Strontium chloride
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| Names | |
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| IUPAC name
Strontium chloride
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| Other names
Strontium(II) chloride
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| Identifiers | |
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3D model (JSmol)
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| ChEBI | |
| ChEMBL | |
| ChemSpider | |
| ECHA InfoCard | 100.030.870 |
| EC Number |
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PubChem CID
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| UNII |
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CompTox Dashboard (EPA)
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| Properties | |
| SrCl2 | |
| Molar mass | 158.53 g/mol (anhydrous) 266.62 g/mol (hexahydrate) |
| Appearance | White crystalline solid |
| Density | 3.052 g/cm3 (anhydrous, monoclinic form) 2.672 g/cm3 (dihydrate) 1.930 g/cm3 (hexahydrate) |
| Melting point | 874 °C (1,605 °F; 1,147 K) (anhydrous) 61 °C (hexahydrate) |
| Boiling point | 1,250 °C (2,280 °F; 1,520 K) (anhydrous) |
| anhydrous: 53.8 g/100 mL (20 °C) hexahydrate: 106 g/100 mL (0 °C) 206 g/100 mL (40 °C) | |
| Solubility | ethanol: very slightly soluble acetone: very slightly soluble ammonia: insoluble |
| −63.0·10−6 cm3/mol | |
Refractive index (nD)
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1.650 (anhydrous) 1.594 (dihydrate) 1.536 (hexahydrate)[1] |
| Structure | |
| Deformed rutile structure | |
| octahedral (six-coordinate) | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
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Irritant |
| NFPA 704 (fire diamond) | |
| Flash point | N/A |
| Related compounds | |
Other anions
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Strontium fluoride Strontium bromide Strontium iodide |
Other cations
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Beryllium chloride Magnesium chloride Calcium chloride Barium chloride Radium chloride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Strontium chloride (SrCl2) is a salt of strontium and chloride. It is a 'typical' salt, forming neutral aqueous solutions. As with all compounds of strontium, this salt emits a bright red colour in flame, and is commonly used in fireworks to that effect. Its properties are intermediate between those for barium chloride, which is more toxic, and calcium chloride.
Preparation[edit]
Strontium chloride can be prepared by treating aqueous strontium hydroxide or strontium carbonate with hydrochloric acid:
- Sr(OH)2 + 2 HCl → SrCl2 + 2 H2O
Crystallization from cold aqueous solution gives the hexahydrate, SrCl2·6H2O. Dehydration of this salt occurs in stages, commencing above 61 °C (142 °F). Full dehydration occurs at 320 °C (608 °F).[2]
Structure[edit]
In the solid state, SrCl2 adopts a fluorite structure.[3][4][5] In the vapour phase the SrCl2 molecule is non-linear with a Cl-Sr-Cl angle of approximately 130°.[6] This is an exception to VSEPR theory which would predict a linear structure. Ab initio calculations have been cited to propose that contributions from d orbitals in the shell below the valence shell are responsible.[7] Another proposal is that polarisation of the electron core of the strontium atom causes a distortion of the core electron density that interacts with the Sr-Cl bonds.[8]
Uses[edit]
Strontium chloride is a precursor to other compounds of strontium, such as yellow strontium chromate, strontium carbonate, and strontium sulfate. Exposure of aqueous solutions of strontium chloride to the sodium salt of the desired anion often leads to formation of the solid precipitate:[9][2]
- SrCl2 + Na2CrO4 → SrCrO4 + 2 NaCl
- SrCl2 + Na2CO3 → SrCO3 + 2 NaCl
- SrCl2 + Na2SO4 → SrSO4 + 2 NaCl
Strontium chloride is often used as a red colouring agent in pyrotechnics. It imparts a much more intense red colour to the flames than most alternatives. It is employed in small quantities in glass-making and metallurgy. The radioactive isotope strontium-89, used for the treatment of bone cancer, is usually administered in the form of strontium chloride. Seawater aquaria require small amounts of strontium chloride, which is consumed during the growth of certain plankton.
