|CAS number||, (hexahydrate)|
|Jmol-3D images||Image 1|
|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)
874 °C (anhydrous)
1250 °C (anhydrous)
|Solubility in water||anhydrous:
53.8 g/100 mL (20 °C)
106 g/100 mL (0 °C)
206 g/100 mL (40 °C)
|Solubility||ethanol: very slightly soluble
acetone: very slightly soluble
|Refractive index (nD)||1.650 (anhydrous)
1.536 (hexahydrate) 
|Crystal structure||Deformed rutile structure|
|EU Index||Not listed|
|Other anions||Strontium fluoride
|Other cations||Beryllium chloride
| (what is: / ?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
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.
- Sr(OH)2 + 2 HCl → SrCl2 + 2 H2O
The solid adopts a deformed rutile structure. In the vapour phase the SrCl2 molecule is non-linear with a Cl-Sr-Cl angle of approximately 130°. This is an exception to VESPR 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. 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.
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:
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.
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.
A commercial company is using a strontium chloride-based artificial solid called AdAmminetm 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. Earlier company research also considered using the stored ammonium as a means to store synthetic Ammonium fuel under the trademark HydrAmminetm and the press name "hydrogen tablet", however this aspect has not been commercialized. Their processes and materials are patented. Their early experiments used magnesium chloride, and is also mentioned in that article.
- Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- 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
- Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419.
- 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
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- Amminex A/S: The solid , retrieved 2013-06-12
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