• Like


Flash Player 9 (or above) is needed to view presentations.
We have detected that you do not have it on your computer. To install it, go here.

2p9 metals and acids 101110

Uploaded on

Metals and acids: S2

Metals and acids: S2

  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
    Be the first to comment
    Be the first to like this
No Downloads


Total Views
On Slideshare
From Embeds
Number of Embeds



Embeds 0

No embeds

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

    No notes for slide


  • 1. Reactions of Metals and Acids 2P9: Wednesday 10/11/10
  • 2. Metals + Water: A quick review
    • Complete the following word equation:
      • Metal + Water 
    • Are the ‘reactants’ on the left or right of this equation?
    • Are the ‘products’ on the left or right of this equation?
    • How do we test for Hydrogen gas?
    • Complete the following word equation:
      • ______ + Water  Magnesium Hydroxide + _____
    • List the metals in order of decreasing reactivity:
      • Magnesium, Calcium, Potassium, Sodium
      • Potassium > Sodium > Calcium > Magnesium
    • Why are Potassium and Sodium stored in oil?
    Metal Hydroxide + Hydrogen
  • 3. Reactions of Metals with Acids
    • Aim: Observe what happens when metals are added to an acid
    • You will need:
      • Test tube rack
      • 4 test tubes
      • Metals: Magnesium, Zinc, Copper
      • Acids: Hydrochloric acid, Sulphuric acid
      • Heat proof mat, Bunsen burner, splint
      • Safety glasses
  • 4. Experimental Method
    • Place test tube in rack and add 10cm 3 1M Hydrochloric acid
    • Add a small piece of Magnesium – immediately place clean test tube (inverted) over the reaction test tube to capture any gas given off
    • Once fizzing stops, test gas with a lit splint
    • Feel the bottom of the reaction test tube to see if the reaction mixture has become hot
    • Repeat all of the above steps using Zinc and Copper
    • Once you have tested all 3 metals with Hydrochloric acid, repeat all three experiments using Sulphuric acid
    • Record your observations in a suitable table
    • When you have completed your experiment, draw a labelled diagram of your apparatus, detail your method and complete your table of results
  • 5. Experimental Results: Metals + Acid Metal Acid Observations Gas given off – test with lit splint Magnesium Hydrochloric acid Fizzing, test tube heats up Hydrogen gas Zinc Hydrochloric acid Few bubbles around surface of metal Hydrogen gas Copper Hydrochloric acid No reaction No gas Magnesium Sulphuric acid Fizzing, test tube heats up Hydrogen gas Zinc Sulphuric acid Slightly more bubbles around the surface of metal Hydrogen gas Copper Sulphuric acid No reaction No gas
  • 6. Conclusions
    • Metals react with an acid to produce a chemical called a salt . Hydrogen gas is also produced in this reaction.
    • General equation for a metal reacting with an acid is:
      • Metal + Acid  Salt + Hydrogen
  • 7. Naming Salts
    • Salts have a first name and a last name:
    • First Name – comes from the metal
    • Last Name – comes from the acid
    • Acid name Salt produced
    • Hydrochloric acid chloride
    • Sulphuric acid sulphate
    • Nitric acid nitrate
  • 8. Examples of Salts
    • From our experiments, the reactions which worked were:
    • Magnesium + Hydrochloric acid 
    • Zinc + Hydrochloric acid 
    • Magnesium + Sulphuric acid 
    • Zinc + Sulphuric acid 
    Magnesium Chloride + Hydrogen Zinc Sulphate + Hydrogen Magnesium Sulphate + Hydrogen Zinc Chloride + Hydrogen
  • 9. Updating our reactivity series
    • Copper metal did not react with either Hydrochloric acid or Sulphuric acid. Copper is therefore not as reactive as Magnesium or Zinc.
    • We can add these metals to our reactivity series:
    • Potassium Most reactive
    • Sodium
    • Calcium
    • Magnesium
    • Zinc
    • Copper Least reactive