1. Chemical Reactions (Energy)

2. I. Energy – Stored in Chemical ______, especially (__-__) bonds.

3. I. Energy – Stored in Chemical Bonds, especially (C-H) bonds. Different forms of energy: A. ________ energy (sunlight) B. ________ energy (chemical bonds) C. ________ energy (movement)

4. I. Energy – Stored in Chemical Bonds, especially (C-H) bonds. Different forms of energy: A. Radiant/Solar energy (sunlight) B. Chemical energy (chemical bonds) C. Kinetic/thermal energy (movement & heat)

5. II. Two Laws of Thermodynamics 1 st Law: Energy cannot be _________ or __________. It is simply ________________.

6. II. Two Laws of Thermodynamics 1 st Law: Energy cannot be created or destroyed. It is simply transferred. Example: Lawnmower gasoline = _______ E bonds break, ________ released Pressure increases, pistons _______

7. II. Two Laws of Thermodynamics 1 st Law: Energy cannot be created or destroyed. It is simply transferred. Example: Lawnmower gasoline = _bond E bonds break, heat released Pressure increases, pistons move **Overall Energy transfer: ______E to ______E **Respiration!! (Consume ______→_____)

8. II. Two Laws of Thermodynamics 1 st Law: Energy cannot be created or destroyed. It is simply transferred. Example: Lawnmower gasoline = bond E bonds break, heat released Pressure increases, pistons move **Overall Energy transfer: bond E to kinetic E **Respiration!! (Consume ______→_____)

9. II. Two Laws of Thermodynamics 1 st Law: Energy cannot be created or destroyed. It is simply transferred. Example: Lawnmower gasoline = bond E bonds break, heat released Pressure increases, pistons move **Overall Energy transfer: bond E to kinetic E **Respiration!! (Consume food → ATP)

10. II. Two Laws of Thermodynamics 2 nd Law: Entropy (disorganization) tends to ___________ as energy is transferred (over time). Ex) Chemical digestion ________________________ ________

11. II. Two Laws of Thermodynamics 2 nd Law: Entropy (disorganization) tends to _increase_ as energy is transferred. Ex) Chemical digestion ________________________ ________

12. II. Two Laws of Thermodynamics 2 nd Law: Entropy (disorganization) tends to _increase_ as energy is transferred. Ex) Chemical digestion 1 polypeptide _________ ________

13. II. Two Laws of Thermodynamics 2 nd Law: Entropy (disorganization) tends to _increase_ as energy is transferred. Ex) Chemical digestion 1 polypeptide 150 Amino Acids

14. II. Two Laws of Thermodynamics Increased disorder (entropy) is offset by biological processes that maintain order.

15. II. Two Laws of Thermodynamics Increased disorder (entropy) is offset by biological processes that maintain order. Living systems do not violate the _______Law (States that entropy increases with time)

16. II. Two Laws of Thermodynamics Increased disorder (entropy) is offset by biological processes that maintain order. Living systems do not violate the _2 nd Law (States that entropy increases with time) How is order maintained? By coupling processes that ________entropy with those that __________order.

17. II. Two Laws of Thermodynamics Increased disorder (entropy) is offset by biological processes that maintain order. Living systems do not violate the _2nd Law (States that entropy increases with time) How is order maintained? By coupling (stacking) processes that increase entropy with those that maintain order.

18. II. Two Laws of Thermodynamics Example: The making of a protein inside a cell: ________ ________ → _______________

19. II. Two Laws of Thermodynamics Example: The making of a protein inside a cell: Amino Acids → Polypeptide_

20. II. Two Laws of Thermodynamics Example: The making of a protein inside a cell: Use of ATP (1 st reaction) Amino Acids → Polypeptide_ (2 nd reaction) **Not a spontaneous reaction – ATP helps in maintaining order.

