Samarium(III) chloride

Names
IUPAC name

samarium(III) chloride

Other names

samarium trichloride
trichlorosamarium

Identifiers

CAS Number

* 10361-82-7 (anhydrous) Y
* 13465-55-9 (hexahydrate) Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 55428 Y

EC Number |

* 233-797-0

PubChem CID

* 10131313

UNII |

* 5J4QGH7J16 Y
* 9874IU4M1V (hexahydrate) Y

InChI

* InChI=1S/3ClH.Sm/h3*1H;/q;;;+3/p-3 Y

Key: BHXBZLPMVFUQBQ-UHFFFAOYSA-K Y

* InChI=1/3ClH.Sm/h3*1H;/q;;;+3/p-3

Key: BHXBZLPMVFUQBQ-DFZHHIFOAZ

SMILES

* Cl[Sm](Cl)Cl

Properties

Chemical formula

| SmCl3
Molar mass | 256.76 g/mol (anhydrous)
364.80 g/mol (hexahydrate)
Appearance  | pale yellow solid (anhydrous)

cream-coloured solid (hexahydrate)

Density | 4.46 g/cm3 (anhydrous)

2.383 g/cm3 (hexahydrate)

Melting point |  682 °C (1,260 °F; 955 K)
Boiling point | decomposes

Solubility in water

| 92.4 g/100 mL (10 °C)
Structure

Crystal structure

| hexagonal, hP8

Space group

| P63/m, No. 176

Coordination geometry

| Tricapped trigonal prismatic
(nine-coordinate)
Hazards
Main hazards | Irritant
GHS pictograms |
GHS Signal word | Warning

GHS hazard statements

| H315, H319

GHS precautionary statements

| P264, P280, P302+352, P305+351+338, P321, P332+313, P337+313, P362
Related compounds

Other anions

| Samarium(III) fluoride
Samarium(III) bromide
Samarium(III) oxide

Other cations

| Samarium(II) chloride
Promethium(III) chloride
Europium(III) chloride

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

Samarium(III) chloride, also known as samarium trichloride, is an inorganic compound of samarium and chloride. It is a pale yellow salt that rapidly absorbs water to form a hexahydrate, SmCl3.6H2O.[1] The compound has few practical applications but is used in laboratories for research on new compounds of samarium.

## Contents

* 1 Structure
* 2 Preparation and reactions
* 3 Uses
* 3.1 In laboratory
* 4 References

## Structure

Like several related chlorides of the lanthanides and actinides, SmCl3 crystallises in the UCl3 motif. The Sm3+ centres are nine-coordinate, occupying trigonal prismatic sites with additional chloride ligands occupying the three square faces.

## Preparation and reactions

SmCl3 is prepared by the "ammonium chloride" route, which involves the initial synthesis of (NH4)2[SmCl5]. This material can be prepared from the common starting materials at reaction temperatures of 230 °C from samarium oxide:[2]

10 NH4Cl + Sm2O3 → 2 (NH4)2[SmCl5] + 6 NH3 \+ 3 H2O

The pentachloride is then heated to 350-400 °C resulting in evolution of ammonium chloride and leaving a residue of the anhydrous trichloride:

(NH4)2[SmCl5] → 2 NH4Cl + SmCl3

It can also be prepared from samarium metal and hydrochloric acid.[3][4]

2 Sm + 6 HCl → 2 SmCl3 \+ 3 H2

Aqueous solutions of samarium(III) chloride can be prepared by dissolving metallic samarium or samarium carbonate in hydrochloric acid.

Samarium(III) chloride is a moderately strong Lewis acid, which ranks as "hard" according to the HSAB concept. Aqueous solutions of samarium chloride can be used to prepare samarium trifluoride:

SmCl3 \+ 3 KF → SmF3 \+ 3 KCl

## Uses

Samarium(III) chloride is used for the preparation of samarium metal, which has a variety of uses, notably in magnets. Anhydrous SmCl3 is mixed with sodium chloride or calcium chloride to give a low melting point eutectic mixture. Electrolysis of this molten salt solution gives the free metal.[5]

### In laboratory

Samarium(III) chloride can also be used as a starting point for the preparation of other samarium salts. The anhydrous chloride is used to prepare organometallic compounds of samarium, such as bis(pentamethylcyclopentadienyl)alkylsamarium(III) complexes.[6]

