facts/Pliny_the_Elder/grx67ghR">Pliny the Elder</a> mentioned in his encyclopedia <i><a href="/facts/Natural_History_(Pliny)/bMp2te1A">Natural History</a></i> that beryl and <a href="/facts/Emerald/pr52yTAD">emerald</a> ("smaragdus") were similar.<a class="footnote-ref" id="fnref:101" href="#fn:101"><sup>101</sup></a> The <a href="/facts/Papyrus_Graecus_Holmiensis/NN5vUV6a">Papyrus Graecus Holmiensis</a>, written in the third or fourth century CE, contains notes on how to prepare artificial emerald and beryl.<a class="footnote-ref" id="fnref:102" href="#fn:102"><sup>102</sup></a> </p> <p>Early analyses of emeralds and beryls by <a href="/facts/Martin_Heinrich_Klaproth/5DAt7l6Q">Martin Heinrich Klaproth</a>, <a href="/facts/Torbern_Olof_Bergman/PssYPozl">Torbern Olof Bergman</a>, <a href="/facts/Franz_Karl_Achard/PMBha6y0">Franz Karl Achard</a>, and Johann Jakob Bindheim [de] always yielded similar elements, leading to the mistaken conclusion that both substances are <a href="/facts/Aluminium_silicate/kmhQYeA7">aluminium silicates</a>.<a class="footnote-ref" id="fnref:103" href="#fn:103"><sup>103</sup></a> Mineralogist <a href="/facts/Ren%C3%A9_Just_Ha%C3%BCy/yQuF9n2T">René Just Haüy</a> discovered that both crystals are geometrically identical, and he asked chemist <a href="/facts/Louis-Nicolas_Vauquelin/ygSb9h9Q">Louis-Nicolas Vauquelin</a> for a chemical analysis.<a class="footnote-ref" id="fnref:104" href="#fn:104"><sup>104</sup></a> </p><p>In a 1798 paper read before the <a href="/facts/Institut_de_France/jrre6kaI">Institut de France</a>, Vauquelin reported that he found a new "earth" by dissolving <a href="/facts/Aluminium_hydroxide/e0pXvDGr">aluminium hydroxide</a> from emerald and beryl in an additional <a href="/facts/Alkali/s6NqPGSP">alkali</a>.<a class="footnote-ref" id="fnref:105" href="#fn:105"><sup>105</sup></a> The editors of the journal <i><a href="/facts/Annales_de_chimie_et_de_physique/sXTtXYmh">Annales de chimie et de physique</a></i> named the new earth "glucine" for the sweet taste of some of its compounds.<a class="footnote-ref" id="fnref:106" href="#fn:106"><sup>106</sup></a><a class="footnote-ref" id="fnref:107" href="#fn:107"><sup>107</sup></a> The name <i>beryllium</i> was first used by <a href="/facts/Friedrich_W%C3%B6hler/D7uh7ySD">Friedrich Wöhler</a> in 1828.<a class="footnote-ref" id="fnref:108" href="#fn:108"><sup>108</sup></a><a class="footnote-ref" id="fnref:109" href="#fn:109"><sup>109</sup></a> Both beryllium and glucinum were used concurrently until 1949, when the <a href="/facts/IUPAC/2AV6myCK">IUPAC</a> adopted beryllium as the standard name of the element.<a class="footnote-ref" id="fnref:110" href="#fn:110"><sup>110</sup></a><a class="footnote-ref" id="fnref:111" href="#fn:111"><sup>111</sup></a> </p> <p><a href="/facts/Friedrich_W%C3%B6hler/D7uh7ySD">Friedrich Wöhler</a><a class="footnote-ref" id="fnref:112" href="#fn:112"><sup>112</sup></a> and <a href="/facts/Antoine_Bussy/bhXcWMhg">Antoine Bussy</a><a class="footnote-ref" id="fnref:113" href="#fn:113"><sup>113</sup></a> independently isolated beryllium in 1828 by the <a href="/facts/Chemical_reaction/GpqWlKrz">chemical reaction</a> of metallic <a href="/facts/Potassium/FWPwS7Rj">potassium</a> with <a href="/facts/Beryllium_chloride/2uepR11V">beryllium chloride</a>, as follows: </p> BeCl2 + 2 K → 2 KCl + Be <p>Using an alcohol lamp, Wöhler heated alternating layers of beryllium chloride and potassium in a wired-shut platinum crucible. The above reaction immediately took place and caused the crucible to become white hot. Upon cooling and washing the resulting gray-black powder, he saw that it was made of fine particles with a dark metallic luster.<a class="footnote-ref" id="fnref:114" href="#fn:114"><sup>114</sup></a> The highly reactive potassium had been produced by the <a href="/facts/Electrolysis/pU75nCDI">electrolysis</a> of its compounds.<a class="footnote-ref" id="fnref:115" href="#fn:115"><sup>115</sup></a> He did not succeed to melt the beryllium particles.<a class="footnote-ref" id="fnref:116" href="#fn:116"><sup>116</sup></a> </p><p>The direct electrolysis of a molten mixture of <a href="/facts/Beryllium_fluoride/4wkNdddq">beryllium fluoride</a> and <a href="/facts/Sodium_fluoride/HHcvwK7s">sodium fluoride</a> by <a href="/facts/Paul_Lebeau/z9H7wNKP">Paul Lebeau</a> in 1898 resulted in the first pure (99.5 to 99.8%) samples of beryllium.<a class="footnote-ref" id="fnref:117" href="#fn:117"><sup>117</sup></a> However, industrial production started only after the First World War. The original industrial involvement included subsidiaries and scientists related to the <a href="/facts/Union_Carbide/kCE5YHal">Union Carbide and Carbon Corporation</a> in Cleveland, Ohio, and <a href="/facts/Siemens_%26_Halske/lAsPJ9sk">Siemens & Halske</a> AG in Berlin. In the US, the process was ruled by Hugh S. Cooper, director of The Kemet Laboratories Company. In Germany, the first commercially successful process for producing beryllium was developed in 1921 by <a href="/facts/Alfred_Stock/qeq9FG3G">Alfred Stock</a> and <a href="/facts/Hans_Goldschmidt/JgGDK2mY">Hans Goldschmidt</a>.