The oxidation number of iron in ferrousofericoxide (Fe3O4) is a combination of Fe(II) and Fe(III) ions. The Fe(II) ions have an oxidation number of +2, while the Fe(III) ions have an oxidation number of +3. Each formula unit of Fe3O4 contains two Fe(III) ions and one Fe(II) ion, resulting in an average oxidation number of +2.67 for iron in this compound.
The formula for iron using the highest oxidation number is Fe2O3, which is iron(III) oxide. In this compound, iron is in the +3 oxidation state.
The oxidation number of iron in Fe3O4 is +8/3. This is calculated by assigning oxygen an oxidation number of -2, and solving for the oxidation number of iron using the formula: (3x) + (4(-2)) = 0.
The oxidation number of iron in the brown ring complex is +2. This complex is [Fe(H2O)5NO]2+ where the iron atom is in the +2 oxidation state.
The oxidation number of iron in Fe3O4 is +2. This is because oxygen is assigned an oxidation number of -2 and the overall charge of the compound is neutral. So, iron must have an oxidation number of +2 to balance out the charges.
The oxidation number of Fe in FeO (iron oxide) is +2. This is because oxygen typically has an oxidation number of -2, and in a neutral compound like FeO, the oxidation numbers must balance out to zero.
The formula for iron using the highest oxidation number is Fe2O3, which is iron(III) oxide. In this compound, iron is in the +3 oxidation state.
The oxidation number of iron in Fe3O4 is +8/3. This is calculated by assigning oxygen an oxidation number of -2, and solving for the oxidation number of iron using the formula: (3x) + (4(-2)) = 0.
The oxidation number of iron in the brown ring complex is +2. This complex is [Fe(H2O)5NO]2+ where the iron atom is in the +2 oxidation state.
The oxidation number of iron in Fe3O4 is +2. This is because oxygen is assigned an oxidation number of -2 and the overall charge of the compound is neutral. So, iron must have an oxidation number of +2 to balance out the charges.
The oxidation number of Fe in FeO (iron oxide) is +2. This is because oxygen typically has an oxidation number of -2, and in a neutral compound like FeO, the oxidation numbers must balance out to zero.
study island answer is +3 -2
The oxidation state of iron in iron (III) compounds is +3. This means that each iron atom in these compounds has lost 3 electrons.
In Fe2O3, iron (Fe) has an oxidation number of +3, and oxygen (O) has an oxidation number of -2. Iron's oxidation number is determined by balancing the overall charge of the compound based on the known oxidation number of oxygen.
The oxidation number of iron is +2 (Fe2+), and the oxidation number of oxygen is -2 (O2-). In iron(II) oxide (Fe2O3), which has two iron ions and three oxygen ions, the overall charge must balance to zero, so the oxidation number of iron is +3.
The oxidation number of iron in sodium nitroprusside is +2. This is because the overall compound has a neutral charge, and since there are 5 cyanide ions each with a -1 charge, the iron must have a +2 oxidation state to balance the charges.
The oxidation number change for the iron atom in a reaction is from Fe^0 (elemental form) to Fe^2+ or Fe^3+ (ionic form). This represents an oxidation of the iron atom, as it loses electrons and increases its oxidation state.
The oxidation number of iron can vary, but it is commonly found at +2 or +3. In some compounds, like Fe2O3, iron is in the +3 oxidation state, while in others, like FeO, it is in the +2 oxidation state.