Strontium chloride

Last updated
Strontium chloride
Strontium chloride hexahydrate.jpg
Names
IUPAC name
Strontium chloride
Other names
Strontium(II) chloride
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.030.870 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 233-971-6
PubChem CID
UNII
  • InChI=1S/2ClH.Sr/h2*1H;/q;;+2/p-2 Yes check.svgY
    Key: AHBGXTDRMVNFER-UHFFFAOYSA-L Yes check.svgY
  • InChI=1S/2ClH.Sr/h2*1H;/q;;+2/p-2
  • Key: AHBGXTDRMVNFER-UHFFFAOYSA-L
  • [Sr+2].[Cl-].[Cl-]
Properties
SrCl2
Molar mass 158.53 g/mol (anhydrous)
266.62 g/mol (hexahydrate)
AppearanceWhite 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
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
Irritant
NFPA 704 (fire diamond)
NFPA 704.svgHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Flash point N/A
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).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

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.

Contents

Preparation

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

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

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

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

Brief strontium chloride exposure induces parthenogenetic activation of oocytes [11] which is used in developmental biological research.

Ammonia storage

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

Strontium chloride is used with citric acid in soil testing as an universal extractant of plant nutrients. [14]

Related Research Articles

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<span class="mw-page-title-main">Acid–base reaction</span> Chemical reaction between an acid and a base

In chemistry, an acid–base reaction is a chemical reaction that occurs between an acid and a base. It can be used to determine pH via titration. Several theoretical frameworks provide alternative conceptions of the reaction mechanisms and their application in solving related problems; these are called the acid–base theories, for example, Brønsted–Lowry acid–base theory.

In chemistry, a salt is a chemical compound consisting of an ionic assembly of positively charged cations and negatively charged anions, which results in a compound with no net electric charge. A common example is table salt, with positively charged sodium ions and negatively charged chloride ions.

<span class="mw-page-title-main">Zinc chloride</span> Chemical compound

Zinc chloride is the name of inorganic chemical compounds with the formula ZnCl2. It forms hydrates. Zinc chloride, anhydrous and its hydrates are colorless or white crystalline solids, and are highly soluble in water. Five hydrates of zinc chloride are known, as well as four forms of anhydrous zinc chloride. This salt is hygroscopic and even deliquescent. Zinc chloride finds wide application in textile processing, metallurgical fluxes, and chemical synthesis. No mineral with this chemical composition is known aside from the very rare mineral simonkolleite, Zn5(OH)8Cl2·H2O.

<span class="mw-page-title-main">Hypochlorite</span> Ion

In chemistry, hypochlorite, or chloroxide is an anion with the chemical formula ClO−. It combines with a number of cations to form hypochlorite salts. Common examples include sodium hypochlorite and calcium hypochlorite. The Cl-O distance in ClO− is 1.69 Å.

<span class="mw-page-title-main">Silver chloride</span> Chemical compound with the formula AgCl

Silver chloride is a chemical compound with the chemical formula AgCl. This white crystalline solid is well known for its low solubility in water and its sensitivity to light. Upon illumination or heating, silver chloride converts to silver, which is signaled by grey to black or purplish coloration in some samples. AgCl occurs naturally as a mineral chlorargyrite.

Neodymium(III) chloride or neodymium trichloride is a chemical compound of neodymium and chlorine with the formula NdCl3. This anhydrous compound is a mauve-colored solid that rapidly absorbs water on exposure to air to form a purple-colored hexahydrate, NdCl3·6H2O. Neodymium(III) chloride is produced from minerals monazite and bastnäsite using a complex multistage extraction process. The chloride has several important applications as an intermediate chemical for production of neodymium metal and neodymium-based lasers and optical fibers. Other applications include a catalyst in organic synthesis and in decomposition of waste water contamination, corrosion protection of aluminium and its alloys, and fluorescent labeling of organic molecules (DNA).

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<span class="mw-page-title-main">Rhodium(III) chloride</span> Chemical compound

Rhodium(III) chloride refers to inorganic compounds with the formula RhCl3(H2O)n, where n varies from 0 to 3. These are diamagnetic solids featuring octahedral Rh(III) centres. Depending on the value of n, the material is either a dense brown solid or a soluble reddish salt. The soluble trihydrated (n = 3) salt is widely used to prepare compounds used in homogeneous catalysis, notably for the industrial production of acetic acid and hydroformylation.

