Metals

• Fullerenes

  Carbon atoms joined together to make large hollow Shape (Hexagonal Rings)
• Graphene

  Single layer of graphite, 1 atom thick. Great electrical conductivity.
• 1 mole

  Relative formula mass In grams
• Concentration

  Measured in (g/dm³)
• A more reactive metal

  Will displace a less reactive metal from its aqueous solution
• Metals can be placed in order

  • Of reactivity by their reactions with water & dilute acid
• Oxidation

  Loss of electrons
• Reduction

  Gain of electrons
• Metals more reactive than carbon cannot be extracted from their ores using carbon
• Making salts

  Reacting a suitable metal with an acid
• Salt Compound: formed when hydrogen in acid is wholly or partially replaced by metal or ammonium ions.
• Concentration(g/dm^3) = Mass of solute(g)/Volume of solution(dm^3)
• Group 0


  Noble gases
• Halogens are poisonous
• Diatomic Molecules


  2 atom molecules
• Halogens can be diatomic molecules by sharing electrons
• As you go down halogens


  Melting and boiling point increase but reactivity decreases
• Noble gases


  • Unreactive as they have full outer shells
• Halide salts are colourless
• Bromine water


  • Orange
• Chlorine water


  • Colourless
• Iodine water


  • Brown
• Harder to lose electrons with high amount of electrons on outer shell


  Requires high amount of energy (e.g. Group 7 electrons)
• Easier to lose electrons with low amount of electrons on outer shell


  (e.g. Group 1 electrons)
• All metals


  • Have metallic bonding (very strong)
  • Are great conductors of electricity and heat
  • Are bad conductors
• All non-metals


  • Are brittle and have low melting and boiling points
• Transition metals


  • Can form more than one ion
  • Are very good catalysts
• Group 1 Alkali metals


  • Are soft
  • Have low density
  • Have low melting points
• Alkali metals


  Are more reactive than other metals
• Potassium + oxygen


  Potassium peroxide = K2O2
• As you go down alkali metals

  Reactivity increases and melting points decrease
• The atomic radius increases going down alkali metals (atoms get larger)
• The force of attraction between the nucleus and outer electron


  Decreases
• The electron is lost more easily (requires less energy to move)
• When alkali metals react with water


  Metal hydroxide and hydrogen are formed