Atomic structure & periodic table C1

• properties of metal

  • Strong and hard to break
  • can be malleable as they can be hammered into different shapes
  • conduct heat and electricity
  • have metallic bonding causing them to have similar basic physical properties
  • high melting and boiling points
• properties of non-metals

  • dull looking
  • more brittle
  • Aren’t always solids at room temperature
  • don’t generally conduct electricity
  • Don’t have metallic bonding
  • lower density
• alkali metals group 1 properties

  • 1 electron in outer shell
  • soft and low density
  • as you go down the group, the reactivity increases since its easier to lose an electron - the most reactive is at the bottom of the group
  • as you go down the group, there are lower melting and boiling points
• halogens group 7 properties

  • as you go down the group, they become less reactive since its harder to gain and electron - the most reactive is at the top
  • as you go down the group, they have higher melting and boiling points
  • as you go down, they have a higher relative atomic mass
  • 7 outer electrons and react in similar ways
• noble gases group 0 properties

  • as you go down the group, their boiling points increase
  • colourless gases at room temperature
  • they are inert and don't react, so they're non-flammable
  • have 8 outer electrons - have a full shell so they are stable
  • as you go down the group relative atomic mass increases
• why do noble gases increase down the group in boiling point?

  the increase in boiling point down the group is due to the number of electrons in each atoms leading to greater intermolecular forces between them that need to be overcome
• fluorine


  a very reactive, poisonous yellow gas
• chlorine


  a fairly reactive, poisonous dense green gas
• bromine 


  a dense, poisonous red-brown volatile liquid
• iodine


  a dark grey crystalline solid or purple vapour
• lithium reaction with oxygen


  lithium oxide - Li2O
• sodium reaction with oxygen


  a mixture of sodium oxide (Na2O) snd sodium peroxide (Na2O2)
• potassium reaction with oxygen


  a mixture of potassium peroxide (K2O2) and potassium superoxide (KO2)