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
1st Law: Energy cannot be _________ or __________. It is simply ________________.

6. II. Two Laws of Thermodynamics
1st 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
1st 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
1st 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
1st 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
2nd Law: Entropy (disorganization) tends to ___________ as energy is transferred (over time).
Ex) Chemical digestion
_______________ _________ ________

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

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

13. II. Two Laws of Thermodynamics
2nd Law: Entropy (disorganization) tends to _increase_ as energy is transferred.
Ex) Chemical digestion
1 polypeptide 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 _2nd 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 (1st reaction)
Amino Acids → Polypeptide_ (2nd 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. . Activation energy- __________ amount of energy required to get a chemical reaction started.
minimum

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

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

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

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

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
_____ + _____ → ______ + _____+ _______

31. 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 ATPs

32. 4. Endergonic reactions= reactants have less energy than products (energy must go into reaction). 5. Exergonic reactions= reactants have more energy than products (energy leaves reaction).

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

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

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

36. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis
CO C6H12O6)

37. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis
CO C6H12O6)
Products are ___________ Stable.

38. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis
CO C6H12O6)
Products are _less_ Stable.

39. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis
CO C6H12O6)
Products are _less_ Stable. (Products have more bond E therefore, more likely to react)

40. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis
CO C6H12O6)
Products are _less_ Stable. (Products have more bond E therefore, more likely to react)
Work Capacity (energy available to the cell) ______________.

41. More Free Energy at end of process (Endergonic reaction) means that Entropy is Decreased. (Example: Photosynthesis
CO C6H12O6)
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)

42. Less Free Energy at end of reaction = ___________ reaction (i. e
Less Free Energy at end of reaction = ___________ reaction (i.e. glucose → CO2 in Respiration) means that:

43. Less Free Energy at end of reaction = Exergonic reaction (i. e
Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO2 in Respiration) means that:

44. Less Free Energy at end of reaction = Exergonic reaction (i. e
Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO2 in Respiration) means that:
Entropy is ____________.

45. Less Free Energy at end of reaction = Exergonic reaction (i. e
Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO2 in Respiration) means that:
Entropy is Increased.

46. Less Free Energy at end of reaction = Exergonic reaction (i. e
Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO2 in Respiration) means that:
Entropy is Increased.
________ _Stable_

47. Less Free Energy at end of reaction = Exergonic reaction (i. e
Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO2 in Respiration)
Entropy is Increased.
More _Stable_

48. Less Free Energy at end of reaction = Exergonic reaction (i. e
Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO2 in Respiration) means that:
Entropy is Increased.
More _Stable_ (Products have less bond E, therefore, are less likely to react)

49. Less Free Energy at end of reaction = Exergonic reaction (i. e
Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO2 in Respiration) means that:
Entropy is Increased.
More _Stable_(Products have less bond E, therefore, are less likely to react)
___________ Work Capacity

50. Less Free Energy at end of reaction = Exergonic reaction (i. e
Less Free Energy at end of reaction = Exergonic reaction (i.e. glucose → CO2 in Respiration) means that:
Entropy is Increased.
More _Stable_(Products have less bond E, therefore, are less likely to react)
Decreased Work Capacity

51. Free Energy Changes Leads to Changes in Entropy, Stability, and Capacity to do Work