Reduction Half-Reaction: MnO4-(aq) → Mn2+(aq)
Oxidation Half-Reaction: Cl-(aq) → Cl2(g)
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Reduction half-reaction: MnO4–(aq) + 8H+(aq) + 5e– → Mn2+(aq) + 4H2O(l) Oxidation half-reaction: Cl–(aq) → Cl2(g) + 2e–
The oxidation state of an element with oxidation state 0 cannot change, as it already has a balance of electrons.
An element that decreases its oxidation number in a chemical reaction is undergoing reduction. In the given reaction, the element that is reduced is the one that gains electrons and decreases its oxidation number.
Iron (Fe) undergoes oxidation when it loses electrons to form Fe2+ ions. This process involves the loss of electrons by iron atoms to form Fe2+ ions, which have a 2+ charge. The iron atoms are oxidized from an oxidation state of 0 to an oxidation state of +2 when they lose electrons.
Oxidation and reduction are two processes that occur simultaneously in chemical reactions. Oxidation involves the loss of electrons, while reduction involves the gain of electrons. Each reaction involves both oxidation and reduction, with one substance being oxidized (losing electrons) while another is reduced (gaining electrons).
The loss of electrons is called oxidation because it involves the increase in oxidation state of an atom or molecule. Oxidation is characterized by the loss of electrons from a substance, leading to an increase in positive charge or a decrease in negative charge.