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, which is directly related to the size of the ions bonded and is also affected by the charge of the ions.

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 and can explain properties of metallic solids such as malleability, conduction, and ductility.

Delocalized electron
The electron involved in metallic bonding that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom.

Metallic bond
The attraction of a metallic cation for delocalized electrons.

Alloy
A mixture of elements that has metallic properties; most commonly forms when the elements are either similar in size or the atoms of one element are much smaller than the atoms of the other.

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. Pairs of dots or lines represent bonding pairs.