<a class="footnote-ref" id="fnref:118" href="#fn:118"><sup>118</sup></a> </p><p>A sample of beryllium was bombarded with <a href="/facts/Alpha_ray/dzNMs9WP">alpha rays</a> from the decay of <a href="/facts/Radium/VWo5gkzn">radium</a> in a 1932 experiment by <a href="/facts/James_Chadwick/nwStNAzI">James Chadwick</a> that uncovered the existence of the <a href="/facts/Neutron/oRCM1geb">neutron</a>.<a class="footnote-ref" id="fnref:119" href="#fn:119"><sup>119</sup></a> This same method is used in one class of radioisotope-based laboratory <a href="/facts/Neutron_source/4BTQAu9l">neutron sources</a> that produce 30 neutrons for every million α particles.<a class="footnote-ref" id="fnref:120" href="#fn:120"><sup>120</sup></a> </p><p>Beryllium production saw a rapid increase during World War II due to the rising demand for hard beryllium-copper alloys and <a href="/facts/Phosphor/vTLjrGDE">phosphors</a> for <a href="/facts/Fluorescent_light/R8SlXCyg">fluorescent lights</a>. Most early fluorescent lamps used <a href="/facts/Zinc_orthosilicate/Gem8lHSH">zinc orthosilicate</a> with varying content of beryllium to emit greenish light. Small additions of magnesium <a href="/facts/Tungstate/ek9P92Tz">tungstate</a> improved the blue part of the spectrum to yield an acceptable white light. Halophosphate-based phosphors replaced beryllium-based phosphors after beryllium was found to be toxic.<a class="footnote-ref" id="fnref:121" href="#fn:121"><sup>121</sup></a> </p><p>Electrolysis of a mixture of <a href="/facts/Beryllium_fluoride/4wkNdddq">beryllium fluoride</a> and <a href="/facts/Sodium_fluoride/HHcvwK7s">sodium fluoride</a> was used to isolate beryllium during the 19th century. The metal's high melting point makes this process more energy-consuming than corresponding processes used for the <a href="/facts/Alkali_metals/IkWbCLk2">alkali metals</a>. Early in the 20th century, the production of beryllium by the thermal decomposition of <a href="/facts/Beryllium_iodide/jFemsCmA">beryllium iodide</a> was investigated following the success of a similar process for the production of <a href="/facts/Zirconium/y7gsoQFz">zirconium</a>, but this process proved to be uneconomical for volume production.<a class="footnote-ref" id="fnref:122" href="#fn:122"><sup>122</sup></a> </p><p>Pure beryllium metal did not become readily available until 1957, even though it had been used as an alloying metal to harden and toughen copper much earlier.<a class="footnote-ref" id="fnref:123" href="#fn:123"><sup>123</sup></a> Beryllium could be produced by reducing beryllium compounds such as <a href="/facts/Beryllium_chloride/2uepR11V">beryllium chloride</a> with metallic potassium or sodium. Currently, most beryllium is produced by reducing beryllium fluoride with <a href="/facts/Magnesium/XyIhd2FG">magnesium</a>.<a class="footnote-ref" id="fnref:124" href="#fn:124"><sup>124</sup></a> The price on the American market for <a href="/facts/Casting_(metalworking)/7mMSBWTs">vacuum-cast</a> beryllium ingots was about $338 per pound ($745 per kilogram) in 2001.<a class="footnote-ref" id="fnref:125" href="#fn:125"><sup>125</sup></a> </p><p>Between 1998 and 2008, the world's production of beryllium had decreased from 343 to about 200 <a href="/facts/Tonne/gMymLmWv">tonnes</a>. It then increased to 230 metric tons by 2018, of which 170 tonnes came from the United States.<a class="footnote-ref" id="fnref:126" href="#fn:126"><sup>126</sup></a><a class="footnote-ref" id="fnref:127" href="#fn:127"><sup>127</sup></a> </p> <h3>Etymology</h3> <p>Beryllium was named for the semiprecious mineral <a href="/facts/Beryl/Fl7q1Hl9">beryl</a>, from which it was first isolated.<a class="footnote-ref" id="fnref:128" href="#fn:128"><sup>128</sup></a><a class="footnote-ref" id="fnref:129" href="#fn:129"><sup>129</sup></a><a class="footnote-ref" id="fnref:130" href="#fn:130"><sup>130</sup></a> Martin Klaproth, having independently determined that beryl and emerald share an element, preferred the name "beryllina" due to the fact that <a href="/facts/Yttria/A7VMIG2D">yttria</a> also formed sweet salts.<a class="footnote-ref" id="fnref:131" href="#fn:131"><sup>131</sup></a><a class="footnote-ref" id="fnref:132" href="#fn:132"><sup>132</sup></a> </p><p>Although <a href="/facts/Humphry_Davy/aDNRfNou">Humphry Davy</a> failed to isolate it, he proposed the name <i>glucium</i> for the new metal, derived from the name <i>glucina</i> for the earth it was found in; altered forms of this name, <i>glucinium</i> or <i>glucinum</i> (symbol Gl) continued to be used into the 20th century.<a class="footnote-ref" id="fnref:133" href="#fn:133"><sup>133</sup></a> </p> <h2 id="applications">Applications</h2> <h3>Radiation windows</h3> <p>Because of its low atomic number and very low absorption for X-rays, the oldest and still one of the most important applications of beryllium is in radiation windows for <a href="/facts/X-ray_tube/tx0dTDqp">X-ray tubes</a>.<a class="footnote-ref" id="fnref:134" href="#fn:134"><sup>134</sup></a> Extreme demands are placed on purity and cleanliness of beryllium to avoid artifacts in the X-ray images. Thin beryllium foils are used as radiation windows for X-ray detectors, and their extremely low absorption minimizes the heating effects caused by high-intensity, low energy X-rays typical of <a href="/facts/Synchrotron/J1oWBgbU">synchrotron</a> radiation. Vacuum-tight windows and beam-tubes for radiation experiments on synchrotrons are manufactured exclusively from beryllium. In scientific setups for various X-ray emission studies (e.g., <a href="/facts/Energy-dispersive_X-ray_spectroscopy/GW0BSTKF">energy-dispersive X-ray spectroscopy</a>) the sample holder is usually made of beryllium because its emitted X-rays have much lower energies (≈100 eV) than X-rays from most studied materials.