Redox Reaction
Definition
Redox reactions involve changes in oxidation states due to transfer of electrons from one molecule or atom to another. They consist of two half-reactions - oxidation (loss of electrons) and reduction (gain of electrons).
Analogy
Think of a redox reaction like a game of hot potato, where the potato is an electron. One molecule passes the "hot potato" to another molecule. The one who throws the potato away (loses an electron) is undergoing oxidation, while the one catching it (gaining an electron) is undergoing reduction.
Related terms
Oxidation: This refers to a process in which a substance loses electrons during a chemical reaction.
Reduction: This refers to a process in which a substance gains electrons during a chemical reaction.
Oxidizing Agent: A substance that causes another substance to be oxidized by accepting its electrons. It's reduced in the process.
"Redox Reaction" appears in:
Study guides (2)
Practice Questions (8)
In the following REDOX reaction, identify the element that is oxidized: Pb(s) + Cl₂(g) → PbCl₂(s)
What is true about the oxidation states in the redox reaction Fe + 2HCl -> FeCl₂ + H₂?
What is true about the redox description in the redox reaction Fe + 2HCl -> FeCl₂ + H₂?
What equation can we use to find the E value for any given redox reaction?
Which of the following is true about the relationship between the standard electrode potential (E°) and the Gibbs free energy change (ΔG°) for a redox reaction?
Faraday’s laws can be used to determine the stoichiometry of the redox reaction occurring in an electrochemical cell with respect to ALL of the following, EXCEPT for:
Faraday’s laws can be used to determine the stoichiometry of the redox reaction occurring in an electrochemical cell with respect to ALL of the following, EXCEPT for:
Faraday’s laws can be used to determine the stoichiometry of the redox reaction occurring in an electrochemical cell with respect to ALL of the following, EXCEPT for:
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