Tin(II) chloride

{{redirect|E512|the road in France|European route E512}} {{chembox | Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 444348698 | Name = Tin(II) chloride | ImageFile = Tin(II) chloride.jpg | ImageFileL1 = Tin-dichloride-gas-molecule-3D-balls.png | ImageFileR1 = Tin(II) chloride space-filling3D.png | ImageName = Tin(II) chloride | ImageCaptionL1 = Ball-and-stick model (gas phase). | ImageCaptionR1 = Space-filling model (gas phase). | IUPACName = Tin(II) chloride<br/>Tin dichloride | OtherNames = {{Unbulleted list|Stannous chloride|Tin salt|Tin protochloride}} | data page pagename = none | SystematicName = | Section1 = {{Chembox Identifiers | CASNo = 7772-99-8 | CASNo_Ref = {{cascite|correct|CAS}} | CASNo2_Ref = {{cascite|correct|CAS}} | CASNo2 = 10025-69-1 | CASNo2_Comment = (dihydrate) | ChEBI_Ref = {{ebicite|correct|EBI}} | ChEBI = 78067 | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID = 22887 | DrugBank = DB11056 | EINECS = 231-868-0 | UNII_Ref = {{fdacite|correct|FDA}} | UNII = R30H55TN67 | UNII2_Ref = {{fdacite|correct|FDA}} | UNII2 = 1BQV3749L5 | UNII2_Comment = (dihydrate) | RTECS = XP8700000 (anhydrous)<br/>XP8850000 (dihydrate) | UNNumber = 3260 | PubChem = 24479 | SMILES = Cl[Sn]Cl | InChI = 1/2ClH.Sn/h2*1H;/q;;+2/p-2 | InChIKey = AXZWODMDQAVCJE-NUQVWONBAJ | StdInChI_Ref = {{stdinchicite|changed|chemspider}} | StdInChI = 1S/2ClH.Sn/h2*1H;/q;;+2/p-2 | StdInChIKey_Ref = {{stdinchicite|changed|chemspider}} | StdInChIKey = AXZWODMDQAVCJE-UHFFFAOYSA-L }} | Section2 = {{Chembox Properties | Formula = SnCl₂ | MolarMass = 189.60 g/mol (anhydrous)<br />225.63 g/mol (dihydrate) | Appearance = White crystalline solid | Odor = odorless | Density = 3.95 g/cm³ (anhydrous)<br />2.71 g/cm³ (dihydrate) | Solubility = 83.9 g/100 ml (0 °C)<br />Hydrolyses in hot water | SolubleOther = soluble in ethanol, acetone, ether, Tetrahydrofuran <br> insoluble in xylene | MeltingPtC = 247 | MeltingPt_notes = (anhydrous) <br> 37.7 °C (dihydrate) | BoilingPtC = 623 | BoilingPt_notes = (decomposes) | MagSus = &minus;69.0·10⁻⁶ cm³/mol }} | Section3 = {{Chembox Structure | MolShape = Bent (gas phase) | Coordination = Trigonal pyramidal (anhydrous)<br/>Dihydrate also three-coordinate | CrystalStruct = Layer structure<br/>(chains of SnCl₃ groups) }} | Section4 = {{Chembox Thermochemistry | DeltaHf = &minus;325 kJ/mol }} | Section7 = {{Chembox Hazards | ExternalSDS = [https://www.ilo.org/dyn/icsc/showcard.display?p_lang=en&p_card_id=0955&p_version=2 ICSC 0955 (anhydrous)]<br/>[https://www.ilo.org/dyn/icsc/showcard.display?p_lang=en&p_card_id=0738&p_version=2 ICSC 0738 (dihydrate)] | MainHazards = Irritant, dangerous for aquatic organisms | GHS_ref = <ref name="GESTIS">{{GESTIS|ZVG=3550}}</ref> | GHSPictograms = {{GHS05}} {{GHS07}} {{GHS08}} | GHSSignalWord = Danger | HPhrases = {{H-phrases |H290|H302+H332|H314|H317|H335|H373|H412}} | PPhrases = {{P-phrases |P260|P273|P280|P303+P361+P353|P304+P340+P312|P305+P351+P338+P310}} | NFPA-H = 3 | NFPA-F = 0 | NFPA-R = 0 | LD50 = 700 mg/kg (rat, oral)<br/>10,000 mg/kg (rabbit, oral)<br/>250 mg/kg (mouse, oral)<ref>{{IDLH|7440315|Tin (inorganic compounds, as Sn)}}</ref> }} | Section8 = {{Chembox Related | OtherAnions = Tin(II) fluoride<br/>Tin(II) bromide<br/>Tin(II) iodide | OtherCations = Germanium dichloride<br/>Tin(IV) chloride<br/>Lead(II) chloride }} }} '''Tin(II) chloride''', also known as '''stannous chloride''', is a white crystalline solid with the formula {{chem2|SnCl2|auto=1}}. It forms a stable dihydrate, but aqueous solutions tend to undergo hydrolysis, particularly if hot. SnCl₂ is widely used as a reducing agent (in acid solution), and in electrolytic baths for tin-plating. Tin(II) chloride should not be confused with the other chloride of tin; tin(IV) chloride or stannic chloride (SnCl₄).

