Yttrium(III) chloride
{{chembox
| Watchedfields = changed
| verifiedrevid = 470635247
| Name = Yttrium(III) chloride
| ImageFile1 = Yttrium(III)-chloride-xtal-one-layer-3D-bs-17.png
| ImageCaption1 = Part of a layer in the crystal structure of YCl3
| ImageName1 = Yttrium(III) chloride
| ImageFileL2 = Yttrium(III)-chloride-xtal-unit-cell-3D-bs-17.png
| ImageCaptionL2 = Unit cell
| ImageFileR2 = Yttrium(III)-chloride-xtal-layers-3D-bs-17.png
| ImageCaptionR2 = Layer packing
| IUPACName = Yttrium(III) chloride
Yttrium trichloride
| Section1 = {{Chembox Identifiers
| index1_label = hexahydrate
| CASNo = 10361-92-9
| CASNo_Ref = {{cascite|correct|CAS}}
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 59696
| ChemSpiderID1 = 175148
| EC_number1 = 233-801-0
| PubChem = 10198055
| PubChem1 = 16211498
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 11521XLD38
| RTECS = ZG3150000
| InChI = 1/3ClH.Y/h3*1H;/q;;;+3/p-3
| InChIKey = PCMOZDDGXKIOLL-DFZHHIFOAW
| SMILES = [Y+3].[Cl-].[Cl-].[Cl-]
| SMILES_Comment = anhydrous
| SMILES1 = [OH2+][Y-3]([OH2+])([OH2+])([OH2+])([OH2+])[OH2+].[Cl-].[Cl-].[Cl-]
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/3ClH.Y/h3*1H;/q;;;+3/p-3
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = PCMOZDDGXKIOLL-UHFFFAOYSA-K
| InChI1=1S/3ClH.6H2O.Y/h3*1H;6*1H2;/q;;;;;;;;;+3/p-3
| InChIKey1 = IINACGXCEZNYTF-UHFFFAOYSA-K
}}
| Section2 = {{Chembox Properties
| Formula = YCl3
| Appearance = white solid
| Density = 2.61 g/cm3{{cite book | editor= Haynes, William M. | year = 2011 | title = CRC Handbook of Chemistry and Physics | edition = 92nd | publisher = CRC Press | isbn = 978-1439855119|page=4.99| title-link = CRC Handbook of Chemistry and Physics }}
| Solubility = 751 g/L (20 °C)
| SolubleOther = 601 g/L ethanol (15 °C)
606 g/L pyridine (15 °C)
{{Citation
| last = Spencer
| first = James F. | year = 1919
| title = The Metals of the Rare Earths | location = New York | publisher = Longmans, Green, and Co | pages = 135
| url = https://books.google.com/books?id=W2zxN_FLQm8C&pg=PA135 }}
| MeltingPtC = 721
| BoilingPtC = 1482
}}
| Section3 = {{Chembox Structure
| CrystalStruct = Monoclinic, mS16
| SpaceGroup = C2/m, No. 12
| LattConst_a = 0.692 nm
| LattConst_b = 1.194 nm
| LattConst_c = 0.644 nm
| LattConst_alpha = 90
| LattConst_beta = 111
| LattConst_gamma = 90
| LattConst_ref =
| LattConst_Comment =
| UnitCellVolume =
| UnitCellFormulas = 4
}}
| Section4 = {{Chembox Hazards
| ExternalSDS = [https://ereztech.com/wp-content/uploads/chemical_sds/SDS-Y1929.pdf External MSDS]
| GHSPictograms = {{GHS07}}
| GHSSignalWord = Warning
| HPhrases = {{H-phrases|315|319|335}}
| PPhrases = {{P-phrases|
261|264|271|280|302 + 352|304 + 340|305 + 351 + 338|312|332 + 313|337 + 313|362
}}
| NFPA-H = 1
| NFPA-F = 0
| NFPA-R = 0
}}
| Section7 =
| Section8 = {{Chembox Related
| OtherAnions = Yttrium(III) fluoride
Yttrium(III) bromide
Yttrium(III) iodide
| OtherCations = Scandium(III) chloride
Lutetium(III) chloride
}}
}}
Yttrium(III) chloride is an inorganic compound of yttrium and chloride. It exists in two forms, the hydrate (YCl3(H2O)6) and an anhydrous form (YCl3). Both are colourless salts that are highly soluble in water and deliquescent.
Structure
Solid YCl3 adopts a cubic{{Citation needed|date=July 2023|reason=how can a cubic structure be layered??}} structure with close-packed chloride ions and yttrium ions filling one third of the octahedral holes and the resulting YCl6 octahedra sharing three edges with adjacent octahedra, giving it a layered structure.Wells A.F. (1984) Structural Inorganic Chemistry 5th edition Oxford Science Publications {{ISBN|0-19-855370-6}}{{ cite journal | first1 = D. H. | last1 = Templeton | first2 = Giles F. | last2 = Carter | title = The Crystal Structures of Yttrium Trichloride and Similar Compounds | journal = J. Phys. Chem. | year = 1954 | volume = 58 | issue = 11 | pages = 940–944 | doi = 10.1021/j150521a002 }} This structure is shared by a range of compounds, notably AlCl3.
Preparation and reactions
YCl3 is often prepared by the "ammonium chloride route," starting from either Y2O3 or hydrated chloride or oxychloride.
{{cite book
| last =Meyer
| first =G.
| title =The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides-The Example of YCl3
| chapter =The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides—The Example of Ycl 3
| series =Inorganic Syntheses
| volume =25
| year =1989
| pages =146–150
| doi =10.1002/9780470132562.ch35
| isbn =978-0-470-13256-2}}
{{cite book |title=Synthetic Methods of Organometallic and Inorganic Chemistry |volume=VI |last=Edelmann |first=F. T. |author2=Poremba, P. |editor=Herrmann, W. A. |year=1997 |publisher=Georg Thieme Verlag |location=Stuttgart |isbn=978-3-13-103021-4 }} or YCl3·6H2O.{{cite journal|last=Taylor|first=M.D.|author2=Carter, C.P. |title=Preparation of anhydrous lanthanide halides, especially iodides|journal=Journal of Inorganic and Nuclear Chemistry|volume=24|issue=4|pages=387–391|doi=10.1016/0022-1902(62)80034-7|year=1962}} These methods produce (NH4)2[YCl5]:
:10 NH4Cl + Y2O3 → 2 (NH4)2[YCl5] + 6 NH3 + 3 H2O
:YCl3·6H2O + 2 NH4Cl → (NH4)2[YCl5] + 6 H2O
The pentachloride decomposes thermally according to the following equation:
: (NH4)2[YCl5] → 2 NH4Cl + YCl3
The thermolysis reaction proceeds via the intermediacy of (NH4)[Y2Cl7].
Treating Y2O3 with aqueous HCl produces the hydrated chloride (YCl3·6H2O). When heated, this salt yields yttrium oxychloride rather than reverting to the anhydrous form.
References
{{reflist}}
{{Yttrium compounds}}
{{Chlorides}}
{{DEFAULTSORT:Yttrium(Iii) Chloride}}