1 / 22

Metals & Metal Compounds

Metals & Metal Compounds. D. Crowley, 2007. Metals & Metal Compounds. To be able to predict the reactions between metals and metal compounds. Reactivity Series. What can you say about the reactivity of metals?

stew
Download Presentation

Metals & Metal Compounds

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 & Metal Compounds D. Crowley, 2007

  2. Metals & Metal Compounds • To be able to predict the reactions between metals and metal compounds

  3. Reactivity Series • What can you say about the reactivity of metals? • Some metals are more reactive than others (remember gold in water is fine, sodium in water is not)! • We can order the reactivity of the metals, from most reactive to least • This is the reactivity series!

  4. Reactivity Series Look at the reactivity series – see if you can come up with a way to remember it… Potassium Sodium Calcium Magnesium Aluminium Zinc Iron Lead (Hydrogen) Copper Silver Gold Platinum Very reactive Fairly reactive Not very reactive Not at all reactive Metals below hydrogen do not react with water or acid – they do not easily tarnish!

  5. Displacement • Some metals are more reactive than others • A displacement reaction is where one metal kicks another out • A more reactive element reacts with a compound and pushes out a less reactive “rival” element

  6. Displacement • E.g. zinc is more reactive than copper – it will react with the copper oxide when heated • The zinc will displace the copper, leaving copper on its own and forming zinc oxide… zinc + copper oxide → zinc oxide + copper Zn + CuO → ZnO + Cu

  7. Displacement • So the more reactive zinc has pushed the copper out, and formed zinc oxide • It’s a bit like a little guy going out with a girl. Everything is fine, until a bigger guy comes along and pushes the little guy away • The big guy gets the girl, the little guy goes home alone… Try the Chem Wars: - http://sycd.co.uk/chemwars In our example, zinc is the big guy, copper the little guy, and the oxide is the girl!

  8. Experiment • To prove the reactivity series, you are going to react a metal and a metal compound together • Firstly you will need a copy of the results sheet…

  9. Results Sheet

  10. Experiment 1 • Get a test tube rack, and 3 test tubes • Fill each test tube up ½ way with copper sulphate • Add a small piece of iron to one • Add a small piece of lead to the second • Add a small piece of magnesium to the third • Has there been a reaction? Look for colour changes on the surface of the metal; colour changes in the solution; bubbles of gas given off; a temperature change • If there was a reaction but a tick in your table; if not put a cross

  11. Experiment 2 • Get a test tube rack, and 3 test tubes • Fill each test tube up ½ way with iron sulphate • Add a small piece of copper to one • Add a small piece of lead to the second • Add a small piece of magnesium to the third • Has there been a reaction? Look for colour changes on the surface of the metal; colour changes in the solution; bubbles of gas given off; a temperature change • If there was a reaction but a tick in your table; if not put a cross

  12. Experiment 3 • Get a test tube rack, and 3 test tubes • Fill each test tube up ½ way with lead nitrate • Add a small piece of copper to one • Add a small piece of iron to the second • Add a small piece of magnesium to the third • Has there been a reaction? Look for colour changes on the surface of the metal; colour changes in the solution; bubbles of gas given off; a temperature change • If there was a reaction but a tick in your table; if not put a cross

  13. Experiment 4 • Get a test tube rack, and 3 test tubes • Fill each test tube up ½ way with magnesium sulphate • Add a small piece of copper to one • Add a small piece of iron to the second • Add a small piece of lead to the third • Has there been a reaction? Look for colour changes on the surface of the metal; colour changes in the solution; bubbles of gas given off; a temperature change • If there was a reaction but a tick in your table; if not put a cross

  14. Reactions • So some metals are more reactive than others – of ours the reactivity series of the metals was: - Magnesium (3 displacements) Iron (2 displacements) Lead (1 displacement) Copper (0 displacements) Magnesium displaces the copper: magnesium + copper oxide → magnesium oxide + copper Iron displaces the copper: iron + copper oxide → iron oxide + copper

  15. Equations - Magnesium The equations for the magnesium was: - copper sulphate + magnesium→ magnesium sulphate + copper (REACTION) iron sulphate + magnesium→ magnesium sulphate + iron (REACTION) lead nitrate + magnesium → magnesium nitrate + lead (REACTION)

  16. Equations - Iron The equations for the lead were: - copper sulphate + iron→ iron sulphate + copper (REACTION) lead nitrate + iron→ iron nitrate + lead (REACTION) magnesium sulphate + iron → magnesium sulphate + iron (NO REACTION)

  17. Equations - Lead The equations for the lead were: - copper sulphate + lead→ lead sulphate + copper (REACTION) iron sulphate + lead→ iron sulphate + lead (NO REACTION) magnesium sulphate + lead → magnesium sulphate + lead (NO REACTION)

  18. Equations - Copper The equations for the lead were: - iron sulphate + copper→ iron sulphate + copper (NO REACTION) lead nitrate + copper→ lead nitrate + copper (NO REACTION) magnesium sulphate + copper → magnesium sulphate + copper (NO REACTION)

  19. Equations - Magnesium The equations for the magnesium was: - copper sulphate + magnesium→ magnesium sulphate + copper CuSO4 + Mg→ MgSO4 + Cu (REACTION) iron sulphate + magnesium→ magnesium sulphate + iron FeSO4 + Mg → MgSO4 + Fe (REACTION) lead nitrate + magnesium → magnesium nitrate + lead Pb(NO3)2 + Mg → Mg(NO3)2 + Pb (REACTION)

  20. Equations - Iron The equations for the lead were: - copper sulphate + iron→ iron sulphate + copper CuSO4 + Fe→ FeSO4 + Cu (REACTION) lead nitrate + iron→ iron nitrate + lead Pb(NO3)2 + Fe → Fe(NO3)2 + Pb (REACTION) magnesium sulphate + iron → magnesium sulphate + iron MgSO4 + Fe → MgSO4 + Fe (NO REACTION)

  21. Equations - Lead The equations for the lead were: - copper sulphate + lead→ lead sulphate + copper CuSO4 + Pb→ PbSO4 + Cu (REACTION) iron sulphate + lead→ iron sulphate + lead FeSO4 + Pb → FeSO4 + Pb (NO REACTION) magnesium sulphate + lead → magnesium sulphate + lead MgSO4 + Pb → MgSO4 + Pb (NO REACTION)

  22. Equations - Copper The equations for the lead were: - iron sulphate + copper→ iron sulphate + copper FeSO4 + Cu→ FeSO4 + Cu (NO REACTION) lead nitrate + copper→ lead nitrate + copper Pb(NO3)2 + Cu → FeSO4 + Cu (NO REACTION) magnesium sulphate + copper → magnesium sulphate + copper MgSO4 + Cu → MgSO4 + Cu (NO REACTION)

More Related