Metallic Bonds

A Closer Look

Metallic Bonds Are formed when metallic atoms overlap the

orbitals of loosely held valence electrons. Metallic bonds are similar to a covalent

bonds except that the atoms don’t care who possesses the electrons. As long as there are enough electrons around they are free to roam.This is referred to as the ‘sea of electrons’

model.

Metallic Bonds(continued) The free roaming, ‘sea of electrons’ are

what gives metals their properties.Electrical conductivity ~ e- are passed alongThermal conductivity ~ e- movement & atomic

vibrations are passed alongLuster ~ e- absorb and reradiate EM energyMalleability ~ nucleus to e- attractions are not

specific so they can be shifted.Ductility ~ same as malleability

Metallic Bond Character

Metals hold their electrons loosely, this results in lower ionization energies.

As you move right and up the atoms hold their electrons more tightly resulting in higher ionization energies.Up and right are less metallic in natureDown and left are more metallic in nature

Metallic Bond Strength

The strength of a metallic bond is affected by the number of free roaming electrons and the nuclear charge of the bonding metals.Many free roaming electrons will lead to more

attractive forces stronger metallic bonds. Increased nuclear charge will lead to more

attractive forces stronger metallic bonds.