1. Metallic Bonds A Closer Look

2. 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.

3. Metallic Bonds (continued) The free roaming, ‘sea of electrons’ are what gives metals their properties.  Electrical conductivity ~ e - are passed along  Thermal conductivity ~ e - movement & atomic vibrations are passed along  Luster ~ e - absorb and reradiate EM energy  Malleability ~ nucleus to e - attractions are not specific so they can be shifted.  Ductility ~ same as malleability

4. 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 nature  Down and left are more metallic in nature

5. 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.