Scandium metal

The production of the first pound of 99% pure scandium metal was announced in 1960. 

Allenyltrimethylsilanes add to ethyl glyoxalate in the presence of a chiral pybox scandium triflate catalyst to afford highly enantioenriched homopropargylic alcohols or dihydrofurans, depending on the nature of the silyl substituent (Tables 9.39 and 9.40) [62]. The trimethylsilyl-substituted silanes give rise to the alcohol products whereas the bulkier t-butyldiphenylsilyl (DPS)-substituted silanes yield only the [3 + 2] cycloadducts. A bidentate complex of the glyoxalate with the scandium metal center in which the aldehyde carbonyl adopts an axial orientation accounts for the observed facial preference ofboth additions. 

Scandium was not produced in any quantities until the late 1930s. Its light weight, resistance to corrosion, and high melting point made it especially useful in the aerospace industries. In the early 1940s contractors for the U.S. Air Force appropriated almost all of the scandium metal for use in the construction of military aircraft. The pure metal form is produced by the electrolysis of a salt of scandium, ScCl The metal has found some other uses in... 

Scandium metal reacts rapidly with most acids hberating hydrogen and forming salts upon evaporation of the solution. Scandium, however, is not attacked by 1 1 mixture of concentrated nitric acid and 48% hydrofluoric acid. A similar behavior is exhibited by yttrium and heavy rare earth metals. 

A 2.25-g sample of scandium metal is reacted with excess hydrochloric acid to produce 0.1502 g hydrogen gas. What is the formula of the scandium chloride produced in the reaction ... 

The substance discovered by Nilson was not pure scandium metal, but a compound of scandium and oxygen—scandium oxide (SC2O3). It is quite difficult to produce pure scandium metal from scandium oxide. In fact, it was not until 1937 that the metal was isolated. Then, it was another 20 years before a large sample (weighing one pound) was produced. Today, companies that use scandium often buy the oxide rather than the pure metal. In 2008, scandium oxide of 99.9995 percent purity cost about 3,260 per kilogram. 

Scandium metal is a silvery-white solid with a slight pink or yellow tint when exposed to air. It has a melting point of 2,800°F (1,538°C) and a... 

Pure scandium metal can be made by reacting scandium fluoride (SCF3) with another active metal, such as calcium or zinc ... 

There are relatively few commercial uses for scandium or its compounds. It is sometimes used to make alloys for special purposes. Scandium metal is lighter than most other metals. It is also resistant to corrosion (rusting) and has a high melting point. These properties make scandium alloys especially desirable for use in sporting equipment, such as baseball bats, lacrosse sticks, and bicycle frames. 

Relatively little is known about the health effects of scandium metal and its compounds. Exposure to scandium dust or most of its compounds is thought to produce irritation of the skin, eyes, and respiratory system. No long-term serious effects of exposure to scandium or its compounds have as yet been found. 

Single crystal X-ray structures of CpDoCp HScCl and CpDoCp HScMe were published. Both molecules showed a similar structure. The Cl complex is one of the very few examples of a di(cyclopentadienyl)scandium chloride without bridging chlorine atoms. This terminal Sc-Cl distance is 2.4574(12) A shorter than in a scandium chloride complex with bridging chlorine atoms like [Cp"2Sc(/r-Cl)]2 with 2.58 A. The scandium metal atom is surrounded by four ligands in a distorted tetrahedral geometry. The coordinated dimethylamino group decreases the Lewis acidity... 

Yelagin, Y.I., Zakharov, V.V. and Rostova, T.D. (1992) Aluminum alloys alloyed with scandium, Metal Science and Thermotreatment of Metals No. 1, 24-28. 

EINECS 231-129-2 Scandium. Metallic element no major industrial use some application in semiconductor field an artificial radioxtive isotope has been used in trxer studies and leak detxtion. mp = 1541 bp = 2836° d = 2.9890. Cerac Rhdne-Poulenc 3973Atomergic Cerx Chemetals Rhone-Pouleno. 

Pollack. L. Smith. E.M. Parpia. J.M. Richardson. R.C. Determination of the electric field gradient and relaxation time measurements in scandium metal at very low temperature. J. Low Temp. Phys. 1992. 87. 753-772. 

Another approach, as described by Carlson and Schmidt (1%7), involved the preparation of yttrium metal by the Ca reduction of YCI3 in the presence of Mg. The Mg and Ca were removed from the Y by a vacuum heat treatment followed by arc melting the resultant Y sponge. In a similar process Schmidt and Carlson (1974) prepared scandium metal by reducing ScCh with Ca and/or Mg. The reduced metal was purified by arc melting or vacuum distillation. 

Schmidt, F.A. and O.N. Carlson, 1974, United States patent No. 3, 846, 121, Method for preparing scandium metal. 

Strongly resembles that of the lanthanides, with most of its compounds being colorless and diamagnetic. This is not surprising as we will see in Section 21.6, the color and magnetism of transition metal compounds usually arise from the d electrons on the metal ion, and Sc + has no d electrons. Scandium metal, which can be prepared by electrolysis of molten ScCls, is not widely used because of its rarity, but it is found in some electronic devices, such as high-intensity lamps. 

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