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Tin(II) oxide

Names
IUPAC name Tin(II) oxide
Other names Stannous oxide Tin monoxide
Identifiers
CAS Number	21651-19-4
3D model (JSmol)	Interactive image
ECHA InfoCard	100.040.439
EC Number	244-499-5
PubChem CID	88989
RTECS number	XQ3700000
UNII	JB2MV9I3LS
CompTox Dashboard (EPA)	DTXSID2066723
InChI InChI=1S/O.Sn
SMILES O=
Properties
Chemical formula	SnO
Molar mass	134.709 g/mol
Appearance	black or red powder when anhydrous, white when hydrated
Density	6.45 g/cm
Melting point	1,080 °C (1,980 °F; 1,350 K)
Solubility in water	insoluble
Magnetic susceptibility (χ)	−19.0·10 cm/mol
Structure
Crystal structure	tetragonal
Thermochemistry
Std molar entropy (S298)	56 J·mol·K
Std enthalpy of formation (ΔfH298)	−285 kJ·mol
Hazards
Flash point	Non-flammable
NIOSH (US health exposure limits):
PEL (Permissible)	none
REL (Recommended)	TWA 2 mg/m
IDLH (Immediate danger)	N.D.
Safety data sheet (SDS)	ICSC 0956
Related compounds
Other anions	Tin sulfide Tin selenide Tin telluride
Other cations	Carbon monoxide Silicon monoxide Germanium(II) oxide Lead(II) oxide
Related tin oxides	Tin dioxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). N verify (what is  ?) Infobox references

Tin(II) oxide (stannous oxide) is a compound with the formula SnO. It is composed of tin and oxygen where tin has the oxidation state of +2. There are two forms, a stable blue-black form and a metastable red form.

Preparation and reactions

Blue-black SnO can be produced by heating the tin(II) oxide hydrate, SnO·xH₂O (x<1) precipitated when a tin(II) salt is reacted with an alkali hydroxide such as NaOH.
Metastable, red SnO can be prepared by gentle heating of the precipitate produced by the action of aqueous ammonia on a tin(II) salt.
SnO may be prepared as a pure substance in the laboratory, by controlled heating of tin(II) oxalate (stannous oxalate) in the absence of air or under a CO₂ atmosphere. This method is also applied to the production of ferrous oxide and manganous oxide.

SnC₂O₄·2H₂O → SnO + CO₂ + CO + 2 H₂O

Tin(II) oxide burns in air with a dim green flame to form SnO₂.

2 SnO + O₂ → 2 SnO₂

When heated in an inert atmosphere initially disproportionation occurs giving Sn metal and Sn₃O₄ which further reacts to give SnO₂ and Sn metal.

4SnO → Sn₃O₄ + Sn

Sn₃O₄ → 2SnO₂ + Sn

SnO is amphoteric, dissolving in strong acid to give tin(II) salts and in strong base to give stannites containing Sn(OH)₃. It can be dissolved in strong acid solutions to give the ionic complexes Sn(OH₂)₃and Sn(OH)(OH₂)₂, and in less acid solutions to give Sn₃(OH)₄. Note that anhydrous stannites, e.g. K₂Sn₂O₃, K₂SnO₂ are also known. SnO is a reducing agent and is thought to reduce copper(I) to metallic clusters in the manufacture of so-called "copper ruby glass".

Structure

Black, α-SnO adopts the tetragonal PbO layer structure containing four coordinate square pyramidal tin atoms. This form is found in nature as the rare mineral romarchite. The asymmetry is usually simply ascribed to a sterically active lone pair; however, electron density calculations show that the asymmetry is caused by an antibonding interaction of the Sn(5s) and the O(2p) orbitals. The electronic structure and chemistry of the lone pair determines most of the properties of the material.

Non-stoichiometry has been observed in SnO.

The electronic band gap has been measured between 2.5eV and 3eV.

