1. Big Idea 2: Cellular Processes in Biological systems
Energy
Growth
Reproduction
Dynamic Homeostasis

2. Learning Objectives:
LO 2.1 The student is able to explain how biological systems use free energy based on empirical data that all organisms require constant energy input to maintain organization, to grow and to reproduce.

3. Learning Objectives:
LO 2.2 The student is able to justify a scientific claim that free energy is required for living systems to maintain organization, to grow or to reproduce, but that multiple strategies exist in different living systems.

4. Learning Objectives:
LO 2.3 The student is able to predict how changes in free energy availability affect organisms, populations and ecosystems.

5. Enduring understanding 2.A:
Growth, reproduction and maintenance of the organization of living systems require free energy and matter.

6. Energy
Energy is the capacity to do work or ability to cause change. Any change in the universe requires energy. Energy comes in 2 forms:
Potential energy is stored energy. No change is currently taking place
Kinetic energy causes change. This always involves some type of motion.

8. 1st Law of Thermodynamics: Energy can be changed from one form to another, but it cannot be created or destroyed. The total amount of energy and matter in the Universe remains constant; it only changes from one form to another.

9. 2nd Law of Thermodynamics: “In all energy exchanges, if no energy enters or leaves the system, the potential energy of the state will always be less than that of the initial state." This is also commonly referred to as entropy.

10. Entropy
It is a measure of disorder: cells are NOT disordered and so have low entropy. In the process of energy transfer, some energy will dissipate as heat. The flow of energy maintains order and life. Entropy wins when organisms cease to take in energy and die.

12. Biological systems follow the laws of thermodynamics, and to offset entropy, energy input must exceed energy lost from and used by an organism to maintain order.

13. Carbohydrate Metabolism
heat
muscle contraction
carbohydrate
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14. Not only can energy deficiencies be detrimental to individual organisms, but changes in free energy availability also can affect population size and cause disruptions at the ecosystem level.

16. Organisms use various energy-related strategies to survive; strategies include different metabolic rates, physiological changes, and variations in reproductive and offspring-raising strategies.

17. Cells and Energy a. Glucose Carbon dioxide and water H2O energy CO2
•more organized
• less stable
• less organized
• more potential energy
• less potential energy
• more stable
low entropy
high entropy
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18. b. Unequal distribution of hydrogen ions+ + H + H
channel protein + H H +
energy + + + H H + H H + H + H + H + + H + H + + H H + H H
Unequal distribution of hydrogen ions
Equal distribution of hydrogen ions
• more organized
• less organized
• more potential energy
• less potential energy
• less stable
• more stable
low entropy
high entropy
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19. All living systems require constant input of free energy
Life requires a highly ordered system.
1. Order is maintained by constant free energy input into the system.
2. Loss of order or free energy flow results in death.
3. Increased disorder and entropy are offset by biological processes that maintain or increase order.

20. The First Law of Thermodynamics
Energy cannot be created or destroyed
Energy can be transferred and transformed
For example, the chemical (potential) energy
in food will be converted to the kinetic
energy of the cheetah’s movement
Chemical
energy

22. Free Energy:
It is the portion of a system’s energy that is able to perform work when temperature and pressure is uniform throughout the system, as in a living cell
Free energy also refers to the amount of energy actually available to break and subsequently form other chemical bonds

23. Free Energy:
Gibbs’ free energy (G): in a cell, the amount of energy contained in a molecule’s chemical bonds
Δ = change
G = free energy
Change in free energy= ΔG and it is calculated as:
energy left in products – energy content of reactants
-ΔG = products have less energy than reactants, and the reaction will occur spontaneously.
+ΔG = products have more energy than the reactants, and the reaction will occur only if there is a constant input of energy

24. Free Energy:
-ΔG reactions are exergonic (free energy releasing reactions)
+ΔG reactions are reactions that requires an input of free energy
Exergonic reactions (G < 0) or
Endergonic reactions (G > 0)
on the basis of whether the free energy of the system decreases or increases during the reaction.

