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{{chembox {{chembox
| Verifiedfields = changed
⚫ | verifiedrevid = 417316717
| Watchedfields = changed
⚫ | Name = Praseodymium(III) chloride
⚫ | verifiedrevid = 428906341
⚫ | ImageFile = Praseodymium(III)-chloride-heptahydrate.jpg
⚫ | Name = Praseodymium(III) chloride
⚫ | ImageFileL1 = UCl3.png
⚫ | ImageFile1 = Praseodymium(III)-chloride-heptahydrate.jpg
| ImageFile2 =
⚫ | ImageFileL1 = UCl3 without caption.png
| ImageFileR1 = Cerium bromide (space filling) 2.png | ImageFileR1 = Cerium bromide (space filling) 2.png
| ImageName = | ImageName =
| IUPACName = Praseodymium(III) chloride | IUPACName = Praseodymium(III) chloride
| OtherNames = Praseodymium chloride; praseodymium trichloride | OtherNames = Praseodymium chloride; praseodymium trichloride
| Section1 = {{Chembox Identifiers |Section1={{Chembox Identifiers
⚫ | CASNo_Ref = {{cascite|correct|CAS}}
| CASNo = 10361-79-2 | CASNo = 10361-79-2
⚫ | CASNo_Ref = {{cascite}}

⚫ | RTECS =
| UNII_Ref = {{fdacite|changed|FDA}}
| UNII = 1JB99PM4G8

⚫ | RTECS =
| PubChem = 66317
| InChI = 1S/3ClH.Pr/h3*1H;/q;;;+3/p-3
| SMILES = Cl(Cl)Cl
}} }}
| Section2 = {{Chembox Properties |Section2={{Chembox Properties
| Formula = PrCl<sub>3</sub> | Formula = PrCl<sub>3</sub>
| MolarMass = 247.24 g/mol (anhydrous)<br/>373.77 g/mol (heptahydrate) | MolarMass = 247.24 g/mol (anhydrous)<br/>373.77 g/mol (heptahydrate)
| Appearance = blue-green solid (anhydrous)<br/>light green solid (heptahydrate) | Appearance = blue-green solid (anhydrous)<br/>light green solid (heptahydrate)
| Density = 4.02 g/cm<sup>3</sup> (anhydrous)<br/>2.250 g/cm<sup>3</sup> (heptahydrate) | Density = 4.02 g/cm<sup>3</sup> (anhydrous)<br/>2.250 g/cm<sup>3</sup> (heptahydrate)
| Solubility = 104.0 g/100 ml (13°C) | Solubility = 104.0 g/100 ml (13 °C)
| MeltingPt = 786 °C | MeltingPtC = 786
| BoilingPt = 1710 °C | BoilingPtC = 1710
| pKa = | pKa =
| pKb = | pKb =
| MagSus = +44.5·10<sup>−6</sup> cm<sup>3</sup>/mol
}} }}
| Section3 = {{Chembox Structure |Section3={{Chembox Structure
| Coordination = Tricapped trigonal prismatic<br />(nine-coordinate) | Coordination = Tricapped trigonal prismatic<br />(nine-coordinate)
| CrystalStruct = ] (]), ] | CrystalStruct = ] (]), ]
| SpaceGroup = P6<sub>3</sub>/m, No. 176 | SpaceGroup = P6<sub>3</sub>/m, No. 176
}} }}
| Section7 = {{Chembox Hazards |Section7={{Chembox Hazards
| ExternalMSDS = | ExternalSDS =
⚫ | MainHazards = Irritant
| EUIndex = Not listed
| FlashPt =
⚫ | MainHazards = Irritant
| FlashPt = | HPhrases =
| RPhrases = | PPhrases =
| SPhrases = | GHS_ref =
}} }}
| Section8 = {{Chembox Related |Section8={{Chembox Related
| OtherAnions = ]<br/>]<br/>] | OtherAnions = ], ]<br/>]<br/>]
| OtherCations = ]<br/>] | OtherCations = ]<br/>]
}} }}
}} }}


'''Praseodymium(III) chloride''' is the ] with the ] ]]<sub>3</sub>. It is a blue-green solid that rapidly absorbs water on exposure to moist air to form a light green hepta]. '''Praseodymium(III) chloride''' is the ] with the ] ]]<sub>3</sub>. Like other ]s, it exists both in the anhydrous and hydrated forms. It is a blue-green solid that rapidly absorbs water on exposure to moist air to form a light green hepta].