<a class="footnote-ref" id="fnref:135" href="#fn:135"><sup>135</sup></a> </p><p>Low <a href="/facts/Atomic_number/bgAr581S">atomic number</a> also makes beryllium relatively transparent to energetic <a href="/facts/Elementary_particle/CTFDM97U">particles</a>. Therefore, it is used to build the <a href="/facts/Beamline/vrfaEtFt">beam pipe</a> around the collision region in <a href="/facts/Particle_physics/YgIuyj2t">particle physics</a> setups, such as all four main detector experiments at the <a href="/facts/Large_Hadron_Collider/XWJCFSqT">Large Hadron Collider</a> (<a href="/facts/A_Large_Ion_Collider_Experiment/Nbg7fpEK">ALICE</a>, <a href="/facts/ATLAS_experiment/hqWY5WQD">ATLAS</a>, <a href="/facts/Compact_Muon_Solenoid/zrdCWwVk">CMS</a>, <a href="/facts/LHCb/PAlpBtnl">LHCb</a>),<a class="footnote-ref" id="fnref:136" href="#fn:136"><sup>136</sup></a> the <a href="/facts/Tevatron/dHkngs84">Tevatron</a> and at <a href="/facts/SLAC/CzX2afas">SLAC</a>. The low density of beryllium allows collision products to reach the surrounding detectors without significant interaction, its stiffness allows a powerful vacuum to be produced within the pipe to minimize interaction with gases, its thermal stability allows it to function correctly at temperatures of only a few degrees above <a href="/facts/Absolute_zero/U3UyPl2K">absolute zero</a>, and its <a href="/facts/Diamagnetic/dgFavn9K">diamagnetic</a> nature keeps it from interfering with the complex multipole magnet systems used to steer and <a href="/facts/Strong_focusing/hG5pbII4">focus</a> the <a href="/facts/Particle_beam/mg5EIlWb">particle beams</a>.<a class="footnote-ref" id="fnref:137" href="#fn:137"><sup>137</sup></a> </p> <h3>Mechanical applications</h3> <p>Because of its stiffness, light weight and dimensional stability over a wide temperature range, beryllium metal is used for lightweight structural components in the defense and <a href="/facts/Aerospace/T6kTLUyV">aerospace</a> industries in high-speed <a href="/facts/Aircraft/EhC4mBep">aircraft</a>, <a href="/facts/Guided_missile/C5VwQClz">guided missiles</a>, <a href="/facts/Spacecraft/YQqQaUw0">spacecraft</a>, and <a href="/facts/Satellite/PTX8c68t">satellites</a>, including the <a href="/facts/James_Webb_Space_Telescope/w4GAWnWX">James Webb Space Telescope</a>. Several <a href="/facts/Liquid-fuel_rocket/TAonrVDn">liquid-fuel rockets</a> have used <a href="/facts/Rocket_engine_nozzle/K4kHCmFX">rocket nozzles</a> made of pure beryllium.<a class="footnote-ref" id="fnref:138" href="#fn:138"><sup>138</sup></a><a class="footnote-ref" id="fnref:139" href="#fn:139"><sup>139</sup></a> Beryllium powder was itself studied as a <a href="/facts/Rocket_fuel/IyFhQEA2">rocket fuel</a>, but this use has never materialized.<a class="footnote-ref" id="fnref:140" href="#fn:140"><sup>140</sup></a> A small number of extreme high-end <a href="/facts/Bicycle_frame/jnDRoA4z">bicycle frames</a> have been built with beryllium.<a class="footnote-ref" id="fnref:141" href="#fn:141"><sup>141</sup></a> From 1998 to 2000, the <a href="/facts/McLaren/yLYrH3BT">McLaren</a> <a href="/facts/Formula_One/BwdePyWY">Formula One</a> team used <a href="/facts/Mercedes-Benz/pGrJrQHC">Mercedes-Benz</a> engines with <a href="/facts/Beryllium-aluminium_alloy/eost1yM9">beryllium-aluminium alloy</a> pistons.<a class="footnote-ref" id="fnref:142" href="#fn:142"><sup>142</sup></a> The use of beryllium engine components was banned following a protest by <a href="/facts/Scuderia_Ferrari/aa79KuLs">Scuderia Ferrari</a>.<a class="footnote-ref" id="fnref:143" href="#fn:143"><sup>143</sup></a> </p><p>Mixing about 2.0% beryllium into <a href="/facts/Copper/I8PEE8oX">copper</a> forms an <a href="/facts/Alloy/I7w7WQWR">alloy</a> called <a href="/facts/Beryllium_copper/YVPmtURb">beryllium copper</a> that is six times stronger than copper alone.<a class="footnote-ref" id="fnref:144" href="#fn:144"><sup>144</sup></a> Beryllium alloys are used in many applications because of their combination of elasticity, high <a href="/facts/Electrical_conductivity/akyCKvMy">electrical conductivity</a> and <a href="/facts/Thermal_conductivity/qWnSG3nQ">thermal conductivity</a>, high strength and <a href="/facts/Hardness_(materials_science)/PtGn6E20">hardness</a>, nonmagnetic properties, as well as good <a href="/facts/Corrosion/lIC7H4we">corrosion</a> and <a href="/facts/Fatigue_(material)/zmJY8hMt">fatigue resistance</a>.<a class="footnote-ref" id="fnref:145" href="#fn:145"><sup>145</sup></a><a class="footnote-ref" id="fnref:146" href="#fn:146"><sup>146</sup></a> These applications include non-sparking tools that are used near flammable gases (beryllium nickel), <a href="/facts/Spring_(device)/jknGXzTq">springs</a>, membranes (beryllium nickel and beryllium iron) used in surgical instruments, and high temperature devices.