Group 2

• Magnesium + steam -> magnesium oxide + hydrogen
• solubility of group 2 hydroxides increases down the group
• First ionisation energy decreases down the group 2 metals because:

  1. number of filled electron shells increases down the group
  2. → increased shielding, increased atomic radius
  3. → weaker force between outer electron and nucleus
  4. → less energy needed to remove electron
• Amphoteric: substance can act as a base or acid
• Group 2 trends:

  Atomic radius down the group

  melting points decrease as charge density decreases

  first ionisation energy decreases

  reactivity increases
• solubility of group 2 sulphates decrease down the group