Strontium chloride
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IUPAC name Strontium chloride | |
| Other names Strontium(II) chloride | |
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ECHA InfoCard | 100.030.870 |
EC Number | 233-971-6 |
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| Properties | |
Chemical formula | 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) |
Solubility in water | 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 |
Magnetic susceptibility (χ) | −63.0·10−6 cm3/mol |
Refractive index (nD) | 1.650 (anhydrous) 1.594 (dihydrate) 1.536 (hexahydrate) [1] |
| Structure | |
Crystal structure | Deformed rutile structure |
Coordination geometry | octahedral (six-coordinate) |
| Hazards | |
| Main hazards | Irritant |
Flash point | Non-flammable |
| Related compounds | |
Other anions | Strontium fluoride Strontium bromide Strontium iodide |
Other cations | 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. Like all compounds of Sr, this salt emits a bright red colour in a flame; in fact it is used as a source of redness in fireworks. Its chemical properties are intermediate between those for barium chloride, which is more toxic, and calcium chloride.
Contents
1 Preparation
2 Structure
3 Uses
3.1 Dental care
3.2 Biological research
3.3 Ammonium storage
4 References
5 External links
Preparation
Strontium chloride can be prepared by treating 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
The solid adopts a deformed rutile structure.[3] In the vapour phase the SrCl2 molecule is non-linear with a Cl-Sr-Cl angle of approximately 130°.[3] 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.[4] 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.[5]
Uses
Strontium chloride is the precursor to other compounds of strontium, such as yellow strontium chromate, which is used as a corrosion inhibitor for aluminium. The precipitation proceeds analogously to the related, isostructural sulfate:[2]
- SrCl2 + Na2CrO4 → SrCrO4 + 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 other 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. Sea water aquaria require small amounts of strontium chloride, which is consumed in the production of the exoskeletons of certain plankton.
Dental care
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 potassium nitrate instead which works as a nerve calming agent rather than a barrier.[3]
Biological research
Brief strontium chloride exposure induces parthenogenetic activation of oocytes[6] which is used in developmental biological research.
Ammonium storage
A commercial company is using a strontium chloride-based artificial solid called AdAmmine as a means to store ammonium 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.[7] Earlier company research also considered using the stored ammonium as a means to store synthetic Ammonium fuel under the trademark HydrAmmine and the press name "hydrogen tablet", however this aspect has not been commercialized.[8] Their processes and materials are patented. Their early experiments used magnesium chloride, and is also mentioned in that article.
References
^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, .mw-parser-output cite.citationfont-style:inherit.mw-parser-output qquotes:"""""""'""'".mw-parser-output code.cs1-codecolor:inherit;background:inherit;border:inherit;padding:inherit.mw-parser-output .cs1-lock-free abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/6/65/Lock-green.svg/9px-Lock-green.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-lock-limited a,.mw-parser-output .cs1-lock-registration abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/Lock-gray-alt-2.svg/9px-Lock-gray-alt-2.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-lock-subscription abackground:url("//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/Lock-red-alt-2.svg/9px-Lock-red-alt-2.svg.png")no-repeat;background-position:right .1em center.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registrationcolor:#555.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration spanborder-bottom:1px dotted;cursor:help.mw-parser-output .cs1-hidden-errordisplay:none;font-size:100%.mw-parser-output .cs1-visible-errorfont-size:100%.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration,.mw-parser-output .cs1-formatfont-size:95%.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-leftpadding-left:0.2em.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-rightpadding-right:0.2em
ISBN 0-07-049439-8
^ ab J. Paul MacMillan, Jai Won Park, Rolf Gerstenberg, Heinz Wagner, Karl Köhler, Peter Wallbrecht "Strontium and Strontium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH: Weinheim. DOI 10.1002/14356007.a25 321
^ ab Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
^ 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
^ O'Neill GT, Rolfe LR, Kaufman MH. "Developmental potential and chromosome constitution of strontium-induced mouse parthenogenones" (1991) Mol. Reprod. Dev. 30:214-219
^ Amminex A/S: The solid [1], retrieved 2013-06-12
^ Tue Johannesen: "'Solidified' ammonia as energy storage material for fuel cell applications", presentation slides, Amminex [2], posted at the NH3 Fuel association website in May 2012, retrieved 2013-06-12
External links
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