Redox Reactions and Ionic Equations

This flashcard set covers key vocabulary concepts related to redox reactions and ionic equations.

Oxidation State

The hypothetical charge of an atom in a molecule, used to track electron transfer.

Reducing Agent

A substance that loses electrons in a redox reaction and is oxidized.

Oxidizing Agent

A substance that gains electrons in a redox reaction and is reduced.

Half Equation

An equation that shows either oxidation or reduction occurring separately in a redox reaction.

Redox Reaction

A chemical reaction involving the transfer of electrons from one substance to another.

Zn2+

The ion formed when zinc loses two electrons.

Cu2+

The ion formed when copper gains two electrons.

Ionic Equation

An equation that shows the particles that participate in a reaction, excluding spectator ions.

Electrons (ē)

Subatomic particles with a negative charge, involved in chemical bonding and reactions.

KMnO4

Potassium permanganate, a strong oxidizing agent in redox reactions.

Ca + AgNO3 -> Ca(NO3)2 + Ag

A reaction where calcium displaces silver from silver nitrate, illustrating a single displacement redox reaction.

Mg + ZnCl2 -> MgCl2 + Zn

An example of a redox reaction where magnesium displaces zinc from zinc chloride.

Oxidation

The process of losing electrons, resulting in an increase in oxidation state.

Reduction

The process of gaining electrons, resulting in a decrease in oxidation state.

Iron (II) Ion (Fe²+)

The oxidation state of iron when it has lost two electrons.

Copper Sulfate Solution (CuSO4)

A common solution used in redox reactions involving copper.

Crystal Violet

A dye that can participate in redox reactions, although not mentioned explicitly in the notes.