<a class="footnote-ref" id="fnref:147" href="#fn:147"><sup>147</sup></a><a class="footnote-ref" id="fnref:148" href="#fn:148"><sup>148</sup></a> As little as 50 parts per million of beryllium alloyed with liquid <a href="/facts/Magnesium/XyIhd2FG">magnesium</a> leads to a significant increase in oxidation resistance and decrease in flammability.<a class="footnote-ref" id="fnref:149" href="#fn:149"><sup>149</sup></a> </p> <p>The high elastic stiffness of beryllium has led to its extensive use in precision instrumentation, e.g. in <a href="/facts/Inertial_guidance/UzUTMhK2">inertial guidance</a> systems and in the support mechanisms for optical systems.<a class="footnote-ref" id="fnref:150" href="#fn:150"><sup>150</sup></a> Beryllium-copper alloys were also applied as a hardening agent in "<a href="/facts/Needlegun_scaler/dPEEkhcC">Jason pistols</a>", which were used to strip the paint from the hulls of ships.<a class="footnote-ref" id="fnref:151" href="#fn:151"><sup>151</sup></a> </p><p>In sound amplification systems, the speed at which sound travels directly affects the resonant frequency of the <a href="/facts/Amplifier/pnRgxncC">amplifier</a>, thereby influencing the range of audible high-frequency sounds. Beryllium stands out due to its exceptionally high speed of sound propagation compared to other metals.<a class="footnote-ref" id="fnref:152" href="#fn:152"><sup>152</sup></a> This unique property allows beryllium to achieve higher resonant frequencies, making it an ideal material for use as a <a href="/facts/Diaphragm_(acoustics)/fYq3PwtC">diaphragm</a> in high-quality loudspeakers.<a class="footnote-ref" id="fnref:153" href="#fn:153"><sup>153</sup></a> </p><p>Beryllium was used for <a href="/facts/Cantilever/Ueu6vIXI">cantilevers</a> in high-performance <a href="/facts/Phonograph/VcNQRYVT">phonograph</a> cartridge styli, where its extreme stiffness and low density allowed for tracking weights to be reduced to 1 gram while still tracking high frequency passages with minimal distortion.<a class="footnote-ref" id="fnref:154" href="#fn:154"><sup>154</sup></a> </p><p>An earlier major application of beryllium was in <a href="/facts/Brake/p8751fV6">brakes</a> for military <a href="/facts/Airplane/81161IpU">airplanes</a> because of its hardness, high melting point, and exceptional ability to <a href="/facts/Heat_dissipation/6WPm3enf">dissipate heat</a>. Environmental considerations have led to substitution by other materials.<a class="footnote-ref" id="fnref:155" href="#fn:155"><sup>155</sup></a> </p><p>A metal matrix composite material combining beryllium with <a href="/facts/Aluminium/7wmR8jYE">aluminium</a> developed under the trade name <a href="/facts/AlBeMet/eost1yM9">AlBeMet</a> for the high performance aerospace industry has low weight but four times the stiffness of aluminum alone.<a class="footnote-ref" id="fnref:156" href="#fn:156"><sup>156</sup></a> </p> <h3>Mirrors</h3> <p>Large-area beryllium <a href="/facts/Mirror/wMu4u6BB">mirrors</a>, frequently with a <a href="/facts/Honeycomb_mirror/q9yCkArI">honeycomb support structure</a>, are used, for example, in <a href="/facts/Meteorological_satellite/yl7QCK8n">meteorological satellites</a> where low weight and long-term dimensional stability are critical. Smaller beryllium mirrors are used in <a href="/facts/Optical_guidance/NSna0Dtk">optical guidance</a> systems and in <a href="/facts/Fire-control_system/HzJ2Nwn4">fire-control systems</a>, e.g. in the German-made <a href="/facts/Leopard_1/EBjHaWfN">Leopard 1</a> and <a href="/facts/Leopard_2/PJEV2Cc2">Leopard 2</a> <a href="/facts/Main_battle_tank/aJz3U1Ta">main battle tanks</a>. In these systems, very rapid movement of the mirror is required, which again dictates low mass and high rigidity. Usually the beryllium mirror is coated with hard <a href="/facts/Electroless_nickel_plating/rtGaEfW3">electroless nickel plating</a> which can be more easily polished to a finer optical finish than beryllium. In some applications, the beryllium blank is polished without any coating. This is particularly applicable to <a href="/facts/Cryogenic/cw7dHAkp">cryogenic</a> operation where thermal expansion mismatch can cause the coating to buckle.<a class="footnote-ref" id="fnref:157" href="#fn:157"><sup>157</sup></a> </p><p>The <a href="/facts/James_Webb_Space_Telescope/w4GAWnWX">James Webb Space Telescope</a> has 18 hexagonal beryllium sections for its mirrors, each plated with a thin layer of gold.<a class="footnote-ref" id="fnref:158" href="#fn:158"><sup>158</sup></a> Because JWST will face a temperature of 33 K, the mirror is made of gold-plated beryllium, which is capable of handling extreme cold better than glass. Beryllium contracts and deforms less than glass and remains more uniform in such temperatures.<a class="footnote-ref" id="fnref:159" href="#fn:159"><sup>159</sup></a> For the same reason, the optics of the <a href="/facts/Spitzer_Space_Telescope/Ic1xXIYb">Spitzer Space Telescope</a> are entirely built of beryllium metal.<a class="footnote-ref" id="fnref:160" href="#fn:160"><sup>160</sup></a> </p> <h3>Magnetic applications</h3> <p>Beryllium is non-magnetic. Therefore, tools fabricated out of beryllium-based materials are used by naval or military <a href="/facts/Explosive_ordnance_disposal/FQJI2y4b">explosive ordnance disposal</a> teams for work on or near <a href="/facts/Naval_mine/jo9uVY9U">naval mines</a>, since these mines commonly have <a href="/facts/Fuze/uGhu5xbF">magnetic fuzes</a>.