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{{chembox {{chembox
| Verifiedfields = changed
| verifiedrevid = 396073021
| Watchedfields = changed
| Name = Tin(II) chloride
| verifiedrevid = 444348698
| ImageFile = Tin(II) chloride.jpg
| Name = Tin(II) chloride
<!--|ImageSize = 200px -->
| ImageName = Tin(II) chloride | ImageFile = Tin(II) chloride.jpg
| ImageFileL1 = Tin-dichloride-gas-molecule-3D-balls.png
| IUPACName = Tin(II) chloride<br/>Tin dichloride
| ImageFileR1 = Tin(II) chloride space-filling3D.png
| OtherNames = Stannous chloride<br/>Tin salt<br/>Tin protochloride
| ImageName = Tin(II) chloride
| Section1 = {{Chembox Identifiers
| 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 = 7772-99-8
| CASNo_Ref = {{cascite|correct|CAS}} | CASNo_Ref = {{cascite|correct|CAS}}
| CASNo2_Ref = {{cascite|correct|CAS}}
| CASOther = <br/>10025-69-1 (dihydrate)
| 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) | RTECS = XP8700000 (anhydrous)<br/>XP8850000 (dihydrate)
| UNNumber = 3260 | UNNumber = 3260
| PubChem = 24479
| SMILES = ClCl
| 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 | Section2 = {{Chembox Properties
| Formula = SnCl<sub>2</sub> | Formula = SnCl<sub>2</sub>
| MolarMass = 189.60 g/mol (anhydrous)<br />225.63 g/mol (dihydrate) | MolarMass = 189.60 g/mol (anhydrous)<br />225.63 g/mol (dihydrate)
| Appearance = White crystalline solid | Appearance = White crystalline solid
| Odor = odorless
| Density = 3.95 g/cm<sup>3</sup> (anhydrous)<br />2.71 g/cm<sup>3</sup> (dihydrate) | Density = 3.95 g/cm<sup>3</sup> (anhydrous)<br />2.71 g/cm<sup>3</sup> (dihydrate)
| Solubility = 83.9 g/100 ml (0 °C)<br />] in hot water | Solubility = 83.9 g/100 ml (0 °C)<br />] in hot water
| SolubleOther = soluble in ], ], ] <br> insoluble in ] | SolubleOther = soluble in ], ], ], ] <br> insoluble in ]
| MeltingPtC = 247
| MeltingPt = 247 °C (anhydrous) <br> 37 °C (dihydrate)
| MeltingPt_notes = (anhydrous) <br> 37.7 °C (dihydrate)
| BoilingPt = 623 °C (896 K) (decomp.)
| BoilingPtC = 623
| BoilingPt_notes = (decomposes)
| MagSus = &minus;69.0·10<sup>−6</sup> cm<sup>3</sup>/mol
}} }}
| Section3 = {{Chembox Structure | Section3 = {{Chembox Structure
| MolShape = ] (gas phase) | MolShape = ] (gas phase)
| Coordination = ] (anhydrous)<br/>Dihydrate also three-coordinate | Coordination = ] (anhydrous)<br/>Dihydrate also three-coordinate
| CrystalStruct = Layer structure<br/>(chains of SnCl<sub>3</sub> groups) | CrystalStruct = Layer structure<br/>(chains of SnCl<sub>3</sub> groups)
}} }}
| Section7 = {{Chembox Hazards | Section4 = {{Chembox Thermochemistry
| DeltaHf = &minus;325 kJ/mol
| ExternalMSDS = <br/>
}}
| Section7 = {{Chembox Hazards
| ExternalSDS = <br/>
| MainHazards = Irritant, dangerous for aquatic organisms | MainHazards = Irritant, dangerous for aquatic organisms
| GHS_ref = <ref name="GESTIS">{{GESTIS|ZVG=3550}}</ref>
| EUIndex = Not listed
| GHSPictograms = {{GHS05}} {{GHS07}} {{GHS08}}
| NFPA-H = 1
| 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-F = 0
| NFPA-R = 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>
| RPhrases =
| SPhrases =
}} }}
| Section8 = {{Chembox Related | Section8 = {{Chembox Related
| OtherAnions = ]<br/>]<br/>] | OtherAnions = ]<br/>]<br/>]
| OtherCations = ]<br/>]<br/>] | OtherCations = ]<br/>]<br/>]
}} }}
}} }}
'''Tin(II) chloride''' (stannous chloride) is a white ]line solid with the formula {{Tin}}{{Chlorine}}<sub>2</sub>. It forms a stable dihydrate, but ] solutions tend to undergo ], particularly if hot. SnCl<sub>2</sub> is widely used as a ] (in acid solution), and in ] baths for ]. Tin(II) chloride should not be confused with the other chloride of tin; ] or stannic chloride (SnCl<sub>4</sub>). '''Tin(II) chloride''', also known as '''stannous chloride''', is a white ]line solid with the formula {{chem2|SnCl2|auto=1}}. It forms a stable ], but ] solutions tend to undergo ], particularly if hot. SnCl<sub>2</sub> is widely used as a ] (in acid solution), and in ] baths for ]. Tin(II) chloride should not be confused with the other chloride of tin; ] or stannic chloride (SnCl<sub>4</sub>).


