Final answer:
Oxidation: 4Al(s)
Reduction: 3O₂
Spectator Ions: None
Step-by-step explanation:
In this chemical equation, 4 moles of aluminum (Al) react with 3 moles of oxygen (O₂) to form 2 moles of aluminum oxide (Al₂O₃). To identify the substance oxidized and reduced, we look at the change in oxidation states. Aluminum starts as elemental Al with an oxidation state of 0 and ends up in the compound Al₂O₃ with an oxidation state of +3. This indicates that aluminum is oxidized, losing electrons. Oxygen starts as O₂ with an oxidation state of 0 and ends in the compound Al₂O₃ with an oxidation state of -2. Therefore, oxygen is reduced, gaining electrons.
The balanced equation shows that all the aluminum atoms are involved in the reaction (4Al(s)), making it the substance oxidized. On the other hand, the oxygen molecules (3O₂) are fully consumed in the formation of aluminum oxide, making them the substance reduced. There are no spectator ions in this reaction because all the species (Al and O₂) involved are participating in the chemical change, with none remaining unchanged or in excess after the reaction.
The reaction between aluminum and oxygen results in the transfer of electrons, leading to the formation of aluminum oxide. This process illustrates the principles of oxidation and reduction, where aluminum loses electrons (oxidation) and oxygen gains electrons (reduction) to form the final product, Al₂O₃.