21. III. Endergonic Reactions Chemical reactions require “start-up” energy known as __________energy.

22. III. Endergonic Reactions Chemical reactions require “start-up” energy known as activation energy. Endergonic (Energy “___”) - Products have _________ free energy (positive ∆G) than reactants.

23. III. Endergonic Reactions Chemical reactions require “start-up” energy known as activation energy. Endergonic (Energy “in”) - Products have more free energy (positive ∆G) than reactants. Example: Photosynthesis ______ + ______ → ______ + _______

24. III. Endergonic Reactions Chemical reactions require “start-up” energy known as activation energy. Endergonic (Energy “in”): Products have more free energy (positive ∆G) than reactants. Example: Photosynthesis carbon dioxide + water → oxygen + glucose Energy Source???

25. IV. Exergonic Reactions Exergonic = Energy “____”- Products have ______ free energy (________ ∆G) than reactants.

26. IV. Exergonic Reactions Exergonic = Energy “out” - Products have less free energy (_________∆G) than reactants.

27. IV. Exergonic Reactions Exergonic = Energy “out” - Products have less free energy (_negative ∆G) than reactants.

28. IV. Exergonic Reactions Exergonic = Energy “out” - Products have less free energy (_negative ∆G) than reactants. Tend to be _________ spontaneous than endergonic reactions!

29. IV. Exergonic Reactions Exergonic = Energy “out” - Products have less free energy (_negative ∆G) than reactants. Tend to be more spontaneous than endergonic reactions! Require less Activation E! Example: Respiration _____ + _____ → ______ + _____+ _______

30. IV. Exergonic Reactions Exergonic = Energy “out” - Products have less free energy (_negative ∆G) than reactants. Tend to be more spontaneous than endergonic reactions! Require less Activation E! Example: Respiration oxygen + glucose → carbon dioxide + water + 36 ATPs

31. V. Free Energy Changes in a Reaction Lead to Changes in Entropy, Stability, and Capacity to do Work

32. More Free Energy at end of process (____________ reaction) means that Entropy is _____________

33. More Free Energy at end of process (Endergonic reaction) means that Entropy is _____________

34. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis CO 2 C 6 H 12 O 6 )

35. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis CO 2 C 6 H 12 O 6 ) Products are ___________ Stable.

36. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis CO 2 C 6 H 12 O 6 ) Products are _less_ Stable.

37. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis CO 2 C 6 H 12 O 6 ) Products are _less_ Stable. (Products have more bond E therefore, more likely to react)

38. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis CO 2 C 6 H 12 O 6 ) Products are _less_ Stable. (Products have more bond E therefore, more likely to react) Work Capacity (energy available to the cell) ______________.

39. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis CO 2 C 6 H 12 O 6 ) Products are _less_ Stable. (Products have more bond E therefore, more likely to react) Work Capacity (energy available to the cell) Increases. (Greater Work Capacity)

40. Less Free Energy at end of reaction = ___________ reaction (i.e. glucose → CO 2 in Respiration) means that:

41. Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO 2 in Respiration) means that:

42. Entropy is ____________.

43. Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO 2 in Respiration) means that: Entropy is Increased.

44. Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO 2 in Respiration) means that: Entropy is Increased. ________ _Stable_

45. Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO 2 in Respiration) Entropy is Increased. More _Stable_

46. Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO 2 in Respiration) means that: Entropy is Increased. More _Stable_ (Products have less bond E, therefore, are less likely to react)

47. Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO 2 in Respiration) means that: Entropy is Increased. More _Stable_(Products have less bond E, therefore, are less likely to react) ___________ Work Capacity

48. Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO 2 in Respiration) means that: Entropy is Increased. More _Stable_(Products have less bond E, therefore, are less likely to react) Decreased Work Capacity

49. Free Energy Changes Leads to Changes in Entropy, Stability, and Capacity to do Work 17. Refer to diagram B. Describe this chemical reaction in relation to entropy, stability & capacity to do work (hint: focus on the end product). A. B.