A reaction involving the transfer of electrons between atoms, leading to changes in oxidation states.

An atom's charge in a compound, showing how many electrons it has gained or lost compared to its neutral state.

The loss of electrons by an atom, resulting in an increase in its oxidation number.

The gain of electrons by an atom, resulting in a decrease in its oxidation number.

A representation showing either the oxidation or reduction process separately, including electrons.

Oxidation: Loss of electrons, oxidation number increases. Reduction: Gain of electrons, oxidation number decreases.

Acidic: Balance using H⁺ ions. Basic: Balance as in acidic, then neutralize H⁺ with OH⁻ to form water.

Oxidation: Oxidation number increases. Reduction: Oxidation number decreases.

Oxidation: Electrons are lost. Reduction: Electrons are gained.

Oxidizing agent: Accepts electrons, gets reduced. Reducing agent: Donates electrons, gets oxidized.

The atom undergoes oxidation, and its oxidation number increases.

The atom undergoes reduction, and its oxidation number decreases.

Water ($H_2O$) is formed, and you must add the same amount of $OH^−$ to the other side of the equation to maintain balance.

The overall equation will not be balanced, leading to incorrect stoichiometric coefficients and an inaccurate representation of the reaction.

$Cr_2O_7^{2−}$ is reduced to $Cr^{3+}$, and $I^−$ is oxidized to $I_2$.