Redox Review 1.1 and 1.2

Vocabulary flashcards covering the basics of redox reactions, oxidation number rules, and identifying agents from the lecture notes.

Redox

A type of chemical reaction in which reduction and oxidation happen simultaneously in one reaction.

Oxidation

The loss of electrons; originally meant reacting with oxygen.

Reduction

The gain of electrons; originally described turning a metal ore into pure metal and reducing its mass.

LEO

An acronym standing for "Loss of Electrons = Oxidation."

GER

An acronym standing for "Gain of Electrons = Reduction."

Electronegativity

An atom's ability to attract or compete for electrons with other atoms it is bonded to.

Oxidation Number Rule 1 (Elements)

The oxidation number for an element by itself is $0$.

Oxidation Number Rule 2 (Monatomic Ion)

The oxidation number of a monatomic ion is equal to its charge.

Oxidation Number Rule 3 (Hydrogen)

Hydrogen is always $+1$ when it is in a compound.

Oxidation Number Rule 4 (Oxygen)

Oxygen is always $-2$ when it is in a compound.

Oxidation Number Rule 5 (Compound Sum)

The sum of oxidation numbers in a compound is $0$.

Oxidation Number Rule 6 (Polyatomic Ion Sum)

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

Reducing Agent

The substance that is oxidized in a reaction, located on the reactant side.

Oxidizing Agent

The substance that is reduced in a reaction, located on the reactant side.

Increase in Oxidation Number

Indicates that the element loses electrons.

Decrease in Oxidation Number

Indicates that the element gains electrons.