==Chemical structure== ==Chemical structure==
SnCl<sub>2</sub> has a ] of ]s, such that the molecule in the gas phase is bent. In the solid state, crystalline SnCl<sub>2</sub> forms chains linked via ] bridges as shown. The dihydrate is also three-coordinate, with one water coordinated on to the tin, and a second water coordinated to the first. The main part of the molecule stacks into double layers in the ], with the "second" water sandwiched between the layers. SnCl<sub>2</sub> has a ] of ]s, such that the molecule in the gas phase is bent. In the solid state, crystalline SnCl<sub>2</sub> forms chains linked via ] 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 ], with the "second" water sandwiched between the layers.


] ]
]s of the crystal structure of SnCl<sub>2</sub><ref>{{cite journal |journal = ]|volume = 57|issue = 1|year = 1996|pages = 7–16|title = The high pressure behaviour of the cotunnite and post-cotunnite phases of PbCl<sub>2</sub> and SnCl<sub>2</sub> |author = J. M. Leger, J. Haines, A. Atouf|doi = 10.1016/0022-3697(95)00060-7}}</ref>]] ]s of the crystal structure of SnCl<sub>2</sub><ref>{{cite journal |journal = ]|volume = 57|issue = 1|year = 1996|pages = 7–16|title = The high pressure behaviour of the cotunnite and post-cotunnite phases of PbCl<sub>2</sub> and SnCl<sub>2</sub> |author1=J. M. Leger |author2=J. Haines |author3=A. Atouf |doi = 10.1016/0022-3697(95)00060-7|bibcode = 1996JPCS...57....7L }}</ref>]]

{{clear|left}}


<br clear = left/>
==Chemical properties== ==Chemical properties==
Tin(II) chloride can dissolve in less than its own mass of water without apparent decomposition, but as the solution is diluted hydrolysis occurs to form an insoluble basic salt: Tin(II) chloride can dissolve in less than its own mass of water without apparent decomposition, but as the solution is diluted, hydrolysis occurs to form an insoluble basic salt:

:SnCl<sub>2</sub> (aq) + H<sub>2</sub>O (l) {{eqm}} Sn(OH)Cl (s) + HCl (aq) :SnCl<sub>2</sub> (aq) + H<sub>2</sub>O (l) {{eqm}} Sn(OH)Cl (s) + HCl (aq)


Therefore if clear solutions of tin(II) chloride are to be used, it must be dissolved in ] (typically of the same or greater molarity as the stannous chloride) to maintain the ] towards the left-hand side (using ]). Solutions of SnCl<sub>2</sub> are also unstable towards ] by the air: Therefore, if clear solutions of tin(II) chloride are to be used, it must be dissolved in ] (typically of the same or greater molarity as the stannous chloride) to maintain the ] towards the left-hand side (using ]). Solutions of SnCl<sub>2</sub> are also unstable towards ] by the air:

