1. Ch. 6 Bonding
6.4 Metallic Bonding

2. Bonding of Metals
the highest energy level for most metal atoms does not contain many electrons
usually have empty p and d block
these vacant overlapping orbitals allow outer electrons to roam freely around the entire metal
the electrons are delocalized – are not with one specific atom

3. Bonding of Metals these roaming electrons form a sea of electrons
around the metal atoms
metal atoms are packed in a crystal lattice
metallic bonding – bonding that results from the attraction between metals atoms and sea of electrons

4. Properties of Metals conductivity luster (shininess)
from the freedom of electrons to move around the atoms
luster (shininess)
contain many orbitals with only small differences in energy
many amounts of energy can be absorbed and emitted

5. Properties of Metals malleability and ductility
bonding is the same in every direction
one layer of atoms can slide past another without friction

6. Bond Strength
depends on the nuclear charge (Z) or the number of protons
depends on the number of electrons in the “sea”
heat of sublimination – amount of heat required to turn solid, bonded metal atoms into gaseous individual atoms

7. Metallic vs. Ionic