Answer:
Explanation:
Oxidation:
Oxidation refers to the process where electrons are lost, resulting in an increase in the oxidation state of an atom of an element.
Reduction:
Reduction is characterized by the acquisition of electrons, leading to a decrease in the oxidation number.
Oxidizing agents:
Oxidizing agents facilitate oxidation of other substances while they themselves undergo reduction.
Reducing agents:
Reducing agents cause the other element to be reduced, while they are oxidized in the process.
Examine the following reaction:
2AgCl + Zn → 2Ag + ZnCl₂
In this instance, the oxidation state of Zn on the left is 0 and rises to +2 on the right, indicating it is oxidized, while the oxidation state of Ag drops from +1 on the left to 0 on the right, showing it is reduced.
4NH₃ + 3O₂ → 2N₂ + 6H₂O
For this reaction, nitrogen's oxidation state shifts from -3 on the left to 0 on the right, signifying it is oxidized, whereas oxygen decreases from 0 to -2, indicating it gets reduced.
Fe₂O₃ + 2Al → Al₂O₃ + 2Fe
Here, the oxidation state of iron reduces from +3 on the left to 0 on the right, meaning it is reduced, while aluminum shifts from 0 to +3, indicating it is oxidized.
