Scandium

Scandium is a chemical element with the symbol Sc and atomic number 21. A silvery-white metallic d-block element, it has historically been classified as a rare-earth element,[6] together with yttrium and the lanthanides. It was discovered in 1879 by spectral analysis of the minerals euxenite and gadolinite from Scandinavia.

Not to be confused with Scandinavium.

"Element 21" redirects here. For the golf company, see Element 21 (company).

Scandium, ₂₁Sc

Scandium
Pronunciation	/ˈskændiəm/ ​(SKAN-dee-əm)
Appearance	silvery white
Standard atomic weight Ar, std(Sc)	44.955908(5)[1]
Scandium in the periodic table
Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson – ↑ Sc ↓ Y calcium ← scandium → titanium
Atomic number (Z)	21
Group	group 3
Period	period 4
Block	d-block
Element category	Transition metal
Electron configuration	[Ar] 3d^1 4s^2
Electrons per shell	2, 8, 9, 2
Physical properties
Phase at STP	solid
Melting point	1814 K ​(1541 °C, ​2806 °F)
Boiling point	3109 K ​(2836 °C, ​5136 °F)
Density (near r.t.)	2.985 g/cm^3
when liquid (at m.p.)	2.80 g/cm^3
Heat of fusion	14.1 kJ/mol
Heat of vaporization	332.7 kJ/mol
Molar heat capacity	25.52 J/(mol·K)
Vapor pressure P (Pa) 1 10 100 1 k 10 k 100 k at T (K) 1645 1804 (2006) (2266) (2613) (3101)
Atomic properties
Oxidation states	0,[2] +1,[3] +2,[4] +3 (an amphoteric oxide)
Electronegativity	Pauling scale: 1.36
Ionization energies	1st: 633.1 kJ/mol 2nd: 1235.0 kJ/mol 3rd: 2388.6 kJ/mol (more)
Atomic radius	empirical: 162 pm
Covalent radius	170±7 pm
Van der Waals radius	211 pm
Color lines in a spectral range Spectral lines of scandium
Other properties
Natural occurrence	primordial
Crystal structure	​hexagonal close-packed (hcp)
Thermal expansion	α, poly: 10.2 µm/(m·K) (at r.t.)
Thermal conductivity	15.8 W/(m·K)
Electrical resistivity	α, poly: 562 nΩ·m (at r.t., calculated)
Magnetic ordering	paramagnetic
Magnetic susceptibility	+315.0·10^−6 cm^3/mol (292 K)[5]
Young's modulus	74.4 GPa
Shear modulus	29.1 GPa
Bulk modulus	56.6 GPa
Poisson ratio	0.279
Brinell hardness	736–1200 MPa
CAS Number	7440-20-2
History
Naming	after Scandinavia
Prediction	Dmitri Mendeleev (1871)
Discovery and first isolation	Lars Fredrik Nilson (1879)
Main isotopes of scandium
Iso­tope Abun­dance Half-life (t1/2) Decay mode Pro­duct ^44m2Sc syn 58.61 h IT ^44Sc γ ^44Sc ε ^44Ca ^45Sc 100% stable ^46Sc syn 83.79 d β^− ^46Ti γ – ^47Sc syn 80.38 d β^− ^47Ti γ – ^48Sc syn 43.67 h β^− ^48Ti γ –

Scandium is present in most of the deposits of rare-earth and uranium compounds, but it is extracted from these ores in only a few mines worldwide. Because of the low availability and the difficulties in the preparation of metallic scandium, which was first done in 1937, applications for scandium were not developed until the 1970s, when the positive effects of scandium on aluminium alloys were discovered, and its use in such alloys remains its only major application. The global trade of scandium oxide is 15–20 tonnes per year.[7]

The properties of scandium compounds are intermediate between those of aluminium and yttrium. A diagonal relationship exists between the behavior of magnesium and scandium, just as there is between beryllium and aluminium. In the chemical compounds of the elements in group 3, the predominant oxidation state is +3.