==Chemical structure== SnCl₂ has a lone pair of electrons, such that the molecule in the gas phase is bent. In the solid state, crystalline SnCl₂ forms chains linked via chloride bridges as shown. The dihydrate has three coordinates as well, with one water on the tin and another water on the first. The main part of the molecule stacks into double layers in the crystal lattice, with the "second" water sandwiched between the layers.

thumb|460px|left|Structures of tin(II) chloride and related compounds [[File:Tin(II)-chloride-xtal-1996-3D-balls-front.png|thumb|460px|left|Ball-and-stick models of the crystal structure of SnCl₂<ref>{{cite journal |journal = J. Phys. Chem. Solids|volume = 57|issue = 1|year = 1996|pages = 7–16|title = The high pressure behaviour of the cotunnite and post-cotunnite phases of PbCl₂ and SnCl₂ |author1=J. M. Leger |author2=J. Haines |author3=A. Atouf |doi = 10.1016/0022-3697(95)00060-7|bibcode = 1996JPCS...57....7L }}</ref>]]

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==Chemical properties== Tin(II) chloride dissolves in less than its own mass of water. Dilute solutions are subject to hydrolysis, yielding an insoluble basic salt: :{{chem2|SnCl2 + H2O {{eqm}} Sn(OH)Cl + HCl}}

Hydrolysis is prevented in the presence of hydrochloric acid, typically of the same or greater molarity as the stannous chloride. Solutions of SnCl₂ are also unstable towards oxidation by the air: :{{chem2|6 SnCl2 + O2 + 2 H2O → 2 SnCl4 + 4 Sn(OH)Cl}}

Oxidation can be prevented by storing the solution over lumps of tin metal.<ref>{{cite book|author = H. Nechamkin|title = The Chemistry of the Elements|url = https://archive.org/details/chemistryofeleme00nech|url-access = registration|publisher = McGraw-Hill|location = New York|year = 1968}}</ref>

Tin(II) chloride acts as a reducing agent for silver and gold salts to the metal, and iron(III) salts to iron(II), for example: :SnCl₂ (aq) + 2 FeCl₃ (aq) → SnCl₄ (aq) + 2 FeCl₂ (aq)

It also reduces copper(II) to copper(I).

Solutions of tin(II) chloride can also serve simply as a source of Sn²⁺ ions, which can form other tin(II) compounds via precipitation reactions. For example, reaction with sodium sulfide produces the brown/black tin(II) sulfide: :SnCl₂ (aq) + Na₂S (aq) → SnS (s) + 2 NaCl (aq)

If alkali is added to a solution of SnCl₂, a white precipitate of hydrated tin(II) oxide forms initially; this then dissolves in excess base to form a stannite salt such as sodium stannite: :SnCl₂(aq) + 2 NaOH (aq) → SnO·H₂O (s) + 2 NaCl (aq) :SnO·H₂O (s) + NaOH (aq) → NaSn(OH)₃ (aq)

Anhydrous SnCl₂ can be used to make a variety of tin(II) compounds in non-aqueous solvents. For example, the lithium salt of 4-methyl-2,6-di-tert-butylphenol reacts with SnCl₂ in THF to give the yellow linear two-coordinate compound Sn(OAr)₂ (Ar = aryl).<ref>{{Cite journal|last1=Cetinkaya|first1=B.|last2=Gumrukcu|first2=I.|last3=Lappert|first3=M. F.|last4=Atwood|first4=J. L.|last5=Rogers|first5=R. D.|last6=Zaworotko|first6=M. J.|display-authors=3|date=1980-03-01|title=Bivalent germanium, tin, and lead 2,6-di-tert-butylphenoxides and the crystal and molecular structures of M(OC6H2Me-4-But2-2,6)2 (M = Ge or Sn)|url=https://doi.org/10.1021/ja00526a054|journal=Journal of the American Chemical Society|volume=102|issue=6|pages=2088–2089|doi=10.1021/ja00526a054|bibcode=1980JAChS.102.2088C |issn=0002-7863|url-access=subscription}}</ref>

Tin(II) chloride also behaves as a weak Lewis acid, forming complexes with ligands such as chloride ion, for example: :{{chem2|SnCl2 + CsCl- → SnCl3-}}

