Wikipedia:WikiProject Chemicals/Chembox validation/VerifiedDataSandbox and Samarium(III) oxide: Difference between pages

{{One source | date= March 2014}}

| verifiedrevid = 464386841

| Name = Samarium(III) oxide

| ImageFile = Samarium(III) oxide.jpg

| ImageName = Samarium(III) oxide

| OtherNames = samarium sesquioxide, samaria

| IUPACName = samarium(III) oxide

| SystematicName =

| CASNo_Ref = {{cascite|correct|CAS}}

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = 91N8739X2N

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| StdInChI_Ref = {{stdinchicite|correct|chemspider}}

| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}

| SMILES = O=[Sm]O[Sm]=O

| SMILES1 = [Sm+3].[Sm+3].[O-2].[O-2].[O-2]

| PubChem = 159425

| EINECS = 235-043-6

| Formula = Sm₂O₃

| MolarMass = 348.72 g/mol

| Appearance = yellow-white crystals

| Density = 8.347 g/cm³

| Solubility = insoluble

| MeltingPtC = 2335

| BoilingPt = Not Stated

| MagSus = +1988.0·10⁻⁶ cm³/mol

| CrystalStruct = Cubic, cI80

| SpaceGroup = Ia-3, No. 206

}}

| Section4 =

| Section5 =

| Section6 =

| GHSPictograms = {{GHS07}}{{GHS09}}

| GHSSignalWord = Warning

| HPhrases = {{H-phrases|319|410}}

| PPhrases = {{P-phrases|264|273|280|305+351+338|337+313|391|501}}

}}

| Section8 = {{Chembox Related

| OtherAnions = [[Samarium(III) chloride]]

| OtherCations = [[Promethium(III) oxide]], [[Europium(III) oxide]]

'''Samarium(III) oxide''' ([[Samarium|Sm₂]][[Oxygen|O₃]]) is a [[chemical compound]]. Samarium oxide readily forms on the surface of [[samarium]] metal under humid conditions or temperatures in excess of 150°C in dry air. Similar to rust on metallic iron, this oxide layer spalls off the surface of the metal, exposing more metal to continue the reaction. The oxide is commonly white to off yellow in color and is often encountered as a highly fine dust like powder.

==Uses==

Samarium(III) oxide is used in optical and infrared absorbing glass to absorb [[infrared radiation]]. Also, it is used as a [[neutron]] absorber in control rods for nuclear power reactors. The oxide catalyzes the dehydration and dehydrogenation of primary and secondary alcohols.<ref>Catalytic properties of samarium oxide with respect to the dehydrogenation and dehydration of alcohols and the dehydrogenation of tetralin. Bulletin of the Academy of Sciences of the USSR, Division of chemical science, January 1964, Volume 13, Issue 1, pp 6–9.</ref> Another use involves preparation of other samarium salts.<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}</ref>

==Preparations==

Samarium(III) oxide may be prepared by two methods:

1. [[thermal decomposition]] of samarium(III) carbonate, hydroxide, nitrate, oxalate or sulfate:

: Sm₂(CO₃)₃ → Sm₂O₃ + 3 CO₂

2. by burning the metal in air or oxygen at a temperature above 150&nbsp;°C:

: 4 Sm + 3 O₂ → 2 Sm₂O₃

==Reactions==

Samarium(III) oxide dissolves in mineral acids, forming salts upon [[evaporation]] and [[crystallization]]:

: Sm₂O₃ + 6 HCl → 2 SmCl₃ + 3 H₂O

The oxide can be reduced to metallic samarium by heating with a [[reducing agent]], such as hydrogen or [[carbon monoxide]], at elevated temperatures.

==References==

{{reflist}}

{{Samarium compounds}}

{{Oxides}}

[[Category:Sesquioxides]]

[[Category:Crystals in space group 206]]

[[Category:Samarium(III) compounds]]