Barium sulfide: Difference between revisions
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{{distinguish|Barium sulfate}} |
{{distinguish|Barium sulfate}} |
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{{chembox |
{{chembox |
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| Watchedfields = changed |
| Watchedfields = changed |
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| verifiedrevid = 443414470 |
| verifiedrevid = 443414470 |
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| ImageFile = NaCl polyhedra.png |
| ImageFile = NaCl polyhedra.png |
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| ImageSize = |
| ImageSize = |
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| IUPACName = |
| IUPACName = |
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| OtherNames = |
| OtherNames = |
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|Section1={{Chembox Identifiers |
|Section1={{Chembox Identifiers |
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| InChI = 1/Ba.S/q+2;-2 |
| InChI = 1/Ba.S/q+2;-2 |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| Gmelin = 13627 |
| Gmelin = 13627 |
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|Section2={{Chembox Properties |
|Section2={{Chembox Properties |
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| Formula = |
| Formula = |
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| Ba=1 | S=1 |
| Ba=1 | S=1 |
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| Appearance = white solid |
| Appearance = white solid |
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| Density = 4.25 g/cm<sup>3</sup> <ref>{{RubberBible87th}}</ref> |
| Density = 4.25 g/cm<sup>3</sup> <ref>{{RubberBible87th}}</ref> |
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| MeltingPtC = 2235<ref name=Stinn2017>Stinn, C., Nose, K., Okabe, T. et al. Metall and Materi Trans B (2017) 48: 2922. https://doi.org/10.1007/s11663-017-1107-5</ref> |
| MeltingPtC = 2235<ref name=Stinn2017>Stinn, C., Nose, K., Okabe, T. et al. Metall and Materi Trans B (2017) 48: 2922. https://doi.org/10.1007/s11663-017-1107-5</ref> |
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| MeltingPt_notes = |
| MeltingPt_notes = |
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| BoilingPt = decomposes |
| BoilingPt = decomposes |
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| RefractIndex = 2.155 |
| RefractIndex = 2.155 |
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}} |
}} |
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|Section3={{Chembox Structure |
|Section3={{Chembox Structure |
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| CrystalStruct = [[Halite]] (cubic), [[Pearson symbol|cF8]] |
| CrystalStruct = [[Halite]] (cubic), [[Pearson symbol|cF8]] |
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| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225 |
| SpaceGroup = Fm<u style="text-decoration:overline">3</u>m, No. 225 |
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| LattConst_a = |
| LattConst_a = |
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}} |
}} |
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|Section7={{Chembox Hazards |
|Section7={{Chembox Hazards |
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| GHSPictograms = {{GHS07}}{{GHS09}} |
| GHSPictograms = {{GHS07}}{{GHS09}} |
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| GHSSignalWord = Warning |
| GHSSignalWord = Warning |
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| NFPA-R = 2 |
| NFPA-R = 2 |
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|Section8={{Chembox Related |
|Section8={{Chembox Related |
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| OtherAnions = [[Barium oxide]] |
| OtherAnions = [[Barium oxide]] |
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| OtherCations = [[Magnesium sulfide]]<br/>[[Calcium sulfide]]<br/>[[Strontium sulfide]] |
| OtherCations = [[Magnesium sulfide]]<br/>[[Calcium sulfide]]<br/>[[Strontium sulfide]] |
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| OtherFunction = |
| OtherFunction = |
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| OtherFunction_label = |
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'''Barium sulfide''' is the [[inorganic compound]] with the formula [[Barium|Ba]][[Sulfide|S]]. BaS is the barium compound produced on the largest scale.<ref>{{Greenwood&Earnshaw2nd|paage=678}}</ref> It is an important precursor to other barium compounds including BaCO<sub>3</sub> and the pigment [[lithopone]], ZnS/BaSO<sub>4</sub>.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref> Like other [[chalcogenide]]s of the alkaline earth metals, BaS is a short [[wavelength]] emitter for [[electronic display]]s.<ref>{{cite conference|last1=Vij|first1=D. R.|last2=Singh|first2= N. |title=Optical and electrical properties of II-VI wide gap semiconducting barium sulfide|journal=[[Proceedings of SPIE]] |year=1992|volume=1523 |conference=Conf. Phys. Technol. Semicond. Devices Integr. Circuits, 1992| |
