Indicate whether each of the following statements is true or false: (c) If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction.

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Understand the definition of a redox reaction: A redox (reduction-oxidation) reaction involves the transfer of electrons between two species, resulting in changes in their oxidation states.

Identify the key characteristic of a redox reaction: The oxidation state of at least one element must change during the reaction.

Analyze the given statement: It claims that if there are no changes in oxidation states, the reaction is not a redox reaction.

Evaluate the statement based on the definition: Since a redox reaction requires a change in oxidation states, if there are no changes, it cannot be a redox reaction.

Conclude the truth value of the statement: The statement is true because the absence of changes in oxidation states means the reaction is not a redox reaction.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Oxidation and Reduction

Oxidation and reduction (redox) reactions involve the transfer of electrons between substances. Oxidation refers to the loss of electrons, resulting in an increase in oxidation state, while reduction refers to the gain of electrons, leading to a decrease in oxidation state. Understanding these processes is crucial for identifying redox reactions.

Oxidation States

Oxidation states (or numbers) are assigned to atoms in a compound to indicate their degree of oxidation. These states help track electron transfer during chemical reactions. A change in oxidation state signifies that a redox reaction has occurred, while no change indicates that the reaction is not a redox process.

Redox Reaction Criteria

For a reaction to be classified as a redox reaction, there must be a change in oxidation states of the reactants and products. If all oxidation states remain constant throughout the reaction, it is not a redox reaction. This criterion is essential for distinguishing redox reactions from other types of chemical reactions.

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Textbook Question

(b) On which side of an oxidation half-reaction do the electrons appear?

Textbook Question

Indicate whether each of the following statements is true or false: (a) If something is oxidized, it is formally losing electrons.

Textbook Question

Indicate whether each of the following statements is true or false: (c) An oxidizing agent is needed to convert CO into CO₂.

Textbook Question

For each of the following balanced oxidation–reduction reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total number of electrons transferred in each reaction. (a) I₂O₅(s) + 5 CO(g) → I₂(s) + 5 CO₂(g) (b) 2 Hg²⁺(aq) + N₂H₄(aq) → 2 Hg(l) + N₂(g) + 4 H⁺(aq) (c) 3 H₂S(aq) + 2 H⁺(aq) + 2 NO₃^-(aq) → 3 S(s) + 2 NO(g) + 4 H₂O(l)

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Textbook Question

For each of the following balanced oxidation–reduction reactions, (i) identify the oxidation numbers for all the elements in the reactants and products and (ii) state the total number of electrons transferred in each reaction. (a) 2 MnO₄^-(aq) + 3 S^2-(aq + 4 H₂O(l) → 3 S(s) + 2 MnO₂(s) + 8 OH^-(aq) (b) 4 H₂O₂(aq) + Cl₂O₇(g) + 2 OH^-(aq) → 2 ClO₂^-(aq) + 5 H₂O(l) + 4 O₂(g) (c) Ba²⁺(aq) + 2 OH^-(aq) + H₂O₂(aq) + 2 ClO₂(aq) → Ba(ClO₂)₂(s) + 2 H₂O(l) + O₂(g)

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