Mg(s) + FeCl2(aq) → MgCl2(aq) + Fe(s). IS THE IRON(II) ION OXIDIZED?
No.
Oxidation is the loss of electrons.
Reduction is the gain of electrons.
Mg(s) with a zero oxidation number changes to Mg^2+ ion with a +2 oxidation number. From zero charge to +2 charge means it had to lose electrons so Mg is oxidized.
Fe^2+ on the left changes to Fe(s) on the right. That must be a gain of electrons so it is reduced.
No, the Iron(II) ion is not oxidized. It probably just realized it left the oven on and hurriedly grabbed a fire extinguisher to put out the flames.
In the reaction Mg(s) + FeCl2(aq) → MgCl2(aq) + Fe(s), iron (II) ion (Fe2+) undergoes oxidation.
To determine if a substance is oxidized, you need to compare the oxidation state of the element before and after the reaction.
In FeCl2(aq), the oxidation state of iron is +2. However, in Fe(s), the oxidation state of iron is 0. This indicates that iron has lost electrons and its oxidation state has increased from +2 to 0.
Therefore, iron (II) ion (Fe2+) is indeed oxidized in the given reaction.
To determine whether the Iron(II) ion (Fe2+) is oxidized in the given chemical equation:
Mg(s) + FeCl2(aq) → MgCl2(aq) + Fe(s)
We need to compare the oxidation states of Iron before and after the reaction.
1. Start by identifying the oxidation states of all elements in the equation:
- In Mg(s), Magnesium (Mg) has an oxidation state of 0 because it is in its elemental state.
- In FeCl2(aq), Chlorine (Cl) usually has an oxidation state of -1 in compounds, so Iron (Fe) must have an oxidation state of +2 to balance the charge of the compound.
- In MgCl2(aq), Chlorine (Cl) still has an oxidation state of -1, so Magnesium (Mg) must have an oxidation state of +2 to balance the charge of the compound.
- In Fe(s), Iron (Fe) has an oxidation state of 0 because it is in its elemental state.
2. Compare the oxidation states of Iron before and after the reaction:
- Before the reaction, Iron (Fe) in FeCl2(aq) has an oxidation state of +2.
- After the reaction, Iron (Fe) in Fe(s) has an oxidation state of 0.
Since the oxidation state of Iron changes from +2 to 0, it decreased. When an element's oxidation state decreases, it is considered a reduction, not an oxidation. Therefore, the Iron(II) ion (Fe2+) is reduced, not oxidized, in the given chemical equation.