HCH031: Redox Reactions and Oxidation Numbers

Flashcards covering key concepts and vocabulary related to redox reactions, oxidation numbers, and IUPAC naming from the lecture notes.

Oxidation-Reduction (redox) reactions

Reactions involving the transfer of electrons from one substance to another.

Oxidation

The process of gaining oxygen or losing hydrogen in a reaction.

Reduction

The process of losing oxygen or gaining hydrogen in a reaction.

Oxidation number (ON)

A value that describes the degree to which an element has been oxidized or reduced.

Oxidizing agent

The reactant that is reduced during a redox reaction.

Reducing agent

The reactant that is oxidized during a redox reaction.

IUPAC naming

The system of naming chemical compounds using rules established by the International Union of Pure and Applied Chemistry.

Fe2+

Iron in the +2 oxidation state, commonly known as Iron (II).

Fe3+

Iron in the +3 oxidation state, commonly known as Iron (III).

Hydrogen in metal hydrides

Has an oxidation number of -1.

Colors of salts for Fe2+ and Fe3+

Fe2+ forms pale green salts, while Fe3+ forms orange-red/brown salts.

Rules for oxidation numbers

Systematic guidelines to determine oxidation states of elements in compounds or ions.

Common oxidizing agents

Substances that gain electrons in redox reactions, often including elements like O2 and Cl2.

Common reducing agents

Substances that lose electrons in redox reactions, such as metals like Mg and Zn.

Electrons transfer

Key characteristic of redox reactions that denotes the interchange of electrons between reactants.