Tin(IV) sulfide Article

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Tin(IV) sulfide
Ball-and-stick model of tin(IV) sulfide
Names
IUPAC name
Tin(IV) sulfide
Other names
Tin disulfide, Stannic sulfide, Mosaic gold
Identifiers
3D model ( JSmol)
ChEBI
ECHA InfoCard 100.013.867
EC Number 215-252-9
PubChem CID
UNII
Properties
S2Sn
Molar mass 182.83 g·mol−1
Appearance Gold-yellow powder
Odor Odorless
Density 4.5 g/cm3 [1]
Melting point 600 °C (1,112 °F; 873 K)
decomposes [1]
Insoluble
Solubility Soluble in aq. alkalis, decompose in aqua regia [1]
Insoluble in alkyl acetates, acetone [2]
Structure
Rhombohedral, hP3 [3]
P3m1, No. 164 [3]
3 2/m [3]
a = 3.65 Å, c = 5.88 Å [3]
α = 90°, β = 90°, γ = 120°
Octahedral (Sn4+) [3]
Hazards
GHS pictograms The exclamation-mark pictogram in the Globally Harmonized System of Classification and Labelling of Chemicals (GHS) [4]
GHS signal word Warning
H302, H312, H315, H319, H332, H335 [4]
P261, P280, P301+312, P302+352, P304+340, P305+351+338, P332+313 [4]
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 1: Exposure would cause irritation but only minor residual injury. E.g., turpentine Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
0
1
0
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Tin(IV) sulfide is a compound with the formula Sn S
2
. The compound crystallizes in the cadmium iodide motif, with the Sn(IV) situated in "octahedral holes' defined by six sulfide centers. [5] It occurs naturally as the rare mineral berndtite. [6] It is useful as semiconductor material with band gap 2.2 eV. [7]

Reactions

The compound precipitates as a brown solid upon the addition of H
2
S
to solutions of tin(IV) species. This reaction is reversed at low pH. Crystalline SnS
2
has a bronze color and is used in decorative coating [8] where it is known as mosaic gold.

The material also reacts with sulfide salts to give a series of thiostannates with the formula [SnS
2
]
m
[S]2n
n
. A simplified equation for this depolymerization reaction is

SnS
2
+ S2−
1/x[SnS2−
3
]
x
.

References

  1. ^ a b c Lide, David R., ed. (2009). CRC Handbook of Chemistry and Physics (90th ed.). Boca Raton, Florida: CRC Press. ISBN  978-1-4200-9084-0.
  2. ^ Comey, Arthur Messinger; Hahn, Dorothy A. (1921-02). A Dictionary of Chemical Solubilities: Inorganic (2nd ed.). New York: The MacMillan Company. p. 1080. Check date values in: |date= ( help)
  3. ^ a b c d e Voort, G.F. Vander, ed. (2004). "Crystal Structure*" (PDF). ASM Handbook. 9 (Metallography and Microstructures): 29–43. doi: 10.1361/asmhba0003722 (inactive 2018-08-27).
  4. ^ a b c d "SDS of Stannic sulfide" (PDF). https://www.pfaltzandbauer.com. Connecticut, USA: Pfaltz & Bauer, Inc. Retrieved 2014-07-13. External link in |website= ( help)
  5. ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN  0-19-855370-6.
  6. ^ Vaughan, D. J.; Craig, J. R. "Mineral Chemistry of Metal Sulfides" Cambridge University Press, Cambridge: 1978. ISBN  0-521-21489-0.
  7. ^ L.A.Burton et al., J. Mater. Chem. A, 2016, 4, 1312-1318 DOI: 10.1039/C5TA08214E.
  8. ^ Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN  0-12-352651-5.

External links