:6 SnCl<sub>2</sub> (aq) + O<sub>2</sub> (g) + 2 H<sub>2</sub>O (l) → 2 SnCl<sub>4</sub> (aq) + 4 Sn(OH)Cl (s) :6 SnCl<sub>2</sub> (aq) + O<sub>2</sub> (g) + 2 H<sub>2</sub>O (l) → 2 SnCl<sub>4</sub> (aq) + 4 Sn(OH)Cl (s)


This can be prevented by storing the solution over lumps of tin metal.<ref>{{cite book|author = H. Nechamkin|title = The Chemistry of the Elements|publisher = McGraw-Hill|location = New York|year = 1968}}</ref> This 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>


There are many such cases where tin(II) chloride acts as a reducing agent, reducing ] and ] salts to the metal, and iron(III) salts to iron(II), for example: There are many such cases where tin(II) chloride acts as a reducing agent, reducing ] and ] salts to the metal, and iron(III) salts to iron(II), for example:

:SnCl<sub>2</sub> (aq) + 2 FeCl<sub>3</sub> (aq) → SnCl<sub>4</sub> (aq) + 2 FeCl<sub>2</sub> (aq) :SnCl<sub>2</sub> (aq) + 2 FeCl<sub>3</sub> (aq) → SnCl<sub>4</sub> (aq) + 2 FeCl<sub>2</sub> (aq)


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Solutions of tin(II) chloride can also serve simply as a source of Sn<sup>2+</sup> ions, which can form other tin(II) compounds via ] reactions. For example, reaction with ] produces the brown/black ]: Solutions of tin(II) chloride can also serve simply as a source of Sn<sup>2+</sup> ions, which can form other tin(II) compounds via ] reactions. For example, reaction with ] produces the brown/black ]:

:SnCl<sub>2</sub> (aq) + Na<sub>2</sub>S (aq) → SnS (s) + 2 NaCl (aq) :SnCl<sub>2</sub> (aq) + Na<sub>2</sub>S (aq) → SnS (s) + 2 NaCl (aq)


If ] is added to a solution of SnCl<sub>2</sub>, a white precipitate of hydrated ] forms initially; this then dissolves in excess base to form a stannite salt such as sodium stannite: If ] is added to a solution of SnCl<sub>2</sub>, a white precipitate of hydrated ] forms initially; this then dissolves in excess base to form a stannite salt such as sodium stannite:

:SnCl<sub>2</sub>(aq) + 2 NaOH (aq) → SnO·H<sub>2</sub>O (s) + 2 NaCl (aq) :SnCl<sub>2</sub>(aq) + 2 NaOH (aq) → SnO·H<sub>2</sub>O (s) + 2 NaCl (aq)

:SnO·H<sub>2</sub>O (s) + NaOH (aq) → NaSn(OH)<sub>3</sub> (aq) :SnO·H<sub>2</sub>O (s) + NaOH (aq) → NaSn(OH)<sub>3</sub> (aq)


Anhydrous SnCl<sub>2</sub> can be used to make a variety of interesting tin(II) compounds in non-aqueous solvents. For example, the ] ] of ] reacts with SnCl<sub>2</sub> in ] to give the yellow linear two-coordinate compound Sn(OAr)<sub>2</sub> (Ar = ]).<ref>{{cite journal|author = B. Cetinkaya, I. Gumrukcu, M. F. Lappert, J. L. Atwood, R. D. Rogers and M. J. Zaworotko|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)|year = 1980|journal = ]|volume = 102|issue = 6|pages = 2088–2089|doi = 10.1021/ja00526a054}}</ref> Anhydrous SnCl<sub>2</sub> can be used to make a variety of interesting tin(II) compounds in non-aqueous solvents. For example, the ] ] of ] reacts with SnCl<sub>2</sub> in ] to give the yellow linear two-coordinate compound Sn(OAr)<sub>2</sub> (Ar = ]).<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=]|volume=102|issue=6|pages=2088–2089|doi=10.1021/ja00526a054|issn=0002-7863}}</ref>


Tin(II) chloride also behaves as a ], forming ] with ]s such as ] ion, for example: Tin(II) chloride also behaves as a ], forming ] with ]s such as ] ion, for example:

