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 statement is not true for oxidation, let's understand the concept of oxidation in chemistry:
- Addition of Oxygen: Oxidation is commonly associated with the addition of oxygen to a substance. This is a traditional definition of oxidation in terms of oxygen transfer. For example, in the formation of magnesium oxide from magnesium and oxygen, magnesium is oxidized.
- Addition of Electronegative Element: Oxidation also involves the addition of any electronegative element, not just oxygen. For example, chlorine can be added to iron to form iron chloride, which is an oxidation process.
- Removal of Hydrogen: Oxidation can also occur by the removal of hydrogen from a compound. For example, in the conversion of ethanol to acetaldehyde, hydrogen is removed from ethanol, indicating an oxidation process.
- Removal of Electronegative Element: Removal of an electronegative element would typically represent a reduction, not oxidation. Therefore, this statement does not describe a process of oxidation.
Given this explanation, the statement that does not accurately describe oxidation is the "removal of electronegative element." This contradicts the general process of oxidation, making it the correct answer to the question.
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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.