==Preparation== ==Preparation==
Praseodymium(III) chloride is prepared by treating praseodymium metal and ]:<ref name=ref7 /><ref name=ref6>L. F. Druding, J. D. Corbett, ''J. Am. Chem. Soc.'' '''83''', 2462 (1961); J. D. Corbett, ''Rev. Chim. Minerale'' '''10''', 239 (1973)<sup>,</sup></ref> Praseodymium(III) chloride is prepared by treating praseodymium metal with ]:<ref name=ref7 /><ref name=ref6>{{cite journal|url=https://pubs.acs.org/doi/10.1021/ja01472a010|author1=L.F. Druding|author2= J.D. Corbett|title=Lower Oxidation States of the Lanthanides. Neodymium(II) Chloride and Iodide|journal=J. Am. Chem. Soc.|volume=83|issue=11|pages=2462-2467|date=1961-06-01|doi=10.1021/ja01472a010}}</ref>

:2 Pr + 6 HCl → 2 PrCl<sub>3</sub> + 3 H<sub>2</sub> :2 Pr + 6 HCl → 2 PrCl<sub>3</sub> + 3 H<sub>2</sub>
It is usually purified by vacuum sublimation.<ref name=ref1 /> It is usually purified by vacuum sublimation.<ref name=ref1 />
Line 53: Line 66:
:Pr<sub>2</sub>(CO<sub>3</sub>)<sub>3</sub> + 6 HCl + 15 H<sub>2</sub>O → 2 Cl<sub>3</sub> + 3 CO<sub>2</sub> :Pr<sub>2</sub>(CO<sub>3</sub>)<sub>3</sub> + 6 HCl + 15 H<sub>2</sub>O → 2 Cl<sub>3</sub> + 3 CO<sub>2</sub>


Anhydrous PrCl<sub>3</sub> can be made by thermal dehydration of the hydrate at 400 °C in the presence of ].<ref name=ref1 /><ref name=ref4>M. D. Taylor, P. C. Carter, ''J. Inorg. Nucl. Chem.'' '''24''', 387 (1962); J. Kutscher, A. Schneider, ''Inorg. Nucl. Chem. Lett.'' '''7''', 815 (1971).</ref> Alternatively the hydrate can be dehydrated using ].<ref name=ref1/><ref name=ref5>J. H. Freeman, M. L. Smith, ''J. Inorg. Nucl. Chem.'' '''7''', 224 (1958).</ref> PrCl<sub>3</sub>∙7H<sub>2</sub>O is a hygroscopic substance, that will not crystallize from the ] unless it is left to dry in a desiccator. Anhydrous PrCl<sub>3</sub> can be made by thermal dehydration of the hydrate at 400&nbsp;°C in the presence of ], the so-called ].<ref name=ref1 /><ref name=ref4>{{cite journal|url=https://www.sciencedirect.com/science/article/abs/pii/0022190262800347|author1=M.D. Taylor|author2=P.C. Carter|title= Preparation of anhydrous lanthanide halides, especially iodides|journal=J. Inorg. Nucl. Chem.|volume=24|issue=4|pages=387-391|date=April 1962|doi=10.1016/0022-1902(62)80034-7}}</ref><ref name="Kutscher">{{cite journal|url=https://www.sciencedirect.com/science/article/abs/pii/0020165071802532|author1=J. Kutscher|author2=A. Schneider|title=Notiz zur Präparation von wasserfreien Lanthaniden-Haloge-niden, Insbesondere von Jodiden|journal=Inorg. Nucl. Chem. Lett.|volume=7|issue=9|pages=815-819|date=September 1971|doi=10.1016/0020-1650(71)80253-2|language=de}}</ref> Alternatively the hydrate can be dehydrated using ].<ref name=ref1/><ref name=ref5>{{cite journal|url=https://www.sciencedirect.com/science/article/abs/pii/0022190258800731|author1=J.H. Freeman|author2=M.L. Smith|title=The preparation of anhydrous inorganic chlorides by dehydration with thionyl chloride|journal=J. Inorg. Nucl. Chem.|volume=7|issue=3|pages=224-227|date=October 1958|doi=10.1016/0022-1902(58)80073-1}}</ref>