:SnCl<sub>2</sub> (aq) + CsCl (aq) → CsSnCl<sub>3</sub> (aq) :SnCl<sub>2</sub> (aq) + CsCl (aq) → CsSnCl<sub>3</sub> (aq)


Most of these complexes are ], and since complexes such as SnCl<sub>3</sub> have a full ], there is little tendency to add more than one ligand. The ] of electrons in such complexes is available for bonding, however, and therefore the complex itself can act as a ] or ligand. This seen in the ]-related product of the following reaction : Most of these complexes are ], and since complexes such as SnCl{{su|b=3|p=&minus;}} have a full ], there is little tendency to add more than one ligand. The ] of electrons in such complexes is available for bonding, however, and therefore the complex itself can act as a ] or ligand. This seen in the ]-related product of the following reaction:

:SnCl<sub>2</sub> + Fe(η<sup>5</sup>-C<sub>5</sub>H<sub>5</sub>)(CO)<sub>2</sub>HgCl → Fe(η<sup>5</sup>-C<sub>5</sub>H<sub>5</sub>)(CO)<sub>2</sub>SnCl<sub>3</sub> + Hg :SnCl<sub>2</sub> + Fe(η<sup>5</sup>-C<sub>5</sub>H<sub>5</sub>)(CO)<sub>2</sub>HgCl → Fe(η<sup>5</sup>-C<sub>5</sub>H<sub>5</sub>)(CO)<sub>2</sub>SnCl<sub>3</sub> + Hg


SnCl<sub>2</sub> can be used to make a variety of such compounds containing metal-metal bonds. For example, the reaction with ]: SnCl<sub>2</sub> can be used to make a variety of such compounds containing metal-metal bonds. For example, the reaction with ]:

:SnCl<sub>2</sub> + Co<sub>2</sub>(CO)<sub>8</sub> → (CO)<sub>4</sub>Co-(SnCl<sub>2</sub>)-Co(CO)<sub>4</sub> :SnCl<sub>2</sub> + Co<sub>2</sub>(CO)<sub>8</sub> → (CO)<sub>4</sub>Co-(SnCl<sub>2</sub>)-Co(CO)<sub>4</sub>


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Anhydrous SnCl<sub>2</sub> is prepared by the action of dry ] gas on ] metal. The dihydrate is made by a similar reaction, using ]: Anhydrous SnCl<sub>2</sub> is prepared by the action of dry ] gas on ] metal. The dihydrate is made by a similar reaction, using ]:


:Sn (s) + 2 HCl (aq) → SnCl<sub>2</sub> (aq) + {{chem|H|2}} (g) :Sn (s) + 2 HCl (aq) → SnCl<sub>2</sub> (aq) + {{chem2|H2}} (g)


The water is then carefully evaporated from the acidic solution to produce crystals of SnCl<sub>2</sub>·2H<sub>2</sub>O. This dihydrate can be ] to anhydrous using ]. The water then carefully evaporated from the acidic solution to produce crystals of SnCl<sub>2</sub>·2H<sub>2</sub>O. This dihydrate can be ] to anhydration using ].<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=], 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== ==Uses==
A solution of tin(II) chloride containing a little ] is used for the ] of steel, in order to make ]s. An electric potential is applied, and ] metal is formed at the ] via ]. A solution of tin(II) chloride containing a little ] is used for the ] of steel, in order to make ]s. An electric potential is applied, and ] metal is formed at the ] via ].


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

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


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


It also finds a use as a catalyst between acetone and hydrogen peroxide to form the tetrameric form of ].
Tin(II) chloride also finds wide use as a ]. This is seen in its use for silvering mirrors, where ] metal is deposited on the glass:

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


:Sn<sup>2+</sup> (aq) + 2 Ag<sup>+</sup> → Sn<sup>4+</sup> (aq) + 2 Ag (s) :Sn<sup>2+</sup> (aq) + 2 Ag<sup>+</sup> → Sn<sup>4+</sup> (aq) + 2 Ag (s)


