Oxidation-Reduction Lecture Notes

These flashcards cover key concepts and definitions related to oxidation-reduction chemistry.

Oxidation Number

The charge assigned to an atom in a molecule, representing the number of electrons that an atom can gain or lose.

Diatomic Elements

Elements that naturally exist as pairs of atoms; for example, O2 (Oxygen), Cl2 (Chlorine), and H2 (Hydrogen).

Oxidation

A process where an atom or molecule loses electrons, resulting in an increase in its oxidation number.

Reduction

A process where an atom or molecule gains electrons, resulting in a decrease in its oxidation number.

Reducing Agent

A substance that donates electrons and is oxidized in a chemical reaction, causing another substance to be reduced.

Oxidizing Agent

A substance that accepts electrons and is reduced in a chemical reaction, causing another substance to be oxidized.

Redox Reaction

A reaction that involves the transfer of electrons between two substances, encompassing both oxidation and reduction.

Charge of Oxygen

In most compounds, oxygen typically has an oxidation number of -2.

Rule for Atoms with No Charge

An atom with no charge has an oxidation number of zero.

Identifying Oxidized and Reduced Species

To find which species is oxidized or reduced, compare the changes in oxidation numbers.