ALUMINUM - Al

Properties of Aluminum:

White light plastic metal. Passivated in water, in the concentrated nitric acid and in solution of a potassium bichromate because of formation of a steady oxidic film. The amalgamated metal reacts with water. The strong reducer, high reactivity. Shows amphoteric properties, reacts with diluted acids and alkalis.


Molar mass g/mol 26.982
Density g/cm3 2.702
Melting point °C 660.37
Boiling point °C 2500

Methods for preparation of Aluminum:

2Al2O3→Electrolysis(in melt of Na3[AlF6])→4Al(cathode)+3O2(anode)↑ (900°C).

2AlCl3(liquid) → Electrolysis → 2Al(on cathode) + 3Cl2(on anode)↑.


Сhemical reactions with metal Aluminum:

2(Al, Hg) + 6H2O = 2Al(OH)3↓ + 3H2↑ + 2Hg↓ (amalgam, normal temp.)

2Al + 6HCl(diluted) = 2AlCl3 + 3H2↑.

8Al + 30HNO3(diluted) = 8Al(NO3)3 + 3NO2 + 15H2O.

8Al + 30HNO3(high diluted) = 8Al(NO3)3 + 3NH4NO3 + 9H2O.

2Al + 2(NaOH·H2O) = 2NaAlO2 + 3H2O (400-500°C).

2Al + 2NaOH(conc.) + 6H2O(hot) = 2Na[Al(OH)4] + 3H2↑.

8Al + 18H2O + 3KNO3 + 5KOH = 8K[Al(OH)4] + NH3↑ (boiling).

4Al(powder) + 3O2 = 2Al2O3 (burning on air).

2Al + 3F2 = 2AlF3 (600°C).

2Al(powder) + 3E2 = 2AlE3 (25°C; E = Cl, Br).

2Al(powder) + 3I2 = 2AlI3 (25°C; catalyst - water drop).

2Al + 3S = Al2S3 (150-200°C).

2Al(powder) + N2 = 2AlN (800-1200°C).

4Al + P4 = 4AlP (500-800°C, in the atm. H2).

4Al + 3C(graphite) = Al4C3 (1500-1700°C).

2Al + 6HF(gas) = 2AlF3 + 3H2 (450-500°C).

2Al + 3H2S = Al2S3 + 3H2 (600-1000°C).

2Al + 2NH3 = 2AlN + 3H2 (over 600°C).

8Al + 3(FeIIFeIII2)O4 = 4Al2O3 + 9Fe (over 2000°C).


 

Did you know?

If you slowly pour a handful of salt into a completely full glass of water, it will not overflow. In fact, the water level will go down.