1. Created By :
Group 1
Lia Agustini (06121010007)
Ranny Rolinda Rusman (06121010020)
Arum Estu Tami (06121010028)
2. 1. Scandium
Scandium derived from latin scandia which means
scandinavia
Scandium was discovered by Lars Nilson in 1879 in
Sweden.
Scandium is found in minerals euxenite, thortveitile,
thortvetile and Gadoline at Scandinavia and
Madagascar.
3. Properties of Scandium
Scandium is a silver-white metal that changes color to
yellow if it reacts with air.
4. physical properties of scandium
Physical properties :
1. Density : 3 g/cm3
2. Melting Point : 1812.2 K
3. Boiling Point : 3021 K
4. Form (25 ° C) : solid
5. Color : white silver
5. Atomic Properties Of Scandium
Atomic Properties
1. Atomic number : 21
2. The mass number : 44,956
3. Electron Configuration : [Ar] 3d1 4S2
4. Atomic Volume : 15 cm3/mol
5. electron affinity : 18.1 kJ / mol
6. 6. Electronegativities : 1.36
7. ionisation energy- first : 631 kJ / mol, second : 1235
kJ / mol, third : 2389 kJ / mol
8. main oxidation states : +3
9. other oxidation states : +1, +2
10. Shape Crystal : Hexagonal Unit Cell
In the solid state of scandium has a hexagonal crystal
structure.
7. Chemical Properties and chemical
reactions
Chemical Properties of Scandium
Reaction with water:
When heated, the Scandium will dissolve in water to
form a solution consisting of ions Sc (III) and
hydrogen gas.
2Sc(s) + 6H2O(aq) ---> 2Sc3+
(aq) + 6OH-
(aq) + 3H2(g)
8. Reaction with oxygen
In the reaction with the air or combustion quickly it
will formscandium (III) oxide.
4Sc(s) + 3O2(g) ---> 2Sc2O3(s)
9. Reactions with halogens
Scandium is very reactive when it reacts with all the
halogens to form trihalides elements.
2Sc(s) + 3F2(g) ---> 2ScF3(s)
2Sc(s) + 3Cl2(g) ---> 2ScCl3(s)
2Sc(s) + 3Br2(l) ---> 2ScBr3(s)
2Sc(s) + 3I2(s) ---> 2ScI3(s)
10. The reaction with acid
Scandium readily soluble in hydrochloric acid to form
a solution containing ions Sc (III) and hydrogen gas.
Sc(s) + 6HCl(aq) ---> 2Sc3+
(aq) + 6Cl-
(aq) + 3H2(g)
11. Useful of Scandium
Clorida Scandium (ScCl3), where these compounds
can be found in halide lamps, fiber optic, and laser
ceramic electrolyte.
primary application of the elements scandium alloy is
as alumunium- scandium is used for sports equipment
(bikes) that have a high quality.
12. other applications is the use of scandium iodide for
lights that provide a high intensity. Sc2O3 is used as a
catalyst in the manufacture of Acetone
13. For Health and Environment Effects
Scandium is not toxic, but need to be careful because
some scandium compounds may be carcinogenic in
humans but it can cause liver damage if it accumulates
in the body.
14. Together with aquatic animals, Sc can cause damage to
the cell membrane, thus providing a negative effect on
the reproductive and nervous systems.
15. Sc can contaminate the environment, especially from
the petroleum industry and from the disposal of
household furniture.
Sc continuously accumulate in the soil, it will trigger
the concentration in the human body and animals.
16. 2. Yitrium
Yitrium is a group IIIB element residing in the period
5.
Yitrium included in the transition metal.
17. Yitrium was discovered by researchers from Finland
named Johan Gadolin and isolated in 1794 by Friedrich
Wohler in 1828 in the form of impure extract of yttria
from yttrium chloride anhydrous reduction (YCl3)
with potassium.
18. Properties of Yitrium
Pyshical Properties
1. Density : 4,5 g/cm3
2. Melting Point : 1799 [or 1526 ° C (2779 ° F)] K
3. Boiling Point : 3609 [or 3.336 ° C (6037 ° F)] K
4. Form (25°C) : solid
5. Color : silver
19. Atomic Properties
1. Atomic Number : 39
2. Mass Number : 88,91
3. Electron Configuration : [Kr] 4d1 5s2
4. Atomic volume : 19,8 cm3/mol
5. Affinity Electron : 29,6 kJ/mol
20. Chemical Properties and Chemical
Reaction
Reaction with water
When heated it Yitrium metal will dissolve in water to
form a solution consisting of ion Y (III) and hydrogen
gas
2Y(s) + 6H2O(aq) → 2Y3+
(aq) + 6OH-
(aq) + 3H2(g)
21. Reaction with oxygen
In the reaction with the air or combustion quickly it
will form Yitrium (III) oxide
4Y(s) + 3O2(g) → 2Y2O3(s)
22. Reactions with halogens
Yitrium is very reactive when it reacts with all the
halogens to form trihalides elements.