'''Barium sulfide''' is the [[inorganic compound]] with the formula [[Barium|Ba]][[Sulfide|S]]. BaS is the barium compound produced on the largest scale.<ref>{{Greenwood&Earnshaw2nd|paage=678}}</ref> It is an important precursor to other barium compounds including BaCO<sub>3</sub> and the pigment [[lithopone]], ZnS/BaSO<sub>4</sub>.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref> Like other [[chalcogenide]]s of the alkaline earth metals, BaS is a short [[wavelength]] emitter for [[electronic display]]s.<ref>{{cite conference|last1=Vij|first1=D. R.|last2=Singh|first2= N. |title=Optical and electrical properties of II-VI wide gap semiconducting barium sulfide|journal=[[Proceedings of SPIE]] |year=1992|volume=1523 |conference=Conf. Phys. Technol. Semicond. Devices Integr. Circuits, 1992|= |doi=10.1117/12.634082|bibcode=1992SPIE.1523..608V}}</ref> It is colorless, although like many sulfides, it is commonly obtained in impure colored forms. |
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==Discovery== |
==Discovery== |
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BaS was prepared by the Italian alchemist |
BaS was prepared by the Italian alchemist (or Vincentinus Casciarolus or Casciorolus, 1571–1624) via the thermo-chemical reduction of [[barium sulfate|BaSO<sub>4</sub>]] (available as the mineral [[barite]]).<ref>F. Licetus, Litheosphorus, sive de lapide Bononiensi lucem in se conceptam ab ambiente claro mox in tenebris mire conservante, Utini, ex typ. N. Schiratti, 1640. See http://www.chem.leeds.ac.uk/delights/texts/Demonstration_21.htm {{Webarchive|url=https://web.archive.org/web/20110813075857/http://www1.chem.leeds.ac.uk/delights/texts/Demonstration_21.htm |date=2011-08-13 }}</ref> It is currently manufactured by an improved version of 's process using [[coke (fuel)|coke]] in place of flour and [[charcoal]]. This kind of conversion is called a [[carbothermic reaction]]: |
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: |
: + → BaS + |
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and also: |
and also: |
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: |
: + → BaS + |
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The basic method remains in use today. BaS dissolves in water. These aqueous solutions, when treated with [[sodium carbonate]] or [[carbon dioxide]], give a white solid of [[barium carbonate]], a source material for many commercial barium compounds.<ref name=Ull>{{Ullmann |doi=10.1002/14356007.a03_325.pub2|title=Barium and Barium Compounds|year=2007|last1=Kresse|first1=Robert|last2=Baudis|first2=Ulrich|last3=Jäger|first3=Paul|last4=Riechers|first4=H. Hermann|last5=Wagner|first5=Heinz|last6=Winkler|first6=Jochen|last7=Wolf|first7=Hans Uwe|isbn=978-3527306732}}</ref> |
The basic method remains in use today. BaS dissolves in water. These aqueous solutions, when treated with [[sodium carbonate]] or [[carbon dioxide]], give a white solid of [[barium carbonate]], a source material for many commercial barium compounds.<ref name=Ull>{{Ullmann |doi=10.1002/14356007.a03_325.pub2|title=Barium and Barium Compounds|year=2007|last1=Kresse|first1=Robert|last2=Baudis|first2=Ulrich|last3=Jäger|first3=Paul|last4=Riechers|first4=H. Hermann|last5=Wagner|first5=Heinz|last6=Winkler|first6=Jochen|last7=Wolf|first7=Hans Uwe|isbn=978-3527306732}}</ref> |
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According to Harvey (1957),<ref name="Harvey_1957">Harvey E. Newton (1957). A History of Luminescence: From the Earliest Times until 1900. Memoirs of the American Physical Society, Philadelphia, J. H. FURST Company, Baltimore, Maryland (USA), Vol. 44, Chapter 1, pp. 11-43.</ref> in 1603, Vincenzo Cascariolo used [[barite]], found at the bottom of Mount Paterno near [[Bologna]], in one of his non-fruitful attempts to produce [[gold]]. After grinding and heating the mineral with charcoal under reducing conditions, he obtained a persistent [[luminescence|luminescent]] material rapidly called ''Lapis Boloniensis'', or Bolognian stone.<ref name="Smet_2010">{{cite journal|last1=Smet|first1=Philippe F.|last2=Moreels|first2=Iwan|last3=Hens|first3=Zeger|last4=Poelman|first4=Dirk|title=Luminescence in Sulfides: A Rich History and a Bright Future|journal=Materials|volume=3|issue=4|year=2010|pages=2834–2883|issn=1996-1944|doi=10.3390/ma3042834|bibcode=2010Mate....3.2834S|doi-access=free}}</ref><ref name="Hardev_2014">{{Cite web |title=History of Luminescence from Ancient to Modern Times |author=Hardev Singh Virk |work=ResearchGate |date=2014 |access-date=6 March 2021 |url= https://www.researchgate.net/publication/259713568}}</ref> The [[phosphorescence]] of the material obtained by Casciarolo made it a curiosity.<ref>{{cite web |
