1.  Living organisms require energy to perform functions. They:  Kidney cells: › to transports materials  Digestive tract: › break macromolecules  Heart: › to pump

3. 3

4. Metabolism : Anabolism : Catabolism : 4

5. Energy : Energy can take many forms: mechanicalelectric current heat light All energy can be classified as: - kinetic energy : - potential energy : 5

6.  stored energy. › ___________________________________ 6

7. 7

8. Potential energy stored in chemical bonds can be transferred from one molecule to another by way of electrons. oxidation : reduction : redox reactions 8

9.  Energy of motion › ________________________________________ 9

10. http://www.youtube.com/watch?v=Jnj8m c04r9E 10

11.  Study of heat and energy flow within chemical reactions 11

12. First Law of Thermodynamics – For example: sunlight energy chemical energy photosynthesis 12

13.  Exercise to lose weight › produce heat and you sweat › heats the air around you.  When you eat a pizza › energy from the chemical bonds in the bread, cheese, etc. is broken down › converted into ATP molecules through cellular respiration. 13

14.  _______________________________________ _______________________________________  The enthalpy change (ΔH) › amount of heat released or absorbed when a chemical reaction occurs at a constant pressure. › ΔH formation = _____________________________ 14

15.  Reactants:  Activation energy (Ea):  Transition state:  Products: 15

16.  some of the reactant's potential energy is released into the surroundings as heat.  enthalpy of the products is ____________________  energy is _____________  ΔH is ____________ 16

17. http://cwx.prenhall.com/petrucci/mediali b/media_portfolio/text_images/019_THER MITE.MOV 17

18. 18

19. 19

20. 20

21. 21

22. Second Law of Thermodynamics : entropy : The 2 nd Law of Thermodynamics states that entropy is always increasing. 22

23. 23

24. Free energy : -denoted by the symbol G (Gibb’s free energy) enthalpy : free energy = enthalpy – (entropy x temp.) G = H - TS 24

25.  Chemical reactions can create changes in free energy.  When products contain more free energy than reactants  G is positive.  When reactants contain more free energy than products  G is negative. 25

26. Chemical reactions can be described by the transfer of energy that occurs: endergonic reaction : exergonic reaction : 26

27. 27

28. Most reactions require some energy to get started. activation energy : catalysts : 28

29. 29

30. C6H12O6 + O2 → CO2 + H2O + Energy (as ATP) ΔG = - 2870 kJ/mol of glucose  release of energy  an increase in entropy  This reaction tends to proceed spontaneously. 30

31. Photosynthesis Chemical Equation CO2 + H2O + Energy → C6H12O6 + O2 ΔG = + 2870 kJ/mol of glucose  energy is absorbed  a decrease in entropy  This reaction does not proceed spontaneously as energy is needed to drive the reaction. 31

32. ATP = adenosine triphosphate ATP structure: 32

33. 33

34. Adenosine Triphosphate (ATP) Section 9.1 P P A P

35. Mono = One phosphate group Di = Two phosphate groups Tri = three phosphates groups Adenosine Triphosphate (ATP) Section 9.1 P P A P

36. The battery of the cell Section 9.1

37. When the bond between phosphates is broken: ATP ADP + P i energy is released ADP = adenosine diphosphate P i = inorganic phosphate This reaction is reversible. 37

38. 38

39. 39

40.  Section 1.3, p.68 1, 2, 5, 10, 11 40