• Metal?atoms are tightly packed together in?lattice?structures
• When the metal atoms are in?lattice?structures, the electrons in their outer shells are free to move throughout the structure
• The free-moving?electrons?are called?‘delocalised'?electrons?and they are not bound to their atom
• When the electrons are?delocalised, the metal atoms become?positively?charged
• The positive charges?repel?each other and keep the neatly arranged lattice in place
• There are very strong?electrostatic?forces between the positive metal centres and the ‘sea’ of delocalised electrons

The positive metal centres are suspended in a ‘sea’ of delocalised electrons

• Metallic compounds are?malleable
  • When a force is applied, the metal layers can slide
  • The?attractive forces?between the metal ions and electrons act in all directions
  • So when the layers slide, the metallic bonds are re-formed
  • The lattice is not broken and has changed shape

• Metallic compounds are?strong?and?hard
  • Due to the strong attractive forces between the metal ions and delocalised electrons
• Metals have?high melting?and?boiling points

Conductivity

• Metals can?conduct electricity?when in the?solid?or?liquid?state
  • As both in the solid and liquid state there are?mobile electrons?which can freely move around and conduct electricity
• Since the bonding in metals is?non-directional, it does not really matter how the?cations?are oriented relative to each other
• The metal?cations?can be moved around and there will still be delocalised electrons available to hold the?cations?together

Metallic Bonding Summary Table

Not all metallic bonds are equal. There are several factors that affect the?strength?of a metallic bond:

The charge on the metal ion

• The?greater?the charge?on the metal ion, the greater the number of electrons in the sea of delocalised electrons and the greater the?charge difference?between the ions and the electrons
• A greater charge difference leads to a?stronger?electrostatic attraction, and therefore a stronger metallic bond
• This effect can be seen in melting point data across a period, as the charge on the metal ion?increases?without a significant change in ionic radius:

The radius of the metal ion

• Metal ions with?smaller ionic radii?exert a greater attraction on the sea of delocalised electrons
• This greater attraction means a?stronger?metallic bond, requiring more energy to break
• This can be seen in data from metals, descending a group, where the charge on the ion remains constant but the ionic radius increases: