Which of the following is not true for oxidation?
- addition of oxygen
- addition of electronegative element
- removal of hydrogen
- removal of electronegative element
The Correct Option is D
Solution and Explanation
To determine which option is not true for oxidation, let's first understand what oxidation means in chemistry. Oxidation is a chemical process that involves:
- Addition of oxygen to a substance.
- Loss of hydrogen from a substance.
- Addition of an electronegative element to a substance.
- Loss of electrons from a substance, also referred to as an increase in oxidation state.
Now, let's evaluate each of the given options based on the above understanding:
- Addition of oxygen: This is a classic interpretation of oxidation. It involves oxygen being added to a substance.
- Addition of an electronegative element: Oxidation often involves gaining elements like chlorine, which are electronegative.
- Removal of hydrogen: This is another classic definition of oxidation. Removing hydrogen aligns with the oxidation of organic compounds.
- Removal of an electronegative element: This does not align with the definition of oxidation. Instead, it typically describes a reduction process, which involves gaining or adding an electronegative element.
Based on this evaluation, the statement that is not true for oxidation is the removal of an electronegative element, as this is contrary to how oxidation processes work.
Thus, the correct answer is: removal of electronegative element
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Concepts Used:
Redox Reactions
Redox Reaction:
Redox reactions are chemical reactions where oxidation and reduction take place simultaneously. In this type of reaction, there is a gain of electrons for one chemical species while the other loses electrons or simply involves transfer of electrons. The species that loses electrons is oxidized while the one that gains electrons is reduced.
Types of Redox Reactions:
Redox reactions can be differentiated into 4 categories namely combination reactions, decomposition reactions, displacement reactions, and disproportionation reactions. Each is explained separately below:
Combination Reaction:
In this, the molecules combine to form new compounds. For example, when magnesium reacts to nitrogen.
Decomposition Reaction:
Opposite to the combination reaction, here there is a breakdown of compounds to simpler substances. For example, electrolysis of water.
Displacement Reaction:
In this, the more reactive metal will displace the less reactive one in a chemical reaction. The reactivity of an element is represented in a series called the reactivity series (arranged in decreasing order of reactivity) which makes it easier to determine the chemical reaction and its products.
Disproportionation Reaction:
This is a peculiar type of reaction where an element showing a particular oxidation state will be oxidized and reduced simultaneously. Another thing to note is that these reactions will always have an element that can exhibit three oxidation states.