Notes

• Whats the structure of metals?

  Metals have a lattice of positively-charged metal cations that are surrounded by a “sea” of delocalised, mobile, valence electrons.
• What are the properties of metal?

  1. High boiling and melting point (except Group 1 metals and mercury)
  2. Good conductors of electricity
  3. Good conductor of heat
  4. Malleable and ductile
  5. High densities
• Why do metals have high melting and boiling points?

  • They have strong electrostatic forces of attraction between the lattice metal cations and the sea of delocalised valence electrons holding the giant metallic lattice structure together.
  • Large amount of energy is needed is absorbed to overcome the strong electrostatic forces of attraction.
• Why are metals good conductors of electricity?

  • Mobile valence electrons can migrate freely through the metallic structure.
  • When connected to a circuit, the mobile valence electrons will move towards the positive terminal, hence more electrons are fed into the metal from the negative terminal.
• Why are metals better conductors of heat than other materials?

  • Metals have free, mobile, valence electrons which can migrate freely throughout the metallic structure. When heated, the free, mobile valence electrons at the heated end will increase in kinetic energy. This causes them to collide with other free, mobile, valence electrons and other metal atoms more often. transferring kinetic energy to them. This causes the average temperature in a metallic structure to increase faster.
• Why are metals malleable and ductile?(AKA soft metals)

  • Metal atoms are packed in a regular and orderly manner, allowing layers of atoms to slide over one another easily when a force is applied
• What is malleability?

  The ability to be deformed without breaking
• What is ductility?

  The ability to be stretched into wires, without breaking.
• Why do metals have high densities?

  Metal atoms are closely packed together.
• What is an alloy?

  It is a mixture of a metal with one or more elements
• Why are alloys favoured over pure metals?

  • Pure metals are soft
  • Pure metals corrode as it reacts with oxygen and water in the environment
• Why are alloys not malleable or ductile?

  • Atoms of another element are different in size compared to the pure metal atoms.
  • This disrupts the regular arrangement of the metal atoms and prevents the layer of atoms from sliding over each other easily, when a force is applied.
• What are the properties of alloys?

  • Increased hardness and strength compared to pure metals
  • Improved appearance compared to pure metals
  • Lower melting points compared to pure metals
  • More resistant to corrosion compared to pure metals
• What are 6 types of alloys? What are their constituents? What are their uses?

  .

  
• What makes a metal more reactive than others?

  A more reactive metal more readily loses its valence electron(s) to form a cation.
• List the reactivity series.

  
  

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  Potassium

  Sodium

  Calcium

  Magnesium

  Aluminium

  Carbon

  Zinc

  Iron

  Lead

  Hydrogen

  Copper

  Silver

  Gold
• How do different metals react with cold water, steam and acid? [1]

  Cold water and steam

  
• How do different metals react with cold water, steam and acid? [2]

  Acid

  
• What is a displacement reaction?

  It is a reaction where a more reactive metal will displace a less reactive metal from its salt solution