==Reactions== ==Reactions==
Praseodymium(III) chloride is ]ic, classified as "hard" according to the ]. Rapid heating of the ] may cause small amounts of ].<ref name=ref1>F. T. Edelmann, P. Poremba, in: ''Synthetic Methods of Organometallic and Inorganic Chemistry'', (W. A. Herrmann, ed.), Vol. 6, Georg Thieme Verlag, Stuttgart, 1997.</ref> PrCl<sub>3</sub> forms a stable Lewis acid-base complex K<sub>2</sub>PrCl<sub>5</sub> by reaction with ]; this compound shows interesting ] and ] properties.<ref name=ref7>J. Cybinska, J. Sokolnicki, J. Legendziewicz, G. Meyer ''Journal of Alloys and Compounds'' '''341''', 115-123 (2002).</ref> Praseodymium(III) chloride is ]ic, classified as "hard" according to the ]. Rapid heating of the ] may cause small amounts of ].<ref name=ref1>{{cite book|author1=F.T. Edelmann|author2= P. Poremba|title=Synthetic Methods of Organometallic and Inorganic Chemistry|volume=6|publisher= Georg Thieme Verlag|location=Stuttgart|date= 1997|isbn=978-31-319-3921-0}}</ref> PrCl<sub>3</sub> forms a stable Lewis acid-base complex K<sub>2</sub>PrCl<sub>5</sub> by reaction with ]; this compound shows interesting ] and ] properties.<ref name=ref7>{{cite journal|url=https://www.semanticscholar.org/paper/Spectroscopic-and-magnetic-studies-of-the-ternary-Cybi%C5%84ska-Sokolnicki/2af96eacdd78d2ec04ac3c0342ca6d875f76130e|author1=J. Cybinska|author2= J. Sokolnicki|author3= J. Legendziewicz|author4= G. Meyer|title=Spectroscopic and magnetic studies of the ternary praseodymium chloride K<sub>2</sub>PrCl<sub>5</sub>|journal=Journal of Alloys and Compounds|volume=341|pages=115–123|date=2002-07-17|doi=10.1016/S0925-8388(02)00089-0}}</ref>


] solutions of praseodymium(III) chloride can be used to prepare insoluble praseodymium(III) compounds. For example, praseodymium(III) phosphate and praseodymium(III) fluoride can be prepared by reaction with ] and ], respectively: ] solutions of praseodymium(III) chloride can be used to prepare insoluble praseodymium(III) compounds. For example, praseodymium(III) phosphate and praseodymium(III) fluoride can be prepared by reaction with ] and ], respectively:
Line 62: Line 75:
:PrCl<sub>3</sub> + K<sub>3</sub>PO<sub>4</sub> → PrPO<sub>4</sub> + 3 KCl :PrCl<sub>3</sub> + K<sub>3</sub>PO<sub>4</sub> → PrPO<sub>4</sub> + 3 KCl
:PrCl<sub>3</sub> + 3 NaF → PrF<sub>3</sub> + 3 NaCl :PrCl<sub>3</sub> + 3 NaF → PrF<sub>3</sub> + 3 NaCl
:2PrCl<sub>3</sub> + 3 Na<sub>2</sub>CO<sub>3</sub>----> Pr<sub>2</sub>CO<sub>3</sub> + 6NaCl
⚫ When heated with alkali metal chlorides, it forms a series of ternary (compounds containing three different elements) materials with the formulae MPr<sub>2</sub>Cl<sub>7</sub>, M<sub>3</sub>PrCl<sub>6</sub>, M<sub>2</sub>PrCl<sub>5</sub>, and M<sub>3</sub>Pr<sub>2</sub>Cl<sub>9</sub> where M = K, Rb, Cs.<ref>{{cite journal|author=Gerd Meyer|title=Ternary Chlorides and Bromides of the Rare-Earth Elements|journal=Inorganic Syntheses|year=1990|volume=30|pages=72–81|doi=10.1002/9780470132616.ch15}}</ref>


]
⚫ When heated with alkali metal chlorides, it forms a series of ternary (compounds containing three different elements) materials with the formulae MPr<sub>2</sub>Cl<sub>7</sub>, M<sub>3</sub>PrCl<sub>6</sub>, M<sub>2</sub>PrCl<sub>5</sub>, and M<sub>3</sub>Pr<sub>2</sub>Cl<sub>9</sub> where M = K, Rb, Cs.<ref>Gerd Meyer "Ternary Chlorides and Bromides of the Rare-Earth Elements" Inorganic Syntheses, 1990, Volume 30, pp. 72–81. {{DOI|10.1002/9780470132616.ch15}}</ref>


