Tin(II) oxide
Template:Short description Script error: No such module "redirect hatnote". Template:Chembox 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
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Blue-black SnO can be produced by heating the tin(II) oxide hydrate, Template:Chem2 (x < 1) precipitated when a tin(II) salt is reacted with an alkali hydroxide such as NaOH.[1]
Metastable, red SnO can be prepared by gentle heating of the precipitate produced by the action of aqueous ammonia on a tin(II) salt.[1]
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.[2][3]
- SnC2O4·2H2O → SnO + CO2 + CO + 2 H2O
Tin(II) oxide burns in air with a dim green flame to form SnO2.[1]
- 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.[1]
- 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−.[1] It can be dissolved in strong acid solutions to give the ionic complexes Sn(OH2)32+ and Sn(OH)(OH2)2+, and in less acid solutions to give Sn3(OH)42+.[1] Note that anhydrous stannites, e.g. K2Sn2O3, K2SnO2 are also known.[4][5][6] SnO is a reducing agent and is thought to reduce copper(I) to metallic clusters in the manufacture of so-called "copper ruby glass".[7]
Structure
Black, α-SnO adopts the tetragonal PbO layer structure containing four coordinate square pyramidal tin atoms.[8] This form is found in nature as the rare mineral romarchite.[9] 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.[10] The electronic structure and chemistry of the lone pair determines most of the properties of the material.[11]
Non-stoichiometry has been observed in SnO.[12]
The electronic band gap has been measured between 2.5eV and 3eV.[13]
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.[14] 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.[15]
References
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- ↑ a b c d e f Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier Template:ISBN
- ↑ Satya Prakash (2000),Advanced Inorganic Chemistry: V. 1, S. Chand, Template:ISBN
- ↑ Arthur Sutcliffe (1930) Practical Chemistry for Advanced Students (1949 Ed.), John Murray - London.
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- ↑ R M Braun R Hoppe Z. Naturforsch. (1982), 37B, 688-694
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- ↑ Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications Template:ISBN
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- ↑ Science and Technology of Chemiresistor Gas Sensors By Dinesh K. Aswal, Shiv K. Gupta (2006), Nova Publishers, Template:ISBN
- ↑ "Red Glass Coloration - A Colorimetric and Structural Study" By Torun Bring. Pub. Vaxjo University.
- ↑ Script error: No such module "Citation/CS1".Script error: No such module "Unsubst".
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