Like {{chem2|SnCl2(H2O)}}, trichlorostannate ({{chem2|SnCl3-}}) ion is pyramidal. Such complexes have a full octet. The lone pair of electrons in such complexes is available for bonding. Therefore, {{chem2|SnCl3-}} itself can serve as a Lewis base or ligand:<ref>{{cite journal |doi=10.1021/ic00133a062 |title=Crystal and Solution Structure of Triphenylmethylphosphonium Pentakis(trichlorostannyl)platinate(II), &#91;Ph₃PCH₃&#93;3&#91;Pt(SnCl₃)₅&#93; |date=1982 |last1=Nelson |first1=John H. |last2=Alcock |first2=Nathaniel W. |journal=Inorganic Chemistry |volume=21 |issue=3 |pages=1196–1200 }}</ref> :SnCl₂ + Fe(η⁵-C₅H₅)(CO)₂HgCl → Fe(η⁵-C₅H₅)(CO)₂SnCl₃ + Hg

SnCl₂ can be used to make a variety of related compounds containing metal-tin bonds. For example, the reaction with dicobalt octacarbonyl: :SnCl₂ + Co₂(CO)₈ → (CO)₄Co-(SnCl₂)-Co(CO)₄

==Preparation== Anhydrous SnCl₂ is prepared by the action of dry hydrogen chloride gas on tin metal. The dihydrate is made by a similar reaction, using hydrochloric acid:

:Sn (s) + 2 HCl (aq) → SnCl₂ (aq) + {{chem2|H2}} (g)

The water then carefully evaporated from the acidic solution to produce crystals of SnCl₂·2H₂O. This dihydrate can be dehydrated to anhydration using acetic anhydride.<ref>{{Cite book |last1=Armarego |first1=W. L. F. |url=https://www.abebooks.com/9781856175678/Purification-Laboratory-Chemicals-Armarego-W.L.F-1856175677/plp |title=Purification of Laboratory Chemicals |last2=Chai |first2=C. L. L. |publisher=Elsevier, Butterwoth-Heinemann |year=2009 |isbn=978-0-08-087824-9 |location=Burlington |language=en |doi=10.1016/B978-1-85617-567-8.50009-3 |access-date=2022-02-03}}</ref>

==Uses== A solution of tin(II) chloride containing a little hydrochloric acid is used for the tin-plating of steel, in order to make tin cans. An electric potential is applied, and tin metal is formed at the cathode via electrolysis.

Tin(II) chloride is used as a mordant in textile dyeing because it gives brighter colours with some dyes e.g. cochineal. This mordant has also been used alone to increase the weight of silk.

In recent years, an increasing number of tooth paste brands have been adding Tin(II) chloride as protection against enamel erosion to their formula, e. g. Oral-B or Elmex.

It is used as a catalyst in the production of the plastic polylactic acid (PLA).

It also finds a use as a catalyst between acetone and hydrogen peroxide to form the tetrameric form of acetone peroxide.

Tin(II) chloride also finds wide use as a reducing agent. This is seen in its use for silvering mirrors, where silver metal is deposited on the glass:

:Sn²⁺ (aq) + 2 Ag⁺ → Sn⁴⁺ (aq) + 2 Ag (s)

A related reduction was traditionally used as an analytical test for {{chem2|auto=1|Hg(2+) (aq)}}. For example, if SnCl₂ is added dropwise into a solution of mercury(II) chloride, a white precipitate of mercury(I) chloride is first formed; as more SnCl₂ is added this turns black as metallic mercury is formed.

Stannous chloride is also used by many precious metals refining hobbyists and professionals to test for the presence of gold salts.<ref>{{Citation |title=How To Make Stannous Chloride for Testing Gold Solutions | date=27 February 2015 |url=https://www.youtube.com/watch?v=v--lPph0nog |access-date=2023-02-10 |language=en}}</ref> When SnCl₂ comes into contact with gold compounds, particularly chloroaurate salts, it forms a bright purple colloid known as purple of Cassius.<ref>{{Cite journal |last1=Fink |first1=Colin |last2=Putnam |first2=Garth |date=1942-06-01 |title=Determination of Small Amounts of Gold with Stannous Chloride |url=https://pubs.acs.org/doi/abs/10.1021/i560106a008 |journal=Industrial & Engineering Chemistry Analytical Edition |language=en |volume=14 |issue=6 |pages=468–470 |doi=10.1021/i560106a008 |issn=0096-4484|url-access=subscription }}</ref> A similar reaction occurs with platinum and palladium salts, becoming green and brown respectively.<ref>{{Cite web |last=Sam |date=2020-07-11 |title=Stannous Chloride – Test For Gold, Platinum and Palladium Presence |url=https://www.goldnscrap.com/post/stannous-chloride-test-for-gold-platinum-and-palladium-presence |access-date=2024-05-05 |website=Gold-N-scrap |language=en}}</ref>

When mercury is analyzed using atomic absorption spectroscopy, a cold vapor method must be used, and tin (II) chloride is typically used as the reductant.