==References== ==References==
Line 71: Line 86:
#<!--old 2--> ''CRC Handbook of Chemistry and Physics'' (58th edition), CRC Press, West Palm Beach, Florida, 1977. #<!--old 2--> ''CRC Handbook of Chemistry and Physics'' (58th edition), CRC Press, West Palm Beach, Florida, 1977.
#<!--old 3--> N. N. Greenwood, A. Earnshaw, ''Chemistry of the Elements'', Pergamon Press, 1984. #<!--old 3--> N. N. Greenwood, A. Earnshaw, ''Chemistry of the Elements'', Pergamon Press, 1984.
#<!--old 8--> S. Sugiyama, T. Miyamoto, H. Hayashi, M. Tanaka, J. B. Moffat ''Journal of Molecular Catalysis A'', '''118''', 129-136 (1997). #<!--old 8--> S. Sugiyama, T. Miyamoto, H. Hayashi, M. Tanaka, J. B. Moffatt, "Effects of chlorine additives in the gas- and solid-phases on the oxidative dehydrogenation of ethane over praseodymium oxide", ''Journal of Molecular Catalysis A'', '''118''', 129-136 (1997).
#<!--old 9--> {{cite journal #<!--old 9--> {{cite journal
| title = Rare Earth Metal-Metal Halide Systems. VI. Praseodymium Chloride | title = Rare Earth Metal-Metal Halide Systems. VI. Praseodymium Chloride
| author = Druding L. F., Corbett J. D., Ramsey B. N. |author1=Druding L. F. |author2=Corbett J. D. |author3=Ramsey B. N. | journal = ]
| journal = ]
| year = 1963 | year = 1963
| volume = 2 | volume = 2
Line 84: Line 98:


{{Praseodymium compounds}} {{Praseodymium compounds}}
{{Chlorides}}
{{Lanthanide halides}}


] ]
] ]
] ]

]

Latest revision as of 17:14, 2 May 2024

Praseodymium(III) chloride
Names
IUPAC name Praseodymium(III) chloride
Other names Praseodymium chloride; praseodymium trichloride
Identifiers
CAS Number
3D model (JSmol)
ECHA InfoCard 100.030.710 Edit this at Wikidata
PubChem CID
UNII
CompTox Dashboard (EPA)
InChI
  • InChI=1S/3ClH.Pr/h3*1H;/q;;;+3/p-3
SMILES
  • Cl(Cl)Cl
Properties
Chemical formula PrCl3
Molar mass 247.24 g/mol (anhydrous)
373.77 g/mol (heptahydrate)
Appearance blue-green solid (anhydrous)
light green solid (heptahydrate)
Density 4.02 g/cm (anhydrous)
2.250 g/cm (heptahydrate)
Melting point 786 °C (1,447 °F; 1,059 K)
Boiling point 1,710 °C (3,110 °F; 1,980 K)
Solubility in water 104.0 g/100 ml (13 °C)
Magnetic susceptibility (χ) +44.5·10 cm/mol
Structure
Crystal structure hexagonal (UCl3 type), hP8
Space group P63/m, No. 176
Coordination geometry Tricapped trigonal prismatic
(nine-coordinate)
Hazards
Occupational safety and health (OHS/OSH):
Main hazards Irritant
Related compounds
Other anions Praseodymium(III) oxide, Praseodymium(III) fluoride
Praseodymium bromide
praseodymium iodide
Other cations Cerium(III) chloride
Neodymium(III) chloride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). ☒N verify (what is  ?) Infobox references
Chemical compound

Praseodymium(III) chloride is the inorganic compound with the formula PrCl3. Like other lanthanide trichlorides, it exists both in the anhydrous and hydrated forms. It is a blue-green solid that rapidly absorbs water on exposure to moist air to form a light green heptahydrate.

Preparation

Praseodymium(III) chloride is prepared by treating praseodymium metal with hydrogen chloride:

2 Pr + 6 HCl → 2 PrCl3 + 3 H2

It is usually purified by vacuum sublimation.

Hydrated salts of praseodymium(III) chloride can be prepared by treatment of either praseodymium metal or praseodymium(III) carbonate with hydrochloric acid:

Pr2(CO3)3 + 6 HCl + 15 H2O → 2 Cl3 + 3 CO2

PrCl3∙7H2O is a hygroscopic substance, that will not crystallize from the mother liquor unless it is left to dry in a desiccator. Anhydrous PrCl3 can be made by thermal dehydration of the hydrate at 400 °C in the presence of ammonium chloride, the so-called ammonium chloride route. Alternatively the hydrate can be dehydrated using thionyl chloride.

