ppt group iii b

Created By :Group 1

Lia Agustini (06121010007)

Ranny Rolinda Rusman (06121010020)Arum Estu Tami (06121010028)

1. Scandium Scandium derived from latin scandia which means

scandinavia

Scandium was discovered by Lars Nilson in 1879 inSweden.

Scandium is found in minerals euxenite, thortveitile,thortvetile and Gadoline at Scandinavia andMadagascar.

Properties of Scandium

Scandium is a silver-white metal that changes color to yellow if it reacts with air.

physical properties of scandiumPhysical 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

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. Electronegativities : 1.36

7. ionisation energy- first : 631 kJ / mol, second : 1235kJ / 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 crystalstructure.

Chemical Properties and chemical reactionsChemical Properties of Scandium

Reaction with water:

When heated, the Scandium will dissolve in water toform a solution consisting of ions Sc (III) andhydrogen gas.

2Sc(s) + 6H2O(aq) ---> 2Sc3+(aq) + 6OH-

(aq) + 3H2(g)

Reaction with oxygen

In the reaction with the air or combustion quickly itwill form scandium (III) oxide.

4Sc(s) + 3O2(g) ---> 2Sc2O3(s)

Reactions with halogens

Scandium is very reactive when it reacts with all thehalogens 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)

The reaction with acid

Scandium readily soluble in hydrochloric acid to forma solution containing ions Sc (III) and hydrogen gas.

Sc(s) + 6HCl(aq) ---> 2Sc3+(aq) + 6Cl-

(aq) + 3H2(g)

Useful of Scandium Clorida Scandium (ScCl3), where these compounds

can be found in halide lamps, fiber optic, and laserceramic electrolyte.

primary application of the elements scandium alloy isas alumunium- scandium is used for sports equipment(bikes) that have a high quality.

other applications is the use of scandium iodide forlights that provide a high intensity. Sc2O3 is used as acatalyst in the manufacture of Acetone

For Health and Environment Effects

Scandium is not toxic, but need to be careful becausesome scandium compounds may be carcinogenic inhumans but it can cause liver damage if it accumulatesin the body.

Together with aquatic animals, Sc can cause damage tothe cell membrane, thus providing a negative effect onthe reproductive and nervous systems.

Sc can contaminate the environment, especially fromthe petroleum industry and from the disposal ofhousehold furniture.

Sc continuously accumulate in the soil, it will triggerthe concentration in the human body and animals.

2. YitriumYitrium is a group IIIB element residing in the period 5.

Yitrium included in the transition metal.

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 yttriafrom yttrium chloride anhydrous reduction (YCl3) with potassium.

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

Atomic Properties1. 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

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)

Reaction with oxygen

In the reaction with the air or combustion quickly itwill form Yitrium (III) oxide

4Y(s) + 3O2(g) → 2Y2O3(s)

Reactions with halogens

Yitrium is very reactive when it reacts with all thehalogens 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)

Reaction with acid

Yitrium easily soluble in hydrochloric acid to form asolution containing ions of Y (III) and hydrogen gas.

2Y(s) + 6HCl(aq) → 2Y3+(aq) + 6Cl-

(aq) + 3H2(g)

Useful of Yitrium

Allumunium Yitrium Garnet Y3All5O12 is used for laser,stimulant and diamond.

Yitrium is also used to increase the strength of themetals aluminum and magnesium alloy

For Health and Environment Effects

Yitrium danger if react with the air is if inhaled byhumans can cause cancer and if it accumulates inexcess amounts in the body causing damage to theliver.

Yitrium can contaminate the environment, especiallyfrom the petroleum industry and from the disposal ofhousehold furniture.

3. Lanthanium

lanthanium discovered in Sweden by Carl GustavMosander which is a great chemist with the nickname"father moses" in 1893

Lanthanium derived from latin “Lanthana” whichmeans hidden.

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.

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.

Chemical Properties Reaction with water

Lanthanum is quite electropositive and reacts slowlywith cold water but fairly quickly if it reacts with hotwater to form hydrogen gas and hydroxide Lanthana.

2La(s)+6H2O(g) → 2La(OH)3(aq)+3H2(g)

Reaction with oxygen

In the reaction with the air or combustion quickly itwill form Lanthana (III) oxide.

4La(s) + 3O2(g) → 2La2O3(s)

Reactions with halogens

Lanthanum metal reacts with all the halogen elementsform 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)

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 anddurability of the steel.

La was used as the main material in the carbonelectrode (carbon arc electrodes).

La salts contained in the zeolite catalysts used in thepetroleum refining process.

One of the uses of the compounds Lanthanida goal isin the film industry for studio lighting and projection.

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 beable to cause embolism.

If the person can breathe La affected by lung cancer.

If accumulates in the body, the La-threatening liverorgan.

La can contaminate the environment, especially fromthe petroleum industry and from the disposal ofhousehold furniture.

4. Actinium The word actinium comes from the Greek, activism,

aktinos, which means “light”.

Actinium was discovered in 1899 by Andre-LouisDebierne a French chemist who separates from themixture actinium. Actinium is separated fromuranium ores

Physical Properties1. 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

Chemical Properties

Actinium shows chemical properties similar tolanthanum

Reaction with Oxygen

Actinium is flammable and form actinium (III) oxide.

4Ac(s) + 3O2(g)→ 2Ac2O3(s)

Useful

The properties of radioactivity of actinium 150 timeslarger than radium, making it possible to use Ac as aneutron source.

Ac-225 is used as a healing agent for the "radio-immunotherapy".

For Health and Environtment Effects Actinium-227 is highly radioactive and adverse health

effects.

The greatest danger from radioactive transform life aswe know it is a danger to the reproductive system andthe nature of the decline.

Even with low-dose carcinogenic which causes adecrease in the immune system.