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Gadolinium(III) chloride
Names
	IUPAC name Gadolinium(III) chloride
	Other names Gadolinium trichloride; Gadolinium chloride
Identifiers
CAS Number	10138-52-0 ; 19423-81-5 (hydrate) ; 13450-84-5 (hexahydrate) ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:37288 ;
ChEMBL	ChEMBL1697696 ;
ChemSpider	55406 ;
ECHA InfoCard	100.030.338
PubChem CID	61486;
UNII	P7082WY76D ;
CompTox Dashboard (EPA)	DTXSID2044761 ;
	InChI InChI=1S/3ClH.Gd/h31H;/q;;;+3/p-3 Key: MEANOSLIBWSCIT-UHFFFAOYSA-K ; InChI=1/3ClH.Gd/h31H;/q;;;+3/p-3 Key: MEANOSLIBWSCIT-DFZHHIFOAP;
	SMILES Cl[Gd](Cl)Cl;
Properties
Chemical formula	GdCl3
Molar mass	263.61 g/mol
Appearance	white crystals; hygroscopic
Density	4.52 g/cm3
Melting point	609 °C (1,128 °F; 882 K)
Boiling point	1,580 °C (2,880 °F; 1,850 K)
Solubility in water	94.65 g/100mL, 25°C
Magnetic susceptibility (χ)	+27,930·10−6 cm3/mol
Structure
Crystal structure	hexagonal, hP8
Space group	P63/m, No. 176
Related compounds
Other anions	Gadolinium(III) fluoride; Gadolinium(III) bromide; Gadolinium(III) oxide
Other cations	Europium(III) chloride; Terbium(III) chloride
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Gadolinium(III) chloride, also known as gadolinium trichloride, is GdCl₃. It is a colorless, hygroscopic, water-soluble solid. The hexahydrate GdCl₃∙6H₂O is commonly encountered and is sometimes also called gadolinium trichloride. Gd³⁺ species are of special interest because the ion has the maximum number of unpaired spins possible, at least for known elements. With seven valence electrons and seven available f-orbitals, all seven electrons are unpaired and symmetrically arranged around the metal. The high magnetism and high symmetry combine to make Gd³⁺ a useful component in NMR spectroscopy and MRI.

Preparation

GdCl₃ is usually prepared by the "ammonium chloride" route, which involves the initial synthesis of (NH₄)₂[GdCl₅]. This material can be prepared from the common starting materials at reaction temperatures of 230 °C from gadolinium oxide:^[2]

10 NH₄Cl + Gd₂O₃ → 2 (NH₄)₂[GdCl₅] + 6 NH₃ + 3 H₂O

from hydrated gadolinium chloride:

4 NH₄Cl + 2 GdCl₃∙6H₂O → 2 (NH₄)₂[GdCl₅] + 12 H₂O

from gadolinium metal:

10 NH₄Cl + 2 Gd → 2 (NH₄)₂[GdCl₅] + 6 NH₃ + 3 H₂

In the second step the pentachloride is decomposed at 300 °C:

(NH₄)₂[GdCl₅] → GdCl₃ + 2 NH₄Cl

This pyrolysis reaction proceeds via the intermediacy of NH₄[Gd₂Cl₇].

The ammonium chloride route is more popular and less expensive than other methods. GdCl₃ can, however, also be synthesized by the reaction of solid Gd at 600 °C in a flowing stream of HCl.^[3]

Gd + 3 HCl → GdCl₃ + 3/2 H₂

Gadolinium(III) chloride also forms a hexahydrate, GdCl₃∙6H₂O. The hexahydrate is prepared by gadolinium(III) oxide (or chloride) in concentrated HCl followed by evaporation.^[4]

Structure

GdCl₃ crystallizes with a hexagonal UCl₃ structure, as seen for other 4f trichlorides including those of La, Ce, Pr, Nd, Pm, Sm, Eu.^[5] The following crystallize in theYCl₃ motif: DyCl₃, HoCl₃, ErCl₃, TmCl₃, YdCl₃, LuCl₃, YCl₃). The UCl₃ motif features 9-coordinate metal with a tricapped trigonal prismatic coordination sphere. In the hexahydrate of gadolinium(III) chloride and other smaller 4f trichlorides and tribromides, six H₂O molecules and 2 Cl⁻ ions coordinate to the cations resulting in a coordination group of 8.

