1. Bond…. Bond Energy

2. All physical stuff is made of … –Matter! (Chemicals – atoms and molecules) In Chemical reactions, atoms rearrange to form new substances –(new molecules)

3. Conservation When new substances are made, the atoms themselves do not change. –They break their old bonds and form new ones. –Mass is CONSERVED! ENERGY is stored in a chemical bonds

4. Bond energies

5. Let’s make some molecules! One molecule of methane and two molecules of oxygen

6. Combustion of methane CH 4(g) + 2O 2(g) 2H 2 O (l) + CO 2(g)

7. Combustion of methane CH 4(g) + 2O 2(g) 2H 2 O (l) + CO 2(g) All reactions involve bond breaking and bond making as the atoms “swap partners”

8. Bond breaking - endothermic Energy is always required to be inputted to break a bond. Bond breaking is always endothermic.

9. Bond making - exothermic Energy is always released when a bond is formed. Bond making is always exothermic.

10. Bond energies The energy released when a bond is formed or absorbed when it is broken is called the bond energy. e.g. the C-H bond in methane has a bond energy of 413 KJ/mol

11. Examples of bond energies BondBond energy KJ/mol H-H436 Cl-Cl242 H-Cl431 C-H413 C-C347 C-O335 O-H464 O=O498

12. Energy level diagrams

13. Exothermic reaction The energy need to break the bonds is less than the energy released when new bonds are made “reaction path” energy CH 4(g) + 2O 2(g) C + 4H + 4O CO 2(g) + 2H 2 O (l) Energy needed to break bonds Energy released by forming bonds Energy released

14. Endothermic reaction The energy need to break the bonds is more than the energy released when new bonds are made “reaction path” energy NH 4 NO 3(s) + H 2 O (l) Energy needed to break bonds Energy released by forming bonds NH 4 NO 3(l) Energy absorbed

15. ΔH – Energy change in a complete reaction If heat is given out, the reaction has lost energy so ΔH is negative

16. ΔH – Energy change in a complete reaction If heat is absorbed (reaction gets colder), the reaction has gained energy so ΔH is positive

17. Calculating ΔH 2H 2(g) + O 2(g) 2H 2 O (l)

18. Calculating ΔH 2H 2(g) + O 2(g) 2H 2 O (l) Bonds broken = 2 x (H-H) + 1 x (O=O) = 2 x 436 + 1 x 498 = 872 + 498 = 1370 KJ/mol

19. Calculating ΔH 2H 2(g) + O 2(g) 2H 2 O (l) Bonds broken = 2 x (H-H) + 1 x (O=O) = 2 x 436 + 1 x 498 = 872 + 498 = 1370 KJ/mol Bonds made = 4 x (O-H) = 4 x -464 = -1856 KJ/mol

20. Calculating ΔH 2H 2(g) + O 2(g) 2H 2 O (l) Bonds broken = 2 x (H-H) + 1 x (O=O) = 2 x 436 + 1 x 498 = 872 + 498 = 1370 KJ/mol Bonds made = 4 x (O-H) = 4 x -464 = -1856 KJ/mol Overall Energy change = 1370 + (-1856) = -486 KJ/mol (Exothermic)

21. Energy in the Chemical Equations Because Energy is released (exothermic), include it as a product: 2H 2(g) + O 2(g) 2H 2 O (l) + Energy If Energy is absorbed (endothermic), you would include it as a reactant!

22. How well have you understood?

23. Bond energies?

24. Energy level diagrams?

25. Using bond energies in calculations?

26. Let’s try Another! CH 4(g) + 4Cl 2(g) CCl 4(g) + 4HCl (g) BondBond energy KJ/mol C-H413 H-Cl431 Cl-Cl242 C-Cl328 C-C347 C-O335 O=O498

29. Homework Homework Book pages 60 – 61 Due TOMORROW Lab Tomorrow as well!

30. Combustion of methane?