- Oxygen in almost all compounds has an oxidation # of (-2).
- Your solving for the oxidation # of Fe so make this (X)
- Creating an equation with what you know:
There are 2 Fe in the compound, so it would be 2X.
There are 3 O in the compound, so it would be (-2 * 3) = -6
2X - 6 = 0
-Do the algebra:
1) 2X = +6
2) X = +6/ 2
3) X = Fe = +3 oxidation number
-2.
The oxidation number of oxygen is almost always -2, unless it is in a superoxide, peroxide, bonded to fluorine, or with itself.
In Fe2O3, we know that the total negative charge must equal the total positive charge.
O3 = -6
Fe = +3 x 2 = +6
It is an increase of 1 as iron goes from the 2+ to the 3+ oxidation state.
+3 for each Fe, -2 for each O.
Note: There is no compound with the formula FeO3 as originally asked in the question.
FeO, iron is +2; Fe2O3 iron is +3. Oxygen is -2 in both compounds
oxidation state is +2
Iron is in oxidation state +3 in Fe2O3
3+
O = 2-, Fe = 3+.
+3 for Fe and -2 for O.
Fe2O3. +3 for Fe, -2 of O.
Fe3O4 can be considered to be 1:1 mixture of FeO and Fe2O3. Oxidation number in FeO: +2 for Fe and -2 of O Oxidation number in Fe2O3: +3 for Fe and -2 of O
+3 for Fe; -2 for O
O = 2-, Fe = 3+.
+3 for Fe and -2 for O.
Fe2O3. +3 for Fe, -2 of O.
Oxidation numbers in Fe2O3 are respectively: Fe => +3 and O => -2
Fe3O4 can be considered to be 1:1 mixture of FeO and Fe2O3. Oxidation number in FeO: +2 for Fe and -2 of O Oxidation number in Fe2O3: +3 for Fe and -2 of O
+3 for Fe; -2 for O
The oxidation number for Fe would be 3+ and for oxygen it would be 2-. This would be Fe2O3
100 will be oxidation no.in Fe2O3.
Usually, oxygen has an oxidation of -2 (that is unless in a compound with peroxides or halogens).
it is +2 it is also done by causing rust
Fe2O3 +3 for each Fe -2 for each O
Ru has oxidation number +8, O has oxidation number of -2