Uses

The dominant use of stannous oxide is as a precursor in manufacturing of other, typically divalent, tin compounds or salts. Stannous oxide may also be employed as a reducing agent and in the creation of ruby glass. It has a minor use as an esterification catalyst.

Cerium(III) oxide in ceramic form, together with Tin(II) oxide (SnO) is used for illumination with UV light.

References

1. Tin and Inorganic Tin Compounds: Concise International Chemical Assessment Document 65, (2005), World Health Organization
2. ^ Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
3. ^ NIOSH Pocket Guide to Chemical Hazards. "#0615". National Institute for Occupational Safety and Health (NIOSH).
4. ^ Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
5. Satya Prakash (2000),Advanced Inorganic Chemistry: V. 1, S. Chand, ISBN 81-219-0263-0
6. Arthur Sutcliffe (1930) Practical Chemistry for Advanced Students (1949 Ed.), John Murray - London.
7. Braun, Rolf Michael; Hoppe, Rudolf (1978). "The First Oxostannate(II): K₂Sn₂O₃". Angewandte Chemie International Edition in English. 17 (6): 449–450. doi:10.1002/anie.197804491.
8. Braun, R. M.; Hoppe, R. (1982). "Über Oxostannate(II). III. K₂Sn₂O₃, Rb₂Sn₂O₃ und Cs₂Sn₂O₃ - ein Vergleich". Zeitschrift für Anorganische und Allgemeine Chemie. 485: 15–22. doi:10.1002/zaac.19824850103.
9. R M Braun R Hoppe Z. Naturforsch. (1982), 37B, 688-694
10. Bring, T.; Jonson, B.; Kloo, L.; Rosdahl, J; Wallenberg, R. (2007), "Colour development in copper ruby alkali silicate glasses. Part I: The impact of tin oxide, time and temperature", Glass Technology, Eur. J. Glass Science & Technology, Part A, 48 (2): 101–108, ISSN 1753-3546
11. Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications ISBN 0-19-855370-6
12. Ramik, R. A.; Organ, R. M.; Mandarino, J. A. (2003). "On Type Romarchite and Hydroromarchite from Boundary Falls, Ontario, and Notes on Other Occurrences". The Canadian Mineralogist. 41 (3): 649–657. Bibcode:2003CaMin..41..649R. doi:10.2113/gscanmin.41.3.649.
13. Walsh, Aron; Watson, Graeme W. (2004). "Electronic structures of rocksalt, litharge, and herzenbergite SnO by density functional theory". Physical Review B. 70 (23): 235114. Bibcode:2004PhRvB..70w5114W. doi:10.1103/PhysRevB.70.235114.
14. Mei, Antonio B.; Miao, Ludi; Wahila, Matthew J.; Khalsa, Guru; Wang, Zhe; Barone, Matthew; Schreiber, Nathaniel J.; Noskin, Lindsey E.; Paik, Hanjong; Tiwald, Thomas E.; Zheng, Qiye (2019-10-21). "Adsorption-controlled growth and properties of epitaxial SnO films". Physical Review Materials. 3 (10): 105202. Bibcode:2019PhRvM...3j5202M. doi:10.1103/PhysRevMaterials.3.105202. S2CID 208008118.
15. Moreno, M. S.; Varela, A.; Otero-Díaz, L. C. (1997). "Cation nonstoichiometry in tin-monoxide-phaseSn1−δOwith tweed microstructure". Physical Review B. 56 (9): 5186–5192. doi:10.1103/PhysRevB.56.5186.
16. Science and Technology of Chemiresistor Gas Sensors By Dinesh K. Aswal, Shiv K. Gupta (2006), Nova Publishers, ISBN 1-60021-514-9
17. "Red Glass Coloration - A Colorimetric and Structural Study" By Torun Bring. Pub. Vaxjo University.
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• Amphoteric compounds
• Oxides
• Reducing agents
• Tin(II) compounds