1 / 33

METALS AND ACIDS

METALS AND ACIDS. METALS AND ACIDS. Metals Magnesium Iron Sodium Calcium. METALS AND ACIDS. Metals Magnesium Iron Sodium Calcium. Acids Hydrochloric acid Sulphuric acid Nitric acid Ethanoic acid. METALS AND ACIDS. Metals Magnesium Iron Sodium Calcium. Acids

annagomez
Download Presentation

METALS AND ACIDS

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. METALS AND ACIDS

  2. METALS AND ACIDS Metals Magnesium Iron Sodium Calcium

  3. METALS AND ACIDS Metals Magnesium Iron Sodium Calcium Acids Hydrochloric acid Sulphuric acid Nitric acid Ethanoic acid

  4. METALS AND ACIDS Metals Magnesium Iron Sodium Calcium Acids Hydrochloric acid Sulphuric acid Nitric acid Ethanoic acid Metal + Acid  Salt + Hydrogen

  5. FORMING SALTS

  6. FORMING SALTS

  7. FORMING SALTS

  8. FORMING SALTS

  9. FORMING SALTS

  10. FORMING SALTS

  11. FORMING SALTS

  12. FORMING SALTS

  13. FORMING SALTS

  14. FORMING SALTS

  15. DISPLACEMENT REACTIONS

  16. DISPLACEMENT REACTIONS • Instructions • Care! You should wear GOGGLES and LAB-COATS at all times during this practical • Obtain a dropping tile • Add a few drops of each of the solutions to individual ‘holes’ in the dropping tile. Make sure you know which solution is which • Choose a metal • Add one piece of that metal to each of the solutions • Observe – you will need to watch carefully for any evidence of a reaction taking place • If a reaction takes place, put a tick into the relevant box. If no reaction takes place, put a cross. • If a reaction takes place, try and describe what is happening • Wash all the reactions into a large beaker – do NOT put any solids into the sink! • Repeat for each metal using fresh solutions

  17. DISPLACEMENT REACTIONS

  18. DISPLACEMENT REACTIONS

  19. DISPLACEMENT REACTIONS

  20. DISPLACEMENT REACTIONS

  21. DISPLACEMENT REACTIONS

  22. DISPLACEMENT REACTIONS

  23. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions

  24. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate 

  25. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate  magnesium nitrate + iron

  26. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate  magnesium nitrate + iron magnesium is more reactive than iron

  27. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate  magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate 

  28. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate  magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate  lead (II) sulphate + copper

  29. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate  magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate  lead (II) sulphate + copper lead is more reactive than copper

  30. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate  magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate  lead (II) sulphate + copper lead is more reactive than copper but copper + lead (II) sulphate 

  31. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate  magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate  lead (II) sulphate + copper lead is more reactive than copper but copper + lead (II) sulphate  no reaction

  32. DISPLACEMENT REACTIONS Summary More reactive metals can displace less reactive metals from their solutions e.g. magnesium + iron (II) nitrate  magnesium nitrate + iron magnesium is more reactive than iron and lead + copper (II) sulphate  lead (II) sulphate + copper lead is more reactive than copper but copper + lead (II) sulphate  no reaction copperis not more reactive than lead

  33. This powerpoint was kindly donated to www.worldofteaching.com http://www.worldofteaching.com is home to over a thousand powerpoints submitted by teachers. This is a completely free site and requires no registration. Please visit and I hope it will help in your teaching.

More Related