<a class="footnote-ref" id="fnref:161" href="#fn:161"><sup>161</sup></a> They are also found in maintenance and construction materials near <a href="/facts/Magnetic_resonance_imaging/Vh9yG9qq">magnetic resonance imaging</a> (MRI) machines because of the high magnetic fields generated.<a class="footnote-ref" id="fnref:162" href="#fn:162"><sup>162</sup></a> </p> <h3>Nuclear applications</h3> <p>High purity beryllium can be used in nuclear reactors as a moderator,<a class="footnote-ref" id="fnref:163" href="#fn:163"><sup>163</sup></a> reflector, or as cladding on fuel elements.<a class="footnote-ref" id="fnref:164" href="#fn:164"><sup>164</sup></a><a class="footnote-ref" id="fnref:165" href="#fn:165"><sup>165</sup></a> Thin plates or foils of beryllium are sometimes used in <a href="/facts/Nuclear_weapon_design/gw0LEc74">nuclear weapon designs</a> as the very outer layer of the <a href="/facts/Plutonium_pit/8HGl80tM">plutonium pits</a> in the primary stages of <a href="/facts/Thermonuclear_bomb/T9zFe3H0">thermonuclear bombs</a>, placed to surround the <a href="/facts/Fissile/XJR9qoxW">fissile</a> material. These layers of beryllium are good "pushers" for the <a href="/facts/Implosion_(mechanical_process)/sQ2J2wQk">implosion</a> of the <a href="/facts/Plutonium-239/eRobTXos">plutonium-239</a>, and they are good <a href="/facts/Neutron_reflector/yDkgmcrE">neutron reflectors</a>, just as in beryllium-moderated <a href="/facts/Nuclear_reactors/8xqjIbge">nuclear reactors</a>.<a class="footnote-ref" id="fnref:166" href="#fn:166"><sup>166</sup></a> </p><p>Beryllium is commonly used in some <a href="/facts/Neutron_source/4BTQAu9l">neutron sources</a> in laboratory devices in which relatively few neutrons are needed (rather than having to use a nuclear reactor or a <a href="/facts/Particle_accelerator/Pkuc08xC">particle accelerator</a>-powered <a href="/facts/Neutron_generator/0cvpTvLu">neutron generator</a>). For this purpose, a target of beryllium-9 is bombarded with energetic alpha particles from a <a href="/facts/Radioisotope/5WpCfbdq">radioisotope</a> such as <a href="/facts/Polonium/G4rzsyjP">polonium</a>-210, <a href="/facts/Radium/VWo5gkzn">radium</a>-226, <a href="/facts/Plutonium/4bUw9zH3">plutonium</a>-238, or <a href="/facts/Americium/rxL9Yc64">americium</a>-241. In the nuclear reaction that occurs, a beryllium nucleus is <a href="/facts/Nuclear_transmutation/MjlvjsV6">transmuted</a> into carbon-12, and one free neutron is emitted, traveling in about the same direction as the alpha particle was heading. Such <a href="/facts/Alpha_decay/rCsHNIUE">alpha decay</a>-driven beryllium neutron sources, named <a href="/facts/Modulated_neutron_initiator/DfBSYYHE">"urchin"</a> neutron initiators, were used in some early <a href="/facts/Atomic_bomb/QVdBcMdm">atomic bombs</a>.<a class="footnote-ref" id="fnref:167" href="#fn:167"><sup>167</sup></a> Neutron sources in which beryllium is bombarded with <a href="/facts/Gamma_ray/5Drf913J">gamma rays</a> from a <a href="/facts/Gamma_decay/5Drf913J">gamma decay</a> radioisotope are also used to produce laboratory neutrons.<a class="footnote-ref" id="fnref:168" href="#fn:168"><sup>168</sup></a> </p> <p>Beryllium is used in fuel fabrication for <a href="/facts/CANDU/fAKl2X0L">CANDU</a> reactors. The fuel elements have small appendages that are resistance brazed to the fuel cladding using an induction brazing process with Be as the braze filler material. Bearing pads are brazed in place to prevent contact between the fuel bundle and the pressure tube containing it, and inter-element spacer pads are brazed on to prevent element to element contact.<a class="footnote-ref" id="fnref:169" href="#fn:169"><sup>169</sup></a> </p><p>Beryllium is used at the <a href="/facts/Joint_European_Torus/faIvLnuY">Joint European Torus</a> <a href="/facts/Nuclear_fusion/hP0gLDqj">nuclear-fusion research laboratory</a>, and it will be used in the more advanced <a href="/facts/ITER/SkpWL87b">ITER</a> to condition the components which face the plasma.<a class="footnote-ref" id="fnref:170" href="#fn:170"><sup>170</sup></a> Beryllium has been proposed as a <a href="/facts/Cladding_(nuclear_fuel)/8RhAomlJ">cladding</a> material for <a href="/facts/Nuclear_fuel_rod/8RhAomlJ">nuclear fuel rods</a>, because of its good combination of mechanical, chemical, and nuclear properties.<a class="footnote-ref" id="fnref:171" href="#fn:171"><sup>171</sup></a> <a href="/facts/Beryllium_fluoride/4wkNdddq">Beryllium fluoride</a> is one of the constituent salts of the eutectic salt mixture <a href="/facts/FLiBe/z8wD05ur">FLiBe</a>, which is used as a solvent, moderator and coolant in many hypothetical <a href="/facts/Molten_salt_reactor/aSvp1qTG">molten salt reactor</a> designs, including the <a href="/facts/Liquid_fluoride_thorium_reactor/3BQ1QVjV">liquid fluoride thorium reactor</a> (LFTR).