Ch 6 Ionic Compounds & Metals and Ch 7 Covalent Bonding

Chemical bond

The force that holds two atoms together; may form by the attraction of a positive ion for a negative ion or by sharing electrons.

Cation

An ion that has a positive charge.

Anion

An ion that has a negative charge.

Ionic bond

The electrostatic force that holds oppositely charged particles together in an ionic compound.

Ionic compound

Compounds that contain ionic bonds.

Crystal lattice

A 3D geometric arrangement of particles in which each positive ion is surrounded by negative ions and each negative ion is surrounded by positive ions.

Electrolyte

An ionic compound whose aqueous solution conducts an electric current.

Lattice energy

The energy required to separate one mole of the ions of an ionic compound, related to the size of the ions and affected by their charge.

Formula unit

The simplest ratio of ions represented in an ionic compound.

Monatomic ion

An ion formed from only one atom.

Polyatomic ion

An ion made up of two or more atoms bonded together that acts as a single unit with a net charge.

Oxyanion

A polyatomic ion composed of an element, usually a nonmetal, bounded to one or more oxygen atoms.

Electron sea model

Proposes that all metal atoms in a metallic solid contribute their valence electrons to form a 'sea' of electrons.

Delocalized electron

The electron in metallic bonding that is free to move easily from one atom to another throughout the metal.

Metallic bond

The attraction of a metallic cation for delocalized electrons.

Alloy

A mixture of elements that has metallic properties.

Covalent bonds

A chemical bond that results from the sharing of valence electrons.

Molecule

Forms when two or more atoms covalently bond and is lower in potential energy than its constituent atoms.

Lewis structure

A model that uses electron-dot structures to show how electrons are arranged in molecules.