Oxidation is defined as:
- AOption (a)
loss of protons
- BOption (b)
gain of neutrons
- COption (c)
loss of electrons
- DOption (d)
gain of electrons
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Correct answer
loss of electrons
Why this answer is correct
The correct answer is loss of electrons.
Key Points
- Oxidation is a chemical process where an atom, ion, or molecule loses electrons during a reaction. This results in an increase in oxidation state.
- Oxidation is often paired with reduction, a process where another substance gains electrons. Together, these processes form a redox reaction.
- In terms of electron transfer, oxidation is defined as the loss of electrons, while reduction is the gain of electrons.
- Oxidation does not involve the loss of protons or gain of neutrons; these are unrelated processes. Hence, options "loss of protons" and "gain of neutrons" are incorrect.
- Similarly, oxidation does not involve "gain of electrons"; gaining electrons is characteristic of reduction, not oxidation.
- For example, in the reaction of sodium (Na) with chlorine (Cl2), sodium loses electrons to form Na+, undergoing oxidation, while chlorine gains electrons to form Cl-, undergoing reduction.
Additional Information
- Redox Reactions:
- Redox reactions are chemical reactions that involve the transfer of electrons between two species.
- Oxidation and reduction always occur simultaneously in redox reactions.
- Example: In the reaction 2Fe3+ + 2I- → 2Fe2+ + I2, Fe3+ is reduced to Fe2+, and I- is oxidized to I2.
- Oxidation State:
- The oxidation state (or oxidation number) is a measure of the degree of oxidation of an atom in a substance.
- An increase in oxidation state indicates oxidation, while a decrease indicates reduction.
- Example: In H2O2, oxygen has an oxidation state of -1, while in O2, it has an oxidation state of 0.
- Examples of Oxidation:
- Rusting of iron: Fe + O2 + H2O → Fe2O3·xH2O.
- Combustion of fuels: CH4 + 2O2 → CO2 + 2H2O.
- Oxidation of glucose in cellular respiration: C6H12O6 + 6O2 → 6CO2 + 6H2O.
- Industrial Applications:
- Oxidation reactions are crucial in industries such as metallurgy, where metals are extracted from ores.
- Oxidation is also used in wastewater treatment to remove impurities.
- In the food industry, oxidation reactions are involved in processes like fermentation and food preservation.
Important Points
- Oxidizing Agents:
- An oxidizing agent (or oxidant) is a substance that causes oxidation by accepting electrons.
- Examples include oxygen (O2), hydrogen peroxide (H2O2), and halogens (Cl2, Br2, etc.).
- Reducing Agents:
- A reducing agent (or reductant) is a substance that causes reduction by donating electrons.
- Examples include hydrogen (H2), carbon monoxide (CO), and metals like Na and Zn.
- Electrochemical Cells:
- Oxidation occurs at the anode, and reduction occurs at the cathode in electrochemical cells.
- These cells are widely used in batteries and fuel cells.