Reactions

Praseodymium(III) chloride is Lewis acidic, classified as "hard" according to the HSAB concept. Rapid heating of the hydrate may cause small amounts of hydrolysis. PrCl3 forms a stable Lewis acid-base complex K2PrCl5 by reaction with potassium chloride; this compound shows interesting optical and magnetic properties.

Aqueous solutions of praseodymium(III) chloride can be used to prepare insoluble praseodymium(III) compounds. For example, praseodymium(III) phosphate and praseodymium(III) fluoride can be prepared by reaction with potassium phosphate and sodium fluoride, respectively:

PrCl3 + K3PO4 → PrPO4 + 3 KCl
PrCl3 + 3 NaF → PrF3 + 3 NaCl
2PrCl3 + 3 Na2CO3----> Pr2CO3 + 6NaCl

When heated with alkali metal chlorides, it forms a series of ternary (compounds containing three different elements) materials with the formulae MPr2Cl7, M3PrCl6, M2PrCl5, and M3Pr2Cl9 where M = K, Rb, Cs.

Praseodymium chloride heptahydrate under different light

References

  1. ^ J. Cybinska; J. Sokolnicki; J. Legendziewicz; G. Meyer (2002-07-17). "Spectroscopic and magnetic studies of the ternary praseodymium chloride K2PrCl5". Journal of Alloys and Compounds. 341: 115–123. doi:10.1016/S0925-8388(02)00089-0.
  2. L.F. Druding; J.D. Corbett (1961-06-01). "Lower Oxidation States of the Lanthanides. Neodymium(II) Chloride and Iodide". J. Am. Chem. Soc. 83 (11): 2462–2467. doi:10.1021/ja01472a010.
  3. ^ F.T. Edelmann; P. Poremba (1997). Synthetic Methods of Organometallic and Inorganic Chemistry. Vol. 6. Stuttgart: Georg Thieme Verlag. ISBN 978-31-319-3921-0.
  4. M.D. Taylor; P.C. Carter (April 1962). "Preparation of anhydrous lanthanide halides, especially iodides". J. Inorg. Nucl. Chem. 24 (4): 387–391. doi:10.1016/0022-1902(62)80034-7.
  5. J. Kutscher; A. Schneider (September 1971). "Notiz zur Präparation von wasserfreien Lanthaniden-Haloge-niden, Insbesondere von Jodiden". Inorg. Nucl. Chem. Lett. (in German). 7 (9): 815–819. doi:10.1016/0020-1650(71)80253-2.
  6. J.H. Freeman; M.L. Smith (October 1958). "The preparation of anhydrous inorganic chlorides by dehydration with thionyl chloride". J. Inorg. Nucl. Chem. 7 (3): 224–227. doi:10.1016/0022-1902(58)80073-1.
  7. Gerd Meyer (1990). "Ternary Chlorides and Bromides of the Rare-Earth Elements". Inorganic Syntheses. 30: 72–81. doi:10.1002/9780470132616.ch15.

