| Physical Properties | The anhydrous chloride is a white hexagonal crystal; hygroscopic; density 3.84 g/cm3; melts at 850°C; soluble in water. The heptahydrate is a white triclinic crystal; decomposes at 91°C; soluble in water and ethanol.
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| Uses | Lanthanum(III) chloride is used to prepare other lanthanum salts. The anhydrous chloride is employed to produce lanthanum metal.
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| Preparation | Lanthanum(III) chloride is formed by dissolving the oxide, hydroxide or carbonate in hydrochloric acid, followed by crystallization. The anhydrous chloride is obtained by heating oxide, hydroxide, or carbonate in an atmosphere of dry hydrogen chloride.
La2(CO3)3 + 6HCl → 2LnCl3 + 3CO2 + 3H2O
Another method involves heating lanthanum oxide with excess ammonium chloride at 300°C.
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| Reactions | When heated in the presence of water vapor, lanthanum oxochloride is formed:
LaCl3 + H2O→LaOCl + 2HCl
Heating with glass at elevated temperatures also forms oxochloride:
LaCl3 + SiO2→2LaOCl + SiCl4
Lanthanum chloride reacts with hydrogen sulfide when heated at 1100°C, forming lanthanum sulfide:
2LaCl3 + 3H2S→La2S3 + 3H2S
Reactions with ammonia and phosphine at elevated temperatures yield lanthanum nitride and phosphide, respectively:
LaCl3 + PH3→LaP + 3HCl
Lanthanum chloride is reduced to lanthanum metal when heated with an alkali or alkaline earth metal at temperatures above 1000°C:
LaCl3 + 3Li→La + 3LiCl
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| Chemical Properties | Lanthanum(III) chloride is white powder or colourless crystals
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| Uses | Lanthanum chloride is used to prepare other lanthanum salts. The anhydrous chloride is employed to produce lanthanum metal. |
| Uses | Lanthanum chloride is a precursor for synthesis of lanthanum phosphate nano rods and used in gamma detectors. It is also used as a catalyst for high pressure oxidative chlorination of methane to chloromethane with hydrochloric acid and oxygen. In organic synthesis, lanthanum trichloride acts as lewis acid for the conversion of aldehydes to acetals. |
| Preparation | The heptahydrate is formed by dissolving the oxide, hydroxide or carbonate in hydrochloric acid, followed by crystallization. The anhydrous chloride is obtained by heating oxide, hydroxide, or carbonate in an atmosphere of dry hydrogen chloride.
La2(CO3)3 + 6HCl → 2LnCl3 + 3CO2 + 3H2O
Another method involves heating lanthanum oxide with excess ammonium chloride at 300°C. |
| General Description | Lanthanum(III) chloride is white crystalline solid. Gives an amber aqueous solution that can cause destruction or irreversible alterations in human skin tissue at the site of contact. Has a severe corrosion rate on steel.
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| Air & Water Reactions | Deliquescent. Water soluble. |
| Reactivity Profile | Aqueous solutions of LANTHANUM CHLORIDE contain moderate concentrations of hydrogen ions and react as acids to neutralize bases. Does not usually react as either oxidizing agents or reducing agents but such behavior is not impossible. May catalyze organic reactions. |
| Health Hazard | TOXIC; inhalation, ingestion or skin contact with material may cause severe injury or death. Contact with molten substance may cause severe burns to skin and eyes. Avoid any skin contact. Effects of contact or inhalation may be delayed. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may be corrosive and/or toxic and cause pollution. |
| Fire Hazard | Non-combustible, substance itself does not burn but may decompose upon heating to produce corrosive and/or toxic fumes. Some are oxidizers and may ignite combustibles (wood, paper, oil, clothing, etc.). Contact with metals may evolve flammable hydrogen gas. Containers may explode when heated. |
