Reactivity Series of Metals & Displacement Reactions

• What is the focus of today's video?

  The reactivity series of metals
• How do metals react with acids?

  They form a salt and hydrogen gas
• What do metals have in common regarding their electron arrangement?

  They have outer shell electrons to lose
• What does the reactivity of a metal indicate?

  How easily it forms positive ions
• Which group of metals is the most reactive?

  Group 1 metals
• Why are carbon and hydrogen included in the reactivity series?

  As references to compare the metals
• What happens when potassium reacts with hydrochloric acid?

  It forms potassium chloride and hydrogen
• How does the reactivity change down the reactivity series?

  Reactions become less violent
• What is observed when magnesium reacts with acid?

  It produces lots of bubbles
• What is necessary for a fair test when comparing metals?

  Same mass and surface area of metals
• What do metals form when they react with water?

  Metal hydroxides and hydrogen
• Which metals do not react with water?

  Zinc, iron, and copper
• What happens when magnesium is placed in iron sulfate solution?

  Magnesium displaces iron to form magnesium sulfate
• What occurs when copper is added to iron sulfate solution?

  Nothing happens because copper is less reactive
• What is the reactivity series of metals?

  • Arrangement of metals by reactivity
  • Most reactive: Group 1 metals
  • Less reactive: Group 2 metals
  • Least reactive: Transition metals
  • Includes carbon and hydrogen for comparison
• How do you determine the reactivity of metals?

  1. React metals with acids or water
  2. Observe reaction speed and violence
  3. Measure temperature change
  4. Ensure fair testing conditions
• What are the outcomes of displacement reactions?

  • More reactive metals displace less reactive ones
  • Example: Magnesium displaces iron in iron sulfate
  • Example: Copper does not displace iron in iron sulfate