Which of following are reducing and oxidising agent respectively.
Which of following are reducing and oxidising agent respectively.
Eu+2, Ce+4
Ce+3, Ce+4
Eu+4, Eu+2
Tb+2, Ce2+
The Correct Option is A
Solution and Explanation
- Eu2+ (Europium in +2 Oxidation State):
- Eu2+ has a tendency to lose an electron and get oxidised to Eu3+, which is a more stable oxidation state for europium due to the half-filled f-orbital configuration (4f7).
- This tendency to donate electrons makes Eu2+ a reducing agent.
- Ce4+ (Cerium in +4 Oxidation State):
- Ce4+ has a tendency to gain an electron and get reduced to Ce3+, which is a more stable oxidation state for cerium due to its 4f1 configuration.
- This ability to accept electrons makes Ce4+ a strong oxidising agent.
Conclusion:
Eu2+ acts as a reducing agent, while Ce4+ acts as an oxidising agent.
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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.