Ionisation

• Blocks

  • S-block : Group 1 and 2
  • P-block : Group 3 to 0
  • D-block : transition metals
  • F-block : radioactive elements
• Atomic radius


  Along a period, atomic radius decreases , due to an increased nuclear charge for the same number of electron shells.
• Outer electrons are pulled in closer to the nucleus as the increased charge produces a greater attraction causing atomic radius to be reduced.
• Ionisation energy

  The energy needed to remove an electron from from an atom or an ion in the gaseous state

  X(g)--X+1(g) + e-
• Along a period, ionisation energy increases because of the increasing nuclear charge and decreasing atomic size.

  • Outer shell held more strongly.
  • More energy required to remove outer electron.
• Down a group, ionisation energy decreases because of the increasing atomic size.

  • Increasing amount of shielding.
  • Nuclear attraction decreases.