<a class="footnote-ref" id="fnref:172" href="#fn:172"><sup>172</sup></a> </p> <h3>Acoustics</h3> <p>The low weight and high rigidity of beryllium make it useful as a material for high-frequency <a href="/facts/Speaker_driver/x3cJaElv">speaker drivers</a>. Because beryllium is expensive (many times more than <a href="/facts/Titanium/53ArnDoy">titanium</a>), hard to shape due to its brittleness, and toxic if mishandled, beryllium <a href="/facts/Tweeter/UrmRhLj1">tweeters</a> are limited to high-end home,<a class="footnote-ref" id="fnref:173" href="#fn:173"><sup>173</sup></a><a class="footnote-ref" id="fnref:174" href="#fn:174"><sup>174</sup></a><a class="footnote-ref" id="fnref:175" href="#fn:175"><sup>175</sup></a> <a href="/facts/Pro_audio/6UyA7U4m">pro audio</a>, and <a href="/facts/Public_address/LlLkJgNz">public address</a> applications.<a class="footnote-ref" id="fnref:176" href="#fn:176"><sup>176</sup></a><a class="footnote-ref" id="fnref:177" href="#fn:177"><sup>177</sup></a> Some high-fidelity products have been fraudulently claimed to be made of the material.<a class="footnote-ref" id="fnref:178" href="#fn:178"><sup>178</sup></a> </p><p>Some high-end <a href="/facts/Magnetic_cartridge/pyfetbvl">phonograph cartridges</a> used beryllium cantilevers to improve tracking by reducing mass.<a class="footnote-ref" id="fnref:179" href="#fn:179"><sup>179</sup></a> </p> <h3>Electronic</h3> <p>Beryllium is a <a href="/facts/P-type_semiconductor/d9GPL5tV">p-type</a> <a href="/facts/Dopant/DvChmeRL">dopant</a> in <a href="/facts/List_of_semiconductor_materials/RMcsYTWQ">III-V compound semiconductors</a>. It is widely used in materials such as <a href="/facts/Gallium_arsenide/BakLFjpp">GaAs</a>, <a href="/facts/AlGaAs/mX3tGQB4">AlGaAs</a>, <a href="/facts/InGaAs/DAHNSFPr">InGaAs</a> and <a href="/facts/InAlAs/dUcEVoR3">InAlAs</a> grown by <a href="/facts/Molecular_beam_epitaxy/zIhe0lMv">molecular beam epitaxy</a> (MBE).<a class="footnote-ref" id="fnref:180" href="#fn:180"><sup>180</sup></a> Cross-rolled beryllium sheet is an excellent structural support for <a href="/facts/Printed_circuit_board/muSR2p43">printed circuit boards</a> in <a href="/facts/Surface-mount_technology/SjFyQbbm">surface-mount technology</a>. In critical electronic applications, beryllium is both a structural support and <a href="/facts/Heat_sink/ccIEdHnq">heat sink</a>. The application also requires a coefficient of <a href="/facts/Thermal_expansion/BP2vjX0N">thermal expansion</a> that is well matched to the alumina and <a href="/facts/Glass-reinforced_plastic/T6MtJ4ep">polyimide-glass</a> <a href="/facts/Substrate_(materials_science)/LwwkV6rX">substrates</a>. The beryllium-beryllium oxide <a href="/facts/Metal_matrix_composite/cWKqblzk">composite</a> "<a href="/facts/E-Material/b3NJFX3d">E-Materials</a>" have been specially designed for these electronic applications and have the additional advantage that the thermal expansion coefficient can be tailored to match diverse substrate materials.<a class="footnote-ref" id="fnref:181" href="#fn:181"><sup>181</sup></a> </p><p><a href="/facts/Beryllium_oxide/o3VnG96d">Beryllium oxide</a> is useful for many applications that require the combined properties of an <a href="/facts/Electrical_insulator/SfSXkrh5">electrical insulator</a> and an excellent heat conductor, with high strength and hardness and a very high melting point. Beryllium oxide is frequently used as an insulator base plate in <a href="/facts/Power_semiconductor_device/5c22S6E6">high-power</a> <a href="/facts/Transistor/Bmr8zwL0">transistors</a> in <a href="/facts/Radio_frequency/aWku7h4R">radio frequency</a> <a href="/facts/Transmitter/nFYghtKv">transmitters</a> for telecommunications. Beryllium oxide is being studied for use in increasing the <a href="/facts/Thermal_conductivity/qWnSG3nQ">thermal conductivity</a> of <a href="/facts/Uranium_dioxide/BqI7GJDq">uranium dioxide</a> <a href="/facts/Nuclear_fuel/8RhAomlJ">nuclear fuel</a> pellets.<a class="footnote-ref" id="fnref:182" href="#fn:182"><sup>182</sup></a> Beryllium compounds were used in <a href="/facts/Fluorescent_light/R8SlXCyg">fluorescent lighting</a> tubes, but this use was discontinued because of the disease <a href="/facts/Berylliosis/yELbTj7r">berylliosis</a> which developed in the workers who were making the tubes.<a class="footnote-ref" id="fnref:183" href="#fn:183"><sup>183</sup></a> </p> <h3>Medical applications</h3> <p>Beryllium is a component of several <a href="/facts/Dental_material/BkjBRwl7">dental alloys</a>.<a class="footnote-ref" id="fnref:184" href="#fn:184"><sup>184</sup></a><a class="footnote-ref" id="fnref:185" href="#fn:185"><sup>185</sup></a> Beryllium is used in X-ray windows because it is transparent to X-rays, allowing for clearer and more efficient imaging.<a class="footnote-ref" id="fnref:186" href="#fn:186"><sup>186</sup></a> In medical imaging equipment, such as CT scanners and mammography machines, beryllium's strength and light weight enhance durability and performance.<a class="footnote-ref" id="fnref:187" href="#fn:187"><sup>187</sup></a> Beryllium is used in analytical equipment for blood, HIV, and other diseases.<a class="footnote-ref" id="fnref:188" href="#fn:188"><sup>188</sup></a> Beryllium alloys are used in surgical instruments, optical mirrors, and laser systems for medical treatments.<a class="footnote-ref" id="fnref:189" href="#fn:189"><sup>189</sup></a><a class="footnote-ref" id="fnref:190" href="#fn:190"><sup>190</sup></a> </p> <h2 id="toxicity-and-safety">Toxicity and safety</h2> <p class="note">Main articles: <a href="/facts/Acute_beryllium_poisoning/pTzLBaNe">Acute beryllium poisoning</a> and <a href="/facts/Berylliosis/yELbTj7r">Berylliosis</a></p> <h3>Biological effects</h3> <p>Approximately 35 micrograms of beryllium is found in the average human body, an amount not considered harmful.