Dental care[edit]
SrCl2 is useful in reducing tooth sensitivity by forming a barrier over microscopic tubules in the dentin containing nerve endings that have become exposed by gum recession. Known in the U.S. as Elecol and Sensodyne, these products are called "strontium chloride toothpastes", although most now use saltpeter (KNO3) instead which works as an analgesic rather than a barrier.[10]
Biological research[edit]
Brief strontium chloride exposure induces parthenogenetic activation of oocytes[11] which is used in developmental biological research.
Ammonia storage[edit]
A commercial company is using a strontium chloride-based artificial solid called AdAmmine as a means to store ammonia at low pressure, mainly for use in NOx emission reduction on Diesel vehicles. They claim that their patented material can also be made from some other salts, but they have chosen strontium chloride for mass production.[12] Earlier company research also considered using the stored ammonia as a means to store synthetic ammonia fuel under the trademark HydrAmmine and the press name "hydrogen tablet", however, this aspect has not been commercialized.[13] Their processes and materials are patented. Their early experiments used magnesium chloride, and is also mentioned in that article.
Soil testing[edit]
Strontium chloride is used with citric acid in soil testing as an universal extractant of plant nutrients.[14]
References[edit]
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- ^ a b MacMillan, J. Paul; Park, Jai Won; Gerstenberg, Rolf; Wagner, Heinz; Köhler, Karl; Wallbrecht, Peter (2000). "Strontium and Strontium Compounds". Ullmann's Encyclopedia of Industrial Chemistry. doi:10.1002/14356007.a25_321. ISBN 3527306730.
- ^ West, Anthony R. (8 January 2014). Solid state chemistry and its applications (Second edition, student ed.). Chichester, West Sussex, UK. ISBN 978-1-118-67625-7. OCLC 854761803.
{{cite book}}: CS1 maint: location missing publisher (link) - ^ Persson, Kristin (2020), Materials Data on SrCl2 by Materials Project, Materials Project, LBNL Materials Project; Lawrence Berkeley National Laboratory (LBNL), Berkeley, CA (United States), doi:10.17188/1199327, retrieved 2020-10-10
- ^ Mark, H.; Tolksdorf, S. (1925). "Ueber das Beugungsvermoegen der Atome fuer Roentgenstrahlen". www.crystallography.net. Retrieved 2020-10-10.
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- ^ Ab initio model potential study of the equilibrium geometry of alkaline earth dihalides: MX2 (M=Mg, Ca Sr, Ba; X=F, Cl, Br, I) Seijo L., Barandiarán Z J. Chem. Phys. 94, 3762 (1991) doi:10.1063/1.459748
- ^ "Ion model and equilibrium configuration of the gaseous alkaline-earth dihalides" Guido M. and Gigli G. J. Chem. Phys. 65, 1397 (1976); doi:10.1063/1.433247
- ^ Aydoğan, Salih; Erdemoğlu, Murat; Aras, Ali; Uçar, Gökhan; Özkan, Alper (2006). "Dissolution kinetics of celestite (SrSO4) in HCl solution with BaCl2". Hydrometallurgy. 84 (3–4): 239–246. Bibcode:2006HydMe..84..239A. doi:10.1016/j.hydromet.2006.06.001.
- ^ "Sensodyne". Sensodyne. Archived from the original on 2008-09-18. Retrieved 2008-09-05.
- ^ O'Neill GT, Rolfe LR, Kaufman MH. "Developmental potential and chromosome constitution of strontium-induced mouse parthenogenones" (1991) Mol. Reprod. Dev. 30:214-219
- ^ "AdAmmine™". Amminex A/S. Archived from the original on 2013-08-01. Retrieved 2013-06-12.
- ^ Tue Johannesen (May 2012). 'Solidified' ammonia as an energy storage material for fuel cell applications (PDF). 2006 Annual NH3 Fuel Conference, October 9 – 10, 2006, Golden, CO. Amminex. Retrieved 2022-11-16. Via NH3 Fuel Association website.
- ^ Simard, R. R. (1 March 1991). "Strontium Chloride-Citric Acid Extraction Evaluated as a Soil-Testing Procedure for Phosphorus". Soil Science Society of America Journal. 55 (2): 414. Bibcode:1991SSASJ..55..414S. doi:10.2136/sssaj1991.03615995005500020021x.
External links[edit]
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