According to Harvey (1957),<ref name="Harvey_1957">Harvey E. Newton (1957). A History of Luminescence: From the Earliest Times until 1900. Memoirs of the American Physical Society, Philadelphia, J. H. FURST Company, Baltimore, Maryland (USA), Vol. 44, Chapter 1, pp. 11-43.</ref> in 1603, Vincenzo Cascariolo used [[barite]], found at the bottom of Mount Paterno near [[Bologna]], in one of his non-fruitful attempts to produce [[gold]]. After grinding and heating the mineral with charcoal under reducing conditions, he obtained a persistent [[luminescence|luminescent]] material rapidly called ''Lapis Boloniensis'', or Bolognian stone.<ref name="Smet_2010">{{cite journal|last1=Smet|first1=Philippe F.|last2=Moreels|first2=Iwan|last3=Hens|first3=Zeger|last4=Poelman|first4=Dirk|title=Luminescence in Sulfides: A Rich History and a Bright Future|journal=Materials|volume=3|issue=4|year=2010|pages=2834–2883|issn=1996-1944|doi=10.3390/ma3042834|bibcode=2010Mate....3.2834S|doi-access=free}}</ref><ref name="Hardev_2014">{{Cite web |title=History of Luminescence from Ancient to Modern Times |author=Hardev Singh Virk |work=ResearchGate |date=2014 |access-date=6 March 2021 |url= https://www.researchgate.net/publication/259713568}}</ref> The [[phosphorescence]] of the material obtained by Casciarolo made it a curiosity.<ref>{{cite web| url = http://www.zeno.org/Lemery-1721/A/Lapis+Boloniensis| title = Lapis Boloniensis| publisher = www.zeno.org}}</ref><ref>{{cite book | url = https://books.google.com/books?id=K25AAAAAcAAJ&pg=PA458 | title =Trait℗e universel des drogues simples | author1 = Lemery, Nicolas | year = 1714 }}</ref><ref>{{cite book | url = https://books.google.com/books?id=jAYAAAAAQAAJ&pg=PA411| title =Recreations in mathematics and natural philosophy .. | author1 = Ozanam, Jacques | author2 = Montucla, Jean Etienne | author3 = Hutton, Charles | year = 1814 }}</ref> |
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==Preparation== |
==Preparation== |
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A modern procedure proceeds from barium carbonate:<ref name=Brauer>{{cite book|author1=P. Ehrlich|chapter=Alkaline Earth Metals|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY,NY|volume=2pages=937}}</ref> |
A modern procedure proceeds from barium carbonate:<ref name=Brauer>{{cite book|author1=P. Ehrlich|chapter=Alkaline Earth Metals|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor=G. Brauer|publisher=Academic Press|year=1963|place=NY,NY|volume=2pages=937}}</ref> |
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:{{chem2|BaCO3 + H2S -> BaS + H2O + CO2}} |
:{{chem2|BaCO3 + H2S -> BaS + H2O + CO2}} |
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BaS crystallizes with the [[NaCl structure]], featuring octahedral Ba<sup>2+</sup> and S<sup>2−</sup> centres. |
BaS crystallizes with the [[NaCl structure]], featuring octahedral Ba<sup>2+</sup> and S<sup>2−</sup> centres. |
Latest revision as of 08:24, 8 July 2024
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Identifiers | |
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3D model (JSmol)
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ChEBI | |
ChemSpider | |
ECHA InfoCard | 100.040.180 |
EC Number |
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13627 | |
PubChem CID
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UNII | |
CompTox Dashboard (EPA)
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Properties | |
BaS | |
Molar mass | 169.39 g/mol |
Appearance | white solid |
Density | 4.25 g/cm3 [1] |
Melting point | 2,235[2] °C (4,055 °F; 2,508 K) |
Boiling point | decomposes |
2.88 g/100 mL (0 °C) 7.68 g/100 mL (20 °C) 60.3 g/100 mL (100 °C) (reacts) | |
Solubility | insoluble in alcohol |
Refractive index (nD)
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2.155 |
Structure | |
Halite (cubic), cF8 | |
Fm3m, No. 225 | |
Octahedral (Ba2+); octahedral (S2−) | |
Hazards | |
GHS labelling: | |
![]() ![]() | |
Warning | |
H315, H319, H335, H400 | |
P261, P264, P271, P273, P280, P302+P352, P304+P340, P305+P351+P338, P312, P321, P332+P313, P337+P313, P362, P391, P403+P233, P405, P501 | |
NFPA 704 (fire diamond) | |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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226 mg/kg humans |
Related compounds | |
Other anions
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Barium oxide Barium selenide Barium telluride Barium polonide |
Other cations
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Beryllium sulfide Magnesium sulfide Calcium sulfide Strontium sulfide Radium sulfide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Barium sulfide is the inorganic compound with the formula BaS. BaS is the barium compound produced on the largest scale.[3] It is an important precursor to other barium compounds including BaCO3 and the pigment lithopone, ZnS/BaSO4.[4] Like other chalcogenides of the alkaline earth metals, BaS is a short wavelength emitter for electronic displays.[5] It is colorless, although like many sulfides, it is commonly obtained in impure colored forms.
