Metals (Edexcel GCSE Chemistry)

The link between metallic bonding and the properties of metals

• Metals have high melting and boiling points
  • There are many strong metallic bonds in giant metallic structures
  • A lot of heat energy is needed to overcome forces and break these bonds

• Metals conduct electricity
  • There are free electrons available to move and carry charge
  • Electrons entering one end of the metal cause a delocalised electron to displace itself from the other end
  • Hence electrons can flow so electricity is conducted

• Metals are malleable and ductile
  • Layers of positive ions can slide over one another and take up different positions
  • Metallic bonding is not disrupted as the valence electrons do not belong to any particular metal atom so the delocalised electrons will move with them
  • Metallic bonds are thus not broken and as a result metals are strong but flexible
  • They can be hammered and bent into different shapes without breaking

Summary Table of the Physical Properties of Metals

Metals and non-metals

• The Periodic Table contains over 100 different elements
• They can be divided into two broad types: metals and non-metals
• Most of the elements are metals and a small number of elements display properties of both types. These elements are called metalloids or semi-metals

The metallic character diminishes moving left to right across the Periodic Table

• The typical properties of metals and non-metals can be compared side-by-side:

Comparison Table of Metals and Non-metals