reactivity

• 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 metals against
• How do we determine the reactivity of metals?

  By reacting them with acid or water
• What happens when potassium reacts with hydrochloric acid?

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

  Reactivity decreases as you go down
• What is observed when magnesium reacts with acid?

  It produces lots of bubbles
• How can we measure the reactivity of metals?

  By measuring temperature changes during reactions
• What must be ensured for a fair test when comparing metals?

  Same mass and surface area of samples
• 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?

  • A list of metals arranged by reactivity
  • Most reactive: Group 1 metals
  • Less reactive: Group 2 metals
  • Least reactive: Transition metals
• What are the key points 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
• What are the products of metal reactions with acids and water?

  • Acids: Salt and hydrogen gas
  • Water: Metal hydroxides and hydrogen
• What factors affect the reactivity of metals?

  • Electron arrangement
  • Ability to lose outer shell electrons
  • Comparison with other metals
• What is the rate of reaction?

  Speed at which reactants turn into products
• How does the rate of reaction change over time?

  Starts quick, then slows as reactants are used
• What is collision theory?

  Particles must collide with enough energy to react
• How does energy affect the rate of reaction according to collision theory?

  More energy leads to more frequent successful collisions
• What effect does temperature have on the rate of reaction?

  Higher temperature increases particle movement
• Why does increased concentration or pressure affect the rate of reaction?

  More particles lead to more frequent collisions
• How does surface area influence the rate of reaction?

  More surface area allows for more collisions
• What role does a catalyst play in a chemical reaction?

  Speeds up reaction by lowering activation energy
• Does a catalyst get used up in a reaction?

  No, it is not used in the reaction
• What are the factors affecting the rate of chemical reactions?

  • Temperature
  • Concentration/Pressure
  • Surface Area
  • Catalyst
• ion


  charged particle