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Key Terms and Definitions:

Bond Energy:  the energy needed to break a bond

Ionic Bonding: electrostatic attractions of closely packed, oppositely charged ions

Ionic Compound: a compound that results when a metal reacts with a nonmetal

Covalent Bonding: A chemical bond formed by the sharing of one or more electrons, especially pairs of electrons, between atoms

Electrolytes: compounds which when dissolved in water produce solutions that conduct an electric current

Nonelectrolytes: compounds which when dissolved in water produce solutions that do not conduct an electric current.

Coulomb’s Law: law used to calculate the energy in forming the ion-pair. It says that the energy of interaction of two ions is directly proportional to the product of their electrical charges and is inversely proportional to the distance between their centers.

Bond Length: the average distance between nuclei of two bonded atoms in a molecule; distance where energy is minimal

Electronegativity:  the ability of an atom in a molecule to attract shared electrons to itself

Lattice Energy: the change in energy that takes place when separated gaseous ions are packed together to form an ionic solid; energy released when an ionic solid forms from its ions

Crystal Lattice: A geometric arrangement of the points in space at which the atoms, molecules, or ions of a crystal occur

Single Bond: bond in which one pair of electrons is shared

Double Bond: bond in which two pair of electrons is shared

Triple Bond: bond in which three pair of electrons is shared

Anion: a negatively charged ion

Cation: a positively charged ion

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