This ppt made by cosnert rabbani, student of chemist departement of andalas university, padang,Indonesia. Contact : Cosnertrabbani@gmail.com

1. History Of Scandium (Sc)
From the Latin word Scandia,
Scandinavia. On the basis of the
Periodic System, Mendeleev predicted
the existence of ekaboron, which
would have an atomic weight between
40 of calcium and 48 of titanium.

3. EKA-BORON
 The name given by Mendeleyev in accordance with the periodic law, and by prediction, to
a hypothetical element then unknown, but since discovered and named scandium. so
called because it was a missing analogue of the boron group.

4.  The element was
discovered by Nilson
in 1878 in the
minerals euxenite and
gadolinite, which had
not yet been found
anywhere except in
Scandinavia.
 euxenite and
gadolinite is
sources of this
element

5. Properties
 Scandium is a silver-white metal which develops a
slightly yellowish or pinkish cast upon exposure to air.
A relatively soft element, scandium resembles yttrium
and the rare-earth metals more than it resembles
aluminum or titanium.
 It is a very light metal and has a much higher melting
point than aluminum, making it of interest to
designers of spacecraft.

6. Source
 Scandium is apparently much more abundant (the
23rd most) in the sun and certain stars than on earth
(the 50th most abundant). It occurs as a principal
component in the rare mineral thortveitite, found in
Scandinavia and Malagasy.
 It is also found in the residues remaining after the
extraction of tungsten from Zinnwald wolframite.

7. How to extrat skandium?
 Pure scandium metal can be made by reacting
scandium fluoride (ScF3) with another active metal,
such as calcium or zinc, eg,
 3Ca + 2ScF3  3CaF2 + 2Sc

8. Reaction
Reaction of scandium with air
 Scandium metal tarnishes in air and burns readily to
form scandium (III) oxide, Sc2O3.
4Sc + 3O2 → 2Sc2O3

9. Reaction of scandium with water
 When finely divided, or heated, scandium metal
dissolves in water to form solutions containing the
aquated Sc(III) ion together with hydrogen gas, H2.
2Sc(s) + 6H2O(aq) → 2Sc3+(aq) + 6OH-(aq) + 3H2(g)

10. Reaction of scandium with the
halogens
Scandium is very reactive towards the halogens
fluorine, F2, chlorine, Cl2 bromine, Br2, and iodine, I2,
and burns to form the trihalides scandium(III)
fluoride, ScF3 , scandium(III) chloride, ScCl3,
scandium(III) bromide, ScBr3, and scandium(III)
iodide, ScI3 respectively.
 2Sc(s) + 3F2(g) → 2ScF3(s)
 2Sc(s) + 3Cl2(g) → 2ScCl3(s)
 2Sc(s) + 3Br2(g) → 2ScBr3(s)
 2Sc(s) + 3I2(g) → 2ScI3(s)

11. Application
 About 20 kg of scandium (as Sc2O3) are used yearly in
the U.S. to produce high-intensity lights.
 The radioactive isotope 46 Sc is used as a tracing agent
in refinery crackers for crude oil, etc.
 Scandium iodide added to mercury vapor lamps
produces a highly efficient light source resembling
sunlight, which is important for indoor or night-time
color TV.

12. Continue..
 The original use of scandium-aluminium alloys was in
the nose cones of some Soviet submarine-launched
ballistic missiles (SLBM).
 Scandium alloys are especially desirable for use in, for
example, baseball bats, lacrosse sticks, and bicycle
frames.
 Fuel cells