Properties

Chemical characteristics

Scandium is a soft metal with a silvery appearance. It develops a slightly yellowish or pinkish cast when oxidized by air. It is susceptible to weathering and dissolves slowly in most dilute acids. It does not react with a 1:1 mixture of nitric acid (HNO₃) and 48% hydrofluoric acid (HF), possibly due to the formation of an impermeable passive layer. Scandium turnings ignite in air with a brilliant yellow flame to form scandium oxide.[8]

Isotopes

Main article: Isotopes of scandium

In nature, scandium is found exclusively as the isotope ⁴⁵Sc, which has a nuclear spin of 7/2; this is its only stable isotope. Thirteen radioisotopes have been characterized with the most stable being ⁴⁶Sc, which has a half-life of 83.8 days; ⁴⁷Sc, 3.35 days; the positron emitter ⁴⁴Sc, 4 h; and ⁴⁸Sc, 43.7 hours. All of the remaining radioactive isotopes have half-lives less than 4 hours, and the majority of these have half-lives less than 2 minutes. This element also has five nuclear isomers, with the most stable being ^44mSc (t_1/2 = 58.6 h).[9]

The isotopes of scandium range from ³⁶Sc to ⁶⁰Sc. The primary decay mode at masses lower than the only stable isotope, ⁴⁵Sc, is electron capture, and the primary mode at masses above it is beta emission. The primary decay products at atomic weights below ⁴⁵Sc are calcium isotopes and the primary products from higher atomic weights are titanium isotopes.[9]

Occurrence

In Earth's crust, scandium is not rare. Estimates vary from 18 to 25 ppm, which is comparable to the abundance of cobalt (20–30 ppm). Scandium is only the 50th most common element on Earth (35th most abundant in the crust), but it is the 23rd most common element in the Sun.[10] However, scandium is distributed sparsely and occurs in trace amounts in many minerals.[11] Rare minerals from Scandinavia[12] and Madagascar[13] such as thortveitite, euxenite, and gadolinite are the only known concentrated sources of this element. Thortveitite can contain up to 45% of scandium in the form of scandium oxide.[12]

The stable form of scandium is created in supernovas via the r-process.[14] Also, in addition, scandium is created by cosmic ray spallation of the more abundant iron nuclei.

• ²⁸Si + 17n → ⁴⁵Si (r-process)
• ⁵⁶Fe + p → ⁴⁵Sc + ¹¹C + n (cosmic ray spallation)

Production

The world production of scandium is in the order of 15-20 tonnes per year, in the form of scandium oxide. The demand is about 50% higher, and both the production and demand keep increasing. In 2003, only three mines produced scandium: the uranium and iron mines in Zhovti Vody in Ukraine, the rare-earth mines in Bayan Obo, China, and the apatite mines in the Kola peninsula, Russia; since then many other countries have built scandium-producing facilities, including 5 tonnes/year (7.5 tonnes/year Sc₂O₃) by Nickel Asia Corporation and Sumitomo Metal Mining in the Philippines.[15][16] In the United States, NioCorp Development hopes to raise $1 billion[17] toward opening a niobium mine at its Elk Creek site in southeast Nebraska[18] which may be able to produce as much as 95 tonnes of scandium oxide annually.[19] In each case scandium is a byproduct from the extraction of other elements and is sold as scandium oxide.[20][21][22]

To produce metallic scandium, the oxide is converted to scandium fluoride and then reduced with metallic calcium.

Madagascar and the Iveland-Evje region in Norway have the only deposits of minerals with high scandium content, thortveitite (Sc,Y)₂(Si₂O₇) but these are not being exploited.[21] The mineral kolbeckite ScPO₄·2H₂O has a very high scandium content but is not available in any larger deposits.[21]

The absence of reliable, secure, stable, long-term production has limited the commercial applications of scandium. Despite this low level of use, scandium offers significant benefits. Particularly promising is the strengthening of aluminium alloys with as little as 0.5% scandium. Scandium-stabilized zirconia enjoys a growing market demand for use as a high-efficiency electrolyte in solid oxide fuel cells.