<a class="footnote-ref" id="fnref:191" href="#fn:191"><sup>191</sup></a> Beryllium is chemically similar to <a href="/facts/Magnesium/XyIhd2FG">magnesium</a> and therefore can displace it from <a href="/facts/Enzyme/DSI1Fh7y">enzymes</a>, which causes them to malfunction.<a class="footnote-ref" id="fnref:192" href="#fn:192"><sup>192</sup></a> Because Be2+ is a highly charged and small ion, it can easily get into many tissues and cells, where it specifically targets cell nuclei, inhibiting many enzymes, including those used for synthesizing DNA. Its toxicity is exacerbated by the fact that the body has no means to control beryllium levels, and once inside the body, beryllium cannot be removed.<a class="footnote-ref" id="fnref:193" href="#fn:193"><sup>193</sup></a> </p> <h3>Inhalation</h3> <p>Chronic beryllium disease (CBD), or <a href="/facts/Berylliosis/yELbTj7r">berylliosis</a>, is a <a href="/facts/Pulmonary/gTWXI6Fj">pulmonary</a> and <a href="/facts/Systemic_circulation/WXwudzzc">systemic</a> <a href="/facts/Granuloma/mqEhHfjS">granulomatous</a> disease caused by inhalation of dust or fumes contaminated with beryllium; either large amounts over a short time or small amounts over a long time can lead to this ailment. Symptoms of the disease can take up to five years to develop; about a third of patients with it die and the survivors are left disabled.<a class="footnote-ref" id="fnref:194" href="#fn:194"><sup>194</sup></a> The <a href="/facts/International_Agency_for_Research_on_Cancer/Pb8KPyTz">International Agency for Research on Cancer</a> (IARC) lists beryllium and beryllium compounds as <a href="/facts/List_of_IARC_Group_1_carcinogens/EY8MuDwQ">Category 1 carcinogens</a>.<a class="footnote-ref" id="fnref:195" href="#fn:195"><sup>195</sup></a> </p> <h3>Occupational exposure</h3> <p>In the US, the <a href="/facts/Occupational_Safety_and_Health_Administration/dCGbW5Ax">Occupational Safety and Health Administration</a> (OSHA) has designated a <a href="/facts/Permissible_exposure_limit/IrQeETWy">permissible exposure limit</a> (PEL) for beryllium and beryllium compounds of 0.2 μg/m3 as an 8-hour time-weighted average (TWA) and 2.0 μg/m3 as a <a href="/facts/Short-term_exposure_limit/RHSQtE4z">short-term exposure limit</a> over a sampling period of 15 minutes. The <a href="/facts/National_Institute_for_Occupational_Safety_and_Health/5WjdDNMN">National Institute for Occupational Safety and Health</a> (NIOSH) has set a <a href="/facts/Recommended_exposure_limit/nexWYeNv">recommended exposure limit</a> (REL) upper-bound threshold of 0.5 μg/m3. The <a href="/facts/IDLH/ektUbSdQ">IDLH</a> (immediately dangerous to life and health) value is 4 mg/m3.<a class="footnote-ref" id="fnref:196" href="#fn:196"><sup>196</sup></a> The toxicity of beryllium is on par with other toxic metalloids/metals, such as <a href="/facts/Arsenic/k1c4f44D">arsenic</a> and <a href="/facts/Mercury_(element)/WlxfoHva">mercury</a>.<a class="footnote-ref" id="fnref:197" href="#fn:197"><sup>197</sup></a><a class="footnote-ref" id="fnref:198" href="#fn:198"><sup>198</sup></a> </p><p>Exposure to beryllium in the workplace can lead to a sensitized immune response, and over time development of <a href="/facts/Berylliosis/yELbTj7r">berylliosis</a>.<a class="footnote-ref" id="fnref:199" href="#fn:199"><sup>199</sup></a> NIOSH in the United States researches these effects in collaboration with a major manufacturer of beryllium products. NIOSH also conducts genetic research on sensitization and CBD, independently of this collaboration.<a class="footnote-ref" id="fnref:200" href="#fn:200"><sup>200</sup></a> </p><p>Acute beryllium disease in the form of <a href="/facts/Chemical_pneumonitis/YMGoFwe3">chemical pneumonitis</a> was first reported in Europe in 1933 and in the United States in 1943. A survey found that about 5% of workers in plants manufacturing <a href="/facts/Fluorescent_lamp/R8SlXCyg">fluorescent lamps</a> in 1949 in the United States had beryllium-related lung diseases.<a class="footnote-ref" id="fnref:201" href="#fn:201"><sup>201</sup></a> Chronic berylliosis resembles <a href="/facts/Sarcoidosis/qgV7Uoe8">sarcoidosis</a> in many respects, and the <a href="/facts/Differential_diagnosis/jLqnn5hA">differential diagnosis</a> is often difficult. It killed some early workers in nuclear weapons design, such as <a href="/facts/Herbert_L._Anderson/49KskgsX">Herbert L. Anderson</a>.<a class="footnote-ref" id="fnref:202" href="#fn:202"><sup>202</sup></a> </p><p>Beryllium may be found in coal slag. When the slag is formulated into an abrasive agent for blasting paint and rust from hard surfaces, the beryllium can become airborne and become a source of exposure.<a class="footnote-ref" id="fnref:203" href="#fn:203"><sup>203</sup></a> </p><p>Although the use of beryllium compounds in fluorescent lighting tubes was discontinued in 1949, potential for exposure to beryllium exists in the nuclear and aerospace industries, in the refining of beryllium metal and the melting of beryllium-containing alloys, in the manufacturing of electronic devices, and in the handling of other beryllium-containing material.