A related reduction was traditionally used as an analytical test for {{Mercury}}<sup>2+</sup>(aq). For example, if SnCl<sub>2</sub> is added ] into a solution of ], a white precipitate of ] is first formed; as more SnCl<sub>2</sub> is added this turns black as metallic mercury is formed. Stannous chloride can be used to test for the presence of ] ]. SnCl<sub>2</sub> turns bright ] in the presence of gold (see '']''). A related reduction was traditionally used as an analytical test for {{chem2|auto=1|Hg(2+) (aq)}}. For example, if SnCl<sub>2</sub> is added ] into a solution of ], a white precipitate of ] is first formed; as more SnCl<sub>2</sub> 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 ] 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 SnCl<sub>2</sub> comes into contact with gold compounds, particularly ] salts, it forms a bright purple colloid known as ].<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}}</ref> A similar reaction occurs with ] and ] 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. 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.


In ], SnCl<sub>2</sub> is mainly used in the ], whereby a ] is reduced (via an ] salt) to an ] which is easily hydrolysed to an ].<ref>{{OrgSynth|title = &beta;-Naphthaldehyde|author = Williams, J. W.|collvol = 3|collvolpages = 626|year = 1955|prep = cv3p0626}}</ref> In ], SnCl<sub>2</sub> is mainly used in the ], whereby a ] is reduced (via an ] salt) to an ] which is easily hydrolysed to an ].<ref>{{OrgSynth|title = β-Naphthaldehyde|author = Williams, J. W.|collvol = 3|collvolpages = 626|year = 1955|prep = cv3p0626}}</ref>


The reaction usually works best with ] nitriles ]-CN. A related reaction (called the Sonn-Müller method) starts with an amide, which is treated with ] to form the imidoyl chloride salt. The reaction usually works best with ] nitriles ]-CN. A related reaction (called the Sonn-Müller method) starts with an amide, which is treated with ] to form the imidoyl chloride salt.
]

]

The Stephen reduction is less used today, because it has been mostly superseded by ] reduction. The Stephen reduction is less used today, because it has been mostly superseded by ] reduction.


Additionally, SnCl<sub>2</sub> is used to selectively reduce ] ] groups to ]s.<ref>{{cite journal|author = F. D. Bellamy and K. Ou|title = Selective reduction of aromatic nitro compounds with stannous chloride in non acidic and non aqueous medium|year = 1984|journal = ]|volume = 25|issue = 8|pages = 839–842|doi = 10.1016/S0040-4039(01)80041-1}}</ref> Additionally, SnCl<sub>2</sub> is used to selectively reduce ] ] groups to ]s.<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 = ]|volume = 25|issue = 8|pages = 839–842|doi = 10.1016/S0040-4039(01)80041-1}}</ref>


] ]
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SnCl<sub>2</sub> also reduces ]s to ]s. SnCl<sub>2</sub> also reduces ]s to ]s.


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


SnCl<sub>2</sub> is used in ] to reduce the radioactive agent ]-99m-] to assist in binding to blood cells.
Finally, aqueous Stannous Chloride is used by many precious metals refining hobbyists as an indicator of ] and ] in solutions.<ref>http://www.goldrefiningforum.com/phpBB3/</ref>


Molten SnCl<sub>2</sub> can be oxidised to form highly crystalline SnO<sub>2</sub> 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|url=https://www.worldcat.org/oclc/5902254906|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|url=https://www.worldcat.org/oclc/5690448892|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>
==Notes==
{{reflist}}


A Stannous reduction is used in ] ] to remove the negative charge from free ] 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>
==References==

Stannous Chloride is used for coating SnO<sub>2</sub> Tin Oxide doped conductive ] 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. * 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. * ''Handbook of Chemistry and Physics'', 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
Line 143: Line 180:
* A. F. Wells, '''Structural Inorganic Chemistry'', 5th ed., Oxford University Press, Oxford, UK, 1984. * 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. * J. March, ''Advanced Organic Chemistry'', 4th ed., p.&nbsp;723, Wiley, New York, 1992.

==References==
{{reflist}}


{{Tin compounds}} {{Tin compounds}}
{{Chlorides}}


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