Properties, with applications to MRI

Gadolinium salts are of primary interest for relaxation agents in magnetic resonance imaging (MRI). This technique exploits the fact that Gd³⁺ has an electronic configuration of f⁷. Seven is the largest number of unpaired electron spins possible for an atom, so Gd³⁺ is a key component in the design of highly paramagnetic complexes.^[6] To generate the relaxation agents, Gd³⁺ sources such as GdCl₃∙6H₂O are converted to coordination complexes. GdCl₃∙6H₂O can not be used as an MRI contrasting agent due to its low solubility in water at the body's near neutral pH.^[7] "Free" gadolinium(III), e.g. [GdCl₂(H₂O)₆]⁺, is toxic, so chelating agents are essential for biomedical applications. Simple monodentate or even bidentate ligands will not suffice because they do not remain bound to Gd³⁺ in solution. Ligands with higher coordination numbers therefore are required. The obvious candidate is EDTA⁴⁻, ethylenediaminetetraacetate, which is a commonly employed hexadentate ligand used to complex to transition metals. In lanthanides, however, exhibit coordination numbers greater than six, so still larger aminocarboxylates are employed.

One representative chelating agent is H₅DTPA, diethylenetriaminepentaacetic acid.^[8] Chelation to the conjugate base of this ligand increases the solubility of the Gd³⁺ at the body's neutral pH and still allows for the paramagnetic effect required for an MRI contrast agent. The DTPA⁵⁻ ligand binds to Gd through five oxygen atoms of the carboxylates and three nitrogen atoms of the amines. A 9th binding site remains, which is occupied by a water molecule. The rapid exchange of this water ligand with bulk water is a major reason for the signal enhancing properties of the chelate. The structure of [Gd(DTPA)(H₂O)]²⁻ is a distorted tricapped trigonal prism.

The following is the reaction for the formation of Gd-DTPA:

References

^ Saeger, Victor William; Spedding, F. H. (November 1960). Some physical properties of rare-earth chlorides in aqueous solution. Ames Laboratory Technical Reports 46. p. 38. Retrieved 19 October 2020.
^ Meyer, G. (1989). The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides-The Example of YCl₃. Inorganic Syntheses. Vol. 25. pp. 146–150. doi:10.1002/9780470132562.ch35. ISBN 978-0-470-13256-2.
^ Corbett, John D. (1983). "Trichlorides of the Rare Earth Elements, Yttrium, and Scandium". Inorganic Syntheses. Inorganic Syntheses. Vol. 22. pp. 39–42. doi:10.1002/9780470132531.ch8. ISBN 978-0-470-13253-1.
^ Quill, L. L.; Clink, George L. (1967). "Preparation of Lanthanide Chloride Methanolates Using 2,2-Dimethoxypropane". Inorganic Chemistry. 6 (7): 1433–1435. doi:10.1021/ic50053a032.
^ Wells, A.F. (1984). Structural Inorganic Chemistry. Oxford: Clarendon Press.
^ Raduchel, B.; Weinmann, H.; Muhler, A. (1996). "Gadolinium Chelates: Chemistry, Safety, & Behavior". Encyclopedia of Nuclear Magnetic Resonance. 4: 2166–2172.
^ Spencer, A. J.; Wilson, S. A.; Batchelor, J.; Reid, A.; Pees, J.; Harpur, E. (1997). "Gadolinium Chloride Toxicity in the Rat". Toxicologic Pathology. 25 (3): 245–255. doi:10.1177/019262339702500301. ISSN 0192-6233. PMID 9210255. S2CID 19838648.
^ Aime, S.; Botta, Mauro; Dastru, Walter; Fasano, Mauro; Panero, Maurizio; Arnelli, Aldo (1993). "Synthesis and Characterization of a Novel DPTA-like Gadolinium(III) Complex: A Potential Reagent for the Determination of Glycated Proteins by Water Proton NMR Relaxation Measurements". Inorganic Chemistry. 32 (10): 2068–2071. doi:10.1021/ic00062a031.