Introduction to Redox Reactions and Oxidation Numbers

Vocabulary flashcards covering fundamental definitions, oxidation state rules, disproportionation, and the metal activity series from Chapter 1 to Chapter 7.

Oxidation

The loss of electrons, an increase in oxidation number, or an atom becoming more positive.

Reduction

The gain of electrons, a decrease in oxidation number, or an atom becoming less positive.

Oxidizing Agent

A substance that oxidizes another substance and itself gets reduced during a redox reaction.

Reducing Agent

A substance that reduces another substance and itself gets oxidized during a redox reaction.

Elemental State Oxidation Number

An oxidation number of $0$ assigned to any atom in its elemental state, with no exceptions.

Monatomic Ion Oxidation State

An oxidation state that is identical to the full charge of the monatomic ion, written as a plus or minus sign followed by a number.

Fluorine Oxidation State in Compounds

An oxidation state of $-1$ in all compound forms, with no exceptions.

Hydrogen Oxidation State Rules

An oxidation state of $+1$ in most molecular compounds, which changes to $-1$ when bonded to a metal.

Oxygen Oxidation State Exceptions

Compounds such as peroxides and superoxides where oxygen does not adopt its typical $-2$ oxidation state.

Disproportionation

A reaction in which a single element starting at one oxidation state undergoes both oxidation and reduction simultaneously.

Activity Series for Metals

A relative ranking of metal reactivity where elements higher on the series are most easily oxidized and serve as strong reducing agents.

Noble Metals

Unreactive metals positioned at the bottom of the activity series that will not react with water or acids.