IB Chemistry Unit 6.1-6.4

Ionic Bonding

Attraction between cations and anions formed by electron transfer from a metal to a nonmetal.

Cation

A positively charged ion that is formed when an atom loses electrons.

Anion

A negatively charged ion that is formed when an atom gains electrons.

Empirical Formula

The simplest whole number ratio of atoms in a compound.

Crystal Lattice Structure

A three-dimensional arrangement of ions in a solid ionic compound.

Lattice Energy

The energy required to separate one mole of an ionic solid into its gaseous ions.

Volatility

The tendency of a substance to evaporate; ionic compounds have low volatility due to strong ionic bonds.

Electrical Conductivity

The ability of a substance to conduct electricity; ionic compounds conduct when dissolved in water or molten.

Solubility

The ability of a substance to dissolve in a solvent; influenced by lattice energy, temperature, and solute-solvent interactions.

Roman Numeral in Naming

Indicates the charge of a transition metal in a compound's name.

Polyatomic Ion

A charged ion composed of two or more atoms.

Alloy

A mixture of metals or a mixture of metals and nonmetals.

Electron Sea Model

A model describing metallic bonding where electrons are delocalized and shared among many atoms.

Ductile

The ability of a metal to be drawn into a wire.

Malleable

The ability of a metal to be shaped into different forms without breaking.

Strength of Metallic Bond

Dependent on the charge of the cation, number of delocalized electrons, and radius of the cation.

Substitutional Alloy

An alloy where atoms of one metal replace atoms in another metal's crystal lattice.

Interstitial Alloy

An alloy formed when smaller atoms fit into the spaces between larger metal atoms.