Metallic bonding

• What is the structure of metal atoms in metallic bonding?

  They are tightly packed in lattice structures
• What happens to the electrons in metal atoms when they form lattice structures?

  Electrons in outer shells move freely
• What are the free-moving electrons in metallic bonding called?

  Delocalised electrons
• What occurs to metal atoms when their electrons are delocalised?

  They become positively charged ions
• Why do positive charges in metallic bonding keep the lattice structure in place?

  They repel each other, maintaining arrangement
• What type of forces exist between positive metal centres and delocalised electrons?

  Very strong forces
• How do delocalised electrons contribute to the properties of metals?

  They allow conductivity and malleability
• What is the definition of metallic bonding?

  The electrostatic attraction between positively charged metal cations and the ‘sea’ of delocalised mobile electrons between them.
• What are some of the properties of metals?

  They are excellent conductors

  They have a high melting point
• Why are metals excellent conductors?

  They have delocalised electrons which can travel throughout the structure and carry a charge.
• Why do metals have a high melting point?

  They have strong metallic bonds as a result of the strong attraction between metal cations and electrons.
• What are some of the properties of pure metals?

  They are malleable and ductile because they ions are arranged in layers which can slide over one another.
• What does malleable mean?

  The material can be hammered into shape.
• What is the definition of ductile?

  The material can be drawn into a wire.
• What does the strength of metals depend upon?

  The charge of the ion

  The size of the ion
• How does the charge of the ion affect the strength of the metal?

  The greater the charge of the ion, the greater number of delocalised electron and the stronger the electrostatic attraction between cations and electrons.
• How does the size of the ion affect the strength of metals?

  The smaller the ion, the closer electrons are to the positive nucleus and the stronger the bond.
• How does the size of an atom change across a period?

  The atoms become smaller as the number of shielding stays the same and there’s an increasing number of protons pulling the shells in closer, making he atoms smaller.