Redox Reactions Overview

These flashcards cover key terms and concepts related to redox reactions, including definitions, rules for assigning oxidation states, and the roles of oxidizing and reducing agents.

Redox Reaction

A chemical reaction involving the transfer of electrons between two species.

Oxidation

The process in which a chemical species loses electrons.

Reduction

The process in which a chemical species gains electrons.

Oxidizing Agent

The substance that helps something else get oxidized and becomes reduced in the process.

Reducing Agent

The substance that helps something else get reduced and becomes oxidized in the process.

Oxidation State Rule 1

An atom in its elemental state has an oxidation number of 0.

Oxidation State Rule 2

An atom in a monatomic ion has an oxidation number equal to its charge.

Hydrogen Oxidation State

Hydrogen is usually +1, except in metal hydrides where it is -1.

Oxygen Oxidation State

Oxygen is usually -2, except in peroxides where it is -1.

Fluorine Oxidation State

Fluorine is always -1 in compounds.

Sum of Oxidation Numbers

The sum of oxidation numbers is 0 for a neutral compound and equals the net charge for a polyatomic ion.