Metallic

• What is the structure of pure metals?

  Tightly-packed layers forming a regular lattice
• What does it mean for electrons to be delocalised?

  They are free to move through the structure
• What happens to the outer electrons of metal atoms?

  They separate and create a sea of electrons
• What is a metallic bond?

  Electrostatic force of attraction between a sea of delocalised electrons and positive metal
• Why do metals have high melting and boiling points?

  Strong forces of attraction between electrons and ions meaning it needs a lot of energy to break it
• What makes metals good conductors of heat and electricity?

  Presence of free electrons carries heat and electricity energy
• How do free electrons contribute to conductivity?

  They carry heat and electrical energy
• What does it mean for metals to be malleable?

  They can be hammered into sheets
• What does it mean for metals to be ductile?

  They can be drawn into wires
• What are the general properties of metals?

  • Good heat conductors
  • Good electricity conductors
  • High melting point
  • High boiling point
  • Malleable
  • Ductile
• Why are pure metals malleable?

  Because the metals ions are layed out in rows making them able to slide over each other and move easily
• What is an alloy?

  A mixture of metals an or other elements
• Example of an alloy

  Rose gold , Stainless steel, Bronze
• Why are alloys stronger than pure metals?

  Because they have a distorted structure of different atoms they are unable to slide over each other like in a pure metal.
• Alloy


  What structure is this?