Price

Because of its rarity, scandium is among the most expensive elements. Price for pure scandium fluctuates between 4000 and 20000 US dollars per kilogram. Meanwhile, the limited market generates a variety of prices at any given time. In 2010, at the peak of the rare-earths shortage, the price of scandium rose to over 15000 US dollars per kilogram, and the widely commercially used scandium oxide (Sc₂O₃) was selling above 7000 US dollars per kilogram. Since then the limited demand coupled with steady production keeps the price at its 20-year average.[23]

Compounds

Scandium chemistry is almost completely dominated by the trivalent ion, Sc³⁺. The radii of M³⁺ ions in the table below indicate that the chemical properties of scandium ions have more in common with yttrium ions than with aluminium ions. In part because of this similarity, scandium is often classified as a lanthanide-like element.

Ionic radii (pm)

Al	Sc	Y	La	Lu
53.5	74.5	90.0	103.2	86.1

Oxides and hydroxides

The oxide Sc
₂O
₃ and the hydroxide Sc(OH)
₃ are amphoteric:[24]

Sc(OH)
₃ + 3 OH⁻
→ [Sc(OH)
₆]³⁻
(scandate ion)

Sc(OH)
₃ + 3 H⁺
+ 3 H
₂O → [Sc(H
₂O)
₆]³⁺

α- and γ-ScOOH are isostructural with their aluminium hydroxide oxide counterparts.[25] Solutions of Sc³⁺
in water are acidic due to hydrolysis.

Halides and pseudohalides

The halides ScX₃, where X= Cl, Br, or I, are very soluble in water, but ScF₃ is insoluble. In all four halides, the scandium is 6-coordinated. The halides are Lewis acids; for example, ScF₃ dissolves in a solution containing excess fluoride ion to form [ScF₆]³⁻. The coordination number 6 is typical for Sc(III). In the larger Y³⁺ and La³⁺ ions, coordination numbers of 8 and 9 are common. Scandium triflate is sometimes used as a Lewis acid catalyst in organic chemistry.

Organic derivatives

Main article: Organoscandium chemistry

Scandium forms a series of organometallic compounds with cyclopentadienyl ligands (Cp), similar to the behavior of the lanthanides. One example is the chlorine-bridged dimer, [ScCp₂Cl]₂ and related derivatives of pentamethylcyclopentadienyl ligands.[26]

Uncommon oxidation states

Compounds that feature scandium in oxidation states other than +3 are rare but well characterized. The blue-black compound CsScCl₃ is one of the simplest. This material adopts a sheet-like structure that exhibits extensive bonding between the scandium(II) centers.[27] Scandium hydride is not well understood, although it appears not to be a saline hydride of Sc(II).[4] As is observed for most elements, a diatomic scandium hydride has been observed spectroscopically at high temperatures in the gas phase.[3] Scandium borides and carbides are non-stoichiometric, as is typical for neighboring elements.[28]

Lower oxidation states (+2, +1, 0) have also been observed in organoscandium compounds.[29][30][31][32]

History

Dmitri Mendeleev, who is referred to as the father of the periodic table, predicted the existence of an element ekaboron, with an atomic mass between 40 and 48 in 1869. Lars Fredrik Nilson and his team detected this element in the minerals euxenite and gadolinite in 1879. Nilson prepared 2 grams of scandium oxide of high purity.[33][34] He named the element scandium, from the Latin Scandia meaning "Scandinavia". Nilson was apparently unaware of Mendeleev's prediction, but Per Teodor Cleve recognized the correspondence and notified Mendeleev.[35][36]

