Paper 1

• Metals (+ions)

  • Metallic bonding
  • Malleable
  • Conducts heat and electricity
  • High melting and boiling point
• Non-metals (-ions)

  • Brittle
  • Dull
  • Low melting and boiling point
  • Lower density
• Alkali (group 1) metals

  • Melting and boiling points decrease
  • Have only 1 electron in outer shell
  • Since they can lose the electron easily they almost always form ionic compounds with non metals
• Ionic compounds


  A metal donates an electron to a non metal so they both have full outer shells, since they are oppositely charged ions they will be attracted to each other by an ionic bond (electrostatic force of attraction)

  • really strong
  • Conduct electricity if melted
  • Dissolve in water forming colorless solutions
• Alkali metals+water ->


  metal hydroxide+hydrogen gas
• Alkali metals+oxygen->


  Metal oxides/peroxides
• Halogens (group 7) - dangerous 


  • Very reactive
  • Melting and boiling points increase and reactivity decrease as you go down
  • More reactive halogens always displace less reactive ones in a reaction
• Ion


  • charged particle
  • Formed when atoms gain or lose electrons which requires energy
• Covalent bonds (sharing electrons)

  • Non metals
  • Make simple molecular substances
  • Make larger substances like polymers
• Simple molecular substances(water)

  • Don't conduct electricity
  • Low temp to melt or boil
• Giant covalent structures

  • A lot of non metal atoms
  • Repeating lattices
  • Very strong
  • High melting and boiling point
  • Don't conduct electricity (except graphite)
• Allotrope


  Different forms of the same element
• Graphite

  • Soft, high melting point
  • Conduct electricity and heat because it has 1 delocalized electrons which carry charge and is free to move
• Alloys


  Mixing together 2 different elements
• Particles - Solid 


  • Strong forces of attraction
  • Fixed position
  • Definite shape or volume
  • Vibrate
• Particles - liquid


  • Weak forces of attraction
  • Free to move
  • Definite volume
  • Shape can change
• Particles - Gas


  • very weak forces of attraction
  • Free to move
  • Random motion
  • No definite shape or volume
• Relative Atomic Mass (Ar)


  Sum of (abundance×mass)÷(all abundance)
• Relative formula mass (Mr)


  Add together the relative Atomic masses (Ar) of all the atoms in the compound
• % Mass


  (Ar of desired element×number of elements atoms)÷Mr of compound

  ×100