Further reading

  1. CRC Handbook of Chemistry and Physics (58th edition), CRC Press, West Palm Beach, Florida, 1977.
  2. N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, Pergamon Press, 1984.
  3. S. Sugiyama, T. Miyamoto, H. Hayashi, M. Tanaka, J. B. Moffatt, "Effects of chlorine additives in the gas- and solid-phases on the oxidative dehydrogenation of ethane over praseodymium oxide", Journal of Molecular Catalysis A, 118, 129-136 (1997).
  4. Druding L. F.; Corbett J. D.; Ramsey B. N. (1963). "Rare Earth Metal-Metal Halide Systems. VI. Praseodymium Chloride". Inorganic Chemistry. 2 (4): 869–871. doi:10.1021/ic50008a055.
Praseodymium compounds
Pr(II)
Pr(III)
Organopraseodymium(III) compounds
  • Pr2(CO3)3
  • Pr2(C2O4)3
    • Pr(III,IV)
    Pr(IV)
    Pr(V)
    Salts and covalent derivatives of the chloride ion
    HCl He
    LiCl BeCl2 B4Cl4
    B12Cl12
    BCl3
    B2Cl4
    +BO3     		C2Cl2
    C2Cl4
    C2Cl6
    CCl4
    +C
    +CO3     		NCl3
    ClN3
    +N
    +NO3     		ClxOy
    Cl2O
    Cl2O2
    ClO
    ClO2
    Cl2O4
    Cl2O6
    Cl2O7
    ClO4
    +O     		ClF
    ClF3
    ClF5     		Ne
    NaCl MgCl2 AlCl
    AlCl3     		Si5Cl12
    Si2Cl6
    SiCl4     		P2Cl4
    PCl3
    PCl5
    +P     		S2Cl2
    SCl2
    SCl4
    +SO4     		Cl2 Ar
    KCl CaCl
    CaCl2     		ScCl3 TiCl2
    TiCl3
    TiCl4     		VCl2
    VCl3
    VCl4
    VCl5     		CrCl2
    CrCl3
    CrCl4     		MnCl2
    MnCl3     		FeCl2
    FeCl3     		CoCl2
    CoCl3     		NiCl2 CuCl
    CuCl2     		ZnCl2 GaCl
    GaCl3     		GeCl2
    GeCl4     		AsCl3
    AsCl5
    +As     		Se2Cl2
    SeCl2
    SeCl4     		BrCl Kr
    RbCl SrCl2 YCl3 ZrCl2
    ZrCl3
    ZrCl4     		NbCl3
    NbCl4
    NbCl5     		MoCl2
    MoCl3
    MoCl4
    MoCl5
    MoCl6     		TcCl3
    TcCl4     		RuCl2
    RuCl3
    RuCl4     		RhCl3 PdCl2 AgCl CdCl2 InCl
    InCl2
    InCl3     		SnCl2
    SnCl4     		SbCl3
    SbCl5     		Te3Cl2
    TeCl2
    TeCl4     		ICl
    ICl3     		XeCl
    XeCl2
    XeCl4
    CsCl BaCl2 * LuCl3 HfCl4 TaCl3
    TaCl4
    TaCl5     		WCl2
    WCl3
    WCl4
    WCl5
    WCl6     		ReCl3
    ReCl4
    ReCl5
    ReCl6     		OsCl2
    OsCl3
    OsCl4
    OsCl5     		IrCl2
    IrCl3
    IrCl4     		PtCl2
    PtCl4     		AuCl
    (Au)2
    AuCl3     		Hg2Cl2
    HgCl2     		TlCl
    TlCl3     		PbCl2
    PbCl4     		BiCl3 PoCl2
    PoCl4     		AtCl Rn
    FrCl RaCl2 ** LrCl3 RfCl4 DbCl5 SgO2Cl2 BhO3Cl 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
    ** AcCl3 ThCl3
    ThCl4     		PaCl4
    PaCl5     		UCl3
    UCl4
    UCl5
    UCl6     		NpCl3 PuCl3 AmCl2
    AmCl3     		CmCl3 BkCl3 CfCl3
    CfCl2     		EsCl2
    EsCl3     		FmCl2 MdCl2 NoCl2
    Lanthanide salts of halides
    La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
    +4 CeF4 PrF4 NdF4 TbF4 DyF4
    +3 LaF3
    LaCl3
    LaBr3
    LaI3     		CeF3
    CeCl3
    CeBr3
    CeI3     		PrF3
    PrCl3
    PrBr3
    PrI3     		NdF3
    NdCl3
    NdBr3
    NdI3     		PmF3
    PmCl3
    PmBr3
    PmI3     		SmF3
    SmCl3
    SmBr3
    SmI3     		EuF3
    EuCl3
    EuBr3
    EuI3     		GdF3
    GdCl3
    GdBr3
    GdI3     		TbF3
    TbCl3
    TbBr3
    TbI3     		DyF3
    DyCl3
    DyBr3
    DyI3     		HoF3
    HoCl3
    HoBr3
    HoI3     		ErF3
    ErCl3
    ErBr3
    ErI3     		TmF3
    TmCl3
    TmBr3
    TmI3     		YbF3
    YbCl3
    YbBr3
    YbI3     		LuF3
    LuCl3
    LuBr3
    LuI3
    +2 LaI2 CeI2 PrI2 NdF2
    NdCl2
    NdBr2
    NdI2     		SmF2
    SmCl2
    SmBr2
    SmI2     		EuF2
    EuCl2
    EuBr2
    EuI2     		GdI2 DyF2
    DyCl2
    DyBr2
    DyI2     		TmF2
    TmCl2
    TmBr2
    TmI2     		YbF2
    YbCl2
    YbBr2
    YbI2
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