Denniston, 7e
Glossary of Key Terms in Chapter Three
angular structure (3.4) planar molecule with bond angles less than 180 o.
boiling point (3.3) the temperature at which the vapor pressure of a liquid is equal to the atmospheric
pressure.
bond energy (3.4) the amount of energy necessary to break a chemical bond.
chemical bond (3.1) the attractive force holding two atomic nuclei together in a chemical compound.
covalent bond (3.1) a pair of electrons shared between two atoms.
crystal lattice (3.1) a unit of a solid characterized by a regular arrangement of components.
dissociation (3.3) production of positive and negative ions when an ionic compound dissolves in water.
double bond (3.4) a bond in which two pairs of electrons are shared by two atoms.
electrolyte (3.3) a material that dissolves in water to produce a solution that conducts an electrical current.
electrolytic solution (3.3) a solvent composed of an electrolytic solute dissolved in water.
electronegativity (3.1) a measure of the tendency of an atom in a molecule to attract shared electrons.
formula (3.2) the representation of the fundamental compound unit using chemical symbols and numerical
subscripts.
intermolecular force (3.5) attractive force that occurs between molecules.
intramolecular force (3.5) attractive force that occurs within molecules.
ionic bonding (3.1) an electrostatic attractive force between ions resulting from electron transfer.
ion pair (3.1) the simplest formula unit for an ionic compound.
isomers (3.4) molecules having the same molecular formula but different chemical structures.
Lewis structure (3.1) representation of a molecule (or polyatomic ion) that shows valence electron
arrangement among the atoms in a molecule (or polyatomic ion).
Lewis symbol (3.1) representation of an atom or ion using the atomic symbol (for the nucleus and core
electrons) and dots to represent valence electrons.
linear structure (3.4) the structure of a molecule in which the bond angle(s) about the central atom(s) is
(are) 180o.
lone pair (3.4) an electron pair that is not involved in bonding.
melting point (3.3) the temperature at which a solid converts to a liquid.
molecule (3.1) a collection of two or more atoms held together by covalent bonds.
monatomic ion (3.2) an ion formed by electron gain or loss from a single atom.
nomenclature (3.2) a system for naming chemical compounds.
nonelectrolyte (3.3) a substance that, when dissolved in water, produces a solution that does not conduct
an electrical current.
polar covalent bonding (3.4) a covalent bond in which the electrons are not equally shared.
polar covalent molecule (3.4) a molecule that has permanent electric dipole moment resulting from an
unsymmetrical electron distribution; a dipolar molecule.
polyatomic ion (3.2) an ion containing a number of atoms.
resonance (3.4) a condition that occurs when more than one valid Lewis structure can be written for a
particular molecule.
resonance form (3.4) one of a number of valid Lewis structures for a particular molecule.
resonance hybrid (3.4) a description of bonding in a molecule resulting from a superimposition of all valid
Lewis structures (resonance forms).
single bond (3.4) a bond in which one pair of electrons is shared by two atoms.
solubility (3.5) the amount of a substance that will dissolve in a given volume of solvent at a specified
temperature.
tetrahedral structure (3.4) a molecule consisting of four groups attached to a central atom which occupy
the four corners of an imagined tetrahedron.
trigonal pyramidal molecule (3.4) a molecular structure resulting from three groups bonded to a central
atom; all groups are equidistant from the central atom.
triple bond (3.4) a bond in which three pairs of electrons are shared by two atoms.
valence shell electron pair repulsion theory (3.4) a model that predicts molecular geometry using the
premise that electron pairs will arrange themselves as far apart as possible, to minimize electron
repulsion.