C4.1.2 - Reactivity Series

• What determines the Reactivity of a metal?

  How tightly the metal holds on to the electrons in its outer most shell.
• Why do displacement reactions occur?

  A more reactive metal takes the place of a less reactive metal within a compound.
• Metal Reactions with Water

  Reaction with water:

  metals above hydrogen react with water - produce bubble of hydrogen gas

  e.g. Ca + 2H2O → Ca(OH)2 + H2

  calcium + water → calcium hydroxide + hydrogen

  
• Metal Reactions with dilute acids

  Reaction with dilute acids:

  All metals above hydrogen (reactivity series) will react with acids - producing bubbles of hydrogen gas.

  more reactive the metal = more vigorous reaction; producing hydrogen gas quicker.

  metals below hydrogen (reactivity series) don't react with acids

  general formula - MASH - Metal + Acid > Salt + Hydrogen

  e.g. Fe + 2HCI → FeCl2 + H2

  • iron + hydrochloric acid → iron(II)chloride + hydrogen

  
• Reactivity Series

  • Potassium – most reactive, so most easily forms positive ions
  • Sodium
  • Lithium
  • Calcium
  • Magnesium
  • Aluminium
  • Carbon
  • Zinc
  • Iron
  • Lead
  • Hydrogen
  • Copper – least reactive, so difficulty forming positive ions
  • Silver
  • Gold
  • Platinum