Bonding ❮ 165(d) PCl 5 must ionize. There are several acceptable equations, all of which must indicate the
formation of ions. Here are two choices:2 PCl 5 PCl 4 + + PCl 6 - or PCl 5 PCl 4 + + Cl-You get 1 point for the explanation and 1 point for either of the equations.
Total your points. There are 10 points possible.❯ Rapid Review
● Compounds are pure substances that have a fixed proportion of elements.
● Metals react with nonmetals to form ionic bonds, and nonmetals react with other non-
metals to form covalent bonds.
● The Lewis electron-dot structure is a way of representing an element and its valence
electrons.
● Atoms tend to lose, gain, or share electrons to achieve the same electronic configuration
as (become isoelectronic to) the nearest noble gas.
● Atoms are generally most stable when they have a complete octet (eight electrons).
● Ionic bonds result when a metal loses electrons to form cations and a nonmetal gains
those electrons to form an anion.
● Ionic bonds can also result from the interaction of polyatomic ions.
● The attraction of the opposite charges (anions and cations) forms the ionic bond.
● The crisscross rule can help determine the formula of an ionic compound.
● In covalent bonding two atoms share one or more electron pairs.
● If the electrons are shared equally, the bond is a nonpolar covalent bond, but unequal
sharing results in a polar covalent bond.
● The element that will have the greatest attraction for a bonding pair of electrons is
related to its electronegativity.
● Electronegativity values increase from left to right on the periodic table and decrease
from top to bottom.
● The N – A = S rule can be used to help draw the Lewis structure of a molecule.
● Molecular geometry, the arrangement of atoms in three-dimensional space, can be
predicted using the VSEPR theory. This theory says the electron pairs around a central
atom will try to get as far as possible from each other to minimize the repulsive forces.
● In using the VSEPR theory, first determine the electron-group geometry, then the
molecular geometry.
● The valence bond theory describes covalent bonding as the overlap of atomic orbitals to
form a new kind of orbital, a hybrid orbital.