<a class="footnote-ref" id="fnref:204" href="#fn:204"><sup>204</sup></a> </p> <h3>Detection</h3> <p>Early researchers undertook the highly hazardous practice of identifying beryllium and its various compounds from its sweet taste. A modern test for beryllium in air and on surfaces has been developed and published as an international voluntary consensus standard, ASTM D7202. The procedure uses dilute <a href="/facts/Ammonium_bifluoride/F433DsdE">ammonium bifluoride</a> for dissolution and fluorescence detection with beryllium bound to sulfonated hydroxybenzoquinoline, allowing up to 100 times more sensitive detection than the recommended limit for beryllium concentration in the workplace. Fluorescence increases with increasing beryllium concentration. The new procedure has been successfully tested on a variety of surfaces and is effective for the dissolution and detection of refractory beryllium oxide and siliceous beryllium in minute concentrations (ASTM D7458).<a class="footnote-ref" id="fnref:205" href="#fn:205"><sup>205</sup></a><a class="footnote-ref" id="fnref:206" href="#fn:206"><sup>206</sup></a> The NIOSH Manual of Analytical Methods contains methods for measuring occupational exposures to beryllium.<a class="footnote-ref" id="fnref:207" href="#fn:207"><sup>207</sup></a> </p> <h2 id="notes">Notes</h2> <h2 id="cited-sources">Cited sources</h2> <ul><li>Emsley, John (2001). <a href="https://archive.org/details/naturesbuildingb0000emsl"><i>Nature's Building Blocks: An A–Z Guide to the Elements</i></a>. Oxford, England, UK: Oxford University Press. <a href="/facts/ISBN_(identifier)/15AdSPa9">ISBN</a> 978-0-19-850340-8.</li> <li><a href="/facts/Mary_Elvira_Weeks/eklpr8u4">Weeks, Mary Elvira</a>; Leichester, Henry M. (1968). <a href="https://archive.org/details/discoveryoftheel002045mbp"><i>Discovery of the Elements</i></a>. Easton, PA: Journal of Chemical Education. LCCCN 68-15217.</li></ul> <h2 id="further-reading">Further reading</h2> <ul><li>Newman LS (2003). "Beryllium". <i>Chemical & Engineering News</i>. 81 (36): 38. <a href="/facts/Doi_(identifier)/muM9Etpq">doi</a>:<a href="https://doi.org/10.1021%2Fcen-v081n036.p038">10.1021/cen-v081n036.p038</a>.</li> <li>Mroz MM, Balkissoon R, and Newman LS. "Beryllium". In: Bingham E, Cohrssen B, Powell C (eds.) <i>Patty's Toxicology</i>, Fifth Edition. New York: John Wiley & Sons 2001, 177–220.</li> <li>Walsh, KA, <a href="https://books.google.com/books?id=3-GbhmSfyeYC"><i>Beryllium Chemistry and Processing</i></a>. Vidal, EE. et al. Eds. 2009, Materials Park, OH:ASM International.</li> <li><a href="https://web.archive.org/web/20190207015758/http://www.bjorklundnutrition.net/2011/11/belpt/">Beryllium Lymphocyte Proliferation Testing (BeLPT).</a> DOE Specification 1142–2001. Washington, DC: U.S. Department of Energy, 2001.</li></ul> <h2 id="external-links">External links</h2> <ul><li><a href="https://www.atsdr.cdc.gov/csem/csem.html">ATSDR Case Studies in Environmental Medicine: Beryllium Toxicity</a> <a href="https://web.archive.org/web/20160204174821/http://www.atsdr.cdc.gov/csem/csem.asp?csem=7&po=7">Archived</a> 4 February 2016 at the <a href="/facts/Wayback_Machine/nmQ3a6JC">Wayback Machine</a> U.S. <a href="/facts/Department_of_Health_and_Human_Services/eS90vYmd">Department of Health and Human Services</a></li> <li><a href="http://education.jlab.org/itselemental/ele004.html">It's Elemental – Beryllium</a></li> <li><a href="/facts/MSDS/jbshEV2W">MSDS</a>: <a href="https://web.archive.org/web/20070928003708/http://espi-metals.com/msds%27s/beryllium.pdf">ESPI Metals</a></li> <li><a href="http://www.periodicvideos.com/videos/004.htm">Beryllium</a> at <i><a href="/facts/The_Periodic_Table_of_Videos/vC5kbN0M">The Periodic Table of Videos</a></i> (University of Nottingham)</li> <li><a href="https://www.cdc.gov/niosh/topics/beryllium/">National Institute for Occupational Safety and Health – Beryllium Page</a></li> <li><a href="http://www.orau.org/nssp/">National Supplemental Screening Program (Oak Ridge Associated Universities)</a></li> <li><a href="https://minerals.usgs.gov/minerals/pubs/commodity/beryllium/100798.pdf">Historic Price of Beryllium in USA</a></li></ul> <h2 id="references">References</h2> <ol> <li id="fn:1"><p>Jakubke, Hans-Dieter; Jeschkeit, Hans, eds. (1994). Concise Encyclopedia Chemistry. trans. rev. Eagleson, Mary. Berlin: Walter de Gruyter. <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li> <li id="fn:2"><p>Jakubke, Hans-Dieter; Jeschkeit, Hans, eds. (1994). Concise Encyclopedia Chemistry. trans. rev. Eagleson, Mary. Berlin: Walter de Gruyter. <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li> <li id="fn:3"><p>Jakubke, Hans-Dieter; Jeschkeit, Hans, eds. (1994). Concise Encyclopedia Chemistry. trans. rev. Eagleson, Mary. Berlin: Walter de Gruyter. <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li> <li id="fn:4"><p>Hoover, Mark D.; Castorina, Bryan T.; Finch, Gregory L.; Rothenberg, Simon J. (October 1989). "Determination of the Oxide Layer Thickness on Beryllium Metal Particles". American Industrial Hygiene Association Journal. 50 (10): 550–553. doi:10.1080/15298668991375146. ISSN 0002-8894. 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