Discovery
[edit]BaS was prepared by the Italian alchemist Vincenzo Cascariolo (also known as Vincentius or Vincentinus Casciarolus or Casciorolus, 1571–1624) via the thermo-chemical reduction of BaSO4 (available as the mineral barite).[6] It is currently manufactured by an improved version of Cascariolo's process using coke in place of flour and charcoal. This kind of conversion is called a carbothermic reaction:
- BaSO4 + 2C → BaS + 2CO2
and also:
- BaSO4 + 4C → BaS + 4CO
The basic method remains in use today. BaS dissolves in water. These aqueous solutions, when treated with sodium carbonate or carbon dioxide, give a white solid of barium carbonate, a source material for many commercial barium compounds.[7]
According to Harvey (1957),[8] in 1603, Vincenzo Cascariolo used barite, found at the bottom of Mount Paterno near Bologna, in one of his non-fruitful attempts to produce gold. After grinding and heating the mineral with charcoal under reducing conditions, he obtained a persistent luminescent material rapidly called Lapis Boloniensis, or Bolognian stone.[9][10] The phosphorescence of the material obtained by Casciarolo made it a curiosity.[11][12][13]
Preparation
[edit]A modern procedure proceeds from barium carbonate:[14]
- BaCO3 + H2S → BaS + H2O + CO2
BaS crystallizes with the NaCl structure, featuring octahedral Ba2+ and S2− centres.
The observed melting point of barium sulfide is highly sensitive to impurities.[2]
Safety
[edit]BaS is quite poisonous, as are related sulfides, such as CaS, which evolve toxic hydrogen sulfide upon contact with water.
References
[edit]- ^ Lide, David R., ed. (2006). CRC Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0487-3.
- ^ a b Stinn, C., Nose, K., Okabe, T. et al. Metall and Materi Trans B (2017) 48: 2922. https://doi.org/10.1007/s11663-017-1107-5 Archived 2024-01-01 at the Wayback Machine
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ^ Vij, D. R.; Singh, N. (1992). Optical and electrical properties of II-VI wide gap semiconducting barium sulfide. Conf. Phys. Technol. Semicond. Devices Integr. Circuits, 1992. Proceedings of SPIE. Vol. 1523. pp. 608–612. Bibcode:1992SPIE.1523..608V. doi:10.1117/12.634082.
- ^ F. Licetus, Litheosphorus, sive de lapide Bononiensi lucem in se conceptam ab ambiente claro mox in tenebris mire conservante, Utini, ex typ. N. Schiratti, 1640. See http://www.chem.leeds.ac.uk/delights/texts/Demonstration_21.htm Archived 2011-08-13 at the Wayback Machine
- ^ Kresse, Robert; Baudis, Ulrich; Jäger, Paul; Riechers, H. Hermann; Wagner, Heinz; Winkler, Jochen; Wolf, Hans Uwe (2007). "Barium and Barium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_325.pub2. ISBN 978-3527306732.
- ^ Harvey E. Newton (1957). A History of Luminescence: From the Earliest Times until 1900. Memoirs of the American Physical Society, Philadelphia, J. H. FURST Company, Baltimore, Maryland (USA), Vol. 44, Chapter 1, pp. 11-43.
- ^ Smet, Philippe F.; Moreels, Iwan; Hens, Zeger; Poelman, Dirk (2010). "Luminescence in Sulfides: A Rich History and a Bright Future". Materials. 3 (4): 2834–2883. Bibcode:2010Mate....3.2834S. doi:10.3390/ma3042834. hdl:1854/LU-1243707. ISSN 1996-1944.
- ^ Hardev Singh Virk (2014). "History of Luminescence from Ancient to Modern Times". ResearchGate. Retrieved 6 March 2021.
- ^ "Lapis Boloniensis". www.zeno.org. Archived from the original on 2012-10-23. Retrieved 2011-01-03.
- ^ Lemery, Nicolas (1714). Trait℗e universel des drogues simples.
- ^ Ozanam, Jacques; Montucla, Jean Etienne; Hutton, Charles (1814). Recreations in mathematics and natural philosophy .
- ^ P. Ehrlich (1963). "Alkaline Earth Metals". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=937. NY, NY: Academic Press.