Name: ____________________________
Bonding Overview
Date: ______________
About 450 BC, the Greek philosopher Democritus proposed that all matter was
composed of tiny, indivisible particles. Unfortunately, Aristotle and other well-known
Greek philosophers did not agree with Democritus’ idea. If matter is composed of such
particles, they argued, then what holds these particles together? Why does matter not
fall apart the way sand castles fall apart in wind? Democritus could not answer such
questions, and so his ideas about atoms were rejected.
The simple answer to this question is that BONDS between particles hold matter
together. BONDS are the forces of attraction (the glue) that hold atoms (or ions, or
molecules) together. Since ELECTRONS (specifically valence electrons) comprise the
boundaries of atoms, ions and molecules, it should come as no surprise that the
attractive forces between particles is the result of the motions and positions of
electrons.
Electron arrangement (configuration) around the atom can be classified in two
categories.
1. ATOMS WITH FEW VALENCE ELECTRONS (1, 2, 3 and occasionally 4
valence electrons). These atoms are classified as METALS.
2. ATOMS WITH MANY VALENCE ELECTRONS (4, 5, 6, 7 or 8 valence
electrons). These atoms are classified as NONMETALS.
Two classifications of atoms create 3 possibilities for bonding.
METALLIC BONDS
 Metal atoms
bonded with
metal atoms
 Produces a
metallic solid
(of a pure metal
or a metal alloy)
 Held together
by metallic
bonds
IONIC BONDS
 Metal atoms
bonded with
nonmetal
atoms
 Produces an
ionic
compound
 Held together
by ionic bonds
COVALENT BONDS
 Nonmetals
bonded with
nonmetal
atoms
 Produces a
molecular
compound
 Held together
by covalent
and
intermolecular
bonds
An organizing principle in all bonding is the OCTET RULE. The OCTET RULE states that
when involved in bonding, atoms tend to gain, lose or share electrons in order to
acquire a full set of valence electrons (8 electrons).
Exceptions are Hydrogen and Helium.
Name: ____________________________
Bonding Overview
Date: ______________
CHARACTERISTICS OF SUBSTANCES
Metallic Bonds
Types of Elements
(metals/nonmetals/metalloids)
How are bonds formed?
(electron-related)
Types of Particles Present
(what is a single unit called?)
Phase of Matter
at Room Temperature
(solid/liquid/gas)
Melting and Boiling Point
Temperatures
(high/low)
Brittle or Malleable
(shatters or dents)
Electrical Conductivity (s)
(high/low)
Electrical Conductivity (l)
(high/low) – melted
Solubility in Water
(does it dissolve easily?)
Electrical Conductivity (aq)
(high/low)
Ionic Bonds
Covalent Bonds