25. Gibbs Free Energy

26. Example 1:

27. HCl(aq) + NaOH(aq)  H2O(l) + NaCl
Example 2
Find the change is Gibbs Free Energy for the reaction at 310C:
HCl(aq) + NaOH(aq)  H2O(l) + NaCl

28. Exergonic reactions (G < 0) or Endergonic reactions (G > 0)

29. Calculate ΔH° and ΔS° for the following reaction:
NH4NO3(s)  + H2O(l)    NH4+ (aq) + NO3- (aq)

30. b) Living systems do not violate the second law of thermodynamics, which states that entropy increases over time. 1. Order is maintained by coupling cellular processes that increase entropy (and so have negative changes in free energy) with those that decrease entropy (and so have positive changes in free energy). 2. Energy input must exceed free energy lost to entropy to maintain order and power cellular processes. 3. Energetically favorable exergonic reactions, such as ATP→ADP, that have a negative change in free energy can be used to maintain or increase order in a system by being coupled with reactions that have a positive free energy change.

32. Exergonic reactions Reactants have more free energy than the products
Involve a net release of energy and/or an increase in entropy
Occur spontaneously (without a net input of energy)
Reactants
Products
Energy
Progress of the reaction
Amount of
energy
released (∆G <0)
Free energy
(a) Exergonic reaction: energy released

33. Endergonic Reactions Reactants have less free energy than the products
Involve a net input of energy and/or a decrease in entropy
Do not occur spontaneously
Energy
Products
Amount of
energy
released (∆G>0)
Reactants
Progress of the reaction
Free energy
(b) Endergonic reaction: energy required

34. Endergonic Exergonic Energy released Product Reactant Reactant Product
Energy supplied
Endergonic
Exergonic
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35. Metabolic Reactions and Energy Transformations
Biology, 9th ed,Sylvia Mader
Chapter 06
Metabolic Reactions and Energy Transformations
Metabolism:
Sum of cellular chemical reactions in cell
Reactants participate in reaction
Products form as result of reaction
Free energy is the amount of energy available to perform work
Exergonic Reactions - Products have less free energy than reactants
Endergonic Reactions - Products have more free energy than reactants
Metabolism

36. ATP and Coupled Reactions
Adenosine triphosphate (ATP)
High energy compound used to drive metabolic reactions
Constantly being generated from adenosine diphosphate (ADP)
Composed of:
Adenine and ribose (adenosine), and
Three phosphate groups
Coupled reactions
Energy released by an exergonic reaction captured in ATP
That ATP used to drive an endergonic reaction

37. adenosine triphosphate
Energy for endergonic reactions
(e.g., protein synthesis, nerve
conduction, muscle contraction)
Energy from exergonic reactions
(e.g., cellular respiration) a.
ATP b. P + P P
inorganic phosphate
adenosine diphosphate
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38. Synthesis of ATP

39. Work-Related Functions of ATP:
Primarily to perform cellular work
Chemical Work: Energy needed to synthesize macromolecules
Transport Work: Energy needed to pump substances across plasma membrane
Mechanical Work: Energy needed to contract muscles, beat flagella, etc.

40. Life Requires Energy

41. Reactions are usually occur in a sequence “A” is Initial Reactant
Metabolic Pathways
Reactions are usually occur in a sequence
Products of an earlier reaction become reactants of a later reaction
Begins with a particular reactant
Proceeds through several intermediates
Terminates with a particular end product
AB C D E FG
“G” is End Product
“A” is Initial Reactant
B, C, D, E, and F
are Intermediates

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43. Krebs cycle Glycolysis Calvin cycle Fermentation
c) Energy-related pathways in biological systems are sequential and may be entered at multiple points in the pathway.
Krebs cycle
Glycolysis
Calvin cycle
Fermentation

44. Biological Order and Disorder
Cells create ordered structures from less ordered materials
Organisms also replace ordered forms of matter and energy with less ordered forms
The evolution of more complex organisms does not violate the second law of thermodynamics
Entropy (disorder) may decrease in an organism, but the universe’s total entropy increases

45. Biological Order and Disorder
Living systems
Increase the entropy of the universe
Use energy to maintain order
A living system’s free energy is energy that can do work under cellular conditions
Organisms live at the expense of free energy
50µm

47. Metabolism: Part 1

48. Equilibrium and Metabolism
Reactions in a closed system eventually reach equilibrium and then do no work
Cells are not in equilibrium; they are open systems experiencing a constant flow of materials

49. Equilibrium and Metabolism
A catabolic pathway in a cell releases free energy in a series of reactions

50. Equilibrium and Metabolism
Closed and open hydroelectric systems can serve as analogies

51. Equilibrium and Metabolism
Closed and open hydroelectric systems can serve as analogies
(b) An open hydroelectric system. Flowing water keeps driving the generator because intake and outflow of water keep the system from reaching equlibrium.
∆G < 0

52. (c) A multistep open hydroelectric system
(c) A multistep open hydroelectric system. Cellular respiration is analogous to this system:
Glucose is broken down in a series of exergonic reactions that power the work of the cell.
The product of each reaction becomes the reactant for the next, so no reaction reaches equilibrium.