===Organic chemistry=== In organic chemistry, SnCl₂ is used in the Stephen reduction, whereby a nitrile is reduced (via an imidoyl chloride salt) to an imine which is easily hydrolysed to an aldehyde.<ref>{{OrgSynth|title = β-Naphthaldehyde|author = Williams, J. W.|collvol = 3|collvolpages = 626|year = 1955|prep = cv3p0626}}</ref>

The reaction usually works best with aromatic nitriles Aryl-CN. A related reaction (called the Sonn-Müller method) starts with an amide, which is treated with PCl₅ to form the imidoyl chloride salt. center|500x500px|The Stephen reduction The Stephen reduction is less used today, because it has been mostly superseded by diisobutylaluminium hydride reduction.

Additionally, SnCl₂ is used to selectively reduce aromatic nitro groups to anilines.<ref>{{cite journal|author1=F. D. Bellamy |author2=K. Ou |name-list-style=amp |title = Selective reduction of aromatic nitro compounds with stannous chloride in non-acidic and non-aqueous medium|year = 1984|journal = Tetrahedron Letters|volume = 25|issue = 8|pages = 839–842|doi = 10.1016/S0040-4039(01)80041-1}}</ref>

center|350px|Aromatic nitro group reduction using SnCl₂

SnCl₂ also reduces quinones to hydroquinones.

Stannous chloride is also added as a food additive with E number '''E512''' to some canned and bottled foods, where it serves as a color-retention agent and antioxidant.

SnCl₂ is used in radionuclide angiography to reduce the radioactive agent technetium-99m-pertechnetate to assist in binding to blood cells.

Molten SnCl₂ can be oxidised to form highly crystalline SnO₂ nanostructures.<ref>{{Cite journal|last1=Kamali|first1=Ali|first2=Reza|last2=Divitini|first3=Giorgio|last3=Ducati|first4=Caterina|last4=Fray|first5=Derek|last5=J|date=2014|title=Transformation of molten SnCl2 to SnO2 nano-single crystals|journal=CERI Ceramics International|language=English|volume=40|issue=6|pages=8533–8538|doi=10.1016/j.ceramint.2014.01.067|issn=0272-8842|oclc=5902254906}}</ref><ref>{{Cite journal|last=Kamali|first=Ali Reza|date=2014|title=Thermokinetic characterisation of tin(II) chloride|journal=Journal of Thermal Analysis and Calorimetry |language=English|volume=118|issue=1|pages=99–104|doi=10.1007/s10973-014-4004-z|s2cid=98207611|issn=1388-6150|oclc=5690448892}}</ref>

A Stannous reduction is used in nuclear medicine bone scans to remove the negative charge from free pertechnetate when it is bound to MDP for radiopharmaceutical studies. Incomplete reduction due to insufficient tin or accidental insufflation of air leads to the formation of free pertechnetate, a finding which can be seen on bone scans due to its inappropriate uptake in the stomach.<ref>{{cite journal |last1=Cabral |first1=RE |last2=Leitão |first2=AC |last3=Lage |first3=C |last4=Caldeira-de-Araújo |first4=A |last5=Bernardo-Filho |first5=M |last6=Dantas |first6=FJ |last7=Cabral-Neto |first7=JB |title=Mutational potentiality of stannous chloride: an important reducing agent in the Tc-99m-radiopharmaceuticals. |journal=Mutation Research |date=7 August 1998 |volume=408 |issue=2 |pages=129–35 |doi=10.1016/s0921-8777(98)00026-3 |pmid=9739815}}</ref>

Stannous Chloride is used for coating SnO₂ Tin Oxide doped conductive iridescent coatings for low e glass.<ref>Electrically conducting coating on glass and other ceramic bodies https://patents.google.com/patent/US2564987A/en</ref>

==Notes== * N. N. Greenwood, A. Earnshaw, ''Chemistry of the Elements'', 2nd ed., Butterworth-Heinemann, Oxford, UK, 1997. * ''Handbook of Chemistry and Physics'', 71st edition, CRC Press, Ann Arbor, Michigan, 1990. * ''The Merck Index'', 7th edition, Merck & Co, Rahway, New Jersey, USA, 1960. * A. F. Wells, '''Structural Inorganic Chemistry'', 5th ed., Oxford University Press, Oxford, UK, 1984. * J. March, ''Advanced Organic Chemistry'', 4th ed., p.&nbsp;723, Wiley, New York, 1992.

==References== {{reflist}}

{{Tin compounds}} {{Chlorides}}

Category:Metal halides Category:Chlorides Category:Tin(II) compounds Category:Coordination complexes Category:Deliquescent materials Category:Reducing agents Category:E-number additives