The oxide which cannot act as a reducing agent is
The oxide which cannot act as a reducing agent is
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Reducing agents are substances that have the capacity to donate electrons, leading to the reduction of another species in a chemical reaction.
- ${NO_2}$
- ${SO_2}$
- ${CO_2}$
- ${ClO_2}$
The Correct Option is C
Approach Solution - 1
The correct answer is Option C) \({CO_2}\)
When a substance loses electrons by increasing its oxidation state, it acts as a reducing agent.
In sulphur dioxide, sulphur has a +4 oxidation state. So, it increases its oxidation state to +6, therefore it acts as a reducing agent.
In Nitrogen Dioxide, nitrogen has a +4 oxidation state. So, it increases its oxidation state to +5, therefore it can also act as a reducing agent.
In carbon dioxide, carbon has the maximum oxidation state of + 4, therefore carbon dioxide \({(CO_2)}\) cannot act as a reducing agent.
In ClO2, chlorine is in a +4 oxidation state, it can increase its oxidation state to +7, therefore it can act as a reducing agent.
Therefore, Option C is the correct answer.
Discover More From Chapter: Redox Reactions
Approach Solution -2
The correct answer is Option C) \({CO_2}\)
Real Life Applications
The real-life application of CO2 includes-
1) Used as a fire extinguisher.
2) CO2 is used in the beverages industry such as in soft drinks and also used to keep them cool.
Question can also be asked as
- What is an Oxidiser? Write some examples of oxidizers.
- Which oxide cannot be oxidized?
- Which oxide has the highest oxidation state?
- Which oxide cannot donate electrons?
- Which oxide is the strongest oxidizing agent?
Approach Solution -3
The correct answer is Option C) \({CO_2}\)
Reducing agents are substances that have the capacity to donate electrons, leading to the reduction of another species in a chemical reaction. In the process, the reducing agent itself is oxidized, losing electrons.
Oxides as Reducing Agents
- Some oxides, particularly those of metals, can act as reducing agents due to their ability to donate electrons.
- These oxides facilitate the reduction of other compounds by providing electrons to the species being reduced.
Sulphur Dioxide (SO2)
- Sulphur dioxide is an oxide composed of sulphur and oxygen, with the chemical formula SO2.
- It is commonly produced through the combustion of sulphur-containing materials, such as fossil fuels.
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Sulphur Dioxide as a Reducing Agent:
- Unlike many other reducing oxides, sulphur dioxide cannot act as a reducing agent.
- This is primarily due to the nature of the sulphur-oxygen bond in SO2.
Stability of Sulphur Dioxide
- The sulphur-oxygen bond in sulphur dioxide is relatively strong, resulting in a stable molecule.
- As a result, sulphur dioxide does not readily donate electrons to other substances, hindering its ability to act as a reducing agent.
Sulphur dioxide, despite being an oxide, cannot act as a reducing agent due to the stability of its sulphur-oxygen bond. While reducing oxides typically donate electrons to facilitate the reduction of other species, sulphur dioxide does not possess this capability. Instead, it exhibits oxidizing properties under certain conditions.
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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.