1. Chemical reaction

2. Chemistry How do we know a chemical reaction has taken place?

3. Chemistry How do we know a chemical reaction has taken place?

4. Chemistry How do we know a chemical reaction has taken place?

5. Chemistry How do we know a chemical reaction has taken place?

6. we know a chemical reaction has taken place if we observe: -Colour change precipitate (solid is formed) -gas or gases are produced -change in mass -light is given out -change in temperature (cold or hot)

7. Review cover lesson Starter. match CH 4 NaCl C 6 H 12 O 6 Extension-name them. METHANEGLUCOSETABLE SALT

8. Some info. You will be tested on this topic G Tuesday 12.05.15 You will not be tested on topics K and L until the June exam. June exam info is all on my web.

9. Practical-Follow the power point first then complete the practical. Saftey Remember clear desks HOT things look like COLD things…if your not sure DO NOT touch it!

10. EXPLAINING CHEMICAL REACTIONS 1. WHY DO SOME REACTIONS GIVE OUT HEAT ? E.g. the chemical reaction between iron and sulfur. IRON + SULFUR IRON SULFIDE

11. First we have to add some heat to break the bonds between the reactants IRON + SULFUR

12. When the new bonds are made we get back energy IRON SULFIDE

13. EXPLAINING CHEMICAL REACTIONS 1. WHY DO SOME REACTIONS GIVE UT HEAT ? IRON + SULFUR IRON SULFIDE

14. Iron sulfide Atoms in compounds made of a metal and a non-metal do not form simple molecules like FeS FeFe FeFe S S

15. Iron sulfide They form LATTICES a regular arrangement of atoms in the RATIO of 1:1 (one Fe for every 1 S)

16. Practical-Follow the power point first then complete the practical. Saftey Remember clear desks HOT things look like COLD things…if your not sure DO NOT touch it!

17. Addition reaction-Iron sulfide FeS(fools gold) 1.State 3 properties of iron 2.State 3 properties of sulfur 3.Does the mixture or iron and sulfur have these same properties? 4.How could you separate a mixture or iron and sulfur? 5.Now put 1 spatula of the iron and sulfur mixture into an ignition tube, place mineral wool in the top of the tube. 6.Using test tube holder heat in the hottest part of a Bunsen flame (top of the inner cone) POINT AWAY from people when you heat. 7.After 1 min take out of the flame and note any observations. 8.Heat for a further 5 mins then place on a heat proof matt. 9.Move on to the other practical's whilst the tube cools down. 10.Describe the iron sulfide you have made 11.Does it have any of the properties of the iron or the sulfur? 12.How could you tell a chemical reaction had taken place? 13.Why did the mixture glow when you removed it from the heat after 1 min ? 14.What is wrong with this diagram of iron sulfide 15.Correct the diagram. FeFe FeFe S S

18. Decomposition reaction-Copper carbonate Decomposition means to break apart. These involve splitting up substances so we usually need to ADD heat to break the bonds between the reactants. Metal carbonates can be heated to produce a metal oxide and carbon dioxide. e.g. MgCO 3 MgO + CO 2

19. Decomposition reaction-Copper carbonate Metal carbonates can be heated to produce a metal oxide and carbon dioxide. e.g. MgCO 3 MgO + CO 2 Reactant Product

20. Decomposition reaction-Copper carbonate We can test for the product carbon dioxide by bubbling the gas through lime water. A positive test will turn the lime water cloudy. e.g. MgCO 3 MgO + CO 2 Lime water turns cloudy or milky

21. Decomposition reaction-Copper carbonate 1.Set up apparatus as shown in the diagram. 2.Heat 3 spatulas of Copper carbonate in the hottest part of a Bunsen flame (use tongs) until you see the limewater turn cloudy. 3.REMOVE LIMEWATER test tube BEFORE you remove copper carbonate from the heat. 4.Describe copper carbonate. 5.Describe copper oxide 6.Describe carbon dioxide 7.Write a chemical equation for the reaction. 8.What was the reactant? 9.What were the products? 10.Lead carbonate reacts in a similar way to copper carbonate. Write a word equation for this reaction Write a chemical equation for this reaction. 11.How could you demonstrate that carbon dioxide was given off. Extension: Why did you need to add so much heat to make this reaction happen ? (link to addition reaction bond breaking and making).

22. Precipitation reactions Some chemical reactions occur without heating. If the REACTANTS are soluble but one of the PRODUCTS is insoluble a PRECIPITATE (suspended solid) will form.

23. Precipitation reactions e.g. Double displacement reactions. Sodium Carbonate Copper Sulfate Copper Carbonate Sodium Sulfate Soluble aq Soluble aq Soluble aq Insoluble Precipitate s

24. Precipitation reactions e.g. Double displacement reactions. Soluble aq Soluble aq Soluble aq Insoluble Precipitate s

25. Precipitation reactions 1.Describe copper sulfate solution. 2.Is copper sulfate soluble? 3.Describe sodium carbonate solution 4.Is sodium carbonate soluble 5.Mix 2cm 3 of copper sulfate solution with 2cm3 of sodium carbonate solution and record your observations. 6.Write a word equation for the reaction. 7.All sodium salts are soluble. In the reaction you have just done what is the name of the precipitate ? 8.Lead nitrate and sodium iodide are mixed, write a word equation for the reaction. 9.One of the products makes a precipitate, name the product.. 10.What is a precipitate?

26. Extension 1. Describe the solutions lead nitrate and potassium iodide. 2.Add two drops of lead nitrate to 2 drops of potassium iodide. 3. Describe the products Write a word equation for the reaction 4. Describe Mg and oxygen.EYES!!!! 5.Heat Mg in a blue bunsen flame 6. Remove from the flame. 7. Describe the product 8. Write word equation for the reaction 9.A star Q ‘’why does the Mg continue to burn after you have removed it from the heat.