Redox reactiosn

Redox Reaction

A process in which electrons are transferred from one species to another.

Reducing Agent

The species that donates electrons and is said to be oxidized.

Oxidizing Agent

The species that gains electrons and is said to be reduced.

OIL RIG

A mnemonic for remembering that Oxidation Is Loss and Reduction Is Gain.

Oxidation

Loss of electrons or an increase in oxidation number.

Reduction

Gain of electrons or a decrease in oxidation number.

Metal-metal ion displacement

A redox reaction where electrons transfer from a more reactive metal to less reactive metal ions.

Halogen-halide ion displacement

A redox reaction where a halogen becomes reduced and halide ions of a less reactive halogen are oxidized.

Combustion

A redox reaction involving the oxidation of fuel and reduction of oxygen gas.

Corrosion

A redox process where a metal is oxidized and oxygen gas is reduced.

Half Equations

Expressions that show the separate oxidation and reduction processes in a redox reaction.

Oxidation Numbers

Numerical values assigned to atoms to track electron exchange in redox reactions.

Oxidation states of elements

All substances in their elemental state have an oxidation number of 0.

Monoatomic ions

These have oxidation numbers equal to the charge of their ion (e.g., Fe3+ = +3).

Combined Oxygen

In most compounds, oxygen has an oxidation number of -2.

Combined Hydrogen

In most compounds, hydrogen has an oxidation number of +1.

Polyatomic Ions

The sum of oxidation numbers in a polyatomic ion equals the charge of the ion.

Balancing redox equations

The process of adjusting the coefficients to balance both mass and charge in redox reactions.

Oxidizing agent

A substance that causes another substance to be oxidized, itself being reduced.

Reducing agent

A substance that causes another substance to be reduced, itself being oxidized.