Lanthanum: the essentials
Lanthanum atoms have 57 electrons and the shell structure is 188.8.131.52.9.2. The ground state electronic configuration of neutral lanthanum is [Xe].5d1.6s2 and the term symbol of lanthanum is 2D3/2.
Lanthanum is silvery white, malleable, ductile, and soft enough to be cut with a knife. It is one of the most reactive of the rare-earth metals. It oxidises rapidly when exposed to air. Cold water attacks lanthanum slowly, and hot water attacks it much more rapidly. The metal reacts directly with elemental carbon, nitrogen, boron, selenium, silicon, phosphorus, sulphur, and with halogens. It is a component of, misch metal (used for making lighter flints).
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Lanthanum: physical properties
Lanthanum: heat properties
- Melting point: 1193 [920 °C (1688 °F)] K
- Boiling point: 3743 [3470 °C (6278 °F)] K
- Enthalpy of fusion: 20.5 kJ mol-1
Lanthanum: atom sizes
- Atomic radius (empirical): 195 pm
- Molecular single bond covalent radius: 180 (coordination number 3) ppm
- van der Waals radius: 298 ppm
- Pauling electronegativity: 1.10 (Pauling units)
- Allred Rochow electronegativity: 1.08 (Pauling units)
- Mulliken-Jaffe electronegativity: (no data)
Lanthanum: orbital properties
- First ionisation energy: 538.09 kJ mol‑1
- Second ionisation energy: 1079.18 kJ mol‑1
- Third ionisation energy: 1850.33 kJ mol‑1
Lanthanum: crystal structure
Lanthanum: biological data
- Human abundance by weight: (no data) ppb by weight
Lanthanum has no biological role.
Reactions of lanthanum as the element with air, water, halogens, acids, and bases where known.
Lanthanum: binary compounds
网络斗地主下载 Binary compounds with halogens (known as halides), oxygen (known as oxides), hydrogen (known as hydrides), and other compounds of lanthanum where known.
Lanthanum: compound properties
Bond strengths; lattice energies of lanthanum halides, hydrides, oxides (where known); and reduction potentials where known.
Lanthanum: historyLanthanum was discovered by Carl Gustaf Mosander in 1839 at Sweden. Origin of name: from the Greek word "lanthanein" meaning "to lie hidden".
The two isotopes of Lanthanum do not appear to have many applications. Only La-139 is used for the production of the medical radioisotope Ce-139.
Isolation: lanthanum metal is available commercially so it is not normally necessary to make it in the laboratory, which is just as well as it is difficult to separate it from as the pure metal. This is largely because of the way it is found in nature. The lanthanoids are found in nature in a number of minerals. The most important are xenotime, monazite, and bastnaesite. The first two are orthophosphate minerals LnPO4 (Ln deonotes a mixture of all the lanthanoids except promethium which is vanishingly rare) and the third is a fluoride carbonate LnCO3F. Lanthanoids with even atomic numbers are more common. The most comon lanthanoids in these minerals are, in order, cerium, lanthanum, neodymium, and praseodymium. Monazite also contains thorium and ytrrium which makes handling difficult since thorium and its decomposition products are radioactive.
For many purposes it is not particularly necessary to separate the metals, but if separation into individual metals is required, the process is complex. Initially, the metals are extracted as salts from the ores by extraction with sulphuric acid (H2SO4), hydrochloric acid (HCl), and sodium hydroxide (NaOH). Modern purification techniques for these lanthanoid salt mixtures are ingenious and involve selective complexation techniques, solvent extractions, and ion exchange chromatography.
Pure lanthanum is available through the reduction of LaF3 with calcium metal.
2LaF3 + 3Ca → 2La + 3CaF2
This would work for the other calcium halides as well but the product CaF2 is easier to handle under the reaction conditions (heat to 50°C above the melting point of the element in an argon atmosphere). Excess calcium is removed from the reaction mixture under vacuum.