The oxidation process creates a change in the oxidation state of a substance, leading to a loss of electrons.
Understanding Oxidation
Oxidation, at its core, is a chemical reaction where a substance loses electrons. This loss of electrons invariably results in an increase in the oxidation state (or oxidation number) of the substance. Thinking about what oxidation "creates" requires understanding its consequences:
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Change in Oxidation State: This is the most fundamental creation of oxidation. An element or compound undergoing oxidation will have a higher oxidation state after the reaction than before.
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Loss of Electrons: While not a physical "creation," oxidation results in the release of electrons from the oxidized species. These electrons must be accepted by another species in a reduction reaction (hence, redox reactions).
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New Chemical Compounds: Depending on the substance being oxidized and the environment, oxidation can create completely new chemical compounds. For example:
- Rust: Iron oxidizes to form iron oxide (rust).
- Oxides of Metals: Many metals react with oxygen to form metal oxides.
- Combustion Products: Burning fuels (oxidation of hydrocarbons) creates carbon dioxide, water, and other products.
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Energy (in some cases): While not a "creation" in the same sense as a chemical compound, many oxidation reactions release energy in the form of heat and/or light. Combustion reactions are a prime example.
Examples of Oxidation
| Process | Reactants | Products (What is "created") |
|---|---|---|
| Rusting | Iron (Fe), Oxygen (O2), Water (H2O) | Iron Oxide (Fe2O3 ·nH2O) - Rust |
| Burning Methane | Methane (CH4), Oxygen (O2) | Carbon Dioxide (CO2), Water (H2O), Heat and Light |
| Tarnish of Silver | Silver (Ag), Sulfur (S) | Silver Sulfide (Ag2S) - Tarnish |
In summary, the oxidation process creates a change in the oxidation state, results in a loss of electrons, and can lead to the formation of new chemical compounds, and in some cases, the release of energy.
