Tin(II) oxide

Tin(II) oxide

Names
IUPAC name Tin(II) oxide
Other names Stannous oxide, tin monoxide
Identifiers
CAS Number	21651-19-4 Y
3D model (Jmol)	Interactive image
ECHA InfoCard	100.040.439
EC Number	244-499-5
PubChem	88989
RTECS number	XQ3700000
InChI InChI=1S/O.Sn
SMILES O=[Sn]
Properties
Chemical formula	SnO
Molar mass	134.709 g/mol
Appearance	black or red powder when anhydrous, white when hydrated
Density	6.45 g/cm3
Melting point	1,080 °C (1,980 °F; 1,350 K)[1]
Solubility in water	insoluble
Structure
Crystal structure	tetragonal
Thermochemistry
Std molar entropy (So298)	56 J·mol−1·K−1[2]
Std enthalpy of formation (ΔfHo298)	−285 kJ·mol−1[2]
Hazards
Safety data sheet	ICSC 0956
Flash point	Non-flammable
US health exposure limits (NIOSH):
PEL (Permissible)	none[3]
REL (Recommended)	TWA 2 mg/m3[3]
IDLH (Immediate danger)	N.D.[3]
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 [77 °F], 100 kPa).
N verify (what is YN ?)
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

Tin(II) oxide burning

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.^[4]
Metastable, red SnO can be prepared by gentle heating of the precipitate produced by the action of aqueous ammonia on a tin(II) salt.^[4]
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.^[5][6]

SnC₂O₄·2H₂O → SnO + CO₂ + CO + 2 H₂O

Tin(II) oxide burns in air with a dim green flame to form SnO₂.^[4]

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.^[4]

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⁻.^[4] 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⁺.^[4] Note that anhydrous stannites, e.g. K₂Sn₂O₃, K₂SnO₂ are also known.^[7][8][9] SnO is a reducing agent and this appears to its role in the manufacture of so-called "copper ruby glass".^[10]

Structure

Black, α-SnO adopts the tetragonal PbO layer structure containing four coordinate square pyramidal tin atoms.^[11] This form is found in nature as the rare mineral romarchite.^[12] 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.^[13]
Non-stoichiometry has been observed in SnO.^[14]

The electronic band gap has been measured between 2.5eV and 3eV.^[15]

Uses

The dominant use of stannous oxide is as a precursor in manufacturing of other, typically trivalent, tin compounds or salts. Stannous oxide may also be employed as a reducing agent and in the creation of ruby glass- See "Red Glass Coloration - A Colorimetric and Structural Study" By Torun Bring. Pub. Vaxjo University.Red Glass Coloration - A Colorimetric and Structural Study. . 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.^[16]

References