Describe how oxidation and reduction involve electrons, change oxidation numbers, and combine in oxidation-reduction reactions.
Question: Describe how oxidation and reduction involve electrons, change oxidation numbers, and combine in oxidation-reduction reactions.
Oxidation and reduction are fundamental chemical processes involving the transfer of electrons and changes in oxidation numbers within oxidation-reduction (redox) reactions.
1. Electron Transfer
Oxidation occurs when an atom, ion, or molecule loses electrons, increasing its oxidation number.
Reduction occurs when an atom, ion, or molecule gains electrons, decreasing its oxidation number.
For example, in the reaction:
Zn
+
Cu
2
+
→
Zn
2
+
+
Cu
Zinc (Zn) loses electrons (oxidized to Zn²⁺).
Copper ion (Cu²⁺) gains electrons (reduced to Cu metal).
2. Changes in Oxidation Numbers
Each element's oxidation number reflects its electron state:
Oxidation increases oxidation number.
Reduction decreases oxidation number.
In the example above:
Zn goes from 0 to +2 (oxidation).
Cu goes from +2 to 0 (reduction).
3. Combination in Redox Reactions
Oxidation and reduction always occur together in redox reactions.
The substance that loses electrons (oxidized) is the reducing agent.
The substance that gains electrons (reduced) is the oxidizing agent.
These reactions are essential in processes like cellular respiration, corrosion, battery function, and industrial chemical production.
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