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.

1. Assign oxidation numbers. 2. Write half-reactions. 3. Balance elements (except O and H). 4. Balance O with H₂O. 5. Balance H with H⁺. 6. Balance charge with e⁻. 7. Combine half-reactions.

1. Balance as in acidic solution. 2. Neutralize H⁺ with OH⁻ to form H₂O. 3. Add the same amount of OH⁻ to the other side. 4. Simplify by canceling H₂O molecules.

1. Assign oxidation numbers. 2. Write half-reactions. 3. Balance elements (except O and H). 4. Balance oxygen atoms by adding H₂O molecules.

5. Balance hydrogen atoms by adding H⁺ ions. 6. Balance the charge by adding electrons. 7. Combine the half-reactions, canceling out any common species.

8. For basic solutions: Neutralize H⁺ ions with OH⁻ to form H₂O, and add the same number of OH⁻ to the other side. 9. Double-check that atoms and charges are balanced.