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Chapter 4: Problem 42

What is the requirement for an element to undergo disproportionation reactions? Name five common elements that are likely to take part in such reactions.

Short Answer

Expert verified
For an element to undergo a disproportionation reaction, it should be able to exist in an intermediate oxidation state and should have stable higher and lower oxidation states to which it can transition during the reaction. Examples of elements that can undergo such reactions include Chlorine, Iodine, Sulfur, Phosphorus, and Hydrogen.

Step by step solution

01

Understanding Disproportionation Reactions

Disproportionation reactions are a special class of redox reactions in which a single element simultaneously undergoes both oxidation and reduction, forming two different products. In essence, for an element to undergo a disproportionation reaction, it should exist in an intermediate oxidation state and should have other stable higher and lower oxidation states to which it can transition.
02

Identifying five elements

Here are five examples of elements that can undergo disproportionation reactions: Chlorine (Cl), Iodine (I), Sulfur (S), Phosphorus (P), and Hydrogen (H). Note that these elements can exist in various oxidation states, making them suitable candidates for disproportionation reactions.

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