Why is the formation of iron hydroxide, Fe(OH)2, from Fe2+ and OH- not considered an oxidation-reduction reaction?

Because there is no change in the Fe2+. It is Fe2+ as the ion and Fe2+ in the hydroxide.

The formation of iron hydroxide, Fe(OH)2, from Fe2+ and OH- is not considered as an oxidation-reduction reaction because there is no change in the oxidation state of the iron ion (Fe2+) during the reaction. In an oxidation-reduction reaction, the oxidation state of at least one of the reacting species will change.

In this case, Fe2+ has an oxidation state of +2, and it remains the same in the product (Fe(OH)2). The hydroxide ion, OH-, also remains unchanged with an oxidation state of -1 throughout the reaction. Since there is no change in oxidation states, the reaction does not involve the transfer of electrons, which is a characteristic of oxidation-reduction reactions.

The formation of iron hydroxide, Fe(OH)2, from Fe2+ and OH- is not considered an oxidation-reduction reaction because there is no change in the oxidation state of the iron (Fe) ion during the reaction.

In an oxidation-reduction (redox) reaction, there is a transfer of electrons between species, resulting in a change in oxidation states. The species that loses electrons is oxidized, while the species that gains electrons is reduced.

In the case of Fe(OH)2 formation, Fe2+ ions (with an oxidation state of +2) react with OH- ions to form Fe(OH)2. The oxidation state of Fe remains at +2 before and after the reaction. There is no transfer of electrons, and hence, no change in oxidation states. Therefore, this reaction is not classified as an oxidation-reduction (redox) reaction.