Lanthanide chlorides are a group of chemical compounds that can form between a lanthanide element (from lanthanum to lutetium) and chlorine. The lanthanides in these compounds are usually in the +2 and +3 oxidation states, although compounds with lanthanides in lower oxidation states exist.

Lanthanide dichlorides

Divalent chlorides are formed by neodymium, samarium, europium, dysprosium, thulium and ytterbium. They can be prepared by reducing the trivalent chloride with lithium metal/naphthalene in tetrahydrofuran:[1]

LnCl3 + Li → LnCl2 + LiCl (Ln=Nd,Sm,Eu)

Reducing the chloride with the metal or hydrogen is also possible:[2][3]

2 LnCl3 + Ln → 3 LnCl2 (Ln=Nd,Sm,Eu?,Dy,Tm,Yb)
2 LnCl3 + H2 → 2 LnCl2 + 2 HCl (Ln=Nd,Sm,Eu,Dy,Tm,Yb)

Lanthanide trichlorides

The lanthanide trichlorides can generally be prepared by dissolving the oxide or carbonate with hydrochloric acid. They are produced commercially by carbothermic reaction of the oxide. To produce the anhydrous forms of these trichlorides, the ammonium chloride route is taken. The anhydrous lanthanide trichlorides have high melting points and are generally pale colored.

Lanthanide trichlorides[4]
MCl3colorstructure typef-configuration
LaCl3colorlessUCl3-typef0
CeCl3colorlessUCl3-typef1, doublet
PrCl3greenUCl3-typef2, triplet
NdCl3pinkUCl3-typef3, quartet
PmCl3greenUCl3-typef4, quintet
SmCl3yellowUCl3-typef5, sextet
EuCl3yellowUCl3-typef6, septet
GdCl3colorlessUCl3-typef7, octet
TbCl3whitePuBr3-typef8, septet
DyCl3whiteAlCl3-typef9, sextet
HoCl3yellowAlCl3-typef10, quintet
ErCl3violetAlCl3-typef11, quartet
TmCl3yellowAlCl3-typef12, triplet
YbCl3colorlessYCl3-typef13, doublet
LuCl3colorlessAlCl3-typef14

See also

References

  1. ↑ Rossmainth, Kurt (1979-01-01). "Herstellung der klassischen Seltenerd(II)-chloride in Lösung" [Preparation of the classical rare earth(II) chlorides in solution]. Anorganische, Struktur- und Physikalische Chemie. 110 (4): 109–114. doi:10.1007/BF00903752. S2CID 91731356.
  2. ↑ Gerd Meyer, Lester R. Morss (1991). Synthesis of lanthanide and actinide compounds. Springer. p. 161. ISBN 0-7923-1018-7.
  3. ↑ Brauer, Georg; Baudler, Marianne (1975). Handbuch der Präparativen Anorganischen Chemie, Band I. (3rd ed.). Stuttgart: Ferdinand Enke. ISBN 3-432-02328-6.
  4. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
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