1. Exothermic Reactions HOT OR COLD

2. Lesson Objectives We are learning to:- Identify exothermic and endothermic reactions What I’m Looking For:- You must be able to be able to assign thermic reactions as +ΔH or –ΔH You should be able to construct a simple energy level diagram for endo- and exo- thermic reaction You should be able to calculate the energy change in a reaction using bond enthalpies

3. Magnesium + Hydrochloric acid Gets hot 25 o C 45 o C magnesium Hydrochloric acid Heat energy given out Exothermic Reactions

4. If heat is given out this energy must have come from chemical energy in the starting materials (reactants). Reactants convert chemical energy to heat energy. The temperature rises. 25 o C 45 o C Exothermic Reactions

5. 45 o C Almost immediately the hot reaction products start to lose heat to the surroundings and eventually they return to room temperature. 25 o C Chemical energy becomes heat energy. The reaction mixture gets hotter. Eventually this heat is lost to the surroundings. It follows that reaction products have less chemical energy than the reactants had to start with. Exothermic Reactions

6. Energy / kJ) Progress of reaction (time) Energy Level Diagram for an Exothermic Reaction reactants Reactants have more chemical energy. Some of this is lost as heat which spreads out into the room. products Products now have less chemical energy than reactants.

7. Energy / kJ Progress of reaction reactants products  H=negative Energy Level Diagram for an Exothermic Reaction 2.  H is how much energy is given out  H is negative because the products have less energy than the reactants. Energy Level Diagram for an Exothermic Reaction

8. Exothermic reactions give out energy. There is a temperature rise and  H is negative. Exothermic Reaction - Definition products Energy / kJ) Progress of reaction reactants  H is negative

9. Activity

10. Endothermic Reactions Endothermic chemical reactions are relatively rare. A few reactions that give off gases are highly endothermic - get very cold. Dissolving salts in water is another process that is often endothermic. Endothermic reactions cause a decrease in temperature.

11. Cools Heat energy taken in as the mixture returns to room temp. Starts 25°C Cools to 5°C Ammonium nitrate Water Endothermic reactions cause a decrease in temperature. Returns to 25°C Endothermic Reactions

12. Extra energy is needed in order for endothermic reactions to occur. This comes from the thermal energy of the reaction mixture which consequently gets colder. Reactants convert heat energy into chemical energy as they change into products. The temperature drops. 25 o C 5 o C Endothermic Reactions

13. 25 o C The cold reaction products start to gain heat from the surroundings and eventually return to room temperature. 5 o C The reactants gain energy. 25 o C This comes from the substances used in the reaction and the reaction gets cold. Eventually heat is absorbed from the surroundings and the mixture returns to room temperature. Overall the chemicals have gained energy. Endothermic Reactions

14. products Energy / kJ) Progress of reaction reactants  H=+ Energy Level Diagram for an Endothermic Process This is positive because the products have more energy than the reactants. This is how much energy is taken in

15. Endothermic reactions take in energy. There is a temperature drop and  H is positive. Endothermic Reaction Definition  H=+ products Energy / kJ Progress of reaction reactants

16. Exothermic reactions give out energy. There is a temperature rise and  H is negative. Exothermic Reaction - Definition products Energy / kJ) Progress of reaction reactants  H is negative

17. Activity

18. Endothermic Reactions Endothermic chemical reactions are relatively rare. A few reactions that give off gases are highly endothermic - get very cold. Dissolving salts in water is another process that is often endothermic. Endothermic reactions cause a decrease in temperature.

19. Are these endothermic or exothermic? 1.A red glow spread throughout the mixture and the temperature rose. 2.The mixture bubbled vigorously but the temperature dropped 15 0 C. 3.Hydrazine and hydrogen peroxide react so explosively and powerfully that they are used to power rockets into space. 4.The decaying grass in the compost maker was considerably above the outside temperature. exo endo exo Activity

20. Sketch the two energy diagrams and label exothermic and endothermic as appropriate.  H=+ products Energy / kJ Progress of reaction reactants products Energy / kJ) Progress of reaction reactants  H=- Activity

21. Breaking chemical bonds Most chemicals will decompose (break up) if we heat them strongly enough. This indicates that breaking chemical bonds requires energy – is an endothermic process. Heat taken in Energy needed to overcome the bonding between the atoms Energy in chemicals Energy needed

22. Making chemical bonds It is reasonable to assume that bond making will be the opposite of bond breaking Energy will be given out in an exothermic process when bonds are formed. Heat given out Energy given out as bonds form between atoms Energy in chemicals Energy given out

23. Changes to chemical bonds Endothermic Reactions In most chemical reactions some existing bonds are broken (endothermic) Energy taken in as old bonds break But new bonds are made (exothermic) Energy in chemicals reactants products Energy given out as new bonds form HH Overall endothermic in this case

24. Changes to chemical bonds Exothermic Reactions Again some existing bonds are broken (endothermic) Energy taken in as old bonds break And new bonds are formed (exothermic) Energy in chemicals reactants products Energy given out as new bonds form HH Overall exothermic – in this case

25. Summary – Bond Changes Where the energy from bond forming exceeds that needed for bond breaking the reaction is exothermic. Where the energy for bond breaking exceeds that from bond forming the reaction is endothermic. Energy in chemicals reactants products HH Bonds break Bond forming Energy in chemicals reactants products HH Bonds break Bonds form Exo Endo