Redox Reactions

Question 1

Disproportionation

Answer 1

Reaction of a single substance with itself to produce two different substances; a type of redox reaction in which an entity is both oxidized and reduced.

Question 2

Half-reaction

Answer 2

Balanced chemical equation that represents either a loss or a gain of electrons by a substance.

Question 3

Oxidation

Answer 3

Chemical process involving the loss of electrons by an entity; an increase in the oxidation number (becomes more positive)

Question 4

Reduction

Answer 4

A chemical process involving the gain of electrons by an entity; a decrease in oxidation number (becomes more negative)

Question 5

Oxidation Number

Answer 5

A positive or negative number corresponding to the oxidation state assigned to an atom or ion.

Question 6

Oxidizing Agent (OA)

Answer 6

An entity that causes or promotes oxidation through removing electrons from another substance. The oxidation number becomes more negative as electrons are gained.

Question 7

Reducing Agent

Answer 7

An entity that causes reduction by donating (losing) electrons to another substance in a redox reaction. It’s oxidation number becomes more positive as a result.

Question 8

Redox Spontaneity Rule

Answer 8

The generalization: a spontaneous redox reaction occurs only if the oxidizing agent (OA) is above the reducing agent (RA) in a table of relative strengths of oxidizing and reducing agents with reduction potentials.