## References

1. ↑ F. T. Edelmann, P. Poremba (1997). W. A. Herrmann. ed. Synthetic Methods of Organometallic and Inorganic Chemistry. 6. Stuttgart: Georg Thieme Verlag.
2. ↑ Meyer, G. (1989). "The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides—The Example of Ycl 3". The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides-The Example of YCl3. Inorganic Syntheses. 25. pp. 146–150. doi:10.1002/9780470132562.ch35. ISBN 978-0-470-13256-2.
3. ↑ L. F. Druding, J. D. Corbett (1961). "Lower Oxidation States of the Lanthanides. Neodymium(II) Chloride and Iodide". J. Am. Chem. Soc. 83 (11): 2462–2467. doi:10.1021/ja01472a010.
4. ↑ J. D. Corbett (1973). "Reduced Halides of the Rare Earth Elements". Rev. Chim. Minérale 10: 239.
5. ↑ Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. ISBN 978-0-08-022057-4. https://books.google.com/books?id=OezvAAAAMAAJ&q=0-08-022057-6&dq=0-08-022057-6&source=bl&ots=m4tIRxdwSk&sig=XQTTjw5EN9n5z62JB3d0vaUEn0Y&hl=en&sa=X&ei=UoAWUN7-EM6ziQfyxIDoCQ&ved=0CD8Q6AEwBA.
6. ↑ G. A. Molander, E. D. Dowdy (1999). Shu Kobayashi. ed. Lanthanides: Chemistry and Use in Organic Synthesis. Berlin: Springer-Verlag. pp. 119–154. ISBN 3-540-64526-8. https://archive.org/details/springer_10.1007-3-540-69801-9.

* v
* t
* e

Samarium compounds

Samarium(II)|

* SmCl2
* SmBr2
* SmB6
* SmI2
* SmS
* SmSe
* SmTe

Samarium(III)|

* SmCl3
* SmBr3
* SmF3
* Sm2O3
* Sm2S3
* Sm2(SO4)3
* Sm(NO3)3
* Sm2(CO3)3

| Organosamarium(III)|

* Sm2(C2O4)3
* Sm(C5H5)3

|

* v
* t
* e

Salts and covalent derivatives of the chloride ion

HCl |  |  |  | He

|
|
|
|

LiCl | BeCl2 | BCl3
B2Cl4 | CCl4 | NCl3
ClN3 | Cl2O
ClO2
Cl2O7 | ClF
ClF3
ClF5 | Ne
NaCl | MgCl2 | AlCl
AlCl3 | SiCl4 | P2Cl4
PCl3
PCl5 | S2Cl2
SCl2
SCl4 | Cl2 | Ar
KCl | CaCl
CaCl2 | ScCl3 | TiCl2
TiCl3
TiCl4 | VCl2
VCl3
VCl4
VCl5 | CrCl2
CrCl3
CrCl4 | MnCl2 | FeCl2
FeCl3 | CoCl2
CoCl3 | NiCl2 | CuCl
CuCl2 | ZnCl2 | GaCl2
GaCl3 | GeCl2
GeCl4 | AsCl3
AsCl5 | Se2Cl2
SeCl4 | BrCl | KrCl
RbCl | SrCl2 | YCl3 | ZrCl3
ZrCl4 | NbCl4
NbCl5 | MoCl2
MoCl3
MoCl4
MoCl5
MoCl6 | TcCl4 | RuCl3 | RhCl3 | PdCl2 | AgCl | CdCl2 | InCl
InCl2
InCl3 | SnCl2
SnCl4 | SbCl3
SbCl5 | Te3Cl2
TeCl4 | ICl
ICl3 | XeCl
XeCl2
CsCl | BaCl2 |  | HfCl4 | TaCl5 | WCl2
WCl3
WCl4
WCl5
WCl6 | Re3Cl9
ReCl4
ReCl5
ReCl6 | OsCl4 | IrCl2
IrCl3
IrCl4 | PtCl2
PtCl4 | AuCl
AuCl3 | Hg2Cl2,
HgCl2 | TlCl | PbCl2,
PbCl4 | BiCl3 | PoCl2,
PoCl4 | AtCl  | RnCl2
FrCl | RaCl2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaCl3 | CeCl3 | PrCl3 | NdCl2,
NdCl3 | PmCl3 | SmCl2,
SmCl3 | EuCl2,
EuCl3 | GdCl3 | TbCl3 | DyCl2,
DyCl3 | HoCl3 | ErCl3 | TmCl2
TmCl3 | YbCl2
YbCl3 | LuCl3
AcCl3 | ThCl4 | PaCl5 | UCl3
UCl4
UCl5
UCl6 | NpCl4 | PuCl3 | AmCl2
AmCl3 | CmCl3 | BkCl3 | CfCl3 | EsCl3 | Fm  | Md  | No  | LrCl3

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*[CID]: Compound ID
*[H315]: Causes skin irritation
*[H319]: Causes serious eye irritation
*[P264]: Wash … thoroughly after handling
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