Redox Reactions Overview

A chemical reaction where atoms change their oxidation states. Oxidation is the loss of electrons, and reduction is the gain of electrons.

The process where an atom or molecule loses electrons.

The process where an atom or molecule gains electrons.

The substance that causes oxidation by gaining electrons. This is the substance that itself undergoes reduction.

The substance that causes reduction by losing electrons. This is the substance that itself undergoes oxidation.

The process where a substance loses electrons and its oxidation state increases.

The process where a substance gains electrons and its oxidation state decreases.

Breaking down a redox reaction into separate parts, one showing the oxidation and the other showing the reduction.

The sum of the oxidation numbers of all atoms in a polyatomic ion must equal the overall charge of the ion.

In a neutral molecule, the sum of oxidation numbers for all atoms is zero.

The oxidation number of an element when it's in its pure, elemental form is always zero.

Oxidation is the process where an atom or molecule loses electrons and its oxidation number increases.

Reduction is the process where an atom or molecule gains electrons and its oxidation number decreases.

A substance that causes oxidation by gaining electrons. It itself undergoes reduction.

A substance that causes reduction by losing electrons. It itself undergoes oxidation.

A chemical reaction involving the transfer of electrons, where one substance is oxidized (loses electrons) and another is reduced (gains electrons).

Breaking down a redox reaction into separate reactions, one showing oxidation and the other showing reduction.

The process of determining the oxidation number of each element in a compound or ion.

A method used for balancing redox reactions, based on the change in oxidation numbers of the elements involved.

The first step in balancing a redox reaction using the oxidation number method, where the reactants and products are written without any balancing coefficients.

The second step in balancing a redox reaction where the oxidation numbers of all elements in the unbalanced equation are assigned.

The third step in the oxidation number method, where you identify which elements are undergoing oxidation (increasing oxidation number) and reduction (decreasing oxidation number).

The fourth step in the oxidation number method, where the oxidation and reduction processes are written as separate equations, showing the changes in oxidation numbers and the movement of electrons.

The movement of electrons between atoms or molecules during a chemical reaction involving the change in oxidation states.

The charge of an atom in a compound, which changes due to electron gain or loss during a redox reaction.

A reaction in which atoms change their oxidation states, one atom losing electrons (oxidation) and another atom gaining electrons (reduction).

A part of a redox reaction that showcases either the oxidation or the reduction process separately, focused on the movement of electrons.

This shows the substance losing electrons, getting oxidized. It's one part of a redox reaction.

This shows the substance gaining electrons, getting reduced. It's one part of a redox reaction.

This number represents the charge an atom would have if the compound was composed of ions. Helps understand electron distribution.

In a neutral compound, the total sum of the oxidation numbers of all the atoms must always add up to zero.

For an element in its pure form, like O₂, N₂, or H₂, the oxidation number of each atom is zero.

A monoatomic ion (an ion made up of a single atom) has an oxidation number equal to its charge.

Oxygen typically has an oxidation number of -2, except in peroxides (where it's -1) or when bonded to fluorine.

Hydrogen usually has an oxidation number of +1, except when combined with metals in hydrides (where it's -1).

Fluorine, being the most electronegative element, always has an oxidation number of -1 in compounds.