Energy and Metabolism

1. Energy and Metabolism

2. Flow of Energy Energy: the capacity to do work -kinetic energy: the energy of motion -potential energy: stored energy

3. Energy forms are inter-convertible

4. Flow of Energy • Most forms of energy can be converted to heat energy. • Thermodynamics = “heatchanges” • 3(2) laws of thermodynamics • Heat energy is measured in kilocalories. • One calorie = the amount of heat required to raise the temp of 1 g of water by 1oC • 1 kilocalorie (kcal) = 1000 calories

5. 13 x 1023 calories/year 4 x 1013 calories/second

6. Flow of Energy Potential energy stored in chemical bonds can be used to do work – breaking bonds can release energy. Potential energy stored in chemical bonds can also be converted to other energy forms. There is always a loss of heat energy in these reactions Bond Bond Energy (kcal/mol) C–H 100 C–O 86 C–N 70 C–C 85 N–H 93

7. 13 x 1023 calories/year 4 x 1013 calories/second heat

8. Flow of Energy Potential energy stored in chemical bonds can be transferred from one molecule to another by way of electrons. oxidation: loss of electrons reduction: gain of electrons redox reactions are coupled to each other.

10. Laws of Thermodynamics First Law of Thermodynamics

12. Laws of Thermodynamics First Law of Thermodynamics – energy cannot be created or destroyed…energy can only be converted from one form to another For example: sunlight energy chemical energy photosynthesis

13. Energy in universe Energy in universe Available to do work Total amount of energy in universe remains constant, but energy available to do work decreases as heat is lost

14. Laws of Thermodynamics Second Law of Thermodynamics

15. Laws of Thermodynamics Second Law of Thermodynamics: disorder is more likely than order entropy: disorder in the universe The 2nd Law of Thermodynamics states that entropy is always increasing.

17. Laws of Thermodynamics • The British scientist and author C.P. Snow had an excellent way of remembering these laws: • You cannot win (that is, you cannot get something for nothing, because matter and energy are conserved). • You cannot break even (you cannot return to the same energy state, because there is always an increase in disorder; entropy always increases).

18. Laws of Thermodynamics Free energy: the energy available to do work -denoted by the symbol G (Gibb’s free energy) enthalpy: energy contained in a molecule’s chemical bonds free energy = enthalpy – (entropy x temp.) G = H - TS

19. Laws of Thermodynamics • Chemical reactions can create changes in free energy: • DG = DH - T DS • When products contain more free energy than reactants – DG is positive. • When reactants contain more free energy than products – DG is negative.

20. Laws of Thermodynamics Chemical reactions can be described by the transfer of energy that occurs: endergonic reaction: a reaction requiring an input of energy - DG is positive exergonic reaction: a reaction that releases free energy - DG is negative

22. ΔG and Spontaneous Processes • ΔG= ΔH - TΔS • • Note that ΔG is composite of both ΔH and ΔS • • A reaction is spontaneous if ΔG < 0. Such that: • If ΔH < 0 and ΔS > 0....spontaneous at any T • If ΔH > 0 and ΔS < 0....not spontaneous at any T • If ΔH < 0 and ΔS < 0....spontaneous at low T • If ΔH > 0 and ΔS > 0....spontaneous at high T

24. Laws of Thermodynamics Most reactions require some energy to get started. activation energy: extra energy needed to get a reaction started -destabilizes existing chemical bonds -required even for exergonic reactions catalysts: substances that lower the activation energy of a reaction

26. Energy Currency of Cells ATP= adenosine triphosphate -the energy “currency” of cells ATP structure: -ribose, a 5-carbon sugar -adenine -three phosphates

28. Energy Currency of Cells ATP stores energy in the bonds between phosphates. Phosphates are highly negative, therefore: -the phosphates repel each other -much energy is required to keep the phosphates bound to each other -much energy is released when the bond between two phosphates is broken

29. Energy Currency of Cells When the bond between phosphates is broken: ATP ADP + Pi energy is released ADP = adenosine diphosphate Pi = inorganic phosphate This reaction is reversible.

31. Energy Currency of Cells The energy released when ATP is broken down to ADP can be used to fuel endergonic reactions. The energy released from an exergonic reaction can be used to fuel the production of ATP from ADP + Pi.

32. Enzymes Enzymes: molecules that catalyze reactions in living cells -most are proteins -lower the activation energy required for a reaction -are not changed or consumed by the reaction

33. Enzymes Enzymes interact with substrates. substrate: molecule that will undergo a reaction active site:region of the enzyme that binds to the substrate Binding of an enzyme to a substrate causes the enzyme to change shape, producing a better induced fit between the molecules.

36. Enzymes Multienzyme complexes offer certain advantages: 1. The product of one reaction can be directly delivered to the next enzyme. 2. The possibility of unwanted side reactions is eliminated. 3. All of the reactions can be controlled as a unit.

37. Enzymes Not all enzymes are proteins. Certain reactions involving RNA molecules are catalyzed by the RNA itself. ribozymes: RNA with enzymatic abilities For example, the ribosome is a ribozyme.

38. Enzymes Enzyme function is affected by its environment. Factors that can change an enzyme’s 3-dimensional shape can change its function. -for example, pH, temperature, regulatory molecules

39. Enzymes Temperature -enzyme activity may be increased with increasing temp, up to the temp optimum -temperatures too far above the temp optimum can denature the enzyme, destroying its function pH – most enzymes prefer pH values from 6 to 8.

41. Enzymes Inhibitors are molecules that bind to an enzyme to decrease enzyme activity. -competitive inhibitors compete with the substrate for binding to the same active site -noncompetitive inhibitors bind to sites other than the enzyme’s active site

42. Enzymes Allosteric enzymes exist in either an active or inactive state. -possess an allosteric site where molecules other than the substrate bind -allosteric inhibitors bind to the allosteric site to inactivate the enzyme allosteric activators bind to the allosteric site to activate the enzyme

44. Metabolism Metabolism: all chemical reactions occurring in an organism Anabolism: chemical reactions that expend energy to make new chemical bonds Catabolism: chemical reactions that harvest energy when bonds are broken

45. Metabolism Some enzymes require additional molecules for proper enzymatic activity. These molecules could be: -cofactors: usually metal ions, found in the active site participating in catalysis -coenzymes: nonprotein organic molecules, often used as an electron donor or acceptor in a redox reaction

46. Metabolism Biochemical pathways are a series of reactions in which the product of one reaction becomes the substrate for the next reaction. Biochemical pathways are often regulated by feedback inhibition in which the end product of the pathway is an allosteric inhibitor of an earlier enzyme in the pathway.