2Y(s) + 3F2(g) → 2YF3(s)
2Y(s) + 3Cl2(g) → 2YCl3(s)
2Y(s) + 3Br2(g) → 2YBr3(s)
2Y(s) + 3I2(g) → 2YI3(s)
23. Reaction with acid
Yitrium easily soluble in hydrochloric acid to form a
solution containing ions of Y (III) and hydrogen gas.
2Y(s) + 6HCl(aq) → 2Y3+
(aq) + 6Cl-
(aq) + 3H2(g)
24. Useful of Yitrium
Allumunium Yitrium Garnet Y3All5O12 is used for laser,
stimulant and diamond.
Yitrium is also used to increase the strength of the
metals aluminum and magnesium alloy
25. For Health and Environment Effects
Yitrium danger if react with the air is if inhaled by
humans can cause cancer and if it accumulates in
excess amounts in the body causing damage to the
liver.
Yitrium can contaminate the environment, especially
from the petroleum industry and from the disposal of
household furniture.
26. 3. Lanthanium
lanthanium discovered in Sweden by Carl Gustav
Mosander which is a great chemist with the nickname
"father moses" in 1893
Lanthanium derived from latin “Lanthana” which
means hidden.
27. Physical Properties of Lanthanium
Lanthanum is a silvery white metal
malleable
strong but soft enough to cut with a knife.
Lanthanium is one of the highly reactive metals.
28. Lanthanium oxidizing rapidly when exposed to air.
Lanthanum has a density of 6,17 g/cm3.
melting point of 1193.2 K
boiling point of 3693 K.
29. Chemical Properties
Reaction with water
Lanthanum is quite electropositive and reacts slowly
with cold water but fairly quickly if it reacts with hot
water to form hydrogen gas and hydroxide Lanthana.
2La(s)+6H2O(g) → 2La(OH)3(aq)+3H2(g)
30. Reaction with oxygen
In the reaction with the air or combustion quickly it
will form Lanthana (III) oxide.
4La(s) + 3O2(g) → 2La2O3(s)
31. Reactions with halogens
Lanthanum metal reacts with all the halogen elements
form Lanthana (III) halide.
2La(s) + 3F2(g) → 2LaF3(s)
2La(s) + 3Cl2(g) → 2LaCl3(s)
2La(s) + 3Br2(g) → 2LaBr3(s)
2La(s) + 3I2(g) → 2LaI3(s)
32. Useful of Lanthanium
La2O2 is used to create a special optical glass (glass
adsorbs infrared, camera and telescope lenses).
If La is added in the steel will increase the softness and
durability of the steel.
La was used as the main material in the carbon
electrode (carbon arc electrodes).
33. La salts contained in the zeolite catalysts used in the
petroleum refining process.
One of the uses of the compounds Lanthanida goal is
in the film industry for studio lighting and projection.
34. For Health and Environment Effects
La is very dangerous if the fog and the smoke inhaled
with the influx of oxygen and in the long term, will be
able to cause embolism.
If the person can breathe La affected by lung cancer.
35. If accumulates in the body, the La-threatening liver
organ.
La can contaminate the environment, especially from
the petroleum industry and from the disposal of
household furniture.
36. 4. Actinium
The word actinium comes from the Greek, activism,
aktinos, which means “light”.
Actinium was discovered in 1899 by Andre-Louis
Debierne a French chemist who separates from the
mixture actinium. Actinium is separated from
uranium ores
37. Physical Properties
1. Density : 10 g/cm3
2. Melting Point : 1323.2 K
3. Boiling Point : 2743 K
4. Form (25 ° C) : solid
5. Color : white silver
6. Melting Heat : 14 kj/mol
7. Heat of evaporation : 400 kj/mol
8. material Capacity : (25 ° C) 27,2 J mol -1 K -1
38. Chemical Properties
Actinium shows chemical properties similar to
lanthanum
Reaction with Oxygen
Actinium is flammable and form actinium (III) oxide.
4Ac(s) + 3O2(g) → 2Ac2O3(s)
39. Useful
The properties of radioactivity of actinium 150 times
larger than radium, making it possible to use Ac as a
neutron source.
Ac-225 is used as a healing agent for the "radio-immunotherapy".
40. For Health and Environtment
Effects
Actinium-227 is highly radioactive and adverse health
effects.
The greatest danger from radioactive transform life as
we know it is a danger to the reproductive system and
the nature of the decline.
Even with low-dose carcinogenic which causes a
decrease in the immune system.
