Aim: How Do Metal
Atoms Bond in a
Metal?
DO NOW: TAKE A SHEET FROM THE
FRONT AND ANSWER THE QUESTIONS.
Metallic Bonding
 Metallic
bonding consists of the
attraction of the free-floating valence
electrons for the positively charged
metal ions
 Positive metal ions in a sea of electrons.
 Electrons are shared amongst every
metal ion.
Structure of Metals
 The
metal ions are in a fixed position of a
crystal lattice and the electrons are free
to move throughout the lattice.
A crystal lattice describes the periodic
arrays of a solid.
 The bond results from the attraction
between the free moving electrons and
the atom’s positive kernel.
Conductivity of Metals
 Metals
conduct electricity because of
the free moving electrons
Electricity is energy due to the flow of
electrons
Malleability of Metals
 Metals
are malleable
 When a force is applies the metal
kernels move to a new location,
changing the shape of a metal.
Crystalline structures
 Metals
are
arranged in very
compact and
orderly patterns.
 Metal atoms
crystallize in
characteristic
patterns.
Ionic
Compounds are
brittle.
Good conductor
of electricity (in
solution and
when
melted)
Metals are
malleable
High melting
points and boiling
points
Good
conductor of
electricity (solid
and liquid)
Alloys
 Alloys
are mixtures composed of two or
more elements, at least of which is a metal.
 Alloys are usually stronger than their
individual components
Steel: iron and carbon, boron, chromium,
manganese, molybdenum, nickel,
tungsten, vanadium.
http://www.drkstreet.com/resources/metallic-bonding-animation.swf
http://www.ausetute.com.au/metallic.html
The ability to conduct electricity in
a solid state is a characteristic of
metallic bonding. This
characteristic is best explained by
 A.
high ionization energies
 B.
high electronegativities
 C.
mobile electrons
 D.
mobile protons
Which element consists of positive
ions immersed in a “sea” of mobile
electrons?
 A.
sulfur
 B.
nitrogen
 C.
calcium
 D.
chlorine