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The oxidation number of Al is +3.
In pure metallic aliminium it is zero . In the majority of its compounds it is +3, e.g. in Al2O3, AlCl3, AlP
0 in the elemental form, +3 in its compounds
Roman Numeral
0 in elemental form +3 in its compounds
+3 for Al and -2 for O is the oxidation number for Al2O3.
Aluminium has an oxidation state (number) of +3 in Al2O3. Al3O3 does not exist.
Aluminium oxide is Al2O3. +3 for each Al and -2 for each O.
In the compound Al2O3, aluminium has an oxidation number of +3, while oxygen's oxidation number is __-2 ____. For aluminium oxide (Al2O3) to form the ionic charges MUST balance. Hence For the 2 aluminiums it is 2 x 3 = +6 For the 3 oxygens it is 3 X -2 = -6 +6 -6 = 0 So the charges balance, hence Al2O3 is neutrally charged compound and NOT an ion.
-2
so you find the ratio of Aluminum to Oxygenin this case it is 2:3and then because the total mole is 2.16for aluminum:2.16/5*2 = 0.864for oxygen:2.16/5*3 = 1.296hope this helped :D
From '0' to '3'. Elemental aluminium is in oxidation state zero (0). When it combines with oxygen to form aluminium oxide , it 'looses' its three outermost electrons to oxygen. Hence aluminium metal becomes the aluminium cation (Al^3+), which is oxidation state '3'.
The oxidation number of Al is +3.
about 267.12g
The oxidation number of Al is +III and S is -II.
Fe2O3 + 2Al ===> Al2O3 + 2FeIn this reaction the number of moles of Al2O3 produced is dependent on the number of moles of Fe2O3 and Al that one starts with. For every 1 mole Fe2O3 and 2 moles Al, one gets 1 moles of Al2O3.
When the oxidation states of reactants in a chemical reaction are changed (parallel phenomena of oxidation and reduction) a redox reaction occur:Fe2O3 + 2 Al = Al2O3 + 2 Fe