Introduction to Electrochemistry and Oxidation States

These flashcards cover key concepts related to electrochemistry, oxidation states, and rules for determining oxidation in chemical compounds.

Electrochemistry

The study of the interchange of chemical and electrical energies.

Oxidation State

The charge of an atom or ion, assuming it has gained or lost the maximum number of electrons based on electronegativity.

Redox Reaction

A chemical reaction involving the transfer of electrons, where oxidation and reduction occur.

Electronegativity

A measure of the tendency of an atom to attract a bonding pair of electrons.

Electrolytic Process

A method involving electrochemical processes to drive chemical reactions.

Oxidation

The process of losing electrons or increasing oxidation state.

Reduction

The process of gaining electrons or decreasing oxidation state.

Sum of Oxidation States

In a molecule or ion, the sum of oxidation states must equal the overall charge.

Monatomic Ion Oxidation State

The oxidation state of a monatomic ion is equal to its charge.

Fluorine Rule

Fluorine always has an oxidation state of -1 in compounds.

Oxygen Rule

Oxygen typically has an oxidation state of -2, except in peroxides where it is -1.

Hydrogen Rule

Hydrogen usually has an oxidation state of +1, with exceptions when combined with certain metals.