Metallic scandium was produced for the first time in 1937 by electrolysis of a eutectic mixture of potassium, lithium, and scandium chlorides, at 700–800 °C.[37] The first pound of 99% pure scandium metal was produced in 1960. Production of aluminium alloys began in 1971, following a US patent.[38] Aluminium-scandium alloys were also developed in the USSR.[39]

Laser crystals of gadolinium-scandium-gallium garnet (GSGG) were used in strategic defense applications developed for the Strategic Defense Initiative (SDI) in the 1980s and 1990s.[40][41]

Red giant stars near the Galactic Center

In early 2018, evidence was gathered from spectrometer data of significant scandium, vanadium and yttrium abundances in red giant stars in the Nuclear Star Cluster (NSC) in the Galactic Center. Further research showed that this was an illusion caused by the relatively low temperature (below 3,500 K) of these stars masking the abundance signals, and that this phenomenon was observable in other red giants.[42]

Applications

Parts of the MiG-29 are made from Al-Sc alloy.[43]

The addition of scandium to aluminium limits the grain growth in the heat zone of welded aluminium components. This has two beneficial effects: the precipitated Al₃Sc forms smaller crystals than in other aluminium alloys,[43] and the volume of precipitate-free zones at the grain boundaries of age-hardening aluminium alloys is reduced.[43] Both of these effects increase the usefulness of the alloy. However, titanium alloys, which are similar in lightness and strength, are cheaper and much more widely used.[44]

The alloy Al₂₀Li₂₀Mg₁₀Sc₂₀Ti₃₀ is as strong as titanium, light as aluminium, and hard as ceramic.[45]

The main application of scandium by weight is in aluminium-scandium alloys for minor aerospace industry components. These alloys contain between 0.1% and 0.5% of scandium. They were used in the Russian military aircraft, specifically the Mikoyan-Gurevich MiG-21 and MiG-29.[43]

Some items of sports equipment, which rely on high-performance materials, have been made with scandium-aluminium alloys, including baseball bats[46] and bicycle frames and components.[47] Lacrosse sticks are also made with scandium. The American firearm manufacturing company Smith & Wesson produces semi-automatic pistols and revolvers with frames of scandium alloy and cylinders of titanium or carbon steel.[48][49]

Dentists use erbium-chromium-doped yttrium-scandium-gallium garnet (Er,Cr:YSGG) lasers for cavity preparation and in endodontics.[50]

The first scandium-based metal-halide lamps were patented by General Electric and initially made in North America, although they are now produced in all major industrialized countries. Approximately 20 kg of scandium (as Sc₂O₃) is used annually in the United States for high-intensity discharge lamps.[51] One type of metal-halide lamp, similar to the mercury-vapor lamp, is made from scandium triiodide and sodium iodide. This lamp is a white-light source with high color rendering index that sufficiently resembles sunlight to allow good color-reproduction with TV cameras.[52] About 80 kg of scandium is used in metal-halide lamps/light bulbs globally per year.

The radioactive isotope ⁴⁶Sc is used in oil refineries as a tracing agent.[51] Scandium triflate is a catalytic Lewis acid used in organic chemistry.[53]

Health and safety

Elemental scandium is considered non-toxic, though extensive animal testing of scandium compounds has not been done.[54] The median lethal dose (LD₅₀) levels for scandium chloride for rats have been determined as 755 mg/kg for intraperitoneal and 4 g/kg for oral administration.[55] In the light of these results, compounds of scandium should be handled as compounds of moderate toxicity.

See also

• Rare-earth element

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Further reading

• Scerri, Eric R. (2007). The Periodic System: Its Story and Its Significance. Oxford, UK: Oxford University Press. ISBN 9780195305739. OCLC 62766695.

External links

• Scandium at The Periodic Table of Videos (University of Nottingham)
• WebElements.com – Scandium
• "Scandium" . Encyclopædia Britannica (11th ed.). 1911.