53. Equilibrium and Metabolism
Cells in our body experience a constant flow of materials in and out, preventing metabolic pathways from reaching equilibrium

54. Energy Coupling
Living organisms have the ability to couple exergonic and endergonic reactions:
Energy released by exergonic reactions is captured and used to make ATP from ADP and Pi
ATP can be broken back down to ADP and Pi, releasing energy to power the cell’s endergonic reactions.

55. The Structure and Hydrolysis of ATP
ATP (adenosine triphosphate)
Is the cell’s energy shuttle
Provides energy for cellular functions O
CH2 H OH N C HC
NH2
Adenine
Ribose
Phosphate groups - CH

56. The Structure and Hydrolysis of ATP
Energy is released from ATP when the terminal phosphate bond is broken P
Adenosine triphosphate (ATP)
H2O +
Energy
Inorganic phosphate
Adenosine diphosphate (ADP)
P i

57. Cellular Work A cell does three main kinds of work Mechanical
Transport
Chemical
Energy coupling is a key feature in the way cells manage their energy resources to do this work
ATP powers cellular work by coupling exergonic reactions to endergonic reactions

58. Energy Coupling - ATP / ADP Cycle
Releasing the third phosphate from ATP to make ADP generates energy (exergonic):
Linking the phosphates together requires energy - so making ATP from ADP and a third phosphate requires energy (endergonic),
Catabolic pathways drive the regeneration of ATP from ADP and phosphate
ATP synthesis from
ADP + P i requires energy
ATP
ADP + P i
Energy for cellular work
(endergonic, energy-
consuming processes)
Energy from catabolism
(exergonic, energy yielding
processes)
ATP hydrolysis to
ADP + P i yields energy

59. How ATP Performs Work?
ATP drives endergonic reactions by phosphorylation, transferring a phosphate group to some other molecule, such as a reactant
The recipient molecule is now phosphorylated
The three types of cellular work (mechanical, transport, and chemical) are powered by the hydrolysis of ATP

60. ATP drives endergonic reactions by phosphorylation, transferring a phosphate to other molecules - hydrolysis of ATP: mechanical

61. ATP drives endergonic reactions by phosphorylation, transferring a phosphate to other molecules - hydrolysis of ATP: transport

62. ATP drives endergonic reactions by phosphorylation, transferring a phosphate to other molecules - hydrolysis of ATP: chemical

63. Activation Energy
All reactions, both endergonic and exergonic, require an input of energy to get started. This energy is called activation energy
The activation energy, EA
Is the initial amount of energy needed to start a chemical reaction
Activation energy is needed to bring the reactants close together and weaken existing bonds to initiate a chemical reaction.
Is often supplied in the form of heat from the surroundings in a system.
Free energy
Progress of the reaction
∆G < O EA A B C D
Reactants
Transition state
Products
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64. Reaction Rates
In most cases, molecules do not have enough kinetic energy to reach the transition state when they collide.
Therefore, most collisions are non-productive, and the reaction proceeds very slowly if at all.
What can be done to speed up these reactions?

65. Increasing Reaction Rates
Add Energy (Heat) - molecules move faster so they collide more frequently and with greater force.

66. Increasing Reaction Rates
Add a catalyst – a catalyst reduces the energy needed to reach the activation state, without being changed itself. Proteins that function as catalysts are called enzymes.
Activation Energy and Catalysis
Energy supplied
Activation
energy
Activation
energy
Reactant
Reactant
Energy released
Product
Product
Uncatalyzed
Catalyzed
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67. Peroxidase Enzyme Activity Advanced Inquiry Lab
Peroxidase enzymes are widely distributed in plants and animals, including bacteria, to protect cells against the effects of oxidative stress and cell damage due to hydrogen peroxide.
Certain enzymes within the peroxisome, use O2, and remove hydrogen atoms from specific organic substrates in an oxidative reaction, producing hydrogen peroxide (H2O2)

68. Peroxidase Enzyme Activity Advanced Inquiry Lab
Peroxidases are easily extracted from turnips and other root vegetables and provide a model enzyme for studying enzyme activity—how the rate of an enzyme-catalyzed reaction depends on biotic and abiotic factors. Enzyme activity studies reflect enzyme structure and function and provide the foundation for understanding the mechanism or theory of enzyme action.

69. Until next time…