<span class="mw-page-title-main">Tetraamminecopper(II) sulfate</span> Chemical compound

Tetra ammine copper(II) sulphate is the salt with the formula [Cu(NH3)4]SO4·H2O. This dark blue to purple solid is a salt of the metal complex [Cu(NH3)4(H2O)]2+. It is closely related to Schweizer's reagent, which is used for the production of cellulose fibers in the production of rayon.

<span class="mw-page-title-main">Metal ammine complex</span>

In coordination chemistry, metal ammine complexes are metal complexes containing at least one ammonia ligand. "Ammine" is spelled this way for historical reasons; in contrast, alkyl or aryl bearing ligands are spelt with a single "m". Almost all metal ions bind ammonia as a ligand, but the most prevalent examples of ammine complexes are for Cr(III), Co(III), Ni(II), Cu(II) as well as several platinum group metals.

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<span class="mw-page-title-main">Ammonium perrhenate</span> Chemical compound

Ammonium perrhenate (APR) is the ammonium salt of perrhenic acid, NH4ReO4. It is the most common form in which rhenium is traded. It is a white salt; soluble in ethanol and water, and mildly soluble in NH4Cl. It was first described soon after the discovery of rhenium.

<span class="mw-page-title-main">Platinum(II) chloride</span> Chemical compound

Platinum(II) chloride is the chemical compound PtCl2. It is an important precursor used in the preparation of other platinum compounds. It exists in two crystalline forms, but the main properties are somewhat similar: dark brown, insoluble in water, diamagnetic, and odorless.

<span class="mw-page-title-main">Magnus's green salt</span> Chemical compound

Magnus's green salt is the inorganic compound with the formula [Pt(NH3)4][PtCl4]. This salt is named after Heinrich Gustav Magnus, who, in the early 1830s, first reported the compound. The compound is a linear chain compound, consisting of a chain of platinum atoms. It is dark green, which is unusual for platinum compounds.

<span class="mw-page-title-main">Strontium carbonate</span> Chemical compound

Strontium carbonate (SrCO3) is the carbonate salt of strontium that has the appearance of a white or grey powder. It occurs in nature as the mineral strontianite.

<span class="mw-page-title-main">Beryllium chloride</span> Chemical compound

Beryllium chloride is an inorganic compound with the formula BeCl2. It is a colourless, hygroscopic solid that dissolves well in many polar solvents. Its properties are similar to those of aluminium chloride, due to beryllium's diagonal relationship with aluminium.

<span class="mw-page-title-main">Pentaamine(dinitrogen)ruthenium(II) chloride</span> Chemical compound

Pentaamine(nitrogen)ruthenium(II) chloride is an inorganic compound with the formula [Ru(NH3)5(N2)]Cl2. It is a nearly white solid, but its solutions are yellow. The cationic complex is of historic significance as the first compound with N2 bound to a metal center. [Ru(NH3)5(N2)]2+ adopts an octahedral structure with C4v symmetry.

<span class="mw-page-title-main">Hexaamminenickel chloride</span> Chemical compound

Hexaamminenickel chloride is the chemical compound with the formula [Ni(NH3)6]Cl2. It is the chloride salt of the metal ammine complex [Ni(NH3)6]2+. The cation features six ammonia (called ammines in coordination chemistry) ligands attached to the nickel(II) ion.

References

  1. ↑ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN   0-07-049439-8
  2. 1 2 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.
  3. ↑ 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)
  4. ↑ 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
  5. ↑ Mark, H.; Tolksdorf, S. (1925). "Ueber das Beugungsvermoegen der Atome fuer Roentgenstrahlen". www.crystallography.net. Retrieved 2020-10-10.
  6. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN   978-0-08-037941-8.
  7. ↑ 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
  8. ↑ "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
  9. ↑ 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.
  10. ↑ "Sensodyne". Sensodyne. Archived from the original on 2008-09-18. Retrieved 2008-09-05.
  11. ↑ O'Neill GT, Rolfe LR, Kaufman MH. "Developmental potential and chromosome constitution of strontium-induced mouse parthenogenones" (1991) Mol. Reprod. Dev. 30:214-219
  12. ↑ "AdAmmine™". Amminex A/S. Archived from the original on 2013-08-01. Retrieved 2013-06